EPA-560/5-77-003
REVIEW OF THE ENVIRONMENTAL
FATE OF SELECTED CHEMICALS
May 1977
Task 3
FINAL REPORT
Office of Toxic Substances
U.S. Environmental Protection Agency
Washington, D.C. 20460
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Document is available to the public through the National Technical Information Service Springfield, Virginia 22151
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STANFORD RESEARCH INSTITUTE
Menlo Park, California 94025 • U.S.A.
EPA-560/5-77-003
Review of the Environmental Fate
of Selected Chemicals
Shirley B. Radding
David H. Liu
Howard L. Johnson
Theodore* Mill
May 1977
Contract No. 68-01-2681
Project Officer - James Darr
Prepared for
Office of Toxic Substances
U.S. Environmental Protection Agency
Washington, D. C. 20460
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NOTICE
This report has been reviewed by the Office of Toxic Substances, EPA,
and approved for publication. Approval does not signify that the contents
necessarily reflect the views and policies of the Environmental Protection
Agency, nor does mention of trade names or commercial products constitute
endorsement or recommendation for use.
ill
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ABSTRACT
A review of the recent literature on sources, production, environ-
mental fate, and bioaccumulation has been carried out by SRI on 26 classes
of compounds. These included epoxides, haloolefins, aldehydes, alkyl and
benzyl halides, peroxides, hydroperoxides and peracids, polyhalomethanes,
aromatic amines, polychlorinated biphenyls, azo dyes, carbamic acid esters,
hydrazines, acyl halides and ketene, phosphoric acid esters, aziridines,
lactones, alkyl sulfates, sultones, aryl dialkyltriazenes, diazoalkanes,
haloalcohols, haloethers, hydroxylamines, nitrosamines, nitrofurans, and
azides.
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CONTENTS
ABSTRACT v
LIST OF TABLES xi
1. INTRODUCTION 1
2. SUMMARY, CONCLUSIONS, AND RECOMMENDATIONS 9
3. METHODOLOGY 13
Literature Search 13
Estimation Procedures for Persistence 13
Kinetic Relationships 13
Chemical Transformations in the Environment 14
Partition Coefficients 28
4. EPOXIDES 37
Production and Properties 37
Environmental Transformation 40
Bioaccumulation 40
5. HALOOLEFINS 43
Production and Properties 43
Environmental Transformations 46
Bioaccumulation 46
6 ALDEHYDES 49
Production and Properties 49
Environmental Transformation 52
Bioaccumulation 52
7 ALKYL AND BENZYL HALIDES 55
Production and Properties 55
Environmental Transformation 59
Bioaccumulation 60
8 PEROXIDES, HYDROPEROXIDES, PERACIDS, AND HYDROGEN PEROXIDE . 63
Production and Properties 63
Environmental Transformation 0 . 66
Bioaccumulation 67
vii
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9. POLYHALOMETHANES 69
Production and Properties
Environmental Transformation
72
Bioaccumulation
10. AROMATIC AMINES 73
•70
Production and Properties
•7O
Environmental Transformation /J
Bioaccumulation '«
11. POLYCHLORINATED BIPHENYLS 79
Production and Properties 79
Environmental Transformation 79
Bioaccumulation 81
12. AZO DYES
Production and Properties 83
Environmental Transformation 81
Bioaccumulation 86
13. CARBAMIC ACID ESTERS 87
Production and Properties 87
Environmental Transformation 87
Bioaccumulation 88
14. HYDRAZINES 89
Production and Properties 89
Environmental Transformation 89
Bioaccumulation 91
15. ACYL HALIDES AND KETENE 93
Production and Properties 93
Environmental Transformation 95
Bioaccumulation 95
16. PHOSPHORIC ACID ESTERS 97
Production and Properties 97
Environmental Transformation 97
Bioaccumulation 99
viii
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17. AZIRIDINES 101
Production and Properties 101
Environmental Transformation 101
Bioaccumulation 103
18. LACTONES 105
Production and Properties 105
Environmental Transformation 105
19. ALKYL SUUFATES , 107
Production and Properties 107
Environmental Transformation .... 1Q7
Bioaccumulation 109
20. SULTONES Ill
Production and Properties Ill
Environmental Transformation Ill
Bioaccumulation Ill
21. ARYL DIALKYLTRIAZENES 113
Production and Properties 113
Environmental Transformation 113
Bioaccumulation 114
22. DIAZOALKANES 115
Production and Properties 115
Environmental Transformation 115
Bioaccumulation 116
23. HALOALCOHOLS
Production and Properties 117
Environmental Transformation 117
Bioaccumulation 117
24. HALOETHERS 119
Production and Properties 119
Environmental Transformation 119
Bioaccumulation 122
ix
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25. HYDROXYLAMINES 123
Production and Properties 123
Environmental Transformation 123
Bioaccumulation 1^
26. NITROSAMINES 127
Production and Properties 127
Environmental Transformation 127
Bioaccumulation 129
27. NITROFURANS 131
Production and Properties 131
Environmental Transformation 131
Bioaccumulation 132
28. AZIDES 133
Production and Properties 133
Environmental Transformation 133
Bioaccumulation 134
29. REFERENCES
135
x
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TABLES
1. Suspected Carcinogens Studied 2
2. Rate Constants and Half-Lives for Reaction of HO Radical 16
with Organic Compounds
3. Rate Constants and Half-Lives for Hydrolysis of
Organic Compounds 23
4. Partition Coefficients 30
5. Producers and Locations for Epoxides 37
6. Physical and Chemical Properties of Epoxides 39
7. Producers and Locations for Haloolefins 43
8. Physical and Chemical Properties of Haloolefins 45
9. Producers and Locations for Aldehydes 49
10. Physical and Chemical Properties of Aldehydes 51
11. Producers and Locations for Alkyl Halides 56
12. Physical and Chemical Properties of Alkyl and Benzyl
Halides 57
13. Producers and Locations for Peroxides 63
14. Physical and Chemical Properties of Peroxides 65
15. Producers and Locations for Polyhalomethanes 70
16. Physical and Chemical Properties of Polyhalomethanes ... 71
17. Producers and Locations for Aromatic Amines 74
18. Physical and Chemical Properties of Aromatic Amines .... 75
19. Physical Properties of Chlorobiphenyls 80
20. Physical and Chemical Properties of Azo Dyes 85
21. Physical and Chemical Properties of Hydrazines 90
22. Physical and Chemical Properties of Acylating Agents ... 94
23. Physical and Chemical Properties of Phosphoric Acid Esters. 98
24. Physical and Chemical Properties of Aziridines 102
25. Physical and Chemical Properties of Alkyl Sulfates .... 108
xi
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26. Physical and Chemical Properties of Haloalcohols 118
27. Physical and Chemical Properties of Haloethers 121
28. Physical and Chemical Properties of Hydroxylamines .... 124
29. Physical and Chemical Properties of Nitrosamines 128
xii
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1. INTRODUCTION
The Office of Toxic Substances (OTS), U.S. Environmental Protection
Agency (EPA), requested SRI to conduct a literature search and evaluation
of the results for the suspected carcinogens listed in Table 1. The EPA
is concerned with information and estimates of the entry and behavior of
these compounds in the environment. A literature search was conducted to
determine what information is available on these compounds to attempt to
predict their environmental fates and the likelihood of their accumulation
in mammals, particularly humans.
The fate of chemicals in the environment depends on a variety of
chemical, physical, and biological interactions, few of which have been
studied in enough detail to predict either the dominant pathways for
transformation or the rates of change in concentration associated with
those pathways. Previous studies have shown that it is difficult to
determine losses of material from manufacturing sites and that the
eventual fate of the material in the environment cannot be predicted on
the basis of published information. However, some intelligent guesses
can be made based on structural analogies within classes of compounds.
For this purpose, emphasis was placed on searching for or estimating
kinetic values for potentially important pathways of chemical degra-
dation, including free radical oxidation, photolysis, and hydrolytic
reactions. Partition coefficients (octanol/water) were calculated for
each compound as one measure of the propensity for biological uptake.
Literature reports on biological uptake and metabolism of these com-
pounds were also reviewed and evaluated.
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Table 1
SUSPECTED CARCINOGENS STUDIED
Class/Name
Epoxides
Ethylene oxide
Propylene oxide
Epichlorohydrin
Styrene oxide
Glycidol
Glycidaldehyde
Haloolef ins
Vinyl chloride
Trichloroethylene
Vinylidene chloride
Chloroprene
CAS Number
75-21-8
75-56-9
106-89-8
96-09-3
556-52-5
765-34-4
75-01-4
79-01-6
75-35-4
126-99-8
Formula
C H 0
2 4
C H O
3 6
C8H8°
C H 0
362
C H O
342
C H Cl
233
C H Cl
222
Aldehydes
Formaldehyde
Acrolein
50-00-0
107-02-8
CH O
Dihaloalkanes
1,2-Ethylene dibromide
1,2-Ethylene dichloride
Polyhalomethanes
Carbon tetrachloride
Chloroform
106-93-4
107-06-0
56-23-3
67-66-3
C H Br
242
C H Cl
242
CGI.
4
CHCl
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Table 1 (continued)
SUSPECTED CARCINOGENS STUDIED
Class/Name
Peroxides
Cumene hydroperoxide
Di-tert-butyl peroxide
Hydrogen peroxide
tert-Butyl hydroperoxide
Succinic acid peroxide
Aromatic amines
4,4'-Methylenebis(2-
chloroaniline)
1-Naphthylamine
3,3-Dichlorobenzidine
Benzidine
2-Biphenylamine
4-Biphenylamine
4,4'-Methylenebis(2-
methylaniline)
2-Naphthylaraine
Polychlorinated biphenyls
. a
Tetrachlorobiphenyl
Pentachlorobiphenyl
a
Hexachlorobiphenyl
CAS Number
80-95-9
110-05-4
7722-84-1
75-9-2
3504-13-0
Alkyl halides and benzyl halides
Benzyl chloride 100-44-7
Methyl chloride 74-87-3
a
101-14-4
134-32-7
91-94-1
92-87-5
90-41-5
92-67-1
838-88-0
91-59-8
26914-33-0
25429-29-2
59291-64-4
Formula
C H 0
9 12 2
C H O
8 18 2
H2°2
C4H18°2
C H O
465
CH Cl
3
C H Cl N
13 12 22
cioV
C12H10CV2
C H N
12 12 2
C H N
12 11
C H N
12 11
C H N
15 18 2
cioV
C H Cl
12 6 4
C12H5C15
C12H4C16
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Table 1 (continued)
SUSPECTED CARCINOGENS STUDIED
Class/Name
Azo dyes
Azobenzene
4-Aminoazobenzene
4-Dimethylaminoazo-
benzene
2-Methyl-4-[(2-methyl-
pheny1)azoJ-benzenamide
Carbamates
Ethyl carbamate
Hydrazines
Hydrazine
1,1-Dimethylhydrazine
Hydrazine carboxamide
1,2-Dimethylhydrazine
Acyl chlorides and ketene
Benzoyl chloride
Diethylcarbamoyl
Dimethylcarbamoyl chloride
Ketene
Phosphates
Triethyl phosphate
Trimethyl phosphate
CAS Number
103-33-3
60-09-3
60-11-7
97-56-3
51-79-6
98-88-4
88-10-8
79-44-7
463-51-4
78-40-0
512-56-1
Formula
C12H10N2
C12H11N3
C14H15N3
C14H15N3
C3H7N°2
302-01-2
57-14-7
57-56-7
540-73-9
H N
4 2
C H N
282
CH N 0
5 3
C H N
282
C H C1NO
3 6
C H O
2 2
C6H15°4P
C3H9°4P
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Table 1 (continued)
SUSPECTED CARCINOGENS STUDIED
Class/Name CAS Number
Aziridines
Ethylenimine 151-56-4
1-Aziridineethanol 1072-52-2
Propylenimine 75-55-8
Lactones
p-Propiolactone 57-57-8
Sulfates
Dimethyl sulfate 77-78-1
Diethyl sulfate 64-67-5
Sultones
1,3-Propane sultone 1120-71-4
1,4-Butane sultone 1633-83-6
Aryl dimethyltriazenes
3,3-Dimethyl-l-phenyltriazene 7227-91-0
l-(p-Chlorophenyl)-3,3-dimethyl- 7203-90-9
triazene
Diazoalkanes
Diazomethane 334-88-3
Chloroalcohols and Ethers
2-Chloroethanol 107-09-3
1-Chloropropanol 127-00-4
Chloromethylmethyl ether 107-30-2
Formula
CRN
2 5
C H NO
4 9
C H N
3 7
C H O
342
C H O S
264
C H O S
4 10 4
C H O S
363
C H 0 S
483
C H N
8 11 3
C H C1N
8 10 3
CH N
2 2
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Table 1 (concluded)
SUSPECTED CARCINOGENS STUDIED
Class/Name
Bis(2-chloroethyl)ether
Bis(chloroethyl)ether
CAS Number
11-44-4
542-88-1
Formula
C H Cl O
422
C H Cl O
242
Hydroxylamine
Hydroxylamine
N-Methylhydroxylamine
0-methylhydroxylamine
Nitrosoamines
N-Nitrosodimethylamine
N-Nitrosodiethylamine
Furans
2-Nitrofuran
N-[4-(5-nitro-2-furanyl)-
2-thiazolyl]-acetamide
N-[4-(5-nitro-2-furanyl)-
2-thiazolylJ-formamide
Azides
Sodium azide
7803-49-8
593-77-1
67-62-0
62-75-9
55-18-5
609-39-2
531-82-8
24554-26-5
26628-22-8
H NO
3
CH NO
CH NO
5
CRN
262
C H N 0
4 10 2
C H NO
433
C H N 0 S
9734
C H N 0 S
8534
N Na
Only the CAS number for the general compound is given here. Each of
these, of course, have numerous isomers with individual CAS numbers.
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The sections of the report covering the individual classes of
compounds have been ordered according to the production estimates for
the class as a whole. Thus, although there are members of the epoxide
class having low production estimates, as a whole the production estimate
for the entire class places it at the top of the list. Where possible,
total production estimates are given for each compound on the list;
producers and plant sites are also listed where available. Physical and
chemical properties have been included. As requested by OTS, EPA, we
have limited discussion to the environmental transformation and bioaccumu-
lation of the compounds and classes of compounds.
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2. SUMMARY, CONCLUSIONS, AND RECOMMENDATIONS
The results of a literature search were combined with estimation
procedures to develop reliable information on the manufacture, environ-
mental transformations, and bioaccumulation of over 70 organic compounds.
These organic compounds represent 22 classes of chemical structures that
are believed to have mutagenic and/or carcinogenic properties.
The objective was to provide the Environmental Protection Agency
with information that can be used to better evaluate the probable
hazard to human and animal populations from exposure to these specific
compounds and to other members of these classes. The rationale for
developing this information lies in the belief that hazard ranking must
take into account at least three factors: (1) exposure of significant
populations of humans or animals to the chemical, as reflected by manu-
facturing data on total production and location of production facilities;
(2) transport, transformation, and persistence, which will govern the
levels of exposure in water, soil, or air and will indicate possible
geographical distribution from point sources; and (3) bioaccumulation
in mammalian species, which together with toxicity or carcinogenicity data
can indicate the probable hazard to life.
This study has several limitations: it does not address the questions
of toxicity, biodegradation, or the possible hazard of transformation
products. Nonetheless, the study does provide a first cut screening of
these compounds and some of their homologs to eliminate compounds that
clearly do not pose a problem of environmental exposure and to focus
attention on those possibly few compounds that are of particular concern
on the basis of wide exposure, long persistence, and significant bioaccu-
mulation. This review also draws attention to important gaps in our
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knowledge of these compounds and their interaction with the environment.
The following evaluation of relative environmental exposure of the
compounds examined in this study is necessarily incomplete and is subject
to revision when additional data are developed.
We have prioritized these compounds for overall environmental
exposure on the basis that the exposure of human populations to a specific
carcinogenic compound is minimal when the compound is manufactured in
amounts of less than 10 Ibs yr , used as an intermediate for in-plant
conversion, is rapidly transformed in the environment, and does not
bioaccumulate. Moderate or severe exposure problems arise from compounds
6 -1
manufactured in large amounts (> 10 Ibs yr ), the chemicals are end
products, are transformed slowly in the environment and bioaccumulate.
Given these limitations, we have classified the compounds into
three categories: minimal, moderate, and severe environmental hazards,
as summarized below.
36 -1
(1) Minimal exposure: production of 10 to 10 Ibs yr and/or
intermediate use only, rapid transformation, and low bio-
accumulation. The following compounds were judged to present
a minimal hazard:
Diazomethane Chloroalkyl ethers
Ketene Peroxides, including hydrogen
Bis(chloromethylether) peroxide
Chloromethyl methyl ether Other diazoalkanes
(2) Moderate exposure production of 1-4 x 10 to 4 x 10 Ibs yr~ ,
rapid transformation in the environment, low propensity to
bioaccumulate. Compounds judged to present a moderate hazard
are:
Chloroform Aziridines
Formaldehyde Nitrosamines
Benzoyl chloride Aryl triazenes
Most alkyl halides Sultones
Lactones Hydrazines
Sulfates Hydroxylamines
Epoxides Haloolefins
10
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6 -1
(3) Severe exposure: in excess of 4 x 10 Ibs yr , slow trans-
formation in the environment, moderate to high propensity to
bioaccumulate. Compounds judged to present severe exposure
are:
Aromatic amines Polychlorinated biphenyls
Chloroalcohols Ethyl aliphatic carbamate
1,2-dihaloalkanes Azo dyes
Carbon tetrachloride Phosphate esters
Although they are likely to pose a minimal problem, there were
too few data on azide ion or nitrofurans to make even a tenta-
tive judgment.
Several of the compounds classified as severe exposure problems,
including carbamates, phosphates, amines, and chloroalcohols, may
biodegrade at significant rates in soil and water. No information on
this subject was sought and is needed to provide more reliable estimates.
Several of these same compounds as well as nitrofurans may also be photo-
transformed at significant rates; data on the uv spectra and quantum yields
for these processes are needed.
Estimated half-lives of these compounds in the atmosphere are based
on a few good data for rates of reaction of HO radical with olefins,
aromatics, and alkanes in the atmosphere, a few data for reactions in
solution with more complex compounds, and a number of intelligent guesses
about solvent and substituent effects on rates of reaction of HO-with
the compounds in this study. The paucity of reliable rate constants
for reactions of HO radical with simple functionalized organic compounds
in the atmosphere remains a serious gap in our knowledge of the environ-
mental transformation of organic compounds.
In this study we have used the partition coefficients (log P as an
index of the propensity of a compound to bioaccumulate on the grounds
that, to a first approximation, log P measures the ease of transfer from
water to tissue (lipophilicity). However, high lipophilicity may be
accompanied by a high rate of metabolism. Thus both factors must be
11
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evaluated to determine the actual extent of bioaccumulation for a
specific compound. Information of this kind was found for only a few
of the compounds examined in this study. Therefore, we recommend that,
for compounds that appear to be significant environmental hazards and
for which this information is lacking, laboratory animal studies be
made of their uptake, distribution, retention, and excretion.
