Nitride Bromide

In chemistry, a nitride is a chemical compound of nitrogen. Nitrides can be inorganic or organic, ionic or covalent. The nitride anion, N³⁻, is very elusive but compounds of nitride are numerous, although rarely naturally occurring. Some nitrides have a found applications, such as wear-resistant coatings (e.g., titanium nitride, TiN), hard ceramic materials (e.g., silicon nitride, Si₃N₄), and semiconductors (e.g., gallium nitride, GaN). The development of GaN-based light emitting diodes was recognized by the 2014 Nobel Prize in Physics. Metal nitrido complexes are also common.

Synthesis of inorganic metal nitrides is challenging because nitrogen gas (N₂) is not very reactive at low temperatures, but it becomes more reactive at higher temperatures. Therefore, a balance must be achieved between the low reactivity of nitrogen gas at low temperatures and the entropy driven formation of N₂ at high temperatures. However, synthetic methods for nitrides are growing more sophisticated and the materials are of increasing technological relevance.

Uses of nitrides

Like carbides, nitrides are often refractory materials owing to their high lattice energy, which reflects the strong bonding of "N³⁻" to metal cation(s). Thus, cubic boron nitride, titanium nitride, and silicon nitride are used as cutting materials and hard coatings. Hexagonal boron nitride, which adopts a layered structure, is a useful high-temperature lubricant akin to molybdenum disulfide. Nitride compounds often have large band gaps, thus nitrides are usually insulators or wide-bandgap semiconductors; examples include boron nitride and silicon nitride. The wide-band gap material gallium nitride is prized for emitting blue light in LEDs. Like some oxides, nitrides can absorb hydrogen and have been discussed in the context of hydrogen storage, e.g. lithium nitride.

Examples

Classification of such a varied group of compounds is somewhat arbitrary. Compounds where nitrogen is not assigned −3 oxidation state are not included, such as nitrogen trichloride where the oxidation state is +3; nor are ammonia and its many organic derivatives.

Nitrides of the s-block elements

Only one alkali metal nitride is stable, the purple-reddish lithium nitride (), which forms when lithium burns in an atmosphere of . Both Sodium nitride and potassium nitride have been synthesized, but remain a laboratory curiosity. The nitrides of the alkaline earth metals that have the formula are however numerous. Examples include beryllium nitride (), magnesium nitride (), calcium nitride (), and strontium nitride (). The nitrides of electropositive metals (including Li, Zn, and the alkaline earth metals) readily hydrolyze upon contact with water, including the moisture in the air:
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Nitrides of the p-block elements

Boron nitride exists as several forms ( polymorphs). Nitrides of silicon and phosphorus are also known, but only the former is commercially important. The nitrides of aluminium, gallium, and indium adopt the hexagonal wurtzite structure in which each atom occupies tetrahedral sites. For example, in aluminium nitride, each aluminium atom has four neighboring nitrogen atoms at the corners of a tetrahedron and similarly each nitrogen atom has four neighboring aluminium atoms at the corners of a tetrahedron. This structure is like hexagonal diamond (lonsdaleite) where every carbon atom occupies a tetrahedral site (however wurtzite differs from sphalerite and diamond in the relative orientation of tetrahedra). Thallium(I) nitride () is known, but thallium(III) nitride (TlN) is not.

Transition metal nitrides

Most metal-rich transition metal nitrides adopt a relatively ordered face-centered cubic or hexagonal close-packed crystal structure, with octahedral coordination. Sometimes these materials are called "interstitial