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Undid revision 768260172 as the hydrogen cyanide article so states, yes. Please discuss on talk page. Our “organic compound” article is clear.
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GHS04 specifically addresses hazards linked to the pressurized storage of gases. As storage methods can vary, that pictogram is not universally applicable to all gaseous compounds.
 
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{{Chembox
{{Chembox
| Watchedfields = changed
|Watchedfields = changed
| verifiedrevid = 470455423
|verifiedrevid = 470455423
| ImageFile = Cyanogen-chloride.png
|ImageFile = Cyanogen-chloride.svg
| ImageFile_Ref = {{chemboximage|correct|??}}
|ImageFile_Ref = {{chemboximage|correct|??}}
| ImageSize = 100
|ImageSize = 100
| ImageName = Skeletal formula of cyanogen chloride
|ImageName = Skeletal formula of cyanogen chloride
| ImageFileL1 = Cyanogen-chloride-3D-balls.png
|ImageFileL1 = Cyanogen-chloride-3D-balls.png
| ImageFileL1_Ref = {{chemboximage|correct|??}}
|ImageFileL1_Ref = {{chemboximage|correct|??}}
| ImageNameL1 = Ball and stick model of cyanogen chloride
|ImageNameL1 = Ball and stick model of cyanogen chloride
| ImageFileR1 = Cyanogen-chloride-3D-vdW.png
|ImageFileR1 = Cyanogen-chloride-3D-vdW.png
| ImageFileR1_Ref = {{chemboximage|correct|??}}
|ImageFileR1_Ref = {{chemboximage|correct|??}}
| ImageNameR1 = Spacefill model of cyanogen chloride
|ImageNameR1 = Spacefill model of cyanogen chloride
| PIN = Carbononitridic chloride
|PIN = Carbononitridic chloride
| SystematicName = Chloroformonitrile
|SystematicName = Chloroformonitrile
| OtherNames = {{Unbulleted list
|OtherNames = {{Unbulleted list
| Chlorine cyanide
|Chlorine cyanide
| Cyanic chloride
|Cyanic chloride
| Chlorocyanogen
|Chlorocyanogen
| Chlorcyan
|Chlorcyan
| Chlorocyanide
|Chlorocyanide
}}
}}
|Section1={{Chembox Identifiers
|Section1={{Chembox Identifiers
| Abbreviations = CK
|Abbreviations = CK
| CASNo = 506-77-4
|CASNo = 506-77-4
| CASNo_Ref = {{cascite|correct|CAS}}
|CASNo_Ref = {{cascite|correct|CAS}}
|UNII_Ref = {{fdacite|correct|FDA}}
⚫
| PubChem = 10477
|UNII = 697I61NSA0
⚫
| ChemSpiderID = 10045
⚫
|PubChem = 10477
⚫
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
⚫
|ChemSpiderID = 10045
⚫
| EINECS = 208-052-8
⚫
|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
⚫
| UNNumber = 1589
⚫
|EINECS = 208-052-8
⚫
| MeSHName = cyanogen+chloride
⚫
|UNNumber = 1589
⚫
| RTECS = GT2275000
⚫
|MeSHName = cyanogen+chloride
⚫
| SMILES = ClC#N
⚫
|RTECS = GT2275000
⚫
| StdInChI = 1S/CClN/c2-1-3
⚫
|SMILES = ClC#N
⚫
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
⚫
|StdInChI = 1S/CClN/c2-1-3
⚫
| StdInChIKey = QPJDMGCKMHUXFD-UHFFFAOYSA-N
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
|StdInChI_Ref = {{stdinchicite|correct|chemspider}}
⚫
|StdInChIKey = QPJDMGCKMHUXFD-UHFFFAOYSA-N
⚫
|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
}}
}}
|Section2={{Chembox Properties
|Section2={{Chembox Properties
| Properties_ref = <ref>{{RubberBible87th}}</ref>
|Properties_ref = <ref>{{RubberBible87th}}</ref>
| Formula = CNCl
|Formula = CNCl
| MolarMass = 61.470 g mol<sup>−1</sup>
|MolarMass = 61.470 g mol<sup>−1</sup>
| Appearance = Colorless gas
|Appearance = Colorless gas
| Odor = acrid
|Odor = acrid
| Density = 2.7683 mg mL<sup>−1</sup> (at 0&nbsp;°C, 101.325 kPa)
|Density = 2.7683 mg mL<sup>−1</sup> (at 0&nbsp;°C, 101.325 kPa)
| MeltingPtC = −6.55
|MeltingPtC = −6.55
| BoilingPtC = 13
|BoilingPtC = 13
| Solubility = soluble
|Solubility = soluble
| SolubleOther = soluble in [[ethanol]], [[ether]]
|SolubleOther = soluble in [[ethanol]], [[diethyl ether|ether]]
| VaporPressure = 1.987 MPa (at 21.1&nbsp;°C)
|VaporPressure = 1.987 MPa (at 21.1&nbsp;°C)
| MagSus = -32.4·10<sup>−6</sup> cm<sup>3</sup>/mol
|MagSus = -32.4·10<sup>−6</sup> cm<sup>3</sup>/mol
}}
}}
|Section3={{Chembox Thermochemistry
|Section3={{Chembox Thermochemistry
| DeltaHf = 137.95 kJ mol<sup>−1</sup>
|DeltaHf = 137.95 kJ mol<sup>−1</sup>
| Entropy = 236.33 J K<sup>−1</sup> mol<sup>−1</sup>
|Entropy = 236.33 J K<sup>−1</sup> mol<sup>−1</sup>
}}
}}
|Section4={{Chembox Hazards
|Section4={{Chembox Hazards
| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics1053.htm inchem.org]
|ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics1053.htm inchem.org]
| MainHazards = Highly toxic;<ref name=niosh>{{ cite web | url = http://www.cdc.gov/niosh/ershdb/EmergencyResponseCard_29750039.html | title = CYANOGEN CHLORIDE (CK)| work = The Emergency Response Safety and Health Database | publisher = NIOSH }}</ref> forms [[cyanide]] in the body<ref name=PGCH/>
|MainHazards = Highly toxic;<ref name=niosh>{{ cite web | url = https://www.cdc.gov/niosh/ershdb/EmergencyResponseCard_29750039.html | title = CYANOGEN CHLORIDE (CK)| work = The Emergency Response Safety and Health Database | date = 9 July 2021| publisher = NIOSH }}</ref> forms [[cyanide]] in the body<ref name=PGCH/>
|GHSPictograms = {{GHS05}} {{GHS06}} {{GHS09}}
⚫
| NFPA-H = 4
|GHSSignalWord = '''DANGER'''
⚫
| NFPA-F = 0
| NFPA-R = 2
|NFPA-H = 4
⚫
|NFPA-F = 0
⚫
| PEL = none<ref name=PGCH>{{PGCH|0162}}</ref>
⚫
|NFPA-R = 2
⚫
| IDLH = N.D.<ref name=PGCH/>
| REL = C 0.3 ppm (0.6 mg/m<sup>3</sup>)<ref name=PGCH/>
|PEL = none<ref name=PGCH>{{PGCH|0162}}</ref>
⚫
|IDLH = N.D.<ref name=PGCH/>
⚫
| FlashPt = nonflammable
| FlashPt_notes = <ref name=PGCH/>
|REL = C 0.3 ppm (0.6 mg/m<sup>3</sup>)<ref name=PGCH/>
⚫
|FlashPt = nonflammable
⚫
|FlashPt_ref = <ref name=PGCH/>
}}
}}
|Section5={{Chembox Related
|Section5={{Chembox Related
| OtherFunction_label = alkanenitriles
|OtherFunction_label = alkanenitriles
| OtherFunction = {{Unbulleted list|[[Hydrogen cyanide]]|[[Thiocyanic acid]]|[[Cyanogen iodide]]|[[Cyanogen bromide]]|[[Cyanogen fluoride]]|[[Acetonitrile]]|[[Aminoacetonitrile]]|[[Glycolonitrile]]|[[Cyanogen]]}}
|OtherFunction = {{Unbulleted list|[[Hydrogen cyanide]]|[[Thiocyanic acid]]|[[Cyanogen iodide]]|[[Cyanogen bromide]]|[[Cyanogen fluoride]]|[[Acetonitrile]]|[[Aminoacetonitrile]]|[[Glycolonitrile]]|[[Cyanogen]]}}
}}
}}
}}
}}
'''Cyanogen chloride''' is an [[organic compound]] with the [[chemical formula|formula]] NCCl. This linear, triatomic [[pseudohalogen]] is an easily condensed colorless gas. More commonly encountered in the laboratory is the related compound [[cyanogen bromide]], a room-temperature solid that is widely used in biochemical analysis and preparation.
'''Cyanogen chloride''' is a highly [[toxicity|toxic]] chemical compound with the [[chemical formula|formula]] CNCl. This linear, triatomic [[pseudohalogen]] is an easily condensed colorless gas. More commonly encountered in the laboratory is the related compound [[cyanogen bromide]], a room-temperature solid that is widely used in biochemical analysis and preparation.


