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Sodium chloride / ˌ s oʊ d i ə m ˈ k l ɔːr aɪ d /, [8] commonly known as edible salt, is an ionic compound with the chemical formula NaCl, representing a 1:1 ratio of sodium and chlorine ions. It is transparent or translucent, brittle, hygroscopic , and occurs as the mineral halite .
The component ions in a salt can be either inorganic, such as chloride (Cl −), or organic, such as acetate (CH 3 COO −). Each ion can be either monatomic (termed simple ion), such as sodium (Na +) and chloride (Cl −) in sodium chloride, or polyatomic, such as ammonium (NH + 4) and carbonate (CO 2− 3) ions in ammonium carbonate.
English: The crystal structure of sodium chloride, NaCl, a typical ionic compound. The __ purple spheres represent sodium cations, Na +, and the __ green spheres represent chloride anions, Cl −. The yellow stipples represent the electrostatic force in each ionic bond.
There occur as many Madelung constants M i in a crystal structure as ions occupy different lattice sites. For example, for the ionic crystal NaCl, there arise two Madelung constants – one for Na and another for Cl. Since both ions, however, occupy lattice sites of the same symmetry they both are of the same magnitude and differ only by sign.
Ionic radius, r ion, is the radius of a monatomic ion in an ionic crystal structure. Although neither atoms nor ions have sharp boundaries, they are treated as if they were hard spheres with radii such that the sum of ionic radii of the cation and anion gives the distance between the ions in a crystal lattice.
English: The crystal structure of sodium chloride, NaCl, a typical ionic compound, emphasising the octahedral environment of one sodium cation, Na +, illustrated as a __ purple sphere and one chloride anion, Cl −, illustrated as a __ green sphere. The yellow stipples represent the electrostatic force in each ionic bond. The crystal lattice ...
The binary compounds sodium chloride (NaCl) and caesium chloride (CsCl) have cubic structures but have different space groups. This can be rationalised in terms of close packing of spheres of different sizes. For example, NaCl can be described as close-packed chloride ions (in a face-centered cubic lattice) with sodium ions in the octahedral holes.
For chemical compounds with regular lattices such as sodium chloride and caesium chloride, a count of the nearest neighbors gives a good picture of the environment of the ions. In sodium chloride each sodium ion has 6 chloride ions as nearest neighbours (at 276 pm) at the corners of an octahedron and each chloride ion has 6 sodium atoms (also ...