12
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3. METHODOLOGY
Literature Search
The basis for the literature search was the list of suspect carcino-
gens (Table 1) as supplied by EPA. Chemical Abstracts was searched from
1965 through 1976 for biological and chemical activity of all compounds
or classes of compounds. The U.S. Government Reports were searched from
1970 through 1976. Primary sources such as current issues of pertinent
journals were scanned. Most of the searching was carried out manually,
but Chemical Abstracts, Volume 84, was searched by Chemical Abstract
Service (CAS) number using the Systems Development Corporation (SDC)
computerized files of Chemical Abstracts.
Manual searching was performed not only under common names and full
chemical names, but also under such terms as environmental fate, bio-
degradation, photolysis, and partition coefficients. The number of
references called in the first search varied considerably for each
compound or class of compounds. Abstracts were studied to limit the
number of full text copies to the most pertinent references only. For
some compounds, Chemical Abstracts was searched as far back as necessary
to find reliable data for specific chemical processes such as hydrolysis.
Estimation Procedures for Persistence
Kinetic Relationships
Estimates of persistence are conveniently expressed as the half-life
(t^) for a substrate (S) under a specific set of conditions, usually
involving one kind of reaction. For the reaction
X + S—*~ Products
13
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the rate law is
dS/dt = k [S][X] (1)
x
Under conditions where X is replaced as consumed, resulting in a constant
or steady-state concentration, the second-order relation (1) becomes
pseudo-first order and may be readily integrated to give
ln(S /S ) = k [X]t + C (2)
o t x
where S is the initial concentration of S and S is the concentration
o t
at time t. At one half-life of S, S /S = 2 and
o t
t, = In 2/k [X] (3)
2 x
If more than one reaction is important for conversion of S, the rate
expression and equation (3) are replaced by more general relations in
which k [X] becomes K [A] + ... k [Nl, the sum of all pseudo-first-
x AN
order rates.
Thus, the half-life in the environment for a specific compound
(S) can be estimated if the concentration of the reactive species (X)
and the rate constant for reaction of X with S are known.
Chemical Transformations in the Environment
At least three important types of transformations of organic com-
pounds in the atmosphere and in aquatic systems can be identified:
oxidation by HO, 0Q, or RO radicals, hydrolysis, and photolysis.
O
Oxidation Processes in the Environment
The major oxidizing species in the atmosphere are HO radical
and ozone; other intermediate radicals are formed but do not control
the rates of oxidation of the initial compound. Our knowledge of the
chemistry of aquatic systems is much more uncertain, but estimates of
14
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reactivity and concentrations of peroxy and alkoxy radicals (RO • and RO-)
^
(where R is H or an organic group) indicate that only RO- (or triplet
ketone biradicals) are likely to be important oxidizers in aquatic
systems. The concentrations of HO« and 0 in the atmosphere are probably
O
known accurately within a factor of 3, while the concentrations of R0« in
water are only order-of-magnitude estimates.
To calculate persistence in the atmosphere, we have used a
concentration of [HO-] = 0.8 x 10 M (average for day and night), based
on measurements of Wang et al. (1975), which are 5.7 times larger
than the earlier estimate by Levy (1971). Concentrations of HO radical
in the atmosphere depend on solar radiation and drop to nearly zero at
night. Therefore we have averaged the values for daylight and dark
periods to take into account this diurnal variation.
Reactions of O with organic compounds are generally much
o
slower than those involving HO*; however, the much higher concentration
-9
of 0 (2 x 10 M in urban clean air) makes some reactions of O competi-
o 3
tive with those of HO radical. For the most part, however, the neglect
of 0 reactions leads to no significant error in estimates of tt (Darnall
3 2
et al., 1976).
Rate constants for reaction of H0»(k ) in air are known
HO
with reasonable accuracy for a wide variety of organic olefins, dienes,
alkanes, and aromatics (Darnall et al., 1976). However, very few data
are available for more complex functionalized molecules; values measured
in water are available (Anbar and Netz, 1967) for many functionalized
compounds and by making some reasonable assumptions about solvent
effects (Walling et al., 1974) and additivity effects of structure we
have estimated values of k and t, for all the compounds in Table 1
HO §
These values are listed in Table 2. Many of the values for k are
HO
probably accurate to no more than a factor of ten. However, the
15
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Table 2
RATE CONSTANTS AND HALF-LIVES FOR REACTION
OF HO RADICAL WITH ORGANIC COMPOUNDS
Class of Compounds
Rate Constant, k.
(M
x 10
~9
HO
Half-Life, t,
(hours)
Epoxides
All aliphatic epoxides
Styrene oxide and other
aromatic epoxides
1.0
2.7
23
8.7
Haloolefins
Chloroethylene
1,2-dichloroethylene
Trichloroethylene
Chlorobutadiene
Monochloroolefins(C -C )
»5 o
Aldehydes
Formaldehyde
Acrolein and other aldehydes
1.9
0.95
0.63
23
8-35
12
26
36
1.1
0.34-3.0
2.6
2.6
Dialkyl halides
1,2-Dichloroethane
1,2-Dibromethane
Dihaloethanes (C-C )
3 D
Peroxides
Di-t-butyl peroxide
t-butyl hydroperoxide
Cumyl hydroperoxide
Perpropionic acid
Hydrogen peroxide
0.1
0.1
0.3-1
0.3
0.3
2.7
0.5
1
234
234
23-77
79
79
8.5
47
23
Alkyl and Benzyl halides
Benzyl chloride
Methyl chloride
2.7
0.2
8.5
117
t = In 2/C0.8 x 10~14)k daylight hours; see text.
1/2 HO
From data of Davis et al (1975).
16
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Table 2 (continued)
RATE CONSTANTS AND HALF-LIVES FOR REACTION
OF HO RADICAL WITH ORGANIC COMPOUNDS
Class of Compounds
Rate Constant, k
x 10
~9
HO
Half-Life, t.,
(hours)
Polyhalomethanes
Chloroform
Carbon tetrachloride
Polychloroethanes(C -C
«j 4
Aromatic amines
All benzidines
All biphenylamines
All naphthylamines
All anilines
0.5
< 0.001
0.05-1.5
2
2
2
2
13
> 23400
16-470
12
12
12
12
Biphenyls and chlorobiphenyls
Biphenyl
Polychlorobiphenyls
4
< 0.5
6
> 47
Azo dyes
All azo dyes
7.9
Carbamates
Ethyl carbamate
0.5
47
Hydrazines
Hydrazine < 0.1
Hydrazine carboxamide < 0.1
Methyl hydrazines
Alkylhydrazines (C -C )
£i 5
10
> 1
> 1
c
c
2.1
2.1
> 2.1
> 23
No reliable data.
17
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Table 2 (continued)
RATE CONSTANTS AND HALF-LIVES FOR REACTION
OF HO RADICAL WITH ORGANIC COMPOUNDS
Class of Compounds
Rate Constant, k
HO
(M"1 s"1) x 10~9
Acyl chlorides and ketene
Dimethylcarbamoyl chloride
Diethylcarbamoyl chloride
Benzoyl chloride
Ketene
Phosphoric acid ester
Trimethyl phosphate
Triethyl phosphate
All alky! phosphate (C3-C6)
Aziridines
All aliphatic aziridines
Azirdine ethanol
Lactones
Propiolactone
All aliphatic lactones C -C
4 10
Alkylsulfates
Dimethylsulfate
Diethylsulfate
Sultones
All five- or six-membered
sultones
0.1
0.5
2.7
3.8
0.5
0.5
0.1
0.1-3
0.02
0.2
0.2
Half-life, t1
(hours) *
230
47
8.5
6.4
< 0.1
0.5
1-3
> 230
47
6.4-23
47
47
230
6.4-230
1170
117
117
Aryl triazenes
All aromatic triazenes
2.7
8.5
18
-------
Table 2 (concluded)
RATE CONSTANTS AND HALF-LIVES FOR REACTION
OF HO RADICAL WITH ORGANIC COMPOUNDS
Class of Compounds
Rate Constant, k
x 10
~9
HO
Half-life, tj
(hours)
Diazoalkanes
Diazomethane
0.1
230
Haloalcohols
2-Chloroethanol
1-Chloropropanol
Haloalcohols C -C
3 6
Haloethers
Chloromethyl methyl
Bis(chloromethyl)
Bis(2-chloroethyl)
0.5
0,5
1
0.1
< 0.1
0.1
47
47
23
230
> 230
230
Hydroxylamines
Hydroxylamine
O- or N-ethylhydroxylamines
> 0.1
< 230
< 230
Nitrosamines
Dimethylnitrosamine
Diethylnitrosamine
Alkylnitrosamines(C -C )
3 6
Aromatic nitrosamines
0.1
0.5
1-3
2
230
8.5~23
12
Nitrofurans
All furans
Aliphatic substituted furans
1.0
3
23
77
Azides
Inorganic azides not found in
atmosphere except as particulate;
no reliable estimate possible
From data of Davis, et al. (1975)
19
-------
reactivity of many functionalized organics toward HO- is high enough
that compounds for which half-lives are predicted to be a few minutes
and which are in fact several hours may still be considered as rela-
tively nonpersistent within the framework of practical environmental
assessment. As a rough rule of thumb, compounds having
9 -1 -1
k > 1 x 10 M s have half-lives in the atmosphere of less than
HO
12 hours and over 90% reaction in 3 days.
The reactions of alkoxy radicals (RO-- where R represents any
organic radical) are not important in air but might be important in the
aqueous phase under some conditions. Concentrations of RO' equal to
-14
~10 M are anticipated for water exposed to sunlight containing
oxygen and light-sensitive compounds that photodissociate (Mill and
Hendry, 1976). Estimates of half-lives use this concentration. The
uncertainty limits range from 1/10 to 10 times reported values. Values
of k for a wide variety of organic compounds are known and are
RO
summarized in the review of Hendry et al. (1974). Only a few compounds
are reactive enough toward RO-for this process to be an important one.
Products of oxidation in the environment generally arise from
one of several possible interactions of peroxy radicals (RO •) with
2j
other radicals or stable molecules. We can predict qualitatively the
kinds of products that will form and can make some generalizations
(Mill, 1976). For example,
• Aromatic compounds will oxidize in air to give mixtures
of phenols, quinones and side chain ketones, alcohols
and aldehydes. In the atmosphere ring oxidation will
probably dominate (> 60%) (Perry, et al., 1974; Kenley and
Hendry, 1977).
• Aliphatic compounds will oxidize in air to give alcohols,
ketones, alkyl nitrates, and mostly cleavage products
arising from intermediate alkoxy radicals.
20
-------
Oxidations in water of both aromatic and aliphatic
compounds will probably proceed through RO'and RO •
radicals to give alcohols, ketones, and hydroperoxides
(Mill et al., 1977).
Hydrolysis
Hydrolysis is an important chemical process in the aquatic
environment for many compounds found in the list. The rate for hydrolysis
of substrate, S, usually can be put in the form
where k , k and k are the second-order rate constants for base-cata-
lyzed, acid-catalyzed, and neutral processes, respectively; in water
k [H 0] is a constant (= k ) . The pseudo-first-order rate constant,
N 2 N
k , is the observed rate constant for hydrolysis at constant pH.
obs
Equation (4) assumes that the individual rate processes for the acid,
base, and neutral hydrolyses are each first order in substrate. With a
few known exceptions, this is usually the case and
kobs = k
From the autoprotolysis water equilibrium, equation (5) may be
rewritten as
[H+][OH~] = K (6)
k K
k = -5— Z + k [H+] + k (7)
obs [H+] AL J N
From equation (7) it is evident how pH affects the overall rate: at
high or low pH (high OH or H ) one of the first two terms is usually
dominant, while at pH 7 the last term can often be most important.
However, the detailed relationship of pH and rate depends on the
21
-------
specific values of k , k , and k . At any fixed pH, the overall rate
B A -^
process is pseudo-first order, and the half-life of the substrate is
independent of its concentration and is simply
t. = In 2/k (8)
\ obs
In cases where rate constants for hydrolysis are reported
only in pH regions outside those of environmental interest (pH 5-9),
a value of k and t, of S at pH 7 can be calculated to give a minimum
obs 2
rate of hydrolysis or maximum persistence. Rate constants and half-lives
for most hydrolyzable compounds in this report are summarized in Table 3.
Some information on hydrolysis is available only in mixed water-organic
solvents or at elevated temperatures. We have relied extensively on
the compilation of hydrolysis kinetic data of Mabey and Mill, (1977) to
o
estimate persistence in aquatic systems at 25 C and pH 7.
Photochemistry
Photochemical transformations in the environment depend on
absorption of photons by a compound in the uv spectrum above 290 nm,
the solar cutoff. The rate of transformation depends on the efficiency
of absorption of photons (the extinction coefficient), the solar
irradiance, and the quantum yield. Although the chemistry of photo-
chemical processes occurring in the environment are variable and often
complex, a few generalizations are possible:
• Aromatic esters may rearrange, or undergo photohydrolysis in
the presence of water; aliphatic and aromatic ketones and
aldehydes will dissociate to radicals.
Halo and nitroaromatics can photohydrolyze or be reduced in
the presence of hydrocarbons (as in aqueous dispersions).
22
-------
Table 3
RATE CONSTANTS AND HALF-LIVES FOR HYDROLYSIS
OF ORGANIC COMPOUNDS
(25°C and pH 7)
Rate Constant
Class/Compound
Half-Life
Reference
Epoxides
1,2-Epoxy-
Ethane
Propane
2-Methylpropane
3-Hydroxy propane
3-Chloropropane
3-Bromopropane
trans-2 , 3 -E poxy-butane
cis-2 ,3-Epoxy -butane
1 ,2-Epoxy-l-phenylethane
trans-1 , 2-epoxy-l-phenyl-
propane
Aliphatic epoxides
6.9
5.5
18.3
2.84
9.8
5
5.12
5.24
5.2
3.7
5.7
(-7)
(-7)
(-7)
(-7)
(-7)
(-7)
(-7)
(-7)
(-7)C
(-7)
(-7)
Haloethers and Alcohols
C1CH2OCH
Chloromethyl Methylether
bis(Chloromethyl)ether
2-Chloroethanol
l-Chloro-2-propanol
Polyhaloraethanes
Dichloromethane
Chloroform
>90
0.018
1.06 (-9)'
1.1 (-8)'
12 days
14.6 days
4.4 days
28 days
8.2 days
16 days
15.7 days
15.3 days
15 days Audier et al.(1968)
21 days Audier et al. (1968)
14 days
<0.007 sec
38 sec
21 yr
2 yr
Cowan et al.(1950)
Cowan et al.(1950)
3.2 (-11) 704 yr
6.9 (-12) 3,500 yr
23
-------
Table 3 (continued)
RATE CONSTANTS AND HALF-LIVES FOR HYDROLYSIS
OF ORGANIC COMPOUNDS
(25°C and pH 7)
Rate Constant
Class/Compound
Tribromomethane
Tetrachloromethane
(s"1)
3.2 (-11)
4.8 (- 7)
Half-Life
686
7000 yr
b
Reference
Alkyl and benzyl halides
(including 1,2-dihalo-
alkanes)
Methyl chloride 1.9 (-8)
Methyl bromide 4.0 (-7)
Ethyl chloride 2.0 (-7)
Ethyl bromide 1.6 (-7)
Isopropyl chloride 2.0 (-7)
Isopropyl bromide 3.7 (-7)
t-Butyl chloride 1.0 (-4)
Benzyl chloride 1.3 (-5)
Benzyl bromide 1.5 (-4)
1,2-Dichloroethane ~5 (-13)
1,2-Dibromoethane ~5 (-12)
Carbamates and carbonates
EtOC(0)NH (ethyl carbamate)
MeOC(0)NHC H 5.5 (-12)
o o
EtOC(0)N(C H )Me 5.0 (-13)
D O
C6H5OC(0)NHC6H5 5.4 (-6)
7 yr
417 days
20 days
40 days
50 days
39 days
2.1 days
1.9 hr
15 hr
1.3 hr
50,000 yrg
5,000 yr Buckley et al.(1967)
20 (-12) 11,000 yr
Dittertand Higuchi
(1963)
4,000 yr
44,000 yr
1.5 days
24
-------
Table 3 (continued)
RATE CONSTANTS AND HALF-LIVES FOR HYDROLYSIS
OF ORGANIC COMPOUNDS
(25°C and pH 7)
Rate Constant
Class/Compound
Half-Life
Reference
C H OC(O)N(C H )Me
65 65
C1CH CH OC(0)NHC H
CC1 CH OC(0)NHC H
EtOC(0)NHMe
EtOC(O)NMe
£1
C H OC(O)OEt
4.2
1.6
3.2
5.7
4.5
2.4
(-12)
(-10)
(- 8)
(-13)
(-13)
(- 8)
5,200
140
252
38,000
39,000
0.9
yr
yr
days
yr
Benzoyl and carbamoyl
chlorides
Benzoyl chloride
4.3 ( -2)
Dimethyl carbamoyl chloride >2.5 ( -3)
Ethyl chloroformate 2.15( -4)
Phosphoric acid esters
Trimethyl phosphate 1.8 ( -8)
Triethyl phosphate 2.2 ( -9)
Diethyl phosphate 6.7 ( -9)
Trithioethyl phosphate 2.6 ( -9)
Triphenyl phosphate 1.7 ( -9)
0-Ethyl-O-p-nitrophenyl- 2.9 ( -6)
S-ethyl phosphate
O,O-Dimethyl-0-p-nitro- 1.1 ( -7)
phenyl thiophosphate
(methyl parathion)
16 sec Kelly and Watson
(1958)
<4.6 min Hall (1955)
53 min Queen (1967)
1.2 yr
10 yr
3.3 yr
8.5 yr
1.3 yr
2.8 days
78 days
25
-------
Table 3 (continued)
RATE CONSTANTS AND HALF-LIVES FOR HYDROLYSIS
OF ORGANIC COMPOUNDS
(25°C and pH 7)
Class/Compound
0,0-Diethyl-O-p-nitro-
phenyl thiophosphate
(parathion)
Rate Constant
(a"1)
4 ( -9)
Half-Life
5.5 yr
Reference
Azirdines
Ethylenimine
Propylenimine
1-Azirideneethanol
5.2 ( -7)
(protonated)
~6 ( -7)
~5 ( -7)
15.4 days
-16 days
-16 days
Lactones
g-Propiolactone 3.3 ( -3) 3.3 hr
y-Butyrolactone and other 8 ( -4) 13 hr
lactones
Alkyl sulfates and
sulfonates
Dimethyl sulfate 1.7 ( -4) 1.2 hr
Diethyl sulfate 1.1 ( -4) 1.7 hr
Ethylene sulfate 7.6 ( -4) 0.25 hr
Trimethylene sulfate 6.3 ( -5) 3.1 hr
Early et al.(1958)
Buist and Lucas
(1957)
Long &. Purchase
(1950)
Long & Purchase
(1950)
Robertson and
Sugamori (1966)
Roberton and
Sugamori (1966)
Kaiser et al.
