Hydrogen chloride

"HCl" redirects here. For the aqueous solution, see Hydrochloric acid. For other uses, see HCL.

Hydrogen chloride  | Skeletal formula of hydrogen chloride with a dimension | Space-filling model of hydrogen chloride with atom symbols

|

Names
IUPAC name

Hydrogen chloride[1]

Systematic IUPAC name

Chlorane[2]

Other names

Hydrochloric acid gas
Hydrochloric gas
Hydrochloride

Identifiers

CAS Number

* 7647-01-0 Y

3D model (JSmol)

* Interactive image

Beilstein Reference

| 1098214
ChEBI |

* CHEBI:17883 Y

ChEMBL |

* ChEMBL1231821 N

ChemSpider |

* 307 Y

EC Number |

* 231-595-7

Gmelin Reference

| 322
KEGG |

* D02057 Y

MeSH | Hydrochloric+acid

PubChem CID

* 313

RTECS number |

* MW4025000

UNII |

* QTT17582CB Y

UN number | 1050

InChI

* InChI=1S/HCl/h1H N

Key: VEXZGXHMUGYJMC-UHFFFAOYSA-N Y

* InChI=1/HCl/h1H

Key: VEXZGXHMUGYJMC-UHFFFAOYAT

SMILES

* Cl

Properties

Chemical formula

| HCl
Molar mass | 36.46 g·mol-1
Appearance  | Colorless gas
Odor | pungent; sharp and burning
Density | 1.49 g/L[3]
Melting point |  −114.22 °C (−173.60 °F; 158.93 K)
Boiling point |  −85.05 °C (−121.09 °F; 188.10 K)

Solubility in water

| 823 g/L (0 °C)
720 g/L (20 °C)
561 g/L (60 °C)
Solubility | soluble in methanol, ethanol, ether and water
Vapor pressure | 4352 kPa (at 21.1 °C)[4]
Acidity (pKa)  | −3.0;[5] −5.9 (±0.4)[6]
Basicity (pKb)  | 17.0
Conjugate acid | Chloronium
Conjugate base | Chloride

Refractive index (nD)

| 1.0004456 (gas)
1.254 (liquid)
Viscosity | 0.311 cP (−100 °C)
Structure

Molecular shape

| linear

Dipole moment

| 1.05 D
Thermochemistry

Heat capacity (C)

| 0.7981 J/(K·g)

Std molar
entropy (S ~~o~~ 298)

| 186.902 J/(K·mol)

Std enthalpy of
formation (ΔfH⦵298)

| −92.31 kJ/mol

Std enthalpy of
combustion (ΔcH⦵298)

| −95.31 kJ/mol
Pharmacology
1=ATC code }}  | A09AB03 (WHO) B05XA13 (WHO)
Hazards
Main hazards | Toxic, corrosive
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H314, H331

GHS precautionary statements

| P261, P280, P303+361+353, P304+340+310, P305+351+338, P410+403
NFPA 704 (fire diamond)  |

COR

Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 238 mg/kg (rat, oral)

LC50 (median concentration)

| 3124 ppm (rat, 1 h)
1108 ppm (mouse, 1 h)[8]

LCLo (lowest published)

| 1300 ppm (human, 30 min)
4416 ppm (rabbit, 30 min)
4416 ppm (guinea pig, 30 min)
3000 ppm (human, 5 min)[8]
NIOSH (US health exposure limits):

PEL (Permissible)

| C 5 ppm (7 mg/m3)[7]

REL (Recommended)

| C 5 ppm (7 mg/m3)[7]

IDLH (Immediate danger)

| 50 ppm[7]
Related compounds

Related compounds

| Hydrogen fluoride
Hydrogen bromide
Hydrogen iodide
Hydrogen astatide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

The compound hydrogen chloride has the chemical formula HCl and as such is a hydrogen halide. At room temperature, it is a colorless gas, which forms white fumes of hydrochloric acid upon contact with atmospheric water vapor.[9] Hydrogen chloride gas and hydrochloric acid are important in technology and industry. Hydrochloric acid, the aqueous solution of hydrogen chloride, is also commonly given the formula HCl.

## Contents

* 1 Reactions
* 1.1 Structure and properties
* 2 Production
* 2.1 Historical routes
* 2.2 Industrial routes
* 2.3 Laboratory methods
* 3 Applications
* 4 History
* 5 Safety
* 6 See also
* 7 References
* 8 External links

## Reactions

Hydrochloric acid vapor turning pH paper red showing that the fumes are acidic

Hydrogen chloride is a diatomic molecule, consisting of a hydrogen atom H and a chlorine atom Cl connected by a polar covalent bond. The chlorine atom is much more electronegative than the hydrogen atom, which makes this bond polar. Consequently, the molecule has a large dipole moment with a negative partial charge (δ−) at the chlorine atom and a positive partial charge (δ+) at the hydrogen atom.[10] In part because of its high polarity, HCl is very soluble in water (and in other polar solvents).

Upon contact, H
2O and HCl combine to form hydronium cations [H
3O]+
and chloride anions Cl−

HCl + H
2O → [H
3O]+
\+ Cl−

The resulting solution is called hydrochloric acid and is a strong acid. The acid dissociation or ionization constant, Ka, is large, which means HCl dissociates or ionizes completely in water. Hydrogen chloride also ionizes in other solvents such as methanol:

HCl + CH
3OH → [CH
3OH
2]+
\+ Cl−

In the absence of such polar solvents, hydrogen chloride functions as a weak acid.

### Structure and properties

The structure of solid DCl, as determined by neutron diffraction of DCl powder at 77 K. DCl was used instead of HCl because the deuterium nucleus is easier to detect than the hydrogen nucleus. The extended linear structure is indicated by the dashed lines.

Frozen HCl undergoes a phase transition at 98.4 K (−174.8 °C; −282.5 °F). X-ray powder diffraction of the frozen material shows that the material changes from an orthorhombic structure to a cubic one during this transition. In both structures the chlorine atoms are in a face-centered array. However, the hydrogen atoms could not be located.[11] Analysis of spectroscopic and dielectric data, and determination of the structure of DCl (deuterium chloride) indicates that HCl forms zigzag chains in the solid, as does HF (see figure on right).[12]

Solubility of HCl (g/L) in common solvents[13] Temperature (°C) | 0 | 20 | 30 | 50

|
|
|
|

Water | 823 | 720 | 673 | 596
Methanol | 513 | 470 | 430 |
Ethanol | 454 | 410 | 381 |
Ether | 356 | 249 | 195 |
Infrared (IR) absorption spectrum One doublet in the IR spectrum resulting from the isotopic composition of chlorine

The infrared spectrum of gaseous hydrogen chloride, shown on the left, consists of a number of sharp absorption lines grouped around 2886 cm−1 (wavelength ~3.47 μm). At room temperature, almost all molecules are in the ground vibrational state v = 0\. Including anharmonicity the vibrational energy can be written as:

Ev=hνe(v+12)+hxeνe(v+12)2

To promote an HCl molecule from the v = 0 to the v = 1 state, we would expect to see an infrared absorption about νo = νe + 2xeνe = 2880 cm−1. However, this absorption corresponding to the Q-branch is not observed due to it being forbidden by symmetry. Instead, two sets of signals (P- and R-branches) are seen owing to a simultaneous change in the rotational state of the molecules. Because of quantum mechanical selection rules, only certain rotational transitions are permitted. The states are characterized by the rotational quantum number J = 0, 1, 2, 3, ... selection rules state that ΔJ is only able to take values of ±1.

E(J)rot=h⋅B⋅J(J+1)

The value of the rotational constant B is much smaller than the vibrational one νo, such that a much smaller amount of energy is required to rotate the molecule; for a typical molecule, this lies within the microwave region. However, the vibrational energy of HCl molecule places its absorptions within the infrared region, allowing a spectrum showing the rovibrational transitions of this molecule to be easily collected using an infrared spectrometer with a gas cell. The latter can even be made of quartz as the HCl absorption lies in a window of transparency for this material.

Naturally abundant chlorine consists of two isotopes, 35Cl and 37Cl, in a ratio of approximately 3:1. While the spring constants are nearly identical, the disparate reduced masses of H35Cl and H37Cl cause measurable differences in the rotational energy, thus doublets are observed on close inspection of each absorption line, weighted in the same ratio of 3:1.

## Production

### Historical routes

In the 17th century, Johann Rudolf Glauber combined sodium chloride salt and sulfuric acid for the preparation of hydrogen chloride. This route is the basis of the Mannheim process. Joseph Priestley prepared hydrogen chloride in 1772,[14] and by 1808 Humphry Davy had proved that the chemical composition included hydrogen and chlorine.[15]

### Industrial routes

Most hydrogen chloride is produced as a byproduct of chlorination processes. Routes to tetrafluoroethylene, chlorobenzene, CFCs, chloroacetic acid, and vinyl chloride are illustrative. In these routes, formally speaking, hydrogen atoms on the hydrocarbon are replaced by chlorine atoms, whereupon the released hydrogen atom recombines with the spare atom from the chlorine molecule, forming hydrogen chloride:

RH + Cl
2 → RCl + HCl

Often the resulting hydrogen chloride is integrated with captive use of it on-site, e.g. oxychlorination. Hydrogen chloride is also produced in some routes to organofluorine compounds:

RCl + HF → RF + HCl

File:Hydrochloric Acid Burner Flame.ogv Hydrogen chloride can be produced by combining chlorine and hydrogen:

