Kloriidide

Kloriidide is the Estonian term used for chlorides, a broad class of chemical compounds that contain chlorine in the form of the chloride ion Cl− or chlorine bound to another element. In many salts, chloride acts as the counteranion, forming ionic lattices with metals or other cations. Chlorides occur widely in nature and industry, and they range from simple inorganic salts to more complex covalent compounds.

Common examples include sodium chloride (NaCl) and potassium chloride (KCl), which are widely used in food and industry; calcium chloride (CaCl2) and magnesium chloride (MgCl2), used in de-icing, dust suppression, and chemistry production; and transition metal chlorides such as iron(III) chloride (FeCl3) and aluminum chloride (AlCl3), which function as catalysts and reagents. Other chlorine-containing chlorides, such as silicon tetrachloride (SiCl4) and phosphorus chlorides (PCl3, PCl5), are molecular chlorides with distinct reactivity.

Properties of chlorides vary significantly. Many metal chlorides are ionic solids with high melting points, while some covalent chlorides are liquids or gases at room temperature. Solubility in water is common, though hydrolysis and moisture sensitivity can occur, especially with highly reactive chlorides like AlCl3 and TiCl4. Chlorides can be produced by reacting chlorine with metals or with hydrogen-containing compounds, or by neutralizing acids with bases.

Applications span food, chemical manufacturing, materials science, and environmental technology. Safety considerations depend on the specific compound; many chlorides are corrosive or toxic in certain forms or exposures, and some release corrosive HCl upon hydrolysis.