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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. In its edible form, it is commonly used as a condiment ...
The crystal structure of sodium chloride, NaCl, a typical salt.The purple spheres represent sodium cations, Na +, and the green spheres represent chloride anions, Cl −.The yellow stipples show the electrostatic forces.
Examples of such crystals are the alkali halides, including potassium fluoride (KF), potassium chloride (KCl), potassium bromide (KBr), potassium iodide (KI), sodium fluoride (NaF). [1] Sodium chloride (NaCl) has a 6:6 co-ordination. The properties of NaCl reflect the strong interactions that exist between the ions.
In crystallography, crystal structure is a description of ordered arrangement of atoms, ions, or molecules in a crystalline material. [1] Ordered structures occur from intrinsic nature of constituent particles to form symmetric patterns that repeat along the principal directions of three-dimensional space in matter.
Pauling estimated that an electronegativity difference of 1.7 (on the Pauling scale) corresponds to 50% ionic character, so that a difference greater than 1.7 corresponds to a bond which is predominantly ionic. [10] Ionic character in covalent bonds can be directly measured for atoms having quadrupolar nuclei (2 H, 14 N, 81,79 Br, 35,37 Cl or ...
The structure of sodium chloride, revealing the tendency of chloride ions (green spheres) to link to several cations. The presence of chlorides, such as in seawater, significantly worsens the conditions for pitting corrosion of most metals (including stainless steels, aluminum and high-alloyed materials).
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 − .
For typical ionic solids, the cations are smaller than the anions, and each cation is surrounded by coordinated anions which form a polyhedron.The sum of the ionic radii determines the cation-anion distance, while the cation-anion radius ratio + / (or /) determines the coordination number (C.N.) of the cation, as well as the shape of the coordinated polyhedron of anions.