2 \+ H
2 → 2 HCl

As the reaction is exothermic, the installation is called an HCl oven or HCl burner. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. This reaction can give a very pure product, e.g. for use in the food industry. The reaction can also be triggered by blue light.[16]

### Laboratory methods

Small amounts of hydrogen chloride for laboratory use can be generated in an HCl generator by dehydrating hydrochloric acid with either sulfuric acid or anhydrous calcium chloride. Alternatively, HCl can be generated by the reaction of sulfuric acid with sodium chloride:[17]

NaCl + H
2SO
4 → NaHSO
4 \+ HCl↑

This reaction occurs at room temperature. Provided there is NaCl remaining in the generator and it is heated above 200 °C, the reaction proceeds further:

NaCl + NaHSO
4 → Na
2SO
4 \+ HCl↑

For such generators to function, the reagents should be dry.

Hydrogen chloride can also be prepared by the hydrolysis of certain reactive chloride compounds such as phosphorus chlorides, thionyl chloride (SOCl
2), and acyl chlorides. For example, cold water can be gradually dripped onto phosphorus pentachloride (PCl
5) to give HCl:

PCl
5 \+ H
2O → POCl
3 \+ 2 HCl↑

## Applications

Most hydrogen chloride is consumed in the production of hydrochloric acid. It is also used in the production of vinyl chloride and many alkyl chlorides.[18] Trichlorosilane, a precursor to ultrapure silicon, is produced by the reaction of hydrogen chloride and silicon at around 300 °C.[19]

Si + 3 HCl → HSiCl
3 \+ H

## History

Around 900, the authors of the Arabic writings attributed to Jabir ibn Hayyan (Latin: Geber) and the Persian physician and alchemist Abu Bakr al-Razi (c. 865–925, Latin: Rhazes) were experimenting with sal ammoniac (ammonium chloride), which when it was distilled together with vitriol (hydrated sulfates of various metals) produced hydrogen chloride.[20] It is possible that in one of his experiments, al-Razi stumbled upon a primitive method to produce hydrochloric acid.[21] However, it appears that in most of these early experiments with chloride salts, the gaseous products were discarded, and hydrogen chloride may have been produced many times before it was discovered that it can be put to chemical use.[22]

One of the first such uses was the synthesis of mercury(II) chloride (corrosive sublimate), whose production from the heating of mercury either with alum and ammonium chloride or with vitriol and sodium chloride was first described in the De aluminibus et salibus ("On Alums and Salts"), an eleventh- or twelfth century Arabic text falsely attributed to Abu Bakr al-Razi and translated into Latin by Gerard of Cremona (1144–1187).[23]

Another important development was the discovery by pseudo-Geber (in the De inventione veritatis, "On the Discovery of Truth", after c. 1300) that by adding ammonium chloride to nitric acid, a strong solvent capable of dissolving gold (i.e., aqua regia) could be produced.[24]

After the discovery in the late sixteenth century of the process by which unmixed hydrochloric acid can be prepared,[25] it was recognized that this new acid (then known as spirit of salt or acidum salis) released vaporous hydrogen chloride, which was called marine acid air. In the 17th century, Johann Rudolf Glauber used salt (sodium chloride) and sulfuric acid for the preparation of sodium sulfate, releasing hydrogen chloride gas (see production, above). In 1772, Carl Wilhelm Scheele also reported this reaction and is sometimes credited with its discovery. Joseph Priestley prepared hydrogen chloride in 1772, and in 1810 Humphry Davy established that it is composed of hydrogen and chlorine.[26]

During the Industrial Revolution, demand for alkaline substances such as soda ash increased, and Nicolas Leblanc developed a new industrial-scale process for producing the soda ash. In the Leblanc process, salt was converted to soda ash, using sulfuric acid, limestone, and coal, giving hydrogen chloride as by-product. Initially, this gas was vented to air, but the Alkali Act 1863 prohibited such release, so then soda ash producers absorbed the HCl waste gas in water, producing hydrochloric acid on an industrial scale. Later, the Hargreaves process was developed, which is similar to the Leblanc process except sulfur dioxide, water, and air are used instead of sulfuric acid in a reaction which is exothermic overall. In the early 20th century the Leblanc process was effectively replaced by the Solvay process, which did not produce HCl. However, hydrogen chloride production continued as a step in hydrochloric acid production.

Historical uses of hydrogen chloride in the 20th century include hydrochlorinations of alkynes in producing the chlorinated monomers chloroprene and vinyl chloride, which are subsequently polymerized to make polychloroprene (Neoprene) and polyvinyl chloride (PVC), respectively. In the production of vinyl chloride, acetylene (C

2) is hydrochlorinated by adding the HCl across the triple bond of the C

2 molecule, turning the triple into a double bond, yielding vinyl chloride.