==Synthesis, basic properties, structure==
==Synthesis, basic properties, structure==
Cyanogen chloride is a molecule with the connectivity ClCN. Carbon and chlorine are linked by a [[single bond]], and carbon and nitrogen by a [[triple bond]]. It is a linear molecule, as are the related cyanogen halides (NCF, [[cyanogen bromide|NCBr]], NCI). Cyanogen chloride is produced by the oxidation of [[sodium cyanide]] with [[chlorine]]. This reaction proceeds via the intermediate [[cyanogen]] ((CN)<sub>2</sub>).<ref>{{ cite journal |author1=Coleman, G. H. |author2=Leeper, R. W. |author3=Schulze, C. C. | title = Cyanogen Chloride | journal = Inorganic Syntheses | year = 1946 | volume = 2 | pages = 90–94 | doi = 10.1002/9780470132333.ch25 }}</ref>
Cyanogen chloride is a molecule with the connectivity {{chem2|Cl\sC\tN}}. Carbon and chlorine are linked by a [[single bond]], and carbon and nitrogen by a [[triple bond]]. It is a linear molecule, as are the related cyanogen halides (NCF, [[cyanogen bromide|NCBr]], NCI). Cyanogen chloride is produced by the oxidation of [[sodium cyanide]] with [[chlorine]]. This reaction proceeds via the intermediate [[cyanogen]] ({{chem2|(CN)2}}).<ref>{{ Cite book |author1=Coleman, G. H. |title=Inorganic Syntheses |author2=Leeper, R. W. |author3=Schulze, C. C. | chapter = Cyanogen Chloride | year = 1946 | volume = 2 | pages = 90–94 | doi = 10.1002/9780470132333.ch25 |isbn=9780470132333 }}</ref>
:NaCN + Cl<sub>2</sub> → ClCN + NaCl
:<chem>NaCN + Cl2 -> ClCN + NaCl</chem>
The compound [[trimer (chemistry)|trimer]]izes in the presence of acid to the heterocycle called [[cyanuric chloride]].
The compound [[trimer (chemistry)|trimer]]izes in the presence of acid to the heterocycle called [[cyanuric chloride]].


