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It has a high ionisation energy (1251.2 kJ/mol), high electron affinity (349 kJ/mol; higher than fluorine), and high electronegativity (3.16). Chlorine is a strong oxidising agent (Cl 2 + 2e → 2HCl = 1.36 V at pH 0). Metal chlorides are largely ionic in nature. The common oxide of chlorine (Cl 2 O 7) is strongly acidic. Liquid bromine
These methods work best when the chloride product is stable to hydrolysis; otherwise, the possibilities include high-temperature oxidative chlorination of the element with chlorine or hydrogen chloride, high-temperature chlorination of a metal oxide or other halide by chlorine, a volatile metal chloride, carbon tetrachloride, or an organic ...
Acidic oxides will typically have a low pK a and may be inorganic or organic. A commonly encountered acidic oxide, carbon dioxide produces an acidic solution (and the generation of carbonic acid) when dissolved. Generally non-metallic oxides are acidic. [2] The acidity of an oxide can be reasonably assumed by its accompanying constituents.
chlorine chlorite, ClOClO, chlorine (I,III) oxide; dichlorine trioxide, Cl 2 O 3 as O−Cl−ClO 2, chlorine (III,V) oxide dichlorine trioxide, Cl 2 O 3 as possible isomer Cl−O−ClO 2, chlorine (I,V) oxide; dichlorine trioxide, Cl 2 O 3 as hypothetical isomer O−Cl−O−Cl−O, chlorine (III) oxide; dichlorine tetroxide, also known as ...
Common examples include sodium hypochlorite (household bleach) and calcium hypochlorite (a component of bleaching powder, swimming pool "chlorine"). [1] The Cl-O distance in ClO − is 1.69 Å. [2] The name can also refer to esters of hypochlorous acid, namely organic compounds with a ClO– group covalently bound to the rest
Chlorous acid is an inorganic compound with the formula HClO 2. It is a weak acid. Chlorine has oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid (Cl oxidation state +1) and chloric acid (Cl oxidation state +5): 2 HClO 2 → HClO + HClO 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.
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure.