Calcium nitride: Difference between revisions
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{{chembox |
{{chembox |
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| verifiedrevid = |
| verifiedrevid = 428740605 |
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| ImageFile = |
| ImageFile = Kristallstruktur Indiumoxid.png |
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| ImageSize = |
| ImageSize = |
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| 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. |
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| IUPACName = Calcium nitride |
| IUPACName = Calcium nitride |
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| OtherNames = tricalcium dinitride |
| OtherNames = tricalcium dinitride |
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|Section1={{Chembox Identifiers |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo = 12013-82-0 |
| CASNo = 12013-82-0 |
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| PubChem = 3387080 |
| PubChem = 3387080 |
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| RTECS = |
| RTECS = |
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| EINECS = 234-592-9 |
| EINECS = 234-592-9 |
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| SMILES = |
| SMILES = [Ca]=N[Ca]N=[Ca] |
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| SMILES2 = [Ca+2].[Ca+2].[Ca+2].[N-3].[N-3] |
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| SMILES3 = [Ca]=[N-].[Ca+2].[N-]=[Ca] |
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| InChI = InChI=1S/3Ca.2N |
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| InChI2 = InChI=1S/3Ca.2N/q3*+2;2*-3 |
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| InChI3 = InChI=1S/3Ca.2N/q;;+2;2*-1 |
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|Section2={{Chembox Properties |
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| Ca |
| Ca=3 | N=2 |
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| Appearance = red-brown crystalline solid |
| Appearance = red-brown crystalline solid |
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| Density = 2.670 g/cm<sup>3</sup> <br> 2.63 g/cm<sup>3</sup> (17 °C) |
| Density = 2.670 g/cm<sup>3</sup> <br> 2.63 g/cm<sup>3</sup> (17 °C) |
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| MeltingPtC = 1195 |
| MeltingPtC = 1195 |
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| BoilingPtC = |
| BoilingPtC