Cyanogen chloride is slowly hydrolyzed by water to release cyanate and chloride ions
Cyanogen chloride is slowly [[hydrolyzed]] by water at neutral [[pH]] to release cyanate and chloride ions:
:ClCN + H<sub>2</sub>O → NCO<sup>−</sup> + Cl<sup>−</sup> + 2H<sup>+</sup>
:<chem>ClCN + H2O -> NCO- + Cl- + 2H+</chem>
:at neutral pH


==Applications in synthesis==
==Applications in synthesis==
Cyanogen chloride is a precursor to the sulfonyl cyanides<ref>{{ OrgSynth | author = Vrijland, M. S. A. | title = Sulfonyl Cyanides: Methanesulfonyl Cyanide | year = 1977 | volume = 57 | pages = 88 | collvol = 6 | collvolpages = 727 | prep = cv6p0727 | url = http://www.orgsyn.org/orgsyn/pdfs/CV6P0727.pdf }}</ref> and [[chlorosulfonyl isocyanate]], a useful reagent in [[organic synthesis]].<ref>{{ OrgSynth | author = Graf, R. | title = Chlorosulfonyl Isocyanate | year = 1966 | volume = 46 | pages = 23 | collvol = 5 | collvolpages = 226 | prep = cv5p0226 | url = http://www.orgsyn.org/orgsyn/pdfs/CV5P0226.pdf }}</ref>
Cyanogen chloride is a precursor to the sulfonyl cyanides<ref>{{ OrgSynth | author = Vrijland, M. S. A. | title = Sulfonyl Cyanides: Methanesulfonyl Cyanide | year = 1977 | volume = 57 | pages = 88 | collvol = 6 | collvolpages = 727 | prep = cv6p0727 | url = http://www.orgsyn.org/orgsyn/pdfs/CV6P0727.pdf }}</ref> and [[chlorosulfonyl isocyanate]], a useful reagent in [[organic synthesis]].<ref>{{ OrgSynth | author = Graf, R. | title = Chlorosulfonyl Isocyanate | year = 1966 | volume = 46 | pages = 23 | collvol = 5 | collvolpages = 226 | prep = cv5p0226 | url = http://www.orgsyn.org/orgsyn/pdfs/CV5P0226.pdf}}</ref>

Further chlorination gives the [[isocyanide dichloride]].


==Safety==
==Safety==
Also known as '''CK''', cyanogen chloride is a highly toxic [[blood agent]], and was once proposed for use in [[chemical warfare]]. It causes immediate injury upon contact with the eyes or respiratory organs. Symptoms of exposure may include [[drowsiness]], [[rhinorrhea]] (runny nose), [[sore throat]], [[cough]]ing, [[confusion]], [[nausea]], [[vomiting]], [[edema]], [[Fainting|loss of consciousness]], [[convulsion]]s, [[paralysis]], and death.<ref name=niosh/> It is especially dangerous because it is capable of penetrating the filters in [[gas mask]]s, according to [[United States|U.S.]] analysts. CK is unstable due to [[polymerization]], sometimes with explosive violence.<ref name="FM 3-8">{{ cite book | title = FM 3-8 Chemical Reference Handbook | publisher = US Army | year = 1967 }}</ref>
Also known as '''CK''', cyanogen chloride is a highly toxic [[blood agent]], and was once proposed for use in [[chemical warfare]]. It causes immediate injury upon contact with the eyes or respiratory organs. Symptoms of exposure may include [[drowsiness]], [[rhinorrhea]] (runny nose), [[sore throat]], [[cough]]ing, [[confusion]], [[nausea]], [[vomiting]], [[edema]], [[Fainting|loss of consciousness]], [[convulsion]]s, [[paralysis]], and death.<ref name=niosh/> It is especially dangerous because it is capable of penetrating the filters in [[gas mask]]s, according to United States analysts. CK is unstable due to [[polymerization]], sometimes with explosive violence.<ref name="FM 3-8">{{cite book | title = FM 3-8 Chemical Reference Handbook | publisher = US Army | year = 1967}}</ref>


