Chloride
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| Names | |||
|---|---|---|---|
| Systematic IUPAC name
Chloride[1] | |||
| Identifiers | |||
3D model (JSmol)
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| 3587171 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| 14910 | |||
IUPHAR/BPS
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| KEGG | |||
PubChem CID
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| UNII | |||
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| Properties | |||
| Cl− | |||
| Molar mass | 35.45 g·mol−1 | ||
| Conjugate acid | Hydrogen chloride | ||
| Thermochemistry | |||
Std molar
entropy (S⦵298) |
153.36 J·K−1·mol−1[2] | ||
Std enthalpy of
formation (ΔfH⦵298) |
−167 kJ·mol−1[2] | ||
| Related compounds | |||
Other anions
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
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The term chloride refers to a compound or molecule that contains either a chlorine anion (Cl−), which is a negatively charged chlorine atom, or a non-charged chlorine atom covalently bonded to the rest of the molecule by a single bond (−Cl). The pronunciation of the word "chloride" is /ˈklɔːraɪd/.[3]
Chloride salts such as sodium chloride are often soluble in water.[4] It is an essential electrolyte located in all body fluids responsible for maintaining acid/base balance, transmitting nerve impulses and regulating liquid flow in and out of cells. Other examples of ionic chlorides include potassium chloride (KCl), calcium chloride (CaCl2), and ammonium chloride (NH4Cl). Examples of covalent chlorides include methyl chloride (CH3Cl), carbon tetrachloride (CCl4), sulfuryl chloride (SO2Cl2), and monochloramine (NH2Cl).
- ^ "Chloride ion - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
- ^ Wells, John C. (2008), Longman Pronunciation Dictionary (3rd ed.), Longman, p. 143, ISBN 9781405881180
- ^ Green, John, and Sadru Damji. "Chapter 3." Chemistry. Camberwell, Vic.: IBID, 2001. Print.