(1963)
Kaiser et al.
(1963)
26
-------
Table 3 (concluded)
RATE CONSTANTS AND HALF-LIVES FOR HYDROLYSIS
OF ORGANIC COMPOUNDS
(25°C and pH 7)
Class/Compound
Rate Constant
(a'1)
Half-Life
Reference
Methylmethane sulfonate 5.0 ( -7)
Ethyl benzenesulfonate 1.0 ( -5)
Sultones
1,3-Propane sultone ~20 ( -6)
1,4-Butane sultone 5 ( -7)
38 hr Robertson and
Sugamori (1966)
16.5 hr Roberton and
Sugamori (1966)
9.6 hr Bordwell et al.
(1959)
16 days
l-Aryl-3,3-dimethyl triazene
Phenyl- 5.5 ( -5)
P-Chlorophenyl-
P-Methoxy-
P-Nitro-
4.8 ( -6)
1.15( -3)
5.0 ( -8)
210 min Kolar and Preus-
mann (1971)
40 hr
10 min
160 days
Numbers in parentheses are exponents of base 10.
Unless otherwise stated, data are from Mabey and Mill (1977).
Extrapolated from 60 C.
Calculated using temperature dependent equation in Cowan et al. (1950)
0
Concentration, 1 ppm.
f
Concentration, 1000 ppm.
£
Estimated to be only one tenth as reactive as dibromoethane.
h o
Measured at 3.2 C.
i o
Measured at 20 C.
J Measured at 37°C.
27
-------
Photooxldation is a common environmental process, but
the mechanisms may involve excited states or free radicals
or both, and details are very dependent on structure.
Although we have tried to estimate the importance of these processes
for compounds that absorb in the solar region, the estimates are usually
educated guesses made in the absence of reliable experimental data.
A reliable method for estimating the rate of a phototrans-
formation in sunlight has been developed by Wolfe et al. (1976). This
method requires only the uv spectrum for the compound and the quantum
yield for the reaction. We have tried to apply the principle of this
method for qualitatively estimating half-lives for some compounds for
which these data are available. However, quantitative estimates
require a machine computation beyond the scope of this study.
Partition Coefficients
Partition coefficients for octanol/water are often used as a re-
liable measure of the propensity of a compound to transfer from water
to a lipid phase and bioaccumulate. The partition coefficient, log P,
is defined as the log (base 10) of the ratio of the concentration in
octanol to the concentration in water. Thus, log P values are directly
proportional to lipophilicity or hydrophobicity as determined by equili-
brium distribution of a compound between lipid and aqueous phases of a
two-phase system.
However, hydrophobicity is only one measure of the tendency of a
compound to bioaccumulate. Such a tendency is frequently offset by
susceptibility to metabolic degradation. Metabolism generally converts
lipophilic compounds to highly polar metabolites, which are readily
28
-------
excreted via the kidneys. Highly polar compounds are frequently ex-
creted rapidly in unchanged form. In contrast, highly lipophilic com-
pounds tend to pass readily into liver microsomes where drug-metabolizing
enzymes are concentrated. Thus, while a high log P value tends to
favor accumulation in body fat and other lipophilic tissues, it also
favors rapid metabolism to easily excreted metabolites depending on the
chemical constitution of the compound. In addition, continued exposure
frequently stimulates such metabolism. In the absence of direct experi-
mental data, accurate prediction of bioaccumulation potential requires
knowledge of metabolic susceptibility in addition to hydrophobicity—
at least in the case of highly lipophilic compounds.
Our conclusions concerning the propensity of each chemical to
bioaccumulate were based primarily on their log P values (see Table 4)
because in most instances, the value was the only information available.
When direct experimental data were available to support or refute
initial conclusions based on log P values, we included them in our dis-
cussion. When available, we also included any information on metabolism
uptake and excretion, and when possible indicated how these factors
might affect bioaccumulation.
Where available, measured values from the literature (Pomona
College medicinal chemistry project data base) are reported. Such
values have either been determined directly in an octanol/water system
or calculated by applying regression equations to data obtained in
other lipid/water systems. Where the data base lists several values
derived by regression equations from measurements in several systems,
a mean value has been calculated. A log P value of 2.0 means that
distribution of a compound between oil (octanol) and water phases is
such that its concentration in the oil phase is favored 100 to 1.
29
-------
Table 4
PARTITION COEFFICIENTS
Class/Name
CAS Number
Log P
Epoxides
Ethylene oxide
Propylene oxide
Epichlorohydrin
Styrene oxide
Glycidol
Glycidaldehyde
Haloolef ins
Vinyl chloride
Trichloroethylene
Vinylidene chloride
Chloroprene
Aldehydes
Formaldehyde
Acrolein
Dihaloalkanes
1,2-Ethylene dibromide
1,2-Ethylene dichloride
Polyhalomethanes
Carbon tetrachloride
Chloroform
75-21-8
75-56-9
106-89-8
96-09-3
556-52-5
765-34-4
75-01-4
79-01-6
75-35-4
126-99-8
50-00-0
107-02-8
106-93-4
107-06-0
56-23-3
67-66-3
a
-0.30
-0.13
0.30
0.98
-2.00
-1.99
0.60
a
2.29
0.73
0.57
-0.96a
-0.90
1.60
1.48a
2.703
a
1.92
30
-------
Table 4 (continued)
PARTITION COEFFICIENTS
Class/Name
Peroxides
Cumene hydroperoxide
Di-tert-butyl peroxide
Hydrogen peroxide
tert-Butyl hydroperoxide
Succinic acid peroxide
CAS Number
80-95-9
110-05-4
7722-84-1
75-9-2
3504-13-0
Alkyl halides and benzyl halides
Benzyl chloride 100-44-7
Methyl chloride 74-87-3
Log P
-0.16
0.68
-1.423
-1.30
-3.04
2.30
1.92'
a
Aromatic amines
4,4'-Methylenebis(2-
chloroaniline)
1-Naphthylamine
3,3-Dichlorobenzidine
Benzidine
2-Biphenylamine
4-Biphenylamine
4,4'-Methylenebis(2-
methylaniline)
2-Naphthylamine
101-14-4
4.02
134-32-7
91-94-1
92-87-5
90-41-5
92-67-1
838-88-0
2.15
3.36
a
1.81
a
2.10
a
1.74
3.92
91-59-8
1.90
Polychlorinated Biphenyls
a
Tetrachlorobiphenyl
a
Pentachlorobiphenyl
a
Hexachlorobiphenyl
26914-33-0
25429-29-2
59291-64-4
7.24
8.05
8.86
31
-------
Table 4 (continued)
PARTITION COEFFICIENTS
Class/Name CAS Number Log p
Azo dyes
a
Azobenzene 103-33-3 3.82
a
4-Aminoazobenzene 60-09-3 3.50
4-Dimethylaminoazo- 60-11-7 4.58
benzene
2-Methyl-4-[(2-methyl- 97-56-3 4.25
phenyl)azoj-benzenamide
Carbamates
Ethyl carbamate 51-79-6 -0.75
Hydrazines
Hydrazine 302-01-2 3-08
1,1-Dimethylhydrazine 57-14-7 -1.94
Hydrazine carboxamide 57-56-7 -2.53
1,2-Dimethylhydrazine 540-73-9 -2.52
Acyl chlorides and ketene
Benzoyl chloride 98-88-4 0.97
Diethylcarbamoyl 88-10-8 -0.12
Dimethylcarbamoyl chloride 79-44-7 -1.20
Ketene 463-51-4 b
Phosphates
Triethyl phosphate 78-40-0 l.ll3
Trimethyl phosphate 512-56-1 -0.52a
32
-------
Table 4 (continued)
PARTITION COEFFICIENTS
Class/Name CAS Number
Aziridines
Ethylenimine 151-56-4
1-Aziridineethanol 1072-52-2
Propylenimine 75-55-8
Lactones
p-Propiolactone 57-57-8
Sulfates
Dimethyl sulfate 77-78-1
Diethyl sulfate 64-67-5
Sultones
1,3-Propane sultone 1120-71-4
1,4-Butane sultone 1633-83-6
Aryl dimethyltriazenes
3,3-Dimethyl-l-phenyltriazene 7227-91-0
l-(p-Chlorophenyl)-3,3-dimethyl- 7203-90-9
triazene
Diazoalkanes
Diazomethane 334-88-3
Chloroalcohols and Ethers
2-Chloroethanol 107-09-3
1-Chloropropanol 127-00-4
Chloromethylmethyl ether 107-30-2
Log P
-1.12
-1.79
-0.46
-0.46
-4.26
-3.18
-2.82
-2.45
2.59£
3.00C
0.03
-0.06
-0.21
33
-------
Table 4 (concluded)
PARTITION COEFFICIENTS
Class/Name
Bis(2-chloroethyl)ether
Bis(chloroethyl)ether
CAS Number
11-44-4
542-88-1
Log P
0.70
-0.38
Hydroxylaraine
Hydroxylamine
N-Methylhydroxylamine
O-methylhydroxylamine
7803-49-8
593-77-1
67-62-0
-3.18
-2.90
-2.47
Nitrosoamines
N-Nitrosodimethylamine
N-Nitrosodiethylamine
62-75-9
55-18-5
0.06
1.14
Furans
2-Nitrofuran
N-[4-(5-nitro-2-furanyl)-
2-thiazolylJ-acetamide
N-[4-(5-nitro-2-furanyl)-
2-thiazolylJ-formamide
609-39-2
531-82-8
24554-26-5
1.86
-0.60
-1.14
Azides
Sodium azide
26628-22-8
a
Literature values; all others are calculated.
b
Insufficient data available; these are reactive, polar compounds with
expected log P <1.0.
rt
"Literature value is for the o-chloro isomer.
34
-------
When no literature data were available, log P was calculated
either from a parent solute and the known additive TT constants for
substituents (Hansch et al., 1973; Leo et al., 1971) as shown by
Equation (9) ;
log PRX = Log PRH + nx (9)
or by summation of fragmental constants (f; assembly of the solute from
its component parts) (Nys et al., 1973; Leo, 1976) as represented by
Equation (10) :
n
log P = £ a f (10)
n n
Either method yields reasonably reliable estimates of lipophilicity
8
within a log P range of more than 10 (less than -1.0 to more than
+ 7.0) .
35
-------
4. EPOXIDES
Production and Properties
Ethylene oxide is produced in the highest quantities of the
chemicals in this group. Production estimates are given below (in
pounds per year):
Ethylene oxide
Propylene oxide
Epichlorohydrin
Styrene oxide
Glycidol
Glycidaldehyde
3893 million (1974)
1756 million (1974)
180 million (1973)
>1000 (1974)
>1000 (1974)
<1000 (1974)
Producers and locations are given in Table 5. Table 6 lists the
synonyms for chemical in this group and some of their physical and
chemical properties.
Table 5
PRODUCERS AND LOCATIONS FOR EPOXIDES
Compound
Producers
Site
Ethylene oxide
BASF Wyandotte Corp.
Cacasiu Chemical Corp.
Celanese Chemical Co.
Dow Chemical Co.
Jefferson Chemical Co.
Northern Petrochemical Co.
Olin Corp.
Oxirane Corp.
PPG Industries
Shell Chemical Co.
Sunolin Chemical Co.
Texas Eastman Co.
Union Carbide Corp.
Geismar, Louisiana
Lake Charles, Louisiana
Clear Lake, Texas
Freeport, Texas
Plaquemine, Louisiana
Port Neches, Texas
East Morris, Illinois
Brandenburg, Kentucky
Channelview, Texas
Beaumont, Texas
Guayanella, Puerto Rico
Geismar, Louisiana
Claymont, Delaware
Longview, Texas
Seadrift, Texas
Taft, Louisiana
Texas City, Texas
Ponce, Puerto Rico
37
-------
Table 5 (Concluded)
PRODUCERS AND LOCATIONS FOR EPOXIDES
Compound
Producers
Site
Propylene oxide
Epichlorohydrin
Styrene oxide
Glycidol
BASF Wyandotte Corp.
Dow Chemical Co.
Jefferson Chemical Co,
Olin Corp.
Oxirane Corp.
Dow Chemical Co.
Shell Chemical Co.
Union Carbide Corp.
Dixie Chemical Co.
FMC Corp.
Wyandotte, Michigan
Freeport, Texas
Plaquemine, Louisiana
Port Neches, Texas
Brandenburg, Texas
Bayport, Texas
Channelview, Texas
Freeport, Texas
Deer Park, Texas
Norco, Louisiana
Taft, Louisiana
Bayport, Texas
Bayport, Texas
38
-------
Table 6
PHYSICAL AND CHEMICAL PROPERTIES OF EPOXIDES
Compound, Synonyms
Mol,
wt.
Ethylene oxide; oxirane; 44.05
dihydrooxirene; dimethyl-
ene oxide; 1,2-epoxy-
ethane.
Propylene oxide; meth- 58.08
yloxirane; 1,2-epoxy-
propane; propene oxide.
Epichlorohydrin ; 1- 92.53
chloro-2,3-epoxy-
propane; chloromethyl-
oxirane; chloropro-
pylene oxide; cy-epi-
chlorohydrin
Styrene oxide; phenyl- 120.16
oxirane; 1,2-epoxy-
ethylbenzene
Glycidol; 2,3-epoxy-l- 74.08
-propanol; oxirane-
methanol; glycidyl al-
cohol; 3-hydroxy-l,2-
epoxy-prop^ ne
M.P.
-111
B.P.
Density
-13.5746 0.882410 1.35977
10
34.3
-48 116.5
60-1
.760
100
194.1
84-5
15
56.5
11
0.859
1.1801
20
1.0523
16
1.117
20
max
(log g)
(gas)
169(3.58)
171(3.57)
1.3670
20
1.4361
20
1.5342
20
Solubility
Soluble in water,
alcohol, ether,
acetone, and benzene
1.4293
16
Infinitely soluble
in water, alcohol
and ether
Slightly soluble in
cold water, decom-
poses in hot water,
infinitely soluble
in alcohol and ether,
soluble in benzene
250sh Insoluble in water,
(2.2),254 soluble in alcohol and
(2.24),260 ether
(2.28) ,265sh
(2.10)in alcohol
Soluble in water,
alcohol, ether, ace-
tone, chloroform, and
benzene
-------
Environmental Transformation
Lower aliphatic epoxides such as ethylene or propylene oxides are
volatile polar compounds that are moderately reactive toward a variety
of nucleophilic species including water via acid, base, and neutral
reactions. In general, structure has little effect on the rates of
hydrolysis of terminal epoxides to diols by neutral water. For example,
aliphatic terminal epoxides have half-lives of 338 ± 200 hours at 25°C;
aromatic substituents such as phenyl or benzyl show this same reactivity
pattern. Data for hydrolysis of a number of epoxides are summarized in
Table 3.
A more detailed analysis of the rate data indicate that more heavily
substituted epoxides (such as isobutylene oxide) probably hydrolyze mostly
by a fast acid-catalyzed process; in acidic waters (pH 5-6) these epoxides
would have half-lives of less than 100 hours.
No photochemical processes are important for simple aliphatic
epoxides; however, aromatic epoxides that absorb in the solar region
probably undergo photohydrolysis in water and this could significantly
reduce the half-life (Hisaoka and Tokumara, 1973). Biodegradation may
be an important competing process for many epoxides, but oxidation in
water is probably very slow.
If dispersed into the atmosphere, epoxides would be oxidized by HO
radical with half-lives of 3 to 11 hours. Products of oxidation probably
include formic esters, CO, C02, and oxidized aliphatic fragments.
Glycidaldehyde would probably photolyse via the aldehyde chromosphere at
about the same rate as oxidation. Washout by rain is likely to be
important only for low molecular weight epoxides.
Bioaccumulation
The log P values for ethylene oxide, propylene oxide, glycidol,
glycidaldehyde, and epichlorhydrin are negative (see Table 4). Only
styrene oxide has a positive log P value (0.98). We believe that none
of these compounds will accumulate significantly in animal tissues.
40
-------
In vitro studies by James and White (1967) and by James et al.
(1976) have shown that styrene oxide is metabolized by the liver of
rats and rabbits and that the reaction is catalyzed by microsomal epoxide
hydrase and by glutathione-s-epoxide transferase. These studies do not
reflect the rate or extent of styrene oxide metabolism in vivo. If
there are enzymes that act on all the epoxides studied, metabolism of
a compound could reduce the extent of accumulation.
41
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5. HALOOLEFINS
Production and Properties
All the compounds in this category are commercially important,
The estimated production figures are given below (in millions of
pounds per year):
Vinyl chloride
Trichloroethylene
Chloroprene
Vinylidene chloride
5621
388
349
60
(1974)
(1974)
(1975)
(1972)
Producers and locations are given in Table 7, and chemical and physical
properties are listed in Table 8.
Compound
Table 7
PRODUCERS AND LOCATIONS FOR HALOOLEFINS
Producer
Vinyl chloride
Allied Chemical Corp.
Borden, Inc.
Continental Oil Co.
Diamond Shamrock
Dow Chemical Co.
Ethyl Corp.
B. F. Goodrich Co.
Monochem, Inc.
PPG Industries
Shell Chemical Co.
Stauffer Chemical Co.
Site
Baton Rouge, Louisiana
Geismar, Louisiana
Westlake, Louisiana
LaPorte, Texas
Freeport, Louisiana
Midland, Michigan
Oyster Creek, Texas
Plaquemine, Louisiana
Baton Rouge, Louisiana
Pasadena, Texas
Calvert City, Kentucky
Geismar, Louisiana
Lake Charles, Louisiana
Guayanilla, Puerto Rico
Deer Park, Texas
Norco, Louisiana
Carson, California
43
-------
Table 7 (Concluded)
PRODUCERS AND LOCATIONS FOR HALOOLEFINS
Compound
Producer
Site
Trichlorethylene
Chloroprene
Diamond Shamrock Corp.
Dow Chemical Co.
Ethyl Corp.
Occidental Petroleum Corp.
PPG Industries
Dow Chemical Co.
Shell Chemical Co.
Vinylidene chloride Dow Chemical Co.
PPG Industries
Deer Park, Texas
Freeport, Texas
Baton Rouge, Louisiana
Taft, Louisiana
Lake Charles, Louisiana
Freeport, Texas
Deer Park, Texas
Norco, Louisiana
Freeport, Texas
Plaquemine, Louisiana
Lake Charles, Louisiana
44
-------
Table 8
PHYSICAL AND CHEMICAL PROPERTIES OF HALOOLEFINS
Compound, Synonyms
Vinyl chloride; chlo-
roethylene; chloro-
ethene;
Trichloroethylene;
trichloroethene;
Chloroprene;
2-chloro-l,3-buta-
diene
Vinylidene chloride;
1,1-dichloroethylene;
1,1-dichloroethene;
Mol.
wt.
62.50
131.39
88.54
96.94
M.P.
°C
B.P.
°C
-153.8 -13.37
760
-73
-122.1
87
760
59.4.