==Chemical weapon==
Cyanogen chloride is listed in [[List of Schedule 3 substances (CWC)|schedule 3]] of the [[Chemical Weapons Convention]]: all production must be reported to the [[OPCW]].{{fact|date=October 2016}}
Cyanogen chloride is listed in [[List of Schedule 3 substances (CWC)|schedule 3]] of the [[Chemical Weapons Convention]]: all production must be reported to the [[Organisation for the Prohibition of Chemical Weapons|OPCW]].<ref>{{Cite web|url=https://www.opcw.org/chemical-weapons-convention/annexes/annex-on-chemicals/schedule-3/|title=Schedule 3 |publisher= www.opcw.org|access-date=16 March 2018}}</ref>

By 1945, the U.S. Army's [[Chemical Corps (United States Army)|Chemical Warfare Service]] developed chemical warfare rockets intended for the new M9 and M9A1 [[Bazooka]]s. An M26 Gas Rocket was adapted to fire cyanogen chloride-filled warheads for these rocket launchers.<ref name="Smart, Jeffrey 1997 p. 32">{{Citation | last = Smart | first = Jeffrey | title = History of Chemical and Biological Warfare: An American Perspective | chapter = 2 | place = Aberdeen, MD, USA | publisher = Army Chemical and Biological Defense Command | year = 1997 | page = 32}}.</ref> As it was capable of penetrating the protective filter barriers in some gas masks,<ref>{{Cite web|url=https://www.cdc.gov/niosh/ershdb/EmergencyResponseCard_29750039.html|title = Cyanogen chloride (CK): Systemic Agent &#124; NIOSH &#124; CDC|date = 9 July 2021}}</ref> it was seen as an effective agent against Japanese forces (particularly those hiding in caves or bunkers) because their standard issue gas masks lacked the barriers that would provide protection against cyanogen chloride.<ref name="Smart, Jeffrey 1997 p. 32" /><ref>{{Citation | title = Field Manual 3-5 | contribution = Characteristics and Employment of Ground Chemical Munitions | place = Washington, DC | publisher = War Department | year = 1946 | pages = 108–19}}</ref><ref>{{Citation | last = Skates | first = John R | title = The Invasion of Japan: Alternative to the Bomb | publisher = [[University of South Carolina Press]] | year = 2000 | isbn = 978-1-57003-354-4 | pages = 93–96}}</ref> The US added the weapon to its arsenal, and considered using it, along with [[hydrogen cyanide]], as part of [[Operation Downfall]], the planned invasion of Japan, but President [[Harry Truman]] decided against it, instead using the atomic bombs developed by the secret [[Manhattan Project]].<ref>{{cite web |url=https://www.youtube.com/watch?v=8CFPaSH84ZU |title=How would have WW2 gone if the US had not used nuclear bombs on Japan? |author=Binkov's Battlegrounds |date=April 27, 2022 |website=YouTube.Com |publisher= |access-date=June 23, 2022 }}</ref> The CK rocket was never deployed or issued to combat personnel.<ref name="Smart, Jeffrey 1997 p. 32"/>


==References==
==References==
Line 96: Line 104:


==External links==
==External links==
* {{ cite web | url = http://www.emedicine.com/emerg/topic910.htm | title = Cyanogen Chloride Poisoning | year = 2011 | author = Murphy-Lavoie, H. | publisher = MedScape | work = eMedicine }}
* {{ Cite journal | url = http://www.emedicine.com/emerg/topic910.htm | title = Cyanogen Chloride Poisoning | year = 2011 | author = Murphy-Lavoie, H. | publisher = MedScape | journal = EMedicine }}
* {{ cite web | url = http://www.npi.gov.au/substances/cyanide/index.html | title = National Pollutant Inventory – Cyanide compounds fact sheet | publisher = Australian Government }}
* {{ cite web | url = http://www.npi.gov.au/substances/cyanide/index.html | title = National Pollutant Inventory – Cyanide compounds fact sheet | publisher = Australian Government }}
* {{ cite web | url = http://www.cdc.gov/niosh/npg/npgd0162.html | title = NIOSH Pocket Guide to Chemical Hazards | publisher = Centers for Disease Control and Prevention }}
* {{ cite web | url = https://www.cdc.gov/niosh/npg/npgd0162.html | title = NIOSH Pocket Guide to Chemical Hazards | publisher = Centers for Disease Control and Prevention }}