The "acetylene process", used until the 1960s for making chloroprene, starts out by joining two acetylene molecules, and then adds HCl to the joined intermediate across the triple bond to convert it to chloroprene as shown here:

This "acetylene process" has been replaced by a process which adds Cl
2 to the double bond of ethylene instead, and subsequent elimination produces HCl instead, as well as chloroprene.

## Safety

Hydrogen chloride forms corrosive hydrochloric acid on contact with water found in body tissue. Inhalation of the fumes can cause coughing, choking, inflammation of the nose, throat, and upper respiratory tract, and in severe cases, pulmonary edema, circulatory system failure, and death.[27] Skin contact can cause redness, pain, and severe chemical burns. Hydrogen chloride may cause severe burns to the eye and permanent eye damage.

The U.S. Occupational Safety and Health Administration and the National Institute for Occupational Safety and Health have established occupational exposure limits for hydrogen chloride at a ceiling of 5 ppm (7 mg/m3),[28] and compiled extensive information on hydrogen chloride workplace safety concerns.[29]

## See also

* Gastric acid, hydrochloric acid secreted into the stomach to aid digestion of proteins
* Chloride, salts of hydrogen chloride
* Hydrogen bromide
* Hydrochloride, organic salts of hydrochloric acid
* Hydrochlorination, addition reaction with alkenes