6.4"
760
100
37
760
Density
D
A
max
(log (
0.910620 1.370020
4
20 20
1.4642 1.4773
2
20
0.9583 1.4583
20
1.218
20
1.4249
20
<200
(vapor)
Solubility
Slightly soluble in
water, soluble in
alcohol, very soluble
in ether
Slightly soluble in
water, infinitely
soluble in alcohol and
ether, soluble in chloro-
form and acetone
223(4.15) Slightly soluble in
(hexane) water, infinitely
soluble in ether, acetone,
benzene, and other organic
solvents
<200 Insoluble in water, soluble
(vapor) in alcohol, acetone, and
benzene, very soluble in
chloroform and ether.
-------
Environmental Transformation
In water, oxidation of haloolefins by RO radical and hydrolysis of
vinylic halides will be extremely slow with half-lives of more than 20
years (Hill et al., 1976). Unless biodegradation is very rapid, the
most likely fate of haloolefins is bioaccumulation or volatilization
to the atmosphere and oxidation.
The relatively low solubility and high volatility of most low
molecular weight chloroolefins will promote their rapid transfer to
the atmosphere, where we estimate that half-lives toward HO radical are
less than 50 hours; for conjugated olefins such as chlorobutadienes
the half-life will be much less than 10 hours. Products formed by
oxidation of these compounds are predicted to be COC12, HC1, and CO
with likelihood of formation of C^O as well. Most simple and conjugated
haloolefins will also oxidize to lower molecular weight acids (Mill and
Hendry, 1976). Oxidation of perhaloolefins by oxygen is a rapid process
with neat substrate but exhibits exceptional sensitivity to inhibitors
(Mayo, 1965). In natural waters we would not expect this process to be
very important.
Bioaccumulation
Based on its log P value and some experimental evidence, vinyl
chloride should not accumulate appreciably in animals. We found no
experimental data demonstrating whether vinylidene chloride and chloro-
prene do or do not accumulate, however, their log P values suggest that
they should not. Trichloroethylene has a high log P value, and experi-
mental evidence indicates that it may bioaccumulate.
Our calculated log P value for vinyl chloride is 0.60, which
indicates that it is slightly lipophilic; however, its affinity for
lipid material is too low to expect significant bioaccumulation.
Green and Hathaway (1975) reported that in rats, the main route of
excretion of vinyl chloride after oral, i.v., or i.p. administration
is pulmonary. Excretion is rapid and the percentage of the dose excreted
increases with the dose. The amount excreted through the lungs may be
46
-------
as high as 99% in 24 hours. Chronic administration (60 days) of vinyl
chloride did not affect elimination of a single dose of 14C-labeled
vinyl chloride. These investigators also studied the metabolism of
vinyl chloride and have devised a metabolic scheme for the compound.
Hefner et al. (1975) determined the amount of radioactivity in
12 tissues, including fat, from rats exposed to 14C-vinyl chloride for
up to 2.5 hours. They found radioactivity only in the liver, bile,
and kidney.
Vinylidene chloride is slightly more lipophilic than vinyl chloride,
having a calculated log P value of 0.73. Like vinyl chloride, it should
not accumulate significantly in animals. Although we found considerable
information about its toxicity, we did not find any information pertinent
to bioaccumulation.
The experimentally determined log P value for trichloroethylene is
2.29, which indicates that it may bioaccumulate.
Cohen and coworkers (1958, cited in Walter et al., 1976) reported
detectable levels of trichloroethylene in the blood, brain, adrenals,
fat, heart, kidney, liver, lung, muscle, pancreas, spinal cord, cerebral
spinal fluid, spleen, and thyroid of animals exposed to the compound
for periods up to 219 hours. The relative amounts of trichloroethylene
in these tissues were not reported in the secondary source because the
data were not adequate for determining the relationship of the concen-
tration in the tissues. We found no other reference to the distribution
of the compound in different tissues and therefore cannot verify the
bioaccumulating potential suggested by the partition coefficient.
According to Stewart and coworkers (1962), trichloroethylene
appears in the blood of humans about 30 minutes after the beginning of
exposure. After cessation of exposure, the blood concentration rapidly
diminishes. Pfaffli and Backman (1972) also observed a rapid reduction
of trichloroethylene in human blood after cessation of exposure;
however, they found detectable levels in the blood and expired air up
to 15 hours after exposure was stopped. Stewart and coworkers (1970)
47
-------
observed that in humans urinary excretion of trichloroacetic acid, a
biotransformation product of trichloroethylene, increased progressively
after cessation of exposure and reached a peak after five days. These
studies suggest that after absorption, trichloroethylene is partly
stored in tissues and released slowly to be excreted unchanged or as
biotransformation products. It is conceivable that repeated exposure
would lead to a buildup of the compound in tissues.
Chloroprene has a calculated log P value of 0.57, which indicates
that it has a low propensity to bioaccumulate. We did not find any
information on its fate, distribution, or retention in animals.
48
-------
6. ALDEHYDES
Production and Properties
Formaldehyde is a very important material commercially, and
acrolein is produced in appreciable quantities, but only in about
one hundredth the amount of formaldehyde. Estimated production (in
millions of pounds per year) is:
Formaldehyde
Acrolein
5765
61
(1974)
(1974)
Sources for formaldehyde are quite extensive and are not limited to any
one area of the country. Producers and locations are given in Table 9.
Synonyms and physical and chemical properties are given in Table 10.
Table 9
PRODUCERS AND LOCATIONS FOR ALDEHYDES
Product
Producer
Location
Formaldehyde
Allied Chemical Co.
Borden, Inc.
Celanese Corp.
E.I. du Pont de Nemours
and Co., Inc.
49
South Point, Ohio
Demopolis, Alabama
Deboll, Texas
Fayetteville, N. Carolina
Geisma, Louisiana
Louisville, Kentucky
Sheboygan, Wisconsin
Fremont, California
Kent, Washington
LaGrande, Oregon
Missoula, Montana
Springfield, Oregon
Bishop, Texas
Newark, New Jersey
Rock Hill, S. Carolina
Belle, W. Virginia
La Porte, Texas
Healings Springs, N.
Carolina
-------
Table 9 (Continued)
PRODUCERS AND LOCATIONS FOR ALDEHYDES
Product
Producer
Location
E.I. du Pont de Nemours
(continued)
G A F Corp.
Georgia-Pacific Corp.
Gulf Oil Corp.
Hercules, Inc.
International Minerals
and Chemical Corp.
Monsanto.Co.
Occidental Petroleum Corp.
Reichhold Chemicals, Inc.
Acrolein
Rohm and Haas Co.
Skelly Oil Co.
Tenneco Inc.
Union Carbide
Univar Corp.
Wright Chemical Corp.
Shell Chemical Co.
Union Carbide Corp.
Linden, New Jersey
Toledo, Ohio
Calvert City, Kentucky
Albany, Oregon
Columbus, Ohio
Coos Bay, Oregon
Crossett, Arkansas
Russellville, S.
Carolina
Taylorsville, Mississippi
Vienna, Georgia
Vicksburg,.Mississippi
Louisiana, Missouri
Wilmington, N. Carolina
Seiple, Pennsylvania
Sterlington, Louisiana
Addyston, Ohio
Chocolate Bayou, Texas
Eugene, Oregon
North Tonawanda, New York
Hampton, S. Carolina
Kansas City, Kansas
Houston, Texas
Malvern, Arkansas
Moncure, N. Carolina
Tacoma, Washington
Tuscaloosa, Alabama
Philadelphia, Pennsylvania
Springfield, Oregon
Winnfield, Louisiana
Fords, New Jersey
Garfield, New Jersey
Bound Brook, New Jersey
Eugene, Oregon
Acme, N. Carolina
Norco, Louisiana
Taft, Louisiana
50
-------
Table 10
PHYSICAL AND CHEMICAL PROPERTIES OF ALDEHYDES
Compound
Formaldehyde;
formalin, meth-
anal; oxomethane,
oxymethylene
Acrolein;
2-propenal; acry-
ladehyde; allyl
aldehyde
Mol.
Wt.
30.03
56.07
M.P.
°C
-92
-86.95
-21
760
-79.6
20
52.5-
53.5
Density
-20
0.815
D
20 20
0.8410 1.4017
4
max
(log
155(4.37)
175(4.26)
(vapor)
207(4.05)
in alcohol
Solubility
Soluble in water,
alcohol, and
chloroform; in-
finitely soluble
in ether, acetone,
and benzene
Very soluble in
water, soluble in
alcohol, ether,
and acetone
-------
Environmental Transformation
Formaldehyde is almost entirely hydrated in water. It is non-
volatile and is inactive toward photochemical dissociation. Higher
aldehydes are less hydrated, more volatile, and absorb weakly in the
solar region dissociating to RCO and H atoms, followed by oxidation to
peroxides and cleavage products (Calvert and Pitts, 1966). Oxidation
by RO radical in water may be fairly rapid to give similar products.
Acrolein would be expected to oxidize at the double bond to give keto
aldehydes and cleavage products. Biotransformation of many aldehydes
in water would be expected to be an important competing process for
which we have no reliable data. In general, neither the aldehydes nor
their oxidation products would be expected to be persistent in water.
In air aldehydes are expected to photodissociate to RCO and H atoms
rapidly and competitively with their oxidation by HO radical, for a
half-life of 2 to 3 hours (Calvert and Pitts, 1966; Hendry, 1977). In
chamber studies N02 accelerates this process (Bufalini et al., 1972) .
The photochemical process would lead to peracylnitrates and peroxy
radicals that would enter the photochemical cycle. Oxidation by HO*
would give the same products, to the extent that HO'removes the
aldehydic H atom, but also could give oxidation of the alkyl chain
in higher aldehydes, phenol from aromatic aldehydes, and addition to
acrolein's double bond. Aldehydes will not persist in the atmosphere,
but their contribution to smog may be significant (Hendry, 1977).
Bioaccumulation
Neither formaldehyde nor acrolein shows a tendency to bioaccumulate.
Their calculated log P values are similar and negative. Formaldehyde is
a normal product of metabolism and is rapidly metabolized to formic acid
and carbon dioxide. We found little information on acrolein and none
of it was pertinent.
Formaldehyde reacts rapidly with tissues to cause crosslinking
and precipitation of proteins. Upon entering the bloodstream, it
52
-------
disappears rapidly by reactions with body tissues and by oxidation to
formic acid (Kitchens et al., 1976). It is a natural metabolic
product that plays an important role in the one-carbon pool (Koivusalo,
1956, 1970). Its experimentally determined log P value of -0.96
suggests that it should not bioaccumulate.
The calculated log P value for acrolein is -.090; hence accumulation
in tissues should be negligible.
53
-------
7. ALKYL AND BENZYL HALIDES
Production and Properties
Alkyl halides such as methyl chloride and ethylene dichloride are
produced in large quantities for use in the production of Freons, vinyl
chloride, and trichloroethylene. Both ethylene dichloride and ethylene
dibromide are used as scavenging agents in gasoline and as fumigants.
Estimated production (in millions of pounds per year) is as follows:
1,2-Ethylene dichloride 9165 (1974)
1,2-Ethylene dibromide 332 (1974)
Methyl chloride 647 (1974)
Producers and locations are given in Table 11. Synonyms and the physical
and chemical properties are listed in Table 12.
Benzyl chloride's principal use is as an intermediate in the
synthesis of other materials. Estimated production was 100 million
pounds per year in 1976. Producers and plant locations are given
below.
Benzyl chloride Monsanto Co. Bridgeport, New Jersey
Stauffer Chemical Co. Edison, New Jersey
Tenneco Chemicals Fords, New Jersey
Synonyms and the physical and chemical properties of benzyl chloride
are also listed in Table 12.
55
-------
Table 11
PRODUCERS AND LOCATIONS FOR ALKYL HALIDES
Compound
Producer
Location
1,2-Ethylene dichloride Allied Chemical Co.
Continental Oil Co.
Diamond Shamrock
Dow Chemical Co.
Ethyl Corp.
B.F. Goodrich Co.
PPG Industries
Shell Chemical Co.
Stauffer Chemical Co.
Union Carbide Corp.
1,2-Ethylene dibromide
Methyl Chloride
Vulcan Materials Co.
Dow Chemical Co.
Ethyl Corp.
Great Lakes Chemical
Corp.
PPG Industries
Allied Chemical Co.
Continental Oil Co.
Diamond Shamrock
Dow Chemical Co.
Dow Corning Corp.
E.I. du Pont de Nemours
and Co., Inc.
Ethyl Corp.
General Electric Co.
Stauffer Chemical Co.
Union Carbide Corp.
Vulcan Materials Co.
Baton Rouge, Louisiana
Westlake, Louisiana
Deer Park, Texas
Freeport, Texas
Oyster Creek, Texas
Plaquemine, Louisiana
Baton Rouge, Louisiana
Calvert City, Kentucky
Lake Charles, Louisiana
Guayanilla, Puerto Rico
Deer Park, Texas
Norco, Louisiana
Carson, California
Taft, Louisiana
Texas City, Texas
Geisma, Louisiana
Magnolia, Arkansas
Midland, Michigan
Magnolia, Arkansas
El Dorado, Arkansas
Beaumont, Texas
Moundsville, W. Virginia
Westlake, Louisiana
Belle, W. Virginia
Freeport, Texas
Plaquemine, Louisiana
Carrollton, Kentucky
Midland, Michigan
Niagara Falls, New York
Baton Rouge, Louisiana
Waterford, New York
Louisville, Kentucky
Institute and South
Charleston, W. Virginia
Newark, New Jersey
56
-------
Table 12
PHYSICAL AND CHEMICAL PROPERTIES OF ALKYL AND BENZYL HALIDES
Compound, Synonyms
Mol,
Wt.
M.P.
B.P.
Density
D
Solubility
Ul
1,2-Ethylene dichl
oride
98.96
760 20 20
-35.36 83.47 1.2351 1.4448
Slightly soluble in
water; soluble in acetone,
chloroform, benzene, and
organic solvents; very
soluble in alcohol;
infinitely soluble in
either
1,2-Ethylene dibro- 187.87
mide
1,2-Dibromoethane;
Freon 150
Methyl chloride;
chloromethane 50.49
9.79 131.36
29.110
760
-97 -23.76
760
20 20
2.1792 1.5387
4
0.92
20
1.3661
-10
Slightly soluble in water;
soluble in acetone, benzene;
very soluble in alcohol;
infinitely soluble in
ether.
Soluble in water and
alcohol; infinitely
soluble in ether and
chloroform
-------
Table 12 (Concluded)
PHYSICAL AND CHEMICAL PROPERTIES OF ALKYL AND BENZYL HALIDES
Ol
00
Compound, Synonyms
cy-Chloro toluene;
(chloromethyl) ben-
zene; tolyl chloride
Mol.
126.56
M.P.
-39
B.P.
Density
D
179.3
760
20 20
1.1002 1.5391
Solubility
Insoluble in water;
infinitely soluble in
alcohol, ether, and
chloroform
X (log r) = 217 (3.85) in alcohol.
max
-------
.Environmental Transformation
Low molecular weight alkyl halides through butyl or pentyl halides
are relatively insoluble, volatile, and unreactive. Thus transfer
to the atmosphere from water or soil is a likely competitive environ-
mental process. Reliable rate constants for hydrolysis of many alkyl
halides are availhble and a number of values are given in Table 3.
Methyl chloride is persistent with a half-life (hydrolysis) of over one
year. Most other simple alkyl halides are much more reactive with
half-lives of 50 days or less. Benzyl halides are very reactive with
half-lives of a few minutes. Vicinal (1,2-dihalo) dihalides and
hydroxyalkyl halides are unreactive in water.
The hydrolysis data suggest the following generalizations about
RX:
The rate of hydrolysis is greatest when X is Brs
least when X is F. Br is more reactive than Cl
by a factor of 5 to 10.
0 Rate of hydrolysis increases as R changes from
primary to secondary to tertiary in the ratio
1:1:1000 for Cl and 1:20 for Br.
° Allylic groups enhance the rate of hydrolysis
of primary halides by a factor of 5 to 100;
benzyl groups enhance the rate by a factor of 50.
0 Geminal (1,1-dihalo) dihalides and 2-hydroxyalkyl
halides are about one-thousandth as reactive as
the simple alkyl halides.
Oxidation of alkyl halides in water by RO radical is not significant
(ti/2 > 100 years). However oxidation in the atmosphere should be
relatively rapid, t]/2 < 20 hours, for most alkyl halides to give acid
halides and halogenated ketones and aldehydes.
Benzyl halides will be more reactive toward HO- than alkyl halides
by a factor of 3 to 10 and give mostly phenols, e.g., chloromethylphenol
from benzyl chloride (Kenley and Hendry, 1977).
59
-------
Bioaccumulation
Methylene dichloride, ethylene dibromide, and methyl chloride
are slightly lipophilic. Log P values for these compounds range from
1.48 to 1.92, indicating that these compounds have a slight tendancy
to accumulate in fatty tissue. However, experimental evidence indicates,
at least for methylene and ethylene dichloride, that these compounds
do not accumulate in lipids.
The experimentally determined value of log P for ethylene
dichloride is 1.48, which indicates that it is slightly lipophilic,
thus has a slight tendency to bioaccumulate. We believe that bio-
accumulation would be minimal. The compound is rapidly excreted mostly
unchanged in the urine of mice, with about 95% excreted in 24 hours
(Yllner, 1971). Ethylene dichloride is metabolized (Heppel and Porter-
field, 1948; Bray et al., 1952; Van Dyke and Wineman, 1971; Yllner, 1971).
Enzymatic dechlorination has been observed in in vitro systems; however,
in intact animals, Yllner (1971) found that the compound is metabolized
to monochloroacetic acid through 2-chloroethanal with liberation of
carbon dioxide.
The calculated log P value for ethylene dibromide is 1.60,
indicating that it is slightly lipophilic and may have a slight tendency
to accumulate. Johns (1976) reported that Lauze (1922) obtained data
indicating a mild tendency of ethylene dibromide to accumulate in the
liver and brain of unspecified laboratory animals. He found that the
compound is excreted unchanged by the lungs and is partially decomposed
in the body, producing bromide that appears in the urine.
A more recent study (Plotnick and Conner, 1976) using radiotracer
techniques, showed that ethylene dibromide, administered intraperitoneally
in guinea pigs, distributed itself throughout the body and concentrated
primarily in the kidneys, liver, and adrenals. The kidney and liver
contained the highest percentage of the injected dose, which is not
surprising because the study showed that the kidney was the major route
of excretion and the liver is usually the organ that metabolizes or
detoxifies foriegn chemicals. Only a small amount of the administered
dose was found in fatty tissue.
60
-------
We
found no information concerning bioaccumulation for methyl chloride
The experimentally determined log P value for this compound is 1.92,
which is higher than the values for methylene dichloride and ethylene
dichloride, but in the same order of magnitude. Although its log P
value indicates that it has a slight affinity for lipids, we do not
expect it to bioaccumulate significantly.
a - Chlorotoluene is lipophilic as indicated by its experimentally
determined log P value of 2.30. We found no other pertinent information
on this compound.