{{Cyanides}}
{{Cyanides}}
{{Chemical warfare}}
{{Chemical warfare}}


{{Use dmy dates|date=March 2018}}
{{DEFAULTSORT:Cyanogen Chloride}}

⚫
[[Category:Chlorides]]
[[Category:Cyanides]]
[[Category:Chlorine compounds]]
[[Category:Inorganic carbon compounds]]
[[Category:Triatomic molecules]]
[[Category:Inorganic nitrogen compounds]]
[[Category:Cyano compounds]]
[[Category:Nonmetal halides]]
[[Category:Nonmetal halides]]
[[Category:Blood agents]]
[[Category:Blood agents]]
⚫
[[Category:Pseudohalogens]]

Latest revision as of 13:43, 30 October 2024

Cyanogen chloride
Skeletal formula of cyanogen chloride
Ball and stick model of cyanogen chloride
Ball and stick model of cyanogen chloride
Spacefill model of cyanogen chloride
Spacefill model of cyanogen chloride
Names
Preferred IUPAC name
Carbononitridic chloride
Systematic IUPAC name
Chloroformonitrile
Other names
  • Chlorine cyanide
  • Cyanic chloride
  • Chlorocyanogen
  • Chlorcyan
  • Chlorocyanide
Identifiers
3D model (JSmol)
Abbreviations CK
ChemSpider
ECHA InfoCard 100.007.321 Edit this at Wikidata
EC Number
  • 208-052-8
MeSH cyanogen+chloride
RTECS number
  • GT2275000
UNII
UN number 1589
  • InChI=1S/CClN/c2-1-3 checkY
    Key: QPJDMGCKMHUXFD-UHFFFAOYSA-N checkY
  • ClC#N
Properties[1]
CNCl
Molar mass 61.470 g mol−1
Appearance Colorless gas
Odor acrid
Density 2.7683 mg mL−1 (at 0 °C, 101.325 kPa)
Melting point −6.55 °C (20.21 °F; 266.60 K)
Boiling point 13 °C (55 °F; 286 K)
soluble
Solubility soluble in ethanol, ether
Vapor pressure 1.987 MPa (at 21.1 °C)
-32.4·10−6 cm3/mol
Thermochemistry
236.33 J K−1 mol−1
137.95 kJ mol−1
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Highly toxic;[2] forms cyanide in the body[3]
GHS labelling:
GHS05: Corrosive GHS06: Toxic GHS09: Environmental hazard
Danger
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no code
4
0
2
Flash point nonflammable[3]
NIOSH (US health exposure limits):
PEL (Permissible)
 none[3]
REL (Recommended)
 C 0.3 ppm (0.6 mg/m3)[3]
IDLH (Immediate danger)
 N.D.[3]
Safety data sheet (SDS) inchem.org
Related compounds
Related alkanenitriles
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Cyanogen chloride is a highly toxic chemical compound with the formula CNCl. This linear, triatomic pseudohalogen is an easily condensed colorless gas. More commonly encountered in the laboratory is the related compound cyanogen bromide, a room-temperature solid that is widely used in biochemical analysis and preparation.

Synthesis, basic properties, structure

[edit]

Cyanogen chloride is a molecule with the connectivity Cl−C≡N. Carbon and chlorine are linked by a single bond, and carbon and nitrogen by a triple bond. It is a linear molecule, as are the related cyanogen halides (NCF, NCBr, NCI). Cyanogen chloride is produced by the oxidation of sodium cyanide with chlorine. This reaction proceeds via the intermediate cyanogen ((CN)2).[4]

The compound trimerizes in the presence of acid to the heterocycle called cyanuric chloride.

