Chloride

Chlorides are compounds of the chemical element chlorine. This may be connected with metals, semi - or non-metals. Metal chlorides such as sodium chloride and cobalt, salts of hydrochloric acid, more commonly known as hydrochloric acid ( chemical formula: HCl). Such chloride ions in its lattice singly negatively charged chlorine ( I ) ions Cl - ( chloride ions usually called ). No metal chlorides such as hydrogen chloride, sulfur chloride, carbon tetrachloride ( tetrachloromethane ) and chlorine dioxide are significantly as molecular weight compounds more volatile than saline chlorides. Chlorinated hydrocarbons are considered and identified in the organic as derivatives of various compounds of hydrocarbons. As methane, in which a hydrogen atom is replaced by a chlorine atom is replaced ( substituted ) was named chloromethane or methylene chloride. Here, however, is not as in the above mentioned ionic compounds before chloride as chloride ion, but is covalently bonded to the carbon atom. However, chloride is in the strict sense only the short name for the singly negatively charged chloride ion. Organic amines form with hydrochloric organic hydrochlorides containing chloride ions.

• 3.1 Inorganic Chloride
• 3.2 Organic chlorides

Proof

For wet chemical qualitative detection of chloride, a solution is first prepared. Advantageously, the Sodaauszug, as in the filtrate numerous interfering cations are separated. Halogenidnachweise then can be performed. Chlorides are precipitated with silver nitrate solution as a white, water-insoluble silver chloride.

The quantitative detection can be done by titration of halides.

Properties

Inorganic Chloride

Chlorides are colorless or colored salts that may be present in various crystal structures. They have very high melting and boiling points.

As melt or in solution they conduct electricity. Chlorides dissolve in protic and polar solvents.

Formation

Inorganic Chloride

Chlorides formed in the redox reaction of metals with elemental chlorine or hydrochloric acid ( only if they are in the voltage range below the hydrogen as hydrochloric acid non-oxidative effect ). But they also occur during the reaction of hydroxides, metal oxides, carbonates, bicarbonates, and generally salts of weaker acids with hydrochloric acid.

Organic chlorides

By substitution and addition reactions of hydrocarbons and carboxylic acids and their derivatives, chlorides can be obtained. There are organic chlorides in which the chlorine is present as a chloride ion, such as the hydrochlorides and N- Acyliminiumchloriden. In the carboxylic acid chlorides, a chlorine atom by a highly polarized atomic bond is bound to an acyl radical. In chloroalkanes - traditional name: alkyl chlorides - the respective chlorine atom bonded via a lower polarized covalent bond to one or more carbon atoms.

Use and examples

The best-known example of a chloride is sodium chloride (chemical formula: NaCl ), better known as cooking and table salt. It is used as a condiment and for preserving.

Other important chlorides are:

• Lithium chloride - LiCl
• Potassium chloride - KCl
• Cesium chloride - CsCl
• Magnesium chloride - MgCl2
• Calcium Chloride - CaCl2
• Lead (II ) chloride - PbCl2
• Iron (II ) chloride - FeCl2
• Iron (III ) chloride - FeCl3
• Silver chloride - AgCl
• Zinc chloride - ZnCl2
• Mercury ( I) chloride - Hg2Cl2
• Mercury (II ) chloride - HgCl2
• Ammonium chloride - NH4Cl
• Barium - BaCl2
• Aluminum chloride - AlCl3
• Diboron - B2Cl4

Many chlorides of these salts form hydrates.

Examples of organic chlorides with the covalent carbon-chlorine bond:

• Methylene chloride ( better naming: dichloromethane ) - CH2Cl2
• Allyl chloride - CH2 = CHCH2Cl
• Benzyl chloride - C6H5CH2Cl

The name of this non-salt organic substances as " chloride " is actually questionable, but nevertheless common.