## References

1. ↑ "hydrogen chloride (CHEBI:17883)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=17883.
2. ↑ Favre, Henri A.; Powell, Warren H., eds (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. Cambridge: The Royal Society of Chemistry. p. 131. ISBN 9781849733069.
3. ↑ Haynes, William M. (2010). Handbook of Chemistry and Physics (91 ed.). Boca Raton, Florida: CRC Press. p. 4–67. ISBN 978-1439820773.
4. ↑ Hydrogen Chloride. Gas Encyclopaedia. Air Liquide
5. ↑ Tipping, E.(2002) [1]. Cambridge University Press, 2004.
6. ↑ Trummal, A.; Lipping, L.; Kaljurand, I.; Koppel, I. A.; Leito, I. "Acidity of Strong Acids in Water and Dimethyl Sulfoxide" J. Phys. Chem. A. 2016, 120, 3663-3669. doi:10.1021/acs.jpca.6b02253
7. ↑ 7.0 7.1 7.2 NIOSH Pocket Guide to Chemical Hazards. "#0332". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0332.html.
8. ↑ 8.0 8.1 "Hydrogen chloride". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/7647010.html.
9. ↑ Rennie, Richard, ed (2020). Dictionary of chemistry. Oxford quick reference (8th ed.). Oxford, United Kingdom ; New York, NY: Oxford University Press. p. 29. ISBN 978-0-19-884122-7.
10. ↑ Ouellette, Robert J.; Rawn, J. David (2015). Principles of Organic Chemistry. Elsevier Science. pp. 6–. ISBN 978-0-12-802634-2. https://books.google.com/books?id=U-CoBAAAQBAJ&pg=PA6.
11. ↑ Natta, G. (1933). "Struttura e polimorfismo degli acidi alogenidrici" (in it). Gazzetta Chimica Italiana 63: 425–439.
12. ↑ Sándor, E.; Farrow, R. F. C. (1967). "Crystal Structure of Solid Hydrogen Chloride and Deuterium Chloride". Nature 213 (5072): 171–172. doi:10.1038/213171a0. Bibcode: 1967Natur.213..171S.
13. ↑ Hydrochloric Acid – Compound Summary. Pubchem
14. ↑ "Observations on different kinds of air [i.e., gases"]. Philosophical Transactions of the Royal Society of London 62: 147–264 (234–244). 1772. doi:10.1098/rstl.1772.0021. https://books.google.com/books?id=aBxWAAAAYAAJ&pg=PA234.
15. ↑ "Electro-chemical researches, on the decomposition of the earths; with observations on the metals obtained from the alkaline earths, and on the amalgam procured from ammonia". Philosophical Transactions of the Royal Society of London 98: 333–370. 1808. doi:10.1098/rstl.1808.0023. Bibcode: 1808RSPT...98..333D. https://books.google.com/books?id=Kg9GAAAAMAAJ&pg=PA343. "p. 343: When potassium was heated in muriatic acid gas [i.e., gaseous hydrogen chloride], as dry as it could be obtained by common chemical means, there was a violent chemical action with ignition; and when the potassium was in sufficient quantity, the muriatic acid gas wholly disappeared, and from one-third to one-fourth of its volume of hydrogene was evolved, and muriate of potash [i.e., potassium chloride] was formed. (The reaction was: 2HCl + 2K → 2KCl + H2)".
16. ↑ Austin, Severin; Glowacki, Arndt (2000). "Hydrochloric Acid". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a13_283. ISBN 978-3-527-30385-4.
17. ↑ Francisco J. Arnsliz (1995). "A Convenient Way To Generate Hydrogen Chloride in the Freshman Lab". J. Chem. Educ. 72 (12): 1139. doi:10.1021/ed072p1139. Bibcode: 1995JChEd..72.1139A. http://jchemed.chem.wisc.edu/journal/Issues/1995/Dec/abs1139.html. Retrieved 6 May 2009.
18. ↑ Austin, Severin; Glowacki, Arndt (2000). Hydrochloric Acid. doi:10.1002/14356007.a13_283. ISBN 3527306730.
19. ↑ Simmler, Walter (2000). "Silicon Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a24_001. ISBN 978-3-527-30385-4.
20. ↑ Kraus, Paul (1942–1943). Jâbir ibn Hayyân: Contribution à l'histoire des idées scientifiques dans l'Islam. I. Le corpus des écrits jâbiriens. II. Jâbir et la science grecque. Cairo: Institut Français d'Archéologie Orientale. ISBN 9783487091150. OCLC 468740510. vol. II, pp. 41–42; Multhauf, Robert P. (1966). The Origins of Chemistry. London: Oldbourne. pp. 141–142.
21. ↑ Stapleton, Henry E.; Azo, R.F.; Hidayat Husain, M. (1927). "Chemistry in Iraq and Persia in the Tenth Century A.D.". Memoirs of the Asiatic Society of Bengal VIII (6): 317–418. OCLC 706947607. http://www.southasiaarchive.com/Content/sarf.100203/231270. p. 333. The relevant recipe reads as follows: "Take equal parts of sweet salt, Bitter salt, Ṭabarzad salt, Andarānī salt, Indian salt, salt of Al-Qilī, and salt of Urine. After adding an equal weight of good crystallised Sal-ammoniac, dissolve by moisture, and distil (the mixture). There will distil over a strong water, which will cleave stone (sakhr) instantly." (p. 333) For a glossary of the terms used in this recipe, see p. 322. German translation of the same passage in Ruska, Julius (1937). Al-Rāzī's Buch Geheimnis der Geheimnisse. Mit Einleitung und Erläuterungen in deutscher Übersetzung. Quellen und Studien zur Geschichte der Naturwissenschaften und der Medizin. VI. Berlin: Springer. p. 182, §5. An English translation of Ruska 1937's translation can be found in Taylor, Gail Marlow (2015). The Alchemy of Al-Razi: A Translation of the "Book of Secrets". CreateSpace Independent Publishing Platform. ISBN 9781507778791. pp. 139–140.
22. ↑ Multhauf 1966, p. 142, note 79.
23. ↑ Multhauf 1966, pp. 160–163.
24. ↑ Karpenko, Vladimír; Norris, John A. (2002). "Vitriol in the History of Chemistry". Chemické listy 96 (12): 997–1005. http://www.chemicke-listy.cz/ojs3/index.php/chemicke-listy/article/view/2266. p. 1002.
25. ↑ Multhauf 1966, p. 208, note 29; cf. p. 142, note 79.
26. ↑ Hartley, Harold (1960). "The Wilkins Lecture. Sir Humphry Davy, Bt., P.R.S. 1778–1829". Proceedings of the Royal Society A 255 (1281): 153–180. doi:10.1098/rspa.1960.0060. Bibcode: 1960RSPSA.255..153H.
27. ↑ Contaminants, National Research Council (US) Committee on Emergency and Continuous Exposure Guidance Levels for Selected Submarine (2009), "Hydrogen Chloride" (in en), Emergency and Continuous Exposure Guidance Levels for Selected Submarine Contaminants: Volume 3 (National Academies Press (US)), https://www.ncbi.nlm.nih.gov/books/NBK219917/, retrieved 2024-04-23
28. ↑ CDC – NIOSH Pocket Guide to Chemical Hazards
29. ↑ "Hydrogen Chloride". 5 March 2012. https://www.cdc.gov/niosh/topics/hydrogen-chloride/.