Cyanogen chloride is slowly hydrolyzed by water at neutral pH to release cyanate and chloride ions:

Applications in synthesis

[edit]

Cyanogen chloride is a precursor to the sulfonyl cyanides[5] and chlorosulfonyl isocyanate, a useful reagent in organic synthesis.[6]

Further chlorination gives the isocyanide dichloride.

Safety

[edit]

Also known as CK, cyanogen chloride is a highly toxic blood agent, and was once proposed for use in chemical warfare. It causes immediate injury upon contact with the eyes or respiratory organs. Symptoms of exposure may include drowsiness, rhinorrhea (runny nose), sore throat, coughing, confusion, nausea, vomiting, edema, loss of consciousness, convulsions, paralysis, and death.[2] It is especially dangerous because it is capable of penetrating the filters in gas masks, according to United States analysts. CK is unstable due to polymerization, sometimes with explosive violence.[7]

Chemical weapon

[edit]

Cyanogen chloride is listed in schedule 3 of the Chemical Weapons Convention: all production must be reported to the OPCW.[8]

By 1945, the U.S. Army's Chemical Warfare Service developed chemical warfare rockets intended for the new M9 and M9A1 Bazookas. An M26 Gas Rocket was adapted to fire cyanogen chloride-filled warheads for these rocket launchers.[9] As it was capable of penetrating the protective filter barriers in some gas masks,[10] it was seen as an effective agent against Japanese forces (particularly those hiding in caves or bunkers) because their standard issue gas masks lacked the barriers that would provide protection against cyanogen chloride.[9][11][12] The US added the weapon to its arsenal, and considered using it, along with hydrogen cyanide, as part of Operation Downfall, the planned invasion of Japan, but President Harry Truman decided against it, instead using the atomic bombs developed by the secret Manhattan Project.[13] The CK rocket was never deployed or issued to combat personnel.[9]

References

[edit]
  1. ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  2. ^ a b "CYANOGEN CHLORIDE (CK)". The Emergency Response Safety and Health Database. NIOSH. 9 July 2021.
  3. ^ a b c d e NIOSH Pocket Guide to Chemical Hazards. "#0162". National Institute for Occupational Safety and Health (NIOSH).
  4. ^ Coleman, G. H.; Leeper, R. W.; Schulze, C. C. (1946). "Cyanogen Chloride". Inorganic Syntheses. Vol. 2. pp. 90–94. doi:10.1002/9780470132333.ch25. ISBN 9780470132333.
  5. ^ Vrijland, M. S. A. (1977). "Sulfonyl Cyanides: Methanesulfonyl Cyanide" (PDF). Organic Syntheses. 57: 88; Collected Volumes, vol. 6, p. 727.
  6. ^ Graf, R. (1966). "Chlorosulfonyl Isocyanate" (PDF). Organic Syntheses. 46: 23; Collected Volumes, vol. 5, p. 226.
  7. ^ FM 3-8 Chemical Reference Handbook. US Army. 1967.
  8. ^ "Schedule 3". www.opcw.org. Retrieved 16 March 2018.
  9. ^ a b c Smart, Jeffrey (1997), "2", History of Chemical and Biological Warfare: An American Perspective, Aberdeen, MD, USA: Army Chemical and Biological Defense Command, p. 32.
  10. ^ "Cyanogen chloride (CK): Systemic Agent | NIOSH | CDC". 9 July 2021.
  11. ^ "Characteristics and Employment of Ground Chemical Munitions", Field Manual 3-5, Washington, DC: War Department, 1946, pp. 108–19
  12. ^ Skates, John R (2000), The Invasion of Japan: Alternative to the Bomb, University of South Carolina Press, pp. 93–96, ISBN 978-1-57003-354-4
  13. ^ Binkov's Battlegrounds (27 April 2022). "How would have WW2 gone if the US had not used nuclear bombs on Japan?". YouTube.Com. Retrieved 23 June 2022.
[edit]

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