61
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8. PEROXIDES, HYDROPEROXIDES, PERACIDS, AND HYDROGEN PEROXIDE
Production and Properties
Organic peroxides are used in a broad spectrum of commercial
and laboratory polymerization reactions. Estimated production figures
for the commercially more important peroxides are given below ( in
pounds per year).
Cumene hydroperoxide
Di-tert-butyl peroxide
Hydrogen peroxide
tert-butyl hydroperoxide
Succinic acid peroxide
3062 million
3 million
1.9 million
>1000
>1000
(1974)
(1974)
(1974)
(1974)
(1974)
Producers and sites are given in Table 13. Table 14 lists the synonyms
and chemical and physical properties of the peroxides.
Compound
Table 13
PRODUCERS AND LOCATIONS FOR PEROXIDES
Producer Location
Cumene hydroperoxide
Allied Chemcial Corp.
Hercules, Inc.
Pennwalt Corp.
Reichhold Chems., Inc.
Di-tert-butyl peroxide Akzona, Inc.
Dart Industries, Inc.
The Norac Co., Inc.
Pennwalt Corp.
Reichhold Chemicals, Inc.
Shell Chemical Co.
Witco Chemical Corp.
Hydrogen peroxide
Allied Chemical Co.
Barium & Chemicals, Inc.
E.I. du Pont de Nemours
FMC Corp.
Pennwalt Corp.
PPG Industries
Shell Chemical Co.
Frankford, Pennsylvania
Gibbstown, New Jersey
Genesco, New York
Austin, Texas
Burt, New York
Elyria, Ohio
Azusa, California
Crosby, Texas
Austin, Texas
Martinez, California
Marshall, Texas
Syracuse, New York
Steubenville, Ohio
Memphis, Tennessee
S. Charleston, W. Virginia
Vancouver, Washington
Wyandotte, Michigan
Barberton, Ohio
Norco, Louisiana
63
-------
Table 13 (Concluded)
Compound Producer Location
tert-Butyl
hydroperoxide Akzona Inc. Burt, New York
Dart Industries, Inc. Elyria, Ohio
The Norac Co., Inc. Azusa, California
Oxirane Corp. Bayport, Texas
Pennwalt Corp. Genesco, New York
Witco Chemical Corp. Marshall, Texas
64
-------
Table 14
PHYSICAL AND CHEMICAL PROPERTIES OF PEROXIDES
Compound. Synonyms
Mol.
wt.
M.P.
C°0
-40
B.P.
20
Density
760
111 20
7Q197 0.794
Di-tert-butyl peroxide; 146.23
Bis (1 , 1-dimethylethyl)
peroxide; tert-butyl
peroxide
Hydrogen peroxide; 34.02 -0.43 152 1.463
hydrogen dioxide
tert-Butyl hydro 90.12 -8 35 " 0.896
peroxide; 1,1-dimethyl-
ether hydroperoxide
20
1.3890
20
1,4007
20
Solubility
Insoluble in water,
soluble in organic sol-
vents, infinitely soluble
in acetone
Mixible with water;
soluble in ether; decom-
posed by many organic
solvents,
Soluble in organic
solvents
-------
Environmental Transformation
Di-t-alkylperoxides such as di-t-butyl peroxide are only slightly
volatile but moderately soluble in water and therefore are most likely
to remain in aquatic systems. Contrary to common belief, tertiary
peroxides are thermally stable to at least 60°C and not very susceptible
to trace metal ion catalysis. These peroxides have weak tailing absorbance
in the solar spectrum, which leads to 0-0 bond cleavage to give RO
radicals, which cleave to ketones and R* radicals (Calvert and Pitts,
1966). This process will be slow: we estimate t]_/2 > 20 hours. Neither
hydrolysis nor oxidation by RO radical is likely to be competitive with
photochemistry in aquatic systems. The same photochemical process will
occur in the atmosphere at a somewhat higher rate (no cage return of
radicals) and compete with oxidation by HO radical, which is relatively
slow.
Hydroperoxides, peracids, and hydrogen peroxide are all more polar,
less volatile, and more reactive than the dialkyl peroxides because of
the relatively weak and polar 0-H bond that makes peroxides susceptible
to radical reactions as well as to reactions with metal ions and light,
2+ 2+
The presence of Fe and Mn in aquatic systems in catalytically
significant amounts (> 1 ppm) suggests that these peroxides will decompose
rapidly (t-^/2 < 10 hours) by reactions with metal ions to give alcohols,
acids, or water (depending on the starting peroxide) (Hiatt et al., 1968).
Photochemical and HO radical oxidation are likely pathways for
transformation of peroxides in the atmosphere. We estimate that half-
lives will be less than a few hours. As an added source of free radicals,
peroxides will contribute to buildup of photochemical smog.
Reliable data on the rates of radical reactions and metal catalyzed
reactions of peroxides in water are lacking. Some recent data indicates
that such reactions may be appreciably different in rate from those
measured in organic solvents (Hiatt, 1977).
66
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Bioaccumulation
Out literature search indicated that little is known about the
fate and distribution of these five peroxides in animals. Their log P
values are less than 1, which indicates that none shows a potential to
bioaccumulate in intact form, i.e., without reacting chemically with
biological constituents.
Much has been published on the role of hydrogen peroxide in
metabolism. It is a normal metabolite in both plants and animals
(Halliwell, 1974; Thurman et al., 1975; Hildebrandt et al., 1973;
Chumakov and Smelyanskaya, 1974). Since the experimentally determined
log P value for hydrogen peroxide is -1.42, bioaccumulation should not
occur.
We did not find any pertinent information on bis(dimethylethyl)
peroxide. Of the five peroxides investigated, it has the highest log P
value (0.68); however, its affinity for lipids is too low to expect
significant accumulation in animals.
Tertiary butyl hydroperoxide has a calculated log P value of -1.30
and should therefore not bioaccumulate. In vitro studies with rats
indicate that the compound is reduced specifically by glutathione
peroxidase in erythrocytes. (Sies, 1972).
No pertinent information on cumene hydroperoxide was found. It has
a calculated log P value of -0.16 and therefore should not bioaccumulate.
Succinic monoperoxy acid is strongly lipopholic, having a calculated
log P value of -3.04. Accumulation of this compound in animals is not
expected.
67
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9. POLYHALOMETHANES
Production and Properties
Polyhalomethane uses range from solvents and grain fumigants to
intermediates and fire extinguishants. Production estimates (in millions
of pounds per year) for 1974 were:
Carbon tetrachloride 1,600
Chloroform 300
Producers and locations are given in Table 15. Synonyms and physical
and chemical properties are given in Table 16.
Environmental Transformation
Carbon tetrachloride is predicted to have a half-life of about
7,000 years in aquatic systems at 1 ppm; in the atmosphere where the
great bulk of CC1 is found, the half-life in the troposphere is at
least 10 years. Indeed, recent detailed analyses of the distribution
of CC1 in the environment indicate that most of what has been produced
4
in the past 60 years is still mostly in the atmosphere with lesser
amounts in soil and water. No natural sources of CC1 have been identi-
4
fied; nor are any needed to account for its present environmental
burden (Singh et al., 1976).
Other polyhalomethanes including CHC1 , CHBr and CH Cl are
o o 2i &
only slightly more reactive in water but much more reactive in the
atmosphere. Hydrolyses of these compounds in water have half-lives of
about 3500 and 700 years, respectively. Oxidation by HO radical will
be relatively rapid: half-lives of one to two months in the
69
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Table 15
PRODUCERS AND LOCATIONS FOR POLYHALOMETHANES
Product
Carbon
tetrachloride
Producer
Location
Chloroform
Allied Chemical Corp.
Dow Chemical Co.
Moundsville, West Virginia
Freeport, Texas
Pittsburg, California
Plaquemine, Louisiana
E.I. du Pont de Nemours Corpus Christi, Texas
and Co., Inc.
South Charleston, West
Virginia
Le Moyne, Alabama
Louisville, Kentucky
Niagara,Fa 11s, New York
Geismar, Louisiana
Wichita, Kansas
FMC Corp.
Stauffer Chemical Co.
Vulcan Materials Co.
Allied Chemical Co.
Diamond Shamrock Corp.
Dow Chemical Co.
Moundsville, West Virginia
Belle, West Virginia
Freeport, Texas
Plaquemine, Louisiana
E.I. du Pont de Nemours Niagara Falls, New York
and Co., Inc.
Stauffer Chemical Co. Louisville, Kentucky
Vulcan Materials Co. Newark, New Jersey
Wichita, Kansas
70
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Table 16
PHYSICAL AND CHEMICAL PROPERTIES OF POLYHALOMETHANES
Chloroform;
trichloromethane
Vapor
Compound /Synonyms
Carbon tetrachloride;
tetrachlorome thane
Mol.
Wt.
153.82
M.P. B.P.
( C) ( C) Density
-22.96 76. 7576° 1.5942,20
4
RD
1.466420
100(23)
40(4.3)
Pressure,
mm( C)
400 (57.8)
Solubility
Insoluble in water,
soluble in alcohol,
infinitely soluble
in ether, benzene,
and chloroform
119.38 -63.5
61.2
760
.18
25
1.4916" 1.4433"" 400 (42.7); Slightly soluble
100 (10.4) in water, soluble
in acetone, in-
finitely soluble
in alcohol, ether,
and benzene
-------
troposphere seem likely, giving COC12 or COB^. These products may be
washed out in rain where they will hydrolyze to CO^ and HC1 or HBr-
Bioaccumulation
The saturated hydrocarbons, methyl chloride, chloroform, and
carbon tetrachloride, have log P values of 1.92, 1.92, and 2.70 respec-
tively. Carbon tetrachloride concentrates rapidly in adipose tissue
(McCollister, et al., 1951; Reynolds, 1967; Rao and Rechnagel, 1969)
and has a long biological half-life as indicated by detectable amounts
found by Stewart and coworkers (1961) in the expired air of human
patients two weeks after exposure to CC1 vapor.
Chloroform also concentrates rapidly in fat. Cohen and Hood (1969)
14
administered C-labeled chloroform by inhalation to mice for 10 minutes,
and sacrificed the animals 0, 15, and 120 minutes after exposure by
immersion in liquid nitrogen. They prepared autoradiograms of longitudi-
nal sections of the body and also analyzed samples of selected tissues
for radioactivity. The tissues analyzed were blood, brain, muscle, lung,
kidney, liver, fat, and brown fat. In animals sacrificed immediately
after exposure, the total concentration of radioactivity in these tissues
was 6550 counts/min/mg, with 25.6% in fat and 48.2% in brown fat. In
animals sacrificed 15 minutes after exposure, these tissues contained a
total of 3270 counts/min/mg of which 29.1% resided in fat and 45.6%
resided in brown fat. The tissues from animals killed 120 minutes after
exposure contained 922 counts/min/mg or about 14% of that found in the
animals killed immediately after exposure. In these animals, 78.8% of
the radioactivity was distributed fairly evenly among the liver (27.1%),
fat (28.8%), and brown fat (22.9%).
We found no information on methyl chloride; however, because its
log P value is the same as that of chloroform, we believe that it may
also accumulate in animal tissues.
72
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10. AROMATIC AMINES
Production and Properties
Most of the compounds in this group have been the subject of a
previous report (Radding et al., 1975) and are important as intermediates
for the production of dyes, antioxidants, or in polymers. Production
figures are given below (in pounds per year).
4,4'-Methylenebis(2-chloroaniline) 7.7 million (1972)
1-Naphthylamine 7 million (1974)
3,3'-Dichlorobenzidine 4.6 million (1972)
Benzidine 1.5 million (1972)
2-Biphenylamine <1000 (1974)
4-Biphenylamine
-------
Table 17
PRODUCERS AND LOCATIONS FOR POLYHALOMETHANES
Compound
Producer
Location
4,4'-Methylenebis(2-
chloroaniline)
1-Naphthylamine
3,3' -Dichlorobenzidine
(as hydrochloride)
Benzidine (as sulfate)
2-Biphenylamine
4-Biphenylamine
4,4'-Methylenebis(2-
methylamine)
2-Naphthylamine
Anderson Development Co
E. I. du Pont de Nemours
& Co., Inc.
American Hoechst Corp.
Lakeway Chemicals, Inc.
The Upjohn Co.
City Chemical Corp.
MacKenzie Chemical Works, Inc,
Aceto Chemical Co., Inc.
N.A.
N.A.
Sigma Chemical Co.
Adrian, Michigan
Deepwater Point,
New Jersey
Coventry, Rhode Island
Muskegon, Michigan
North Haven, Connecticut
Jersey City, New Jersey
Central Is lip, New York
Carlstadt, New Jersey
N.A.
N.A.
St. Louis, Missouri
74
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Table 18
PHYSICAL AND CHEMICAL PROPERTIES OF AROMATIC AMINES
Oi
Compound
4 ,4 ' -Methylenebis(2-chloroaniline);
4,4'-Methylenebis(2-chlorobenzamine);
Bis(3-chloro-4-aminophenyl)-methane
1-Naphthylamine; 1-aminonaphthalene;
2-naphthylamine; 2-naphthylamine
Benzidine; 4,4'-diaminobiphenyl; C.I.
Azoic Diazo Component 112; (1,1'-biphenyl)-
4 ,4 '-diamine
2-Biphenylamine;
2-phenylaniline ;
2-biphenylamine
3,3'-Dichlorobenzidine; (1,1 -biphenyl)-
4, 4'-diamine,3',3'-dichloro-; C.I. 23060
4-Biphenylamine;
4-phenylaniline; Zenylamine;
4-biphenylylamine
4,4'-Methylenebis(2-methylaniline);
4,4'-methylene-di-o-toluidine;
4,4'-methylenebis(2-roethylbenzenamine)
2-Naphthylamine;
j-naphthylamine;
C.I. 37270
MoL
Wt.
267
M.P.
110
B.P.
Density
max
(log e)
Solubility
760
1.43.19
184.24
169.23
50
122-
128
51-3
300.8 1.1229 1.6703
160 12
sublimes
400 74°
299760
242(4.27)
320(3.71)
in alcohol
287(4.4)
in alcohol
300(3.5)
in alcohol
253.13 132-3
169.23 53.4 302.
191
15
143.19 113
306.1
no
1.06144
Slightly soluble in water; very
soluble in alcohol and ether
Slightly soluble in hot water^
very soluble in alcohol and ether
Insoluble in water; soluble in
alcohol, ether, and benzene
Almost insoluble in water, readily
soluble in alcohol and benzene
278(4.24) Slightly soluble in water; soluble
in alcohol in alcohol, ether, and chloroform
236(4.78)
280(3.82)
292(3.73)
340(3.28)
in alcohol
Very soluble in hot water, soluble
in cold water, alcohol, and ether
-------
In the atmosphere, oxidation by HO-to phenols and amine oxides,
hydroxylamines and ring open structures is probably rapid. Chlorine
substitution should have little effect on rates of oxidation in the
atmosphere but may retard oxidation in water by RO radical.
Reliable data on the oxidation, photochemical, and sorption pro-
perties of aromatic amines in water are lacking and are badly needed
for reliable assessment.
Bioaccumulation
The partition coefficient (log P) for benzidine is reported as 1.81.
We calculated the log P to be 1.4. Both reported and calculated values
indicate that benzidine should not accumulate appreciably in the body.
This hypothesis is supported by data obtained by Kellner and coworkers
(1973), who found in rats, dogs, and monkeys, almost no radioactivity
14
in the tissues 7 days after intravenous administration of C-labeled
benzidine. They reported that although the urine of these animals con-
tained benzidine, most of the radioactivity was associated with meta-
bolites. Bradshaw and Clayson (1955), Clayson (1959), and Fabre (1960)
identified these metabolites as 4'-acetoamido-4-aminodiphenyl, 3-hydro-
xybenzidine, 4,4'-diamino-3-diphenylyl hydrogen sulfate, 4'-acetamido-
4-amino-3-diphenylyl hydrogen sulfate, 4'-amino-4-diphenylyl sulfamic
acid, and N-glucuronides. They also found several acid-stable unknowns.
We calculated the partition coefficient for 3,3'-dichlorobenzidine
(DCS) as 2.8. No empirically determined values were found in the
literature. Our calculated value suggests that the compound has a slight
propensity to accumulate in body tissues.
Kellner and coworkers (1973) reported that DCB is excreted almost
unchanged in the urine of rats, dogs, and monkeys and that it is
76
-------
excreted less rapidly than benzidine. Aksamitnaya (1959) found four
metabolites in the urine of rats given DCB orally over a long period
and in a single large dose; one of the metabolites was benzidine. The
compound has been identified in the urine of workers in a pigment plant
(Akiyama, 1970).
Our calculated partition coefficient for o>-naphthylamine is 1.8.
The value reported in the literature is 2.15. The partition coefficient
for @-naphthylamine is probably in the same range. Neither compound
should accumulate significantly in body tissues. Both compounds are
metabolized by a mixed-function oxidase. Both have also been detected
in the urine of workers in factories where these compounds are manu-
factured (Takemura et al., 1972).
No information was found concerning the accumulation of 4,4'-
methylene-bis(2-chloraniline) in animal tissues. It and certain metabolites
have been identified in the urine of workers in plants where the compound
is manufactured (Linch et al., 1971). The compound has a calculated par-
tition coefficient of 3.5, and therefore may accumulate significantly in
animal tissues.
We found no information concerning the fate or distribution of
4,4'-methylenebis(2-methyl)benzenamine in animals. It has a relatively
high potential for bioaccumulation as indicated by its calculated log P
value of 3.92.
77
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11. POLYCHLORINATED BIPHENYLS
Production and Properties
Many polychlorinated biphenyls have been produced commercially
under the names of Aroclor, Chlorextal, Dykanol, Inerteen, Noflamol,
Pyranol, and Therminol. Most, however, are being phased out and at
the present time Monsanto may be the only producer at the Sanget,
Illinois, plant. In 1974, total production was estimated as 40
million pounds per year.
The physical properties of chlorobiphenyls (tetrachloro- or
higher) are given in Table 19.
Environmental Transformations
Biphenyl and its chlorinated derivatives (PCBs) are lipophilic,
nonvolatile, unreactive compounds that tend to bioaccumulate. They
present a well-established environmental problem, and little can be
added to what has already been summarized in several reviews of their
pathways (Durfee et al., 1976). They are ubiquitous in the environ-
ment and persist for long periods in water- Evaporation to the atmos-
phere is also thought to be important. Some of the chlorinated and
polychlorinated biphenyls starting with 4,4-dichlorobiphenyl will
absorb above 300 nm. Crosby and Moilanen (1973) report that suspensions
of these compounds in water undergo dechlorination and photohydrolysis
to give 4-chlorobiphenyl, 4-chloro-4'-hydroxybiphenyl, and trace amounts
of 2-chlorobenzofurans. Ruzo et al. (1972) and Herring et al. (1972)
found similar photoreduction in hexane solvent or in neat mixtures.
