Kloriid

Kloriid, in chemistry often referred to as chloride, denotes a family of compounds that contain chlorine in the form of the chloride ion Cl− or as covalently bound chlorine atoms. The most familiar example is sodium chloride, NaCl, a salt composed of Na+ and Cl− ions arranged in a lattice and widely used as a seasoning and preservative.

Chlorides are commonly divided into inorganic chlorides and organic chlorides. Inorganic chlorides include metal chlorides such as NaCl, KCl, FeCl3, and AlCl3, which are typically ionic and many are water-soluble, though some (like AgCl or PbCl2) are sparingly soluble. Organic chlorides feature covalent carbon–chlorine bonds, with examples such as chloromethane (CH3Cl) and carbon tetrachloride (CCl4). Organic chlorides vary widely in reactivity and toxicity and are frequently used as solvents, intermediates, or monomers in industry.

Occurrence and production: Chlorides occur naturally in seawater, brines, and mineral deposits such as halite (rock salt). Industrially, chlorides are produced by mining or evaporating seawater to obtain NaCl, by direct chlorination of metals to form metal chlorides, or by reactions that introduce chlorine into organic substrates.

Uses: Sodium chloride is essential in food and many processes; chlorides like calcium chloride are used for de-icing and dehumidification; organic chlorides serve as solvents, reagents, or monomers (for example vinyl chloride in PVC production).

Safety: Solids and solutions of chlorides can be corrosive or irritants in some contexts. Several organic chlorides are toxic or environmentally persistent and require proper handling and containment.