## External links

* International Chemical Safety Card 0163
* Thames & Kosmos Chem C2000 Experiment Manual

* v
* t
* e

Hydrogen compounds

* H3AsO3
* H3AsO4
* HArF
* HAt
* HSO3F
* HBF4
* HBr
* HBrO
* HBrO2
* HBrO3
* HBrO4
* HCl
* HClO
* HClO2
* HClO3
* HClO4
* HCN
* HCNO
* H2CrO4/H2Cr2O7
* H2CO3
* H2CS3
* HF
* HFΟ
* HI
* HIO
* HIO2
* HIO3
* HIO4
* HMnO4
* H2MoO4
* HNC
* NaHCO3
* HNCO
* HNO
* HNO2
* HNO3
* H2N2O2
* HNO5S
* H3NSO3
* H2O
* H2O2
* H2O3
* H3PO2
* H3PO3
* H3PO4
* H4P2O7
* H5P3O10
* H2PtCl6
* H2S
* H2S2
* H2Se
* H2SeO3
* H2SeO4
* H4SiO4
* H2SiF6
* HSCN
* HNSC
* H2SO3
* H2SO4
* H2SO5
* H2S2O3
* H2S2O6
* H2S2O7
* H2S2O8
* CF3SO3H
* H2Te
* H2TeO3
* H6TeO6
* H4TiO4
* H2Po
* HCo(CO)4

* v
* t
* e

Molecules detected in outer space

Molecules|

| Diatomic|

* Aluminium monochloride
* Aluminium monofluoride
* Aluminium monoxide
* Argonium
* Carbon monophosphide
* Carbon monosulfide
* Carbon monoxide
* Carborundum
* Cyanogen radical
* Diatomic carbon
* Fluoromethylidynium
* Helium hydride ion
* Hydrogen chloride
* Hydrogen fluoride
* Hydrogen (molecular)
* Hydroxyl radical
* Iron(II) oxide
* Magnesium monohydride cation
* Methylidyne radical
* Nitric oxide
* Nitrogen (molecular)
* Nitrogen monohydride
* Nitrogen sulfide
* Oxygen (molecular)
* Phosphorus monoxide
* Phosphorus mononitride
* Potassium chloride
* Silicon carbide
* Silicon mononitride
* Silicon monoxide
* Silicon monosulfide
* Sodium chloride
* Sodium iodide
* Sulfur monohydride
* Sulfur monoxide
* Titanium oxide

|
|

Triatomic|

* Aluminium hydroxide
* Aluminium isocyanide
* Amino radical
* Carbon dioxide
* Carbonyl sulfide
* CCP radical
* Chloronium
* Diazenylium
* Dicarbon monoxide
* Disilicon carbide
* Ethynyl radical
* Formyl radical
* Hydrogen cyanide (HCN)
* Hydrogen isocyanide (HNC)
* Hydrogen sulfide
* Hydroperoxyl
* Iron cyanide
* Isoformyl
* Magnesium cyanide
* Magnesium isocyanide
* Methylene radical
* N2H+
* Nitrous oxide
* Nitroxyl
* Ozone
* Phosphaethyne
* Potassium cyanide
* Protonated molecular hydrogen
* Sodium cyanide
* Sodium hydroxide
* Silicon carbonitride
* c-Silicon dicarbide
* SiNC
* Sulfur dioxide
* Thioformyl
* Thioxoethenylidene
* Titanium dioxide
* Tricarbon
* Water

Four
atoms|

* Acetylene
* Ammonia
* Cyanic acid
* Cyanoethynyl
* Cyclopropynylidyne
* Formaldehyde
* Fulminic acid
* HCCN
* Hydrogen peroxide
* Hydromagnesium isocyanide
* Isocyanic acid
* Isothiocyanic acid
* Ketenyl
* Methylene amidogen
* Methyl radical
* Propynylidyne
* Protonated carbon dioxide
* Protonated hydrogen cyanide
* Silicon tricarbide
* Thioformaldehyde
* Tricarbon monoxide
* Tricarbon sulfide
* Thiocyanic acid

Five
atoms|

* Ammonium ion
* Butadiynyl
* Carbodiimide
* Cyanamide
* Cyanoacetylene
* Cyanoformaldehyde
* Cyanomethyl
* Cyclopropenylidene
* Formic acid
* Isocyanoacetylene
* Ketene
* Methane
* Methoxy radical
* Methylenimine
* Propadienylidene
* Protonated formaldehyde
* Protonated formaldehyde
* Silane
* Silicon-carbide cluster

Six
atoms|

* Acetonitrile
* Cyanobutadiynyl radical
* E-Cyanomethanimine
* Cyclopropenone
* Diacetylene
* Ethylene
* Formamide
* HC4N
* Ketenimine
* Methanethiol
* Methanol
* Methyl isocyanide
* Pentynylidyne
* Propynal
* Protonated cyanoacetylene

Seven
atoms|

* Acetaldehyde
* Acrylonitrile
* Vinyl cyanide
* Cyanodiacetylene
* Ethylene oxide
* Glycolonitrile
* Hexatriynyl radical
* Methylacetylene
* Methylamine
* Methyl isocyanate
* Vinyl alcohol

Eight
atoms|

* Acetic acid
* Aminoacetonitrile
* Cyanoallene
* Ethanimine
* Glycolaldehyde
* Heptatrienyl radical
* Hexapentaenylidene
* Methylcyanoacetylene
* Methyl formate
* Propenal

Nine
atoms|

* Acetamide
* Cyanohexatriyne
* Cyanotriacetylene
* Dimethyl ether
* Ethanol
* Methyldiacetylene
* Octatetraynyl radical
* Propene
* Propionitrile

Ten
atoms
or more|

* Acetone
* Benzene
* Benzonitrile
* Buckminsterfullerene (C60, C60+, fullerene, buckyball)
* C70 fullerene
* Cyanodecapentayne
* Cyanopentaacetylene
* Cyanotetra-acetylene
* Ethylene glycol
* Ethyl formate
* Methyl acetate
* Methyl-cyano-diacetylene
* Methyltriacetylene
* Propanal
* n-Propyl cyanide
* Pyrimidine

Deuterated
molecules|

* Ammonia
* Ammonium ion
* Formaldehyde
* Formyl radical
* Heavy water
* Hydrogen cyanide
* Hydrogen deuteride
* Hydrogen isocyanide
* Methylacetylene
* N2D+
* Trihydrogen cation

Unconfirmed|

* Anthracene
* Dihydroxyacetone
* Ethyl methyl ether
* Glycine
* Graphene
* H2NCO+
* Linear C5
* Naphthalene cation
* Phosphine
* Pyrene
* Silylidine

Related|

* Abiogenesis
* Astrobiology
* Astrochemistry
* Atomic and molecular astrophysics
* Chemical formula
* Circumstellar envelope
* Cosmic dust
* Cosmic ray
* Cosmochemistry
* Diffuse interstellar band
* Earliest known life forms
* Extraterrestrial life
* Extraterrestrial liquid water
* Forbidden mechanism
* Homochirality
* Intergalactic dust
* Interplanetary medium
* Interstellar medium
* Photodissociation region
* Iron–sulfur world theory
* Kerogen
* Molecules in stars
* Nexus for Exoplanet System Science
* Organic compound
* Outer space
* PAH world hypothesis
* Panspermia
* Polycyclic aromatic hydrocarbon (PAH)
* RNA world hypothesis
* Spectroscopy
* Tholin

* Category:Astrochemistry
*   *   *

* v
* t
* e

Chlorine compounds

* ClF
* ClF3
* ClF5
* ClNO3
* ClO
* ClOF3
* Cl2O2
* ClO2
* ClO2F
* ClO3F
* Cl2O
* Cl2O4
* Cl2O6
* Cl2O7
* HCl
* SiCl4

* v
* t
* e

Salts and covalent derivatives of the chloride ion

HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | BCl3
B2Cl4 | CCl4 | NCl3
ClN3 | Cl2O
ClO2
Cl2O7 | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | SiCl4 | P2Cl4
PCl3
PCl5 | S2Cl2
SCl2
SCl4 | Cl2 | Ar
KCl | CaCl
CaCl2 | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl2
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5 | Se2Cl2
SeCl4 | BrCl | KrCl
RbCl | SrCl2 | YCl3 | ZrCl3
ZrCl4 | NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl4 | RuCl3 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
CsCl | BaCl2 |  | HfCl4 | TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | Re3Cl9
ReCl4
ReCl5
ReCl6 | OsCl4 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
AuCl3 | Hg2Cl2,
HgCl2 | TlCl | PbCl2,
PbCl4 | BiCl3 | PoCl2,
PoCl4 | AtCl  | RnCl2
FrCl | RaCl2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaCl3 | CeCl3 | PrCl3 | NdCl2,
NdCl3 | PmCl3 | SmCl2,
SmCl3 | EuCl2,
EuCl3 | GdCl3 | TbCl3 | DyCl2,
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3 | LuCl3
AcCl3 | ThCl4 | PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl3 | Fm  | Md  | No  | LrCl3

* v
* t
* e

Binary compounds of hydrogen

Alkali metal (Group 1) hydrides|

* LiH
* NaH
* KH
* RbH
* CsH

Lithium hydride, LiH
ionic metal hydride

Beryllium hydride
Left (gas phase): BeH2
covalent metal hydride
Right: (BeH2)n (solid phase)
polymeric metal hydride

Borane and diborane
Left: BH3 (special conditions), covalent metalloid hydride
Right: B2H6 (standard conditions), dimeric metalloid hydride