79
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Table 19
PHYSICAL PROPERTIES OF CHLOROBIPHENYLS
Melting Boiling Point
Compound Point (°C) °C (mm Hg)
3,4,3',4'-Tetrachlorobiphenyl 172 230 (50)
3,4,2',5'-Tetrachlorobiphenyl 103
2,6,2',6'-Tetrachlorobipnenyl 198
2,5,3',5'-Tetrachlorobiphenyl 162
2,4,2',4'-Tetrachlorobiphenyl 83
2,5,2',5'-Tetrachlorobiphenyl 84-85
2,4,5,3',4'-Pentachlorobiphenyl 179 195-220 (10)
3,4,5,3',4',5'-Hexachlorobiphenyl 198
2,4,6,2',4',6'-Hexachlorobiphenyl 111.5-112
2,3,4,5,2',4',5'-Heptachlorobiphenyl 240-280 (20
2,3,5,6,2',3',5',6',-Octachlorobiphenyl 161
2,3,4,5,6,2',3',4',5',6',-Decachlorobiphenyl 330
80
-------
Quantitative data on the fate of chlorinated biphenyls in aquatic
systems are not yet available, but we think it is likely that photo-
lysis will lead mainly to reduction in aquatic systems.
PCBs may be absorbed on particulates and dispersed in the atmos-
phere. In this form they may be oxidized by HO radical with half-lives
in excess of 8 hours. Products would be phenols and quinones. Direct
photolysis to less chlorinated products might also occur and would
give products less susceptible to photolysis (shorter wavelength
absorbance) but more reactive to HO radical (t, < 8 hours). Again, the
2
quantitative aspects of these reactions have not been examined.
Bioaccumulation
It is well-known that polychlorinated biphenyls accumulated in
animal tissues and that some accumulate to a greater degree than others.
Much of the knowledge of the environmental and health effects of PCBs
is reviewed in the Proceedings of the National Conference of Polychlori-
nated Biphenyls (Ayer, 1976). We reviewed that report as well as many
others, but have cited only a few that we feel are significant.
It appears that the degree of PCB accumulation in animal tissues
increases with the number of chlorines attached to the biphenyl
molecule. A survey conducted by Kutz and Strassman (In Ayer, 1976)
of PBCs in adipose tissue of people living in the United States,
showed that the most frequently encountered forms of PCBs are the
penta-, hexa, and heptachlorobiphenyls.
Matthews and Anderson (1975) found that chlorobiphenyl, dichloro-
biphenyl, pentachlorobiphenyl, and hexachlorobiphenyl are rapidly
removed from the blood of rats after a single intravenous injection
and stored initially in the liver and muscles. From the liver and
81
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muscles, PCB is redistributed to the skin and adipose tissue, and the
rate of deposition in these tissues increases with the degree of
chlorination. The rate of removal of these PCBs from the skin and
adipose tissue, excretion in the urine, and total excretion decreases
as the degree of chlorination increases. During the 42-day obser-
vation period, more than 90% of administered dose of mono-, di-, and
pentachlorobiphenyls was excreted; however, these investigators calc-
ulated that less than 20% of the administered dose of hexachlorobiphenyl
would ever be excreted. Excretion was not appreciable until the
parent compound had been metabolized to more polar compounds.
These two studies indicate that the polychlorinated biphenyls
with at least five chlorine molecules have the greatest potential for
accumulating in animal tissues and that susceptibility to metabolic
degradation to more polar compounds has a considerable influence in
the magnitude of bioaccumulation of a compound. We calculated log P
values of 7.24, 8.05, and 8.86 for tetrachloro-, pentachloro, and
hexachlorobiphenyl, respectively. Although these values indicate that
these PCBs have a very strong affinity for lipids, pentachloro- and
perhaps tetrachlorobiphenyl are metabolized and excreted.
82
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12. AZO DYES
Production and Properties
Azo dyes form the largest class of dyes and have found wide appli-
cation in almost all manufactured goods. Estimated production is given
below (in pounds per year) for the four compounds in this study.
2HMethyl-4-[(2-methylphenyl)-
azo ] -benzenamide
4-Aminoazobenzene
4-Dimethylaminoazobenzene
Azobenzene
Solvent dyes are produced by several companies; however, it is
difficult to determine exactly which of the solvent dyes are produced
by each company and where. Manufacturing sites and manufacturers are
given below for the general class of solvent dyes.
450,000
330,000
10,000
< 1,000
(1973)
(1974)
(1971)
(1974)
Company
Site
Allied Chemical Company
American Color and Chemical Corp.
American Cyanamid Co.
Atlantic Chemical Industries, Inc,
Ciba-Geigy Corp.
Dye Specialties, Inc.
GAP Corp.
Kewanee Industries, Inc.
Morton-Norwich Products, Inc.
Nyanza, Inc.
Passaic Color & Chemical Co.
Hilton-Davis Chemical Co.
Buffalo, New York
Lock Haven, Pennsylvania
Bound Brook, New Jersey
Damascus, Virginia
Marietta, Ohio
Nutley, New Jersey
Mclntosh, Alabama
Jersey City, New Jersey
Rensselaer, New York
Louisville, Kentucky
Paterson, New Jersey
Ashland, Massachusetts
Paterson, New Jersey
Cincinnati, Ohio
83
-------
Physical and chemical properties along with synonyms are given in
Table 20.
Environmental Transformations
Simple azobenzene dyes including azobenzene are polar and nonvolatile
compounds that probably exhibit little propensity to transfer to the
atmosphere from water. However, their high lipophilicity may lead to
significant absorption by sediments having significant organic content.
Those azo dyes with primary amino groups, such as 4-aminoazobenzene,
should exhibit chemical properties in water similar to those of aromatic
amines including rapid oxidation by RO to hydroxylamines and nitrosamines
(Sections 28 and 29). The azo groups are strong chromophores that effi-
ciently absorb visible and near UV solar radiation and may lead to a
variety of photochemical transformations. Meier (1971) has provided a
detailed discussion of the photochemistry of azo dyes and notes (p. 462)
that very little information is available other than that both oxidation
and reduction of azo dyes occur slowly and that oxygen inhibits reduction.
We conclude that, in aquatic systems where natural organics may be
present in low concentrations of 5-10 ppm along with oxygen, photoreduction
to hydrazines and amines is possible but is likely to be very slow
except in oxygen-poor water. Some experiments to measure these rates
are obviously needed. Biogradation is a likely fate along with bio-
accumulation .
Dispersions of any azo dye in the atmosphere are likely to be
oxidized by HO radical at rates comparable to those found for other
aromatics, i.e., half-lives of 8 hours or less.
84
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Table 2O
PHYSICAL AND CHEMICAL PROPERTIES OF AZO DYES
00
Compound, Synonyms
2-Methyl-4-[(2-methyl-
phenyl)azo] benzenamide;
C.I. Solvent yellow 3;
4-(o-tolylazo)-
o-toluidine; o-amino-
azotoluene
4-Aminoazobenzene;
C.I. Solvent Yellow 1;
4-(phenylazo) -
benzenamine
4-Dimethylaminoazo-
benzene; C.I. Solvent
Yellow 2; N,N-dimethyl-
4-(phenylazo)-
benzenamine; butter
yellow
Azobenzene;
benzeneazobenzene;
diphenyldiazene
Mol.
Wt.
M.P.
B.P.
Density _Q (
225.28 101-102
225.30
117 Decomp.
182.23
71
293
1.20
326C4.28)
490(3.40)
in alcohol
Solubility
Insoluble in water,
soluble in alcohol,
ether, and chloroform
251(4.0) Slightly soluble in
384(4.4) hot water; soluble in
in alcohol hot alcohol, benzene,
cold chloroform, ether
Insoluble in water;
soluble in ether,
chloroform, benzene,
petroleum ether, mineral
acids, oils
243(4.02) Slightly soluble in
281(3.72) water; soluble in alcohol,
433(3.18) ether, and benzene
in alcohol
-------
Bioaccumulation
The log P values for azobenzene, 4-aminoazobenzene, 4-dimethyl-
aminoazobenzene, and 2-methyl-4-[(2-methylphenyl)azo] benzenamide are
3.82, 3.50, 4.58, and 4.24, respectively. These values indicate that
these compounds are highly lipophilic. We did not find any information
concerning their distribution or retention in animal tissues. These
are probably good examples of the fact that highly lipophilic compounds
are frequently metabolized extensively. Robinson and coworkers (1964)
postulated that 4-aminoazobenzene may become bound in tissues, perhaps
by a reaction between the amino group and tissue constituents. The
compound is metabolized to a number of different compounds (Matsumoto
and Terayama, 1962; Ishidate and Hashimoto, 1962); however, it does not
undergo methylation to form more potent carcinogins such as 4-methyl-
aminoazobenzene or 4-dimethylaminoazobenzene (Matsumoto, 1965).
4-M.methylaminoazobenzene binds to DNA and other proteins (Warwick,
1969; Roberts, 1969; Chauveau and Benoit, 1973). Its metabolism has
been extensively studied, and many of its biotransformation products
have been identified.
We found no information on the distribution or retention of 2-methyl-
4-[(2-methylphenyl)azo] benzenamine in animals. Its high log P value
(experimental) suggests that it has a high tendency to bioaccumulate.
86
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13. CARBAMIC ACID ESTERS
Production and Properties
Carbamates (or urethanes) are used in plastics, pesticides, phar-
maceuticals, surface-active agents, dye intermediates, and corrosion
inhibitors. Ethyl carbamate, the only compound considered here, is
used as an intermediate in organic synthesis, in pesticide formulations,
and as a solvent. Annual estimated production was 100,000 pounds per
year in 1972 .
Synonyms for ethyl carbamate are: carbamic acid, ethyl ester, and
urethane. Physical and chemical properties are given below.
Molecular weight 89.10
Melting point (°C) 48.5-50
Boiling point ( C) 185
21
Density 0.9862
n 1.414452
D
Solubility Very soluble in water,
alcohol, ether, benzene,
chloroform
Environmental Transformation
Simple carbamate esters such as ethyl carbamate are polar, soluble
in water, and nonvolatile. They will not transfer to the atmosphere or
absorb in sediments to any significant extent. Hydrolysis of carbamates
to alcohol, amine or ammonia, and CO is generally extremely slow at 25°C
^
and pH 7. Half-lives for hydrolysis in Table 3 indicates that, with the
exception of aromatic esters having an ArOC(0)NHAr structure, they will
87
-------
not hydrolyse at 25°C and pH 7 for centuries. Oxidation is also negli-
gbly slow. Photohydrolysis of aromatic carbabates is a possible, faster
process. Biodegradation may be a facile process for many carbamates,
preventing their accumulation, but we have not looked for data on this
process.
We estimate that in the atmosphere ethyl carbamate will oxidize
with HO radical with a half-life of 47 hours. Products would probably
include ammonia, CO , and acetaldehyde. Aromatic carbamates might
£
photolyse, but we have found no data.
Bioaccumulatj.on
Ethyl ester of carbamic acid, commonly called urethane, has an
experimentally determined log P value of -0.75; therefore, bioaccumulation
of this compound is not expected. Studies have shown that the compound
or its metabolites binds with DNA (Pound and Lawson, 1976; Prodi et al.,
1073; Lawson, 1974; Lawson and Pound, 1972, 1973); however,- this is not
evidence of bioaccumulation.
The compound is metabolized by laboratory animals (Nery, 1968;
Grogan et al., 1970). Repeated administration stimulates metabolism of
the compound (Braeunlich, 1968).
88
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14. HYDRAZINES
Production and Properties
Hydrazines are used over a broad spectrum of industries ranging
from agricultural chemicals, medicinals, textile agents, and plastics,
to propellant mixes. The production figures for the compounds listed in
this class are given below (in pounds per year).
Hydrazine 3.1 million (1971)
1,1-Dimethylhydrazine < 1.1 million (1973)
Hydrazine carboxamide > 1000 (1974)
1,2-Dimethylhydrazine < 1000 (1974)
Producers and locations are as follows:
Compound
Hydrazine Fairmont Chemical Co.,Inc. Newark, New Jersey
Hummel Chemical Co., Inc. South Plainfield, New Jersey
Olin Corp. Lake Charles, Louisiana
Uniroyal, Inc. Geismar, Louisiana
1,1-Dimethylhydrazine FMC Corp. Baltimore, Maryland
Olin Corp. Lake Charles, Louisiana
Hydrazine Carboxamide Fairmount Chemical Co.,Inc.Newark, New Jersey
Olin Corp. Rochester, New York
1,2-Dimethylhydrazine N.A. N.A.
Synonyms and physical and chemical properties are given in Table 21.
Environmental Transformations
Data on likely environmental fates of hydrazines are sparse. However,
from their properties and from work in this laboratory we can make some
reasonable assumptions as to likely pathways.
89
-------
Table 21
PHYSICAL AND CHEMICAL PROPERTIES OF HYDRAZINES
VD
O
Mol.
wt.
M.P. B.P.
Compounds, Synonyms
Hydrazine
1,1-Dimethylhydrazine,
dimazine; N,N-
dimethylhydrazine
Hydrazine carbox-
amide; aminourea;
carbazamide;
carbamic acid,
hydrazide;
semicarbazide
1,2-Dimethylhydrazine; 60.11
N,N '-dimethylhydrazine;
hydrazomethane
32.05
60.11
75.07
81
753
Density
15
1.4 113.5 1.011
752 22
63 0.7914
96
0.8274
20
D
max
(log ?)
1.470
22
1.4075
22
Solubility
Very soluble in cold water,
soluble in alcohol
Very soluble in water,
alcohol, ether
231(1.2) Insoluble in ether, benzene,
in chloroform; soluble in
alcohol alcohol; very soluble in
water
20
1.4209 235(4.0) Infinitely soluble in
280(3.1) water, alcohol, and ether
in
alcohol
-------
All the simple hydrazine derivatives are polar, nonvolatile, and
soluble in water. As a result none of these compounds will transfer to
the atmosphere at significant rates; nor are they likely to absorb to
sediments in significant amounts.
In water, oxidation by molecular oxygen to diimides and then to
nitrogen, possibly catalyzed by metal ions
0
2
RNHNH - [RN = NH] - RH + N + H 0
£ £ £
(Wagnerova et al., 1973) may be the most important fate (Ross et al.,
1971).
Methylhydrazine reacts rapidly with oxygen in the gas phase at con-
centrations of < 0.01 M (t± < 1 hour), dimethylhydrazine more slowly,
from which we conclude that these compounds will not persist in water
or in the atmosphere. Oxidation by HO radical in the gas phase is
reported to be rapid with a half-life of less than 1 hour (Hack et al.,
1974) .
Bioaccumulation
The log P values for hydrazine, 1,1-dimethylhydrazine, 1,2-dimethyl-
hydrazine, and hydrazine carboxamide are negative, indicating that none
of these compounds should accumulate in animal tissues. However, high
levels of hydrazine and 1,1-dimethylhydrazine appear to impair kidney
function. This could prevent normal excretion of these compounds and
their metabolites and increase the overall body burden, which in turn
would increase the probability of binding of the compounds to proteins
or deposition in adipose tissue.
Hydrazine has a calculated log P value of -3.08. A study by Smith
and Clark (1972) showed that hydrazine is rapidly absorbed into the
91
-------
blood stream of dogs but that blood levels decline slowly after reaching
a peak. After administration of high levels of hydrazine, blood levels
peaked and remained elevated. This suggested an impairment of detoxication
and/or renal function. Continued elevated hydrazine blood levels can
contribute to bioaccumulation. Mass action could increase the probability
of binding of hydrazine to cellular constituents as well as of deposition
of hydrazine in adipose tissue.
We found no pertinent information concerning hydrazine carboxamide.
Its calculated log P value of -2.53 indicates that it should not normally
bioaccumulate.
92
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15. ACYL HALIDES AND KETENE
Production and Properties
While the compounds listed here do have some end-use as is,
most are used as intermediates in the preparation of Pharmaceuticals,
pesticides, textile finishing compounds, and so on. Production estimates
are given below (in pounds per year).
Benzoyl chloride 15,000,000
Diethylcarbamoyl chloride 15,000
Dimethylcarbamoyl chloride <1000 (1974)
Ketene N.A.
Producers and locations are as follows:
Compound
Producer
Location
Benzoyl chloride
Diethylcarbamoyl
chloride
Dimethylcarbamoyl
chloride
Ketene (as dimer)
Velsicol Chemical Corp.
Hooker Chemical Corp.
Stauffer Chemical Co.
Aldrich Chemical Co.
Ashland Chemical Co.
Ashland Chemical Co.
Eastman Chemical
Products, Inc.
FMC Corp.
Chattanooga, Tennessee
Niagara Falls, New York
Edison, New York
Milwaukee, Wisconsin
Great Meadows, New Jersey
Great Meadows, New Jersey
Kingsport, Tennessee
Meadville, Pennsylvania
Synonyms and physical and chemical properties are given in Table 22.
93
-------
Table 22
PHYSICAL AND CHEMICAL PROPERTIES OF ACYIATING AGENTS
Compound, Synonyms
Benzoyl chloride; ben-
zoic acid, chloride;
benzenecarbonyl
chloride
Mol. M.P.
wt. °C
140.57
B.P.
o Density
760 20
197.2 1.2120.
§ 4
71
D
max
(log
1.5537
20
Solubility
Decomposes in water and
alcohol; soluble in ben-
zene and carbon disulfide;
infinitely soluble in ether
Diethylcarbamoyl chlo-
ride; diethylcarbamic
chloride; diethylcar-
bamyl chloride
135.60 186
Decomposes in hot water
or hot alcohol
Dimethylcarbamoyl
chloride; dimethylcar-
bamyl chloride; di-
methylcarbamic chloride
Ketene; carbomethene;
ethonone; methylene
ketene
42.04
-151 -56,
-41'
760
330(1.0) Decomposes in water,
gas alcohol, and ammonia;
slightly soluble in ether
and acetone
-------
Environmental Transformation
In water, acyl chlorides hydrolyze rapidly with half-lives of only
a few seconds for benzoyl chloride to an hour or so for ethyl
chloroformates (Table 3); dimethylcarbamyl chloride has a half-life of
less than 5 minutes. In all cases hydrolysis products include HC1 but
otherwise are probably not harmful or persistent. Because of these
compounds' high reactivity toward water, other processes cannot compete
under most conditions in aquatic systems. Ring substituents in benzoyl
chloride such as nitro or methyl can increase the rate by factors of
five to ten (Hudson and Wardill, 1950).
In the atmosphere we calculate that half-lives for hydrolysis in
moist air (50% humidity) will be about 40 times longer than in pure
water assuming no special solvent effects. Thus half-lives will be
10 minutes, 3 hours, and 40 hours for benzoyl, dimethylcarbamyl
chlorides, and ethyl chloroformate, respectively. Oxidation by HO
radical will be an important process only for the chloroformate.
