Calcium nitride: Difference between revisions

| verifiedrevid = 428740605

| ImageFile = Kristallstruktur Indiumoxid.png

| ImageCaption = Unit cell containing 31 nitride ions (red) and 48 calcium ions (white). Each nitride is surrounded by six calcium, and each calcium by four nitride ions.

|Section1={{Chembox Identifiers

| CASNo_Ref = {{cascite|correct|??}}

| RTECS =

| SMILES = [Ca]=N[Ca]N=[Ca]

| SMILES2 = [Ca+2].[Ca+2].[Ca+2].[N-3].[N-3]

| SMILES3 = [Ca]=[N-].[Ca+2].[N-]=[Ca]

| InChI = InChI=1S/3Ca.2N

| InChI2 = InChI=1S/3Ca.2N/q3*+2;2*-3

| InChI3 = InChI=1S/3Ca.2N/q;;+2;2*-1

|Section2={{Chembox Properties

| Ca=3 | N=2

| BoilingPtC =

|Section3={{Chembox Structure

|Section7={{Chembox Hazards

| MainHazards =

| FlashPt =

| AutoignitionPt =

| Section8 = {{Chembox Related

| OtherCations = [[Beryllium nitride]]<br />[[Magnesium nitride]]<br>[[Strontium nitride]]<br>[[Barium nitride]]<br>[[Radium nitride]]<br>[[Zinc nitride]]<br>[[Aluminium nitride]]<br>[[Lithium nitride]]<br>[[Sodium nitride]]<br>[[Potassium nitride]]

| OtherAnions = {{ubl|[[Calcium fluoride]]|[[Calcium oxide]]}}

| OtherCompounds = {{ubl|[[Ammonia]]|[[Calcium amide]]|[[Calcium imide]]}}

}}

'''Calcium nitride''' is the [[inorganic compound]] with the [[chemical formula]] [[Calcium|Ca]]₃[[Nitride|N]]₂.<ref>{{ Cite book | title = Concise Encyclopedia Chemistry | author = Eagleson, M. | year = 1994 | publisher = Walter de Gruyter | page = [https://archive.org/details/conciseencyclope00eagl/page/160 160] | url = https://archive.org/details/conciseencyclope00eagl | url-access = registration | quote = Calcium nitride. | isbn = 3-11-011451-8 }}</ref> It exists in various forms ([[Isomorphism (crystallography)|isomorph]]s), α-calcium nitride being more commonly encountered.

==Structure==

α-Calcium nitride adopts an anti-[[bixbyite]] structure, similar to [[Manganese(III) oxide|Mn₂O₃]], except that the positions of the ions are reversed: calcium (Ca²⁺) take the oxide (O²⁻) positions and nitride ions (N³⁻) the manganese (Mn³⁺). In this structure, Ca²⁺ occupies tetrahedral sites, and the nitride centres occupy two different types of octahedral sites.<ref>Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. {{ISBN|0-19-855370-6}}.</ref>

==Synthesis and reactions==

Calcium nitride is formed along with the oxide, [[calcium oxide|CaO]], when calcium burns in air. It can be produced by direct reaction of the elements:<ref> P. Ehrlich “Calcium, Strontium, Barium Nitrides Ca₃N₂, Sr₃N₂, Ba₃N₂” in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 940-1.</ref>

:3 Ca + N₂ → Ca₃N₂

It reacts with water or even the moisture in air to give [[ammonia]] and [[calcium hydroxide]]:<ref>{{ cite journal | title = The Vibrational Spectra and Decomposition of α-Calcium Nitride (α-Ca₃N₂) and Magnesium Nitride (Mg₃N₂) | year = 1998 | author = Heyns, A. | journal = Journal of Solid State Chemistry | volume = 137 | issue = 1 | pages = 33–41 | doi = 10.1006/jssc.1997.7672 | bibcode = 1998JSSCh.137...33H }}</ref>

:Ca₃N₂ + 6 H₂O → 3 Ca(OH)₂ + 2 NH₃

Like [[sodium oxide]], calcium nitride absorbs hydrogen above 350 °C:

:Ca₃N₂ + 2 H₂ → 2 CaNH + [[calcium hydride|CaH₂]]

* {{Greenwood&Earnshaw}}

== References ==

{{Nitrides}}