Methane, CH4
covalent nonmetal hydride

Ammonia, NH3
covalent nonmetal hydride

Water, H2O
covalent nonmetal hydride

Hydrogen fluoride, HF
covalent nonmetal hydride

Alkaline (Group 2) earth hydrides|

| Monohydrides|

* BeH
* MgH
* CaH
* SrH
* BaH

|

Dihydrides|

* BeH2
* MgH2
* CaH2
* SrH2
* BaH2

|

Group 13 hydrides|

| Boranes|

* BH3
* B2H6
* B2H2
* B2H4
* B4H10
* B5H9
* B5H11
* B6H10
* B6H12
* B10H14
* B18H22

|

Alanes|

* AlH3
* Al2H6

|

Gallanes|

* GaH3
* Ga2H6

|

Indiganes|

* InH3
* In2H6

|

Thallanes|

* TlH3
* Tl2H6

|

Group 14 hydrides|

| Linear alkanes|

* CH4
* C2H6
* C3H8
* C4H10
* C5H12
* C6H14
* C7H16
* C8H18
* C9H20
* C10H22
* more...

|

Linear alkenes|

* C2H4
* C3H6
* C4H8
* C5H10
* C6H12
* C7H14
* C8H16
* C9H18
* C10H20
* more...

|

Linear alkynes|

* C2H2
* C3H4
* C4H6
* C5H8
* C6H10
* C7H12
* C8H14
* C9H16
* C10H18
* more...

|

Silanes|

* SiH4
* Si2H6
* Si3H8
* Si4H10
* Si5H12
* Si6H14
* Si7H16
* Si8H18
* Si9H20
* Si10H22
* more...

|

Silenes|

* Si2H4

|

Silynes|

* Si2H2
* SiH

|

Germanes|

* GeH4
* Ge2H6
* Ge3H8
* Ge4H10
* Ge5H12

|

Stannanes|

* SnH4
* Sn2H6

|

Plumbanes|

* PbH4

|

* CH
* CH2
* CH3
* C2H
* Cycloalkanes
* Cycloalkenes
* Annulenes
* Many more

Pnictogen (Group 15) hydrides|

| Azanes|

* NH3
* N2H4
* N3H5
* N4H6
* N5H7
* N6H8
* N7H9
* N8H10
* N9H11
* N10H12
* more...

|

Azenes|

* N2H2
* N3H3
* N4H4

|

Phosphanes|

* PH3
* P2H4
* P3H5
* P4H6
* P5H7
* P6H8
* P7H9
* P8H10
* P9H11
* P10H12
* more...

|

Phosphenes|

* P2H2
* P3H3
* P4H4

|

Arsanes|

* AsH3
* As2H4

|

Stibanes|

* SbH3

|

Bismuthanes|

* BiH3

|

* HN3
* NH
* radical

Hydrogen chalcogenides (Group 16 hydrides)|

| Polyoxidanes|

* H2O
* H2O2
* H2O3
* H2O4
* H2O5
* H2O6
* H2O7
* H2O8
* H2O9
* H2O10
* more...

|

Polysulfanes|

* H2S
* H2S2
* H2S3
* H2S4
* H2S5
* H2S6
* H2S7
* H2S8
* H2S9
* H2S10
* more...

|

Selanes|

* H2Se
* H2Se2

|

Tellanes|

* H2Te
* H2Te2

|

Polanes|

* PoH2

|

* HO
* HO2
* HO3
* H2O+–O–
* H2S=S
* (HS)2S+–S–
* HS
* HDO
* D2O
* T2O

Hydrogen halides (Group 17 hydrides)|

* HF
* HCl
* HBr
* HI
* HAt

Transition metal hydrides|

* ScH2
* YH2
* YH3
* TiH2
* ZrH2
* HfH2
* VH
* VH2
* NbH
* NbH2
* TaH
* CrH
* CrH2
* CrHx
* NiH
* PdHx (x < 1)
* FeH
* FeH2
* FeH5
* CuH
* ZnH2
* CdH2
* HgH2

Lanthanide hydrides|

* LaH2
* LaH3
* LaH10
* CeH2
* CeH3
* PrH2
* PrH3
* NdH2
* NdH3
* SmH2
* SmH3
* EuH2
* GdH2
* GdH3
* TbH2
* TbH3
* DyH2
* DyH3
* HoH2
* HoH3
* ErH2
* ErH3
* TmH2
* TmH3
* YbH2
* YbH2.5
* LuH2
* LuH3

Actinide hydrides|

* AcH2
* ThH2
* Th4H15
* PaH3
* UH3
* NpH2
* NpH3
* PuH2
* PuH3
* AmH2
* AmH3
* CmH2

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Original source: https://en.wikipedia.org/wiki/Hydrogen chloride. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Hydrogen_chloride&oldid=4433885"
*[CID]: Compound ID
*[H314]: Causes severe skin burns and eye damage
*[H331]: Toxic if inhaled
*[P261]: Avoid breathing dust/fume/gas/mist/vapours/spray
*[P280]: Wear protective gloves/protective clothing/eye protection/face protection
*[P303+361+353]: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water/shower
*[P304+340+310]: IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing. Immediately call a POISON CENTER or doctor/physician
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
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