Ketene is a powerful acylating agent that reacts rapidly with a
variety of nucleophiles under laboratory conditions to give, with H«0,
acetic acid and, with alcohols, acetate esters. In the aquatic environ-
ment these reactions probably are slow, but we have found no recent
data on which to base reliable estimates of persistence. Photolysis
of ketene in the UV region up to 320 nm gives CO and methylene (CH2);
methylene reacts rapidly (k > 108 M"1 s"1) with a wide variety of
organic compounds including oxygen. Available data (Calvert and Pitts,
1967) suggest that photolysis in the atmosphere will be rapid
(t-, ij < 10 hours) and will compete with oxidation by HO radical. Products
probably include CH20, C02, and CO.
95
-------
Bioaccumulation
Our literature search did not produce any information concerning
the fate or distribution of benzyl chloride, dimethylcarbamoyl chloride,
diethylcarbamoyl chloride, or ketene in animals. The log P values for
these compounds indicate that their tendency to bioaccumulate is in-
significant.
The calculated log P values for dimethylcarbamoyl chloride, diethyl-
carbamoyl chloride, and benzoyl chloride are -1.20, -0.12, and 0.97,
respectively.
We could not calculate a log P value for ketene because of insuf-
ficient information; however, ketene is a reactive polar compound that
would probably have a log P value of less than 1 and therefore is not
expected to accumulate appreciably in animal tissues.
96
-------
16. PHOSPHORIC ACID ESTERS
Production and Properties
In general, phosphoric acid esters are intermediates in synthesis,
in organophosphorus insecticides, and as alkylating agents. The estimated
production rates for 1974 for the two esters discussed here are given
below (in pounds per year).
Diethyl phosphate 7 million (1974)
Dimethyl phosphate < 1000 (1974)
Triethyl phosphate is produced by Eastman Chemical Products, Inc., in
Kingsport, Tennessee. Synonyms and physical and chemical properties
are given in Table 23.
Environmental Transformation
Simple trialkylphosphates are nonvolatile, very polar, and water
soluble. Transfer to the atmosphere will be negligible. Kinetic data
for hydrolysis of several alkyl and aryl phosphates are listed in
Table 3. Half-lives are generally over 1 year for all but the nitrophenyl
phosphates (methyl parathion and parathion), and unless biodegradation
of these esters is facile they will persist. Adsorption of the esters
to sediments is probably unimportant, as is oxidation in water. Photo-
hydrolysis of suitably substituted arylphosphates is much faster than
thermal hydrolysis and might become important in oligotrophic waters
(Mabey et al., 1976).
Rates of oxidation of phosphate esters by HO radical are similar to
those for sulfate esters and other organic esters: very slow unless
activating groups such as phenyl or long alkyl chains are present;
half-lives are over 100 hours. Direct photochemical processes in the
atmosphere are probably not important even for aromatic esters.
97
-------
Table 23
PHYSICAL AND CHEMICAL PROPERTIES OF PHOSPHORIC ACID ESTERS
00
Compound,
Synonyms
Mol.
wt.
M.P.
°C
B.P.
°C
760
Density
20
D Solubility
20
Triethyl phosphate; 182.16 -56.4
phosphoric acid;
triethyl ester
Trimethyl phosphate; 140.08 -42(a)
phosphoric acid, -62(0)
trimethyl ester
215-6
103
25
197.2
8524
760
1.0695
1.2144
20
1.4053 Soluble in water with
slight decomposition;
Soluble in ether and
benzene; very soluble
in alcohol
20
1.3967 Slightly soluble in
alcohol; soluble in
ether, very soluble
in water
-------
Bioaccumulation
The log P values for triethyl and trimethyl phosphate indicate that
neither should bioaccumulate significantly. Triethyl phosphate is
somewhat lipophilic as indicated by its experimentally determined log P
value of 1.11. Trimethyl phosphate is slightly lipophilic, having an
empirical log P value of -0.52.
99
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17. AZIRIDINES
Production and Properties
Ethylenimine (aziridine) was discussed in Task Order Report I
(Radding et al. , 1975) and only an update is included here in addition
to other aziridines. Estimated production for 1974 is given below
(in pounds per year).
Ethylenimine <4.8 million
1-Aziridineethanol 10,000
Propylenimine >1,000
Ethylenimine is produced by Dow Chemical Company in Freeport, Texas.
Physical and chemical properties and synonyms are given in Table 24.
Environmental. Trans format ion
Hydrolyses of aziridines to amino alcohols generally and of
ethylenimine (El) specifically to give 2-hydroxyethylamine are acid-
catalyzed processes for which there are no direct measurements at pH 7
and 25°C. However, kinetic analysis of the pK data for El reported
3.
by Buist and Lucas (1957) and the data of Early et al. (1958) on
hydrolysis of El in strong acid provide an estimate of the persistence
of El under environmental conditions.
Ethylenimine is weakly basic (pK = 8); thus at pH 8 half of El is
Q.
protonated and at pH 7, 90% is protonated. Early (1958) found the
rate constant for hydrolysis k of protonated El to be 5.2 x 10 sec
at 25°C. Thus the persistence of El at pH 7 in water is ^ 370 hours,
very similar to the persistence of epoxides. At pH 6 (CC^-buffered)
the half-life will be only slightly shorter because 99% of El will be
protonated rather than 90%; however, at pH 8 where only 50% of El is
protonated, the half-life will be nearly doubled. Other aziridines
101
-------
TABLE 24
PHYSICAL AND CHEMICAL PROPERTIES OF AZIRIDINES
o
ro
Compound, Synonyms
Ethylenimine;
Aziridine; dehydro-
azirine; azirane;
1-Aziridinethanol;
2-(Hydroxyethyl)ethyl-
enimine; N-(2-hydroxy-
ethyl)aziridine;
2-(l-aziridinyl)ethanol
Propylenimine;
2-methylaziridine;
2-me thyle thylenimine
Mol.
Wt.
43.07
M.P.
B.P.
Density
n,.
56756 0.8321?°
4
6G-6775 0.812
A max
(log £)
Solubility
soluble in alcohol;
very soluble in ether,
acetone, and benzene;
infinitely soluble in
water and other organic
solvents
-------
should hydrolyze at nearly the same rate as El based on the similarity
of rates for most aliphatic epoxides (see above), but no specific rate
data were found.
Oxidation of El in water by RO- is probably very slow. Although El
is volatile, escape to the atmosphere probably will be very slow because
of the basicity and polarity of El. Similarly sorption to sediments
or organisms will be low. Good data on physical transport processes
for aziridines are lacking.
The fate of aziridines in the atmosphere is expected to be oxidation
by HO radical with t, ,„ of 56 hours for aziridine and methylaziridine
but 22 hours for aziridineethanol. No photochemical or hydrolytic
processes appear important, but this conclusion could be modified if
aziridines were absorbed on acidic particulates fly ash where
hydrolysis would be a likely fate. No specific information is avail-
able on this matter.
Bioaccumulation
With the exception of ethylenimine, our literature search produced
no information directly or indirectly concerned with bioaccumulation
of the three aziridines. The log P values of these aziridines were
less than zero, which indicates that they tend to be hydrophilic and
therefore should have little tendency to bioaccumulate.
For ethylenimine, we calculated a log P value of -1.12. According
to Wright and Rowe (1967), this compound is rapidly excreted by rats.
About 55% of the injected dose was excreted in 96 hours. The kidneys
play a major role in the excretion of this compound. Unexcreted
ethylenimine was found evenly distributed throughout the body; very
little was found in fatty tissue.
The calculated log P value for propylenimine is -0.46. We do not
expect this compound to accumulate in fatty tissue.
103
-------
1-Aziridineethanol is slightly more hydrophilic than ethylenimine
and has a calculated log P of -1.79. It should not accumulate in fatty
tissue.
104
-------
18. LACTONES
Production and Properties
3-Propiolactone was discussed in Task One Report (Radding et al. ,
1975) and only an update is included here. Production has been
estimated at less than 1000 pounds per year for 1974.
Synonyms for g-propiolactone are: 3-hydroxy propanoic acid and
lactone. Physical and chemical properties are given below.
Molecular weight 72.06
Melting point (°C) -33.4
Boiling point (°C) 162 decomposition, 5110
Density 1.1460^°
nD 1.410520
Solubility Decomposes in water and alcohol;
soluble in chloroform; infinitely
soluble in ether
Environmental Transformation
Lactones are subject to rapid hydrolysis in aquatic systems. A
careful study of the hydrolysis of g-propiolactone (PL) to give
3-hydroxypropionic acid was made by Long and Purchase (1950). The
reaction is rapid at 25°C, independent of acidity, and only weakly
catalyzed by hydroxide ion. Based on the rate constant for hydrolysis
in neutral water (k ) of 3.3 10~3 min"1, we estimate the half-life
w
of PL in water at 25°C and pH 7 to be 3.5 hours and appreciably less
in ocean or brackish water where chloride ion will also cleave the
lactone ring. Base-catalyzed hydrolysis is not important to PL until
the pH reaches 11 (k^ = 100 liter mol"1 min~l). Butyrolactone is
reported by the same workers to be only a fourth as reactive as PL.
We expect higher lactones to resemble butyrolactone in their reactivity
toward water at pH 7.
105
-------
Oxidation of lactones by RO'in water are estimated to have half-
lives of over 20 years.
The high boiling points, high solubilities, and polarities, coupled
with the rapid hydrolysis rates in water, make it likely that the major
fate of lactones will be to remain in water to hydrolyze to the hydroxy
acids.
If released in the atmosphere, lactones will be oxidized to mixtures
of bifunctional 1-, 2-, and 3-carbon compounds with half-lives of ^ 100
hours. Rain is likely to wash out lactones to soil and streams.
Photochemical cleavage of lactones in the atmosphere seems unlikely
since they have no significant absorption in the solar region.
We uncovered no information concerning bioaccumulation of
3-propiolactone. However, it has a partition coefficient of -0.3
(calculated), is rapidly hydrolyzed, and is highly reactive. These
factors strongly suggest that it does not accumulate in tissues.
106
-------
19. ALKYL SULFATES
Production and Properties
Both the dimethyl and the diethyl sulfates are used as alkylating
agents. Production estimates for 1974 show greater than 1000 pounds
per year manufactured for both.
Dimethyl sulfate is produced by E.I. du Pont de Nemours & Co., Inc.
at Bell, West Virginia, and at Linden, New Jersey. Diethyl sulfate is
produced by Union Carbide Corporation at Texas City, Texas.
Synonyms and physical and chemical properties are given in
Table 25.
Environmental Transformation
Sulfate esters are relatively polar and nonvolatile compounds that
are not likely to transfer to the atmosphere from water. Hydrolysis of
sulfates at pH 7 and 25°C is a facile process (see Table 3) with half-
lives of only 1 to 2 hours for ethyl and methyl sulfates. Cyclic
sulfates are also readily hydrolyzed under these conditions. Some data
on sulfonate esters, included for comparison, show that they are much
more resistant to hydrolysis (t, /2 '^17-40 hours). The product sulfuric
or sulfonic acids would be damaging only in concentrated spills. Oxida-
tion of these esters in water is negligible, as is bioaccumulation and
absorption to sediments.
Simple alkyl sulfates in the atmosphere would wash out in rain
and hydrolyze. Oxidation by HO radical would be very slow for dimethyl
sulfate and only moderately rapid for diethyl sulfate. Products
probably would be sulfonic acid, CH?0, CO, and CO^.
107
-------
Table 25
PHYSICAL AND CHEMICAL PROPERTIES OF ALKYL SULFATES
o
oo
Compound/Synonyms
Diethyl sulfate;
Sulfuric acid, diethyl
ester; ethyl sulfate;
DES
Dimethyl sulfate;
sulfuric acid,
dimethyl ester; methyl
sulfate; DMS
96
15
Density
126.13 -31.75 188.5760 1.3283
20
154.19 -24.5 208(sl. 1.1774^° 1.4004
decomp.
20
1.3874
20
X. max
(log )
265
(undil.)
Solubility
Insoluble in cold water;
decomposes in hot water
and in hot alcohol;
infinitely soluble in
alcohol and ether
Insoluble in carbon
disulfide; soluble in
water, ether, and
benzene; infinetely
solution in alcohol
-------
Bioaccumulation
Dimethyl sulfate and diethyl sulfate are strongly lipophobic and
are not expected to bioaccumulate. Dimethyl sulfate is rapidly broken
down in the body. Diethyl sulfate may behave similarly; however, we
found no information concerning its fate in biological systems.
Our calculated log P value for dimethyl sulfate and diethyl sulfate
are -4.26 and -3.18, respectively. Swann (1968) reported that the
dimethyl sulfate disappears completely from the blood of rats within
three minutes after intravenous injection. The concentration in the
blood one minute after injection was one-sixth of that expected if the
compound had distributed itself evenly in body water; hence, the author
concluded that the compound undergoes rapid breakdown.
109
-------
20. SULTONES
Production and Properties
Sultones are becoming increasingly important as intermediates in
organic synthesis to introduce sulfo-groups into materials. Production
of each in 1974 was estimated at less than 1000 pounds per year.
Synonyms for the propane sultone are: 1,2-oxathiolane, 2,2-dioxide
and 3-hydroxy-l-propanesulfonic acid, gamma-sultone. For butane sultone,
there is: 1,2-oxathiarie, 2,2-dioxide; 4-hydroxy-l-butanesulfonic acid,
delta sultone; and delta-valerosultone.
Environmental Transformations
These cyclic esters of hydroxysulfonic acids are very polar and
nonvolatile. Like lactones, these esters hydrolyze relatively quickly
in neutral water by a. base-catalyzed process, the rate of which depends
on ring size: 1,3-sultones hydrolyze about 40 times as fast as
1,4-sultones compared with a factor of only 4 times for lactones.
Bordwell et al., (1959) showed that methyl substituents on 1,3-sultones
retarded the rate of hydrolysis for steric reasons, and we can probably
generalize that observation to include other substituents particularly
in the a and B (to oxygen) positions. The rate effect of methyl groups
is substantial: about 200 times for a,B trimethylsulfone.
The atmospheric chemistry of sultones is unknown; hydrolysis in
moist air is negligibly slow. We have estimated that oxidations by
HO radical will be slow with half-lives over 50 hours.
Bioaccumulation
We did not find any information on the uptake, fate, distribution,
excretion, or accumulation of 1,3-propane sultone or 1,4-butane
sultone in biological systems. 1,3-Propane sultone is hydrophilic and
111
-------
not expected to accumulate in body tissues. For this compound, we
calculated a log P value of -2.82. Like 1,3-propane sultone, 1,4-butane
sultone is hydrophilic and has a calculated log P of -2.45.
112
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21. ARYL DIALKYLTRIAZENES
Production and Properties
Triazenes are used not only as intermediates, but also as herbicides,
rodent repellents, and as antineoplastic agents. Production for 1974 has
been estimated at less than 1000 pounds per year for both l-phenyl-3,3-
dimethyltriazene and l-(4-chlorophenyl)-3,3-dimethyltriazene considered
here .
Synonyms are given below for each compound.
• 3,3-Dimethyl-l-phenyltriazene;
l-phenyl-3,3-dimethyltriazene
• l-(4-Chlorophenyl)-3,3-dimethyltriazene;
1-(4-Chlorophenyl)-3,3-dimethyl-l-triazene
Environmental Transformation
The most reliable data relating to environmental chemistry of
triazenes are those of Kolar and Preussmann (1971) on the hydrolysis of
14 substituted l-aryl-3,3-dimethyltriazenes at 37°C and pH 7. They
reported half-lives ranging from 10 minutes for p-MeO-phenyl to 250 days
for m-NO -phenyl ; the phenyl dimethyltriazene has a half-life of 210
£t
minutes, and p-chlorophenyl dimethyltriazene has a half-life of 40 to
45 hours. No temperature dependence is given, but we estimate that
half-lives would increase by about a factor of 2 at 25°C.
113
-------
Triazenes absorb strongly (e > 10,000) around 310-360 nm and
exhibit fairly rapid phototransformations in organic solvents (Le Fevre
and Liddicoet, 1951). These workers described photolysis of many aryl
dimethyltriazenes on exposure to 4 hours of sunlight. From their data,
we estimate that half-lives of several triazenes including phenyl dimethyl
triazene may be as short as 100 hours. Products are not known; nor do we
know the effect of solvent on the rate of the photoprocess. In the
unlikely event that a triazene were dispersed into the atmosphere, it
would be rapidly oxidized by HO radical (t^ < 4 hours). Products in part
2
would consist of phenols, but some attack at the triazene structure
is likely.
Bioaccumulation
We found no information directly or indirectly concerned with
bioaccumulation of 3,3-dimethyl-l-phenyltriazene or l-(p-chlorophenyl)-
3,3-dimethyltriazene. Experimentally determined log P values for these
compounds indicate that they may accumulate in fatty tissue. 3,3-Dimethyl
1-phenyltriazene has a log P value of 2.59, and the experimentally
determined log P value for the o-chloro isomer of l-(p-chlorophenyl)-3,3-
dimethyltriazene is 3.00.
114
-------
22. DIAZOALKANES
Production and Properties
Diazoalkanes are powerful alkylating agents. Only diazomethane was
selected to represent this class of compounds. Production of diazomethane
was estimated at less than 1000 pounds per year in 1974. Synonyms,
physical and chemical properties are given below.
Mol. M.P. B.P. X max
Compound, Synonyms Wt. (°C) (°C) (log e) Solubility
Diazomethane; 42.04 -145 -2.3 380(0.5) Decomposes in
water; soluble
Azimethylene 408(0.5)
in hot alcohol;
435(0.5) .
soluble in ether
Gas
Environmental Transformations
The simplist diazoalkane, diazomethane, is a yellow explosive gas,
only slightly soluble in water. The extreme reactivity of diazomethane
toward acids, metal ions, surfaces, and visible light makes it unlikely
that diazomethane or other simple diazoalkanes will ever constitute a
significant environmental pollution problem. In water we would expect
rapid decomposition on reaction with natural organics and with particu-
lates to remove it quickly, but we know of no quantitative data. Higher
diazoalkanes particularly phenyl and diphenyldiazomethane are much less
reactive in general, but also exhibit strong visible absorbance and might
persist except for photolysis.
In the atmosphere diazomethane will photolyze fairly rapidly owing
to a very broad absorbance band from 320 to 540 nm (e ~ M cm ) (Brinton
and Volman, 1951; Pitts and Calvert, 1967). Decomposition of diazomethane
on particulates is also a reasonable possibility.
115
-------
Bioaccumulation
We did not find any information on the fate of diazomethane in
biological systems; nor were we able to calculate a log P value for it
because of insufficient data. The compound is reactive and polar and
probably would have a log P of less than 1. We do not expect it to
accumulate significantly.
116
-------
23. HALOALCOHOLS
Production and Properties
Haloalcohols are used as solvents and as intermediates, for example,
in the preparation of insecticides. Production has been estimated as
less than 1000 pounds per year in 1974 for 2-chloroethanol, which is
produced by Union Carbide Corporation at Institute and South Charleston,
West Virginia. l-Chloro-2-propanol is produced by Eastman Kodak Company
at Rochester, New York, and by R.S.A. Corporation at Ardsley, New York.
Synonyms and physical and chemical properties are given in Table 26.
Environmental Transport
Haloalcohols are discussed in Section 7 as alkyl halides.
Bioaccumulation
We found no information on the distribution or retention of
2-chloroethanol or l-chloro-2-propanol in animal tissues. The experi-
mentally determined log P value for 2-chloroethanol is 0.03, and the
calculated log P value for l-chloro-2-propanol is 0.06. These values
indicate that neither compound should accumulate significantly in
animal tissues.
117
-------
Table 26
PHYSICAL AND CHEMICAL PROPERTIES OF HALOALCOHOLS
00
Compound , Synonyms
2-chloroethanol ;
Mol.
Wt.
80.52
M.P.
(°C)
-67.5
B.P.
128760
4420
Density
1.2002720
2-chloroethyl alcohol;
ethylene chlorohydrin
l-Chloro-2-propanol;
lOchloroisopropyl
alcohol; propylene
chlorohydrin
94.54 126-7
750
1.115
20
20
1.44189
20
1.4392
20
Vapor
X max Pressure
(log E) mm(°C)
Solubility
Slightly soluble in
ether; infinitely
soluble in water,
alcohol
Infinitely soluble
in water, alcohol,
and ether
-------
24. HALOETHERS
Production and Properties
One of the compounds included in this class, bis(chloromethyl)
ether was included in the Task One Report (Radding et al. , 1975) and
only an update is given here. Haloethers have been used as textile
finishing agents, as chloromethylation agents in organic synthesis,
and even as solvents. Estimations of production for 1974 are given
below (in pounds per year).
Chloromethyl ether > 1000
Bis(chloromethyl)ether < 1000
Bis(2-chloroethyl)ether < 1000
Producers and locations are given below.
Compound Producers Location
Chloromethylmethyl ether Stauffer Chemical Co. Edison, New Jersey
Bis(2-chloroethyl)ether Buckman Laboratories Cadet, Missouri
Memphis, Tennessee
Synonyms and physical and chemical properties are given in Table 27.
Environmental Transformation^
The carcinogenic properties of bis(chloromethyl)ether (BCME) have
prompted some studies of its chemical properties in the past two years
with the result that reliable estimates can be made of its rates of
hydrolysis and formation under environmental conditions. A few data
on the monochloroether are also available.
Hydrolysis of BCME is complicated by its reformation from t^O,
CH90, and HC1 through a series of rapid reversible reactions. The data
of Frankel et al. (1974) indicate that the net equilibrium constant is
nearly 10~7. Thus
119
-------
K = BCME/(CH20)(HC1) = 10 7
with 4000 ppm CH.,,0 and 40,000 ppm HC1, about 13 ppm of BCME were found
at equilibrium.
Hydrolysis of BCME in water is driven by the large excess of water
(55 M) with the result that, by careful measurements on 1 ppm BCME
dissolved in water, Tou et al., (1974) showed that hydrolysis of BCME
is pH independent and that the rate constant at 20°C is 0.018 sec
Thus, the half-life of BCME at 20°C in water is only ^ 38 seconds. In
moist air (50% relative humidity) Tou and Kallos (1974) found that
k, = 00047 min , corresponding to t.. ,„ = 25 minutes.
IF BCME were spilled in any quantity into water, its low solubility
(ppm range) would minimize hydrolysis except at the interface and promote
volatilization. In the atmosphere, oxidation by HO-to products such as
formic acid, CO, and C02 is likely to be slow (t.. ,„ = >_ 100 hours) but
may compete with hydrolysis at low humidity levels. No direct photolytic
processes can be important; however, formaldehyde formed on hydrolysis
porbably photolyses rapidly (t ,„ < 2 hours), thus preventing reformation
of BCME.
Solvolysis of methyl chloromethyl ether to HC1, CH20, and CH-OH is
extremely rapid. Jones and Thornton (1967) reported that at 25°C in
10 percent dioxane the half-life is only 2.3 seconds. Nichols and
Merritt (1973) claim the relative reactivities of mono- and bis(chloro-
methyl) ether are over 5000/1 in dioxane-water. In pure water the
half-life is probably <0.1 second, and in moist air the half-life would
be <4 seconds. On this basis the persistence of the chloroether in
water or air is fleeting and should not .constitute an environmental
pollutant except under very arid conditions.
120
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Table 27
PHYSICAL AND CHEMICAL PROPERTIES OF HALOETHERS
Compound/Synonyms
Chloromethylmethyl ether;
chloromethoxymethane;
methoxymethyl chloride
Mol. M.P.
Wt. (°C)
80.52
B.P.
Density
-103.5 59.1576° 1.0605 °
A. max
(log E)
1.3974
20
Solubility
Decomposes in
water; soluble
in alcohol,
ether, acetone,
and chloroform
Bis(2-chloroethyl)ether;
2,2'-dichloroethyl ether;
l,l'-oxybis(2-chloroethane);
1,1"-dichloroether
143.02
Bis(2-chloromethyl) ether;
oxybis(chloromethane);
chloromethyl ether
114.96
-24.5
-41.5
178
760
75
20
104
760
1.2199,
20
1.328
15
1.4575
20
1.435
21
Insoluble in
water, slightly
soluble in hot
water; soluble
in alcohol,
ether, and ace-
tone; infinitely
soluble in benzene
and methanol
Decomposes in
water; infinitely
soluble in al-
cohol and ether
-------
Bioaccumulation
Based on the calculated octanol/water partition coefficients (log P) ,
bis(chloromethyl)ether, bis(2-chloroethyl)ether, and chloromethylmethyl
ether show little or no propensity towards accumulating in body tissues.
Bis(chloromethyl)ether has a calculated log P value of -.0.38;
chloromethylmethylether, -0.21; and bis(2-chloroethyl)ether, 0.70.
This last value indicates that bis(2-chloroethyl)ether is slightly
lipophilic, but not enough to cause bioaccumulation problems. Our
search did not produce any experimental data concerning the distribution
of these compounds in tissues or organs.
122
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25. HYDROXYLAMINES
Production and Properties
Hydroxylamines are widely used in the preparation of other inter-
mediates in the chemical industry. The estimation of production for
the year 1974 for each of the three compounds considered in this class
is less than 1000 pounds per year.
Producers and locations are given below for hydroxylamine as both
the hydrochloride and sulfate salts as well as for N-methylhydroxylamine
and 0-methylhydroxylamine.
Compound Producer Location
Hydroxylamine G. Frederick Smith
Chemical Co. Columbus, Ohio
Dow Badische Co. Freeport, Texas
Commercial Solvents
Corp. Sterlington, Louisiana
Virginia Chemical
Inc. Portsmouth, Virginia
N-Methylhydroxylamine Aldrich Chemical CO. Milwaukee, Wisconsin
0-Methylhydroxylamine Eastman Kodak Co. Rochester, New York
Synonyms and physical and chemical properties are given in Table 28.
Environmental Transformations
Because they are polar and water soluble, hydroxylamines should not
transfer from water to the atmosphere or to sediments at significant
rates. Oxidation in water by RO radicals may be rapid, but there are
no reliable data.
123
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S3
-p-
N-Methylhydroxylamine;
N-Hydroxymethanamine;
TABLE 28
PHYSICAL AND CHEMICAL PROPERTIES OF HYDROXYLAMINES
Vapor
Compound ,
Synonyms
Hydroxylamine
Mol.
Wt.
33.03
M
(0,
33
.P.
C)
.05
B.P.
56.5
Density
1.204
Xmax
nD (log e)
Pressure
mm(°C)
10(47.2)
1 (solid)
Solubility
Decomposes in h
water ; soluble
47.06 42 62.515 1.0003^° 1.416420
cold water, acids, alcohol;
very slightly soluble
in ether, chloroform,
benzene, and carbon
disulfide
Slightly soluble in
ether and benzene;
very soluble in
water, methanol, and
ethanol
0-Methylhydroxylamine;
me thoxyami ne
47.06
49.50
Miscible with water,
alcohol, and ether
-------
Oxidation in air by HO radical should be rapid; the aminoxy radicals
can further react to give NO and/or N02> but we know of no experimental
data for these processes.
Bioaccumulation
We did not find any information concerning the distribution of
hydroxylamine or of N-methyl- or 0-methylhydroxylamine in organs and
tissues. Our calculated log P values for these compounds indicate that
they should not bioaccumulate. The calculated log P values for
hydroxylamine, N-methylhydroxylamine, and 0-methylhydroxylamine are
-3.18, -2.90, and -2.47, respectively. The metabolism of these compounds,
particularly hydroxylamine, has been studied (Kadlubar et al.,1973;
Neunhoeffer, 1973).
125
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26. NITROSAMINES
Production and Properties
Nitrosamine derivatives are used, for example, as fuel additives,
antioxidants, pesticides, plasticizers, and in rocket fuels. The two
nitrosamines considered here are estimated to be produced at <1000
pounds per year. Synonyms and physical and chemical properties are
given in Table 29.
Environmental Transformation
Simple nitrosamines, particularly dimethylnitrosamine (DMNA), are
volatile compounds readily formed from the parent amine and nitrous
acid and are potent carcinogens (.Lijinsky and Epstein, 1970). The high
volatility of simple nitrosamines suggests that they will volatilize
rapidly from water if formed there, but Tate et al. (1975) found that
dimethyl, diethyl, and dipropyl nitrosamines appeared to be stable in
soil and water at 250 or 20 ppm for up to 100 days in the dark. Some
rapid initial loss of nitrosamines at 250 ppm due to volatilization to
the atmosphere was noted, but biodegradation appears to be unimportant.
Hanst et al. (1976) calculated that in air DMNA would be formed
rapidly from the amine and HN02: at 0.04 ppm of HN02, any added amine
would form the DMNA at the rate of 2% hr~ . However, photolysis of DMNA
is rapid in sunlight with a half-life of less than an hour during most
parts of the day to give CO, HO, CH 0, and an unknown product. Photolysis
of HNO? is also rapid. Most nitrosamines absorb strongly out to 360 nm
and would be expected to photolyse rapidly also.
We calculate that direct oxidation of DMNA and higher nitrosamines
by HO radical in the atmosphere would be relatively slow, and the evidence
indicates that the dominant process for removal of nitrosamines from the
atmosphere will be rapid photolysis. Recent ambient air analyses by Fine
et al. (1976) confirm that little nitrosamine is present.
127
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Table 29
PHYSICAL AND CHEMICAL PROPERTIES OF NITROSAMINES
Mol.
Compound, Synonyms Wt .
Dimethylnitrosamine; 74.08
N-nitrosadimethylamine;
N-methyl-N-nitrosomethan-
araine ; DMN , DMNA
Diethylnitrosamine; 102.14
N-ethyl-N-nitrosoethan-
amine;nitrosoethyl-
amine; DENA ;
B.P. A. max
°C Density RD (log e)
760 20 20
154 1.0059 1.4358 231(3.85)
346(2.0)
in alcohol
760 20 20
176.9 0.9472 1.4386 233(3.7)
350(1.95)
in alcohol
Solubility
Soluble in
water,
alcohol ,
and ether
Soluble in
water,
alcohol ,
and ether
N-nitrosodiethylamine
-------
Photolysis of nitrosamines in water and other solvents has been
investigated, but the results are in conflict. Chow (1964) and Burgess
and Lavanish (1964) indicate that simple dialkylnitrosamines are nearly
inert to photolysis in solvents. However, Sander et al. (1974) and
Ballweg and Schmael (1967) report that several simple nitrosamines in
water at low concentrations, including DMNA, photolyze rapidly in sun-
light with half-lives of only a few hours.
Hydrolysis of nitrosamines occurs only in relatively acidic solvents
and oxidation by ROwill be very slow.
Bioaccumulation
N-Nitrosodimethylamine and N-nitrosodiethylamine are potent carci-
nogens that are rapidly metabolized and have low log P values, indicating
that the bioaccumulation potential of these compounds is low. The
calculated log P value for N-nitrosodimethylamine is 0.06, which indicates
that it shows nearly equal affinity for octanol and for water and should
therefore not accumulate in body tissues.
There is evidence that both compounds can be synthesized in the
body by bacterial flora. Grilli and coworkers (1975) observed binding
of nitrosodimethylamine to DNA of the calf; and Swann and Magee (1968)
reported evidence for alkylation of nucleic acids of the rat by the
compound. There is evidence that the compound is synthesized in the
intact animal from secondary amines and nitrite (Sen et al., 1969) and
by bacteria in human saliva (Ishiwata et al., 1976).
129
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27. NITROFURANS
Production and Properties
Nitrofuran derivatives are used as food additives, feed additives,
and drugs. In 1974, the estimated production for the three compounds
investigated was less than 1000 pounds per year for each. Synonyms
and some physical and chemical properties are given below:
Compound/ Synonyms Mol
Wt.
M.P-
2-Nitrofuran
B.P.
113.07 29 133.5
123
X max
( log )
Solubility
22.5(3.53) Soluble in water,
3.5(3.91) alcohol, and
ether
Environmental Transformation
Very little data were found to indicate the probable environmental
pathways for these nitrofuran derivatives. As amides they will be stable
for many years toward hydrolysis. 2-Nitrofuran undergoes photosubstitution
by water to give the hydroxy compound (Groens and Havinga, 1974). Other
thiazole nitrofurans should also be susceptible to this same transform-
ation. The relatively intense absorption by nitrofuran around 310-320
nm (e > 10000) (Raffauf, 1950) suggests that this process could be rapid
for all nitrofurans. Unfortunately, no quantum yield data are available
with which to calculate the actual rates of photolysis. If found in
131
-------
the atmosphere, they would probably oxidize with HO radical at rates
comparable to those for other aromatic structures (t.. ,„ < 8 hours).
Bioaccumulation
We found no information concerning the distribution or retention
of the three nitrofurans in animal tissues. 2-Nitrofuran, N-[4-(5-nitro-
2-furanyl)-2-thiazolyl]-acetamide and formamide are metabolized by
laboratory mammals, and reduced acetamide appears to bind to the sulf-
hydryl group of microsomal protein.
2-Nitrofuran shows a tendency to accumulate in animal lipids.
This is suggested by its calculated log P value of 1.86. Paul et al.
(1949) reported finding some unidentified metabolic products of
2-nitrofuran in the urine of rats to which the compound was administered
orally; however, this study was not extensive enough to permit inferences
regarding tissue accumulation.
N-[4(5-nitro-2-furanyl)-2-thiazolyl]- acetamide has a calculated
log P value of -0.60, which suggests that the compound should not
bioaccumulate. One of its metabolites appear to bind to microsomal
protein sulfhydryl groups (Wang et al., 1975). The metabolite is not
a deacylation product (Wang et al., 1974).
N-4-[(5-nitro-2-furanyl)-2-thiazolylJ-formamide is not lipophilic
as indicated by its calculated log P value of -1.14. It should there-
fore not bioaccumulate. Wang and coworkers (1974) observed that the
compound is deformylated in the stomach and intestines of a number of
laboratory mammals.
132
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28. AZIDES
Production and Properties
The only compound considered here is sodium azide, which is used
as an intermediate. Estimate of production for 1974 was less than
1000 pounds per year. Physical and chemical properties are given below.
Solubility
Mol.
Wt.
65.01
M.P.
(°C)
decomp
B.P.
(°C)
decomp
in vacuo
Density
1.84620
41.7 g/100 cc at 17°C in
water
0.314 g/100 cc at 16°C in
alcohol
Environmental Transformation
Inorganic azides are ionic solids with low vapor pressure and (in
some cases) modest solubility in water. Alkali metal azides are rela-
tively stable, but other metal azides are notoriously sensitive to
detonation and are used as primary explosives in detonator caps. Simple
azides such as sodium azide are stable in water in the dark but appear
to be susceptible to photodecomposition with solar radiation. Data on
solution photolysis are not susceptible to detailed analyses in terms
of persistence in sunlight.
The chemistry of azides is ably summarized by Hudson et al. (1969).
Photolysis of the solid azides produces metal nitrides initially and
eventually the free metal and nitrogen (Verneker, 1967). We have found
no information concerning the quantum yields for such processes or the
effect of solution on the efficiency of the process. Burak et al. (1970)
reported on the chemistry of photolysis of azide ion in solution using
light of 214 nm; the chemistry is probably similar at higher wavelengths.
No information is available to evaluate the reactivity of azides toward
RO radical.
133
-------
The likelihood that azide salts would be found in the atmosphere
appears low except as particulate readily washed down with rain.
Photolysis is a plausible pathway for removal of azides under those
conditions, but we know of no data bearing on the matter.
Bioaccumulation
Sodium azide is a reactive, polar compound that should not
accumulate significantly in animal tissues. We were not able to cal-
culate its log P value because of insufficient data, but believe that
the value should be less than 1. We found no data concerning the
distribution or retention of this compound in animal tissues.
134
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TECHNICAL REPORT DATA
(Please read Instructions on the reverse before completing!
. REPORT NO.
EPA 560/5-77-003
3. RECIPIENT'S ACCESSION>NO.
4. TITLE AND SUBTITLE
Review of the Environmental Fate of Selected
Chemicals
5. REPORT DATE
May 1977
6. PERFORMING ORGANIZATION CODE
7. AUTHORlS)
Shirley B. Radding, David H. Liu, Howard L. Johnson,
Theordore Mill
8. PERFORMING ORGANIZATION REPORT NO.
Final
9, PERFORMING ORGANIZATION NAME AND ADDRESS
Stanford Research Institute
333 Ravenswood Avenue
Menlo Park, CA. 94025
10. PROGRAM ELEMENT NO.
2LS676
11. CONTRACT/GRANT NO.
EPA 68-01-2681
12. SPONSORING AGENCV NAME AND ADDRESS
Office of Toxic Substances
U.S. Environmental Protection Agency
Washington, B.C. 20460
13. TYPE OF REPORT AND PERIOD COVERED
Final
14. SPONSORING AGENCY CODE
15.SUPPLEMENTARY NOTES
16. ABSTRACT
A review of the recent literature on sources, production, environ-
mental fate, and bioaccumulation has been carried out by SRI on 26 classes
of compounds. These included epoxides, haloolefins, aldehydes, alkyl and
benzyl halides, peroxides, hydroperoxides and peracids, polyhalomethanes,
aromatic amines, polychlorinated biphenyls, azo dyes, carbamic acid esters,
hydrazines, acyl halides and ketene, phosphoric acid esters, aziridines,
lactones, alkyl sulfates, sultones, aryl dialkyltriazenes, diazoalkanes,
haloalcohols, haloethers, hydroxylamines, nitrosamines, nitrofurans, and
azides.
KEY WORDS AND DOCUMENT ANALYSIS
DESCRIPTORS
b.IDENTIFIERS/OPEN ENDED TERMS
COSATI Field/Group
Environmental fate,
bioaccumulation,
sources, partition
coefficients
6A, 6F, 7C,
13B
8. DISTRIBUTION STATEMENT
Document is available to the public through
the National Technical Information Service
«.. .._. __jj,-^i^ Virginia 22151
19. SECURITY CLASS (ThisReport)
Unclassified
21. NO. OF PAGES
147
20. SECURITY CLASS (Thispage)
Unclassified
22. PF1ICE
EPA Form 2220-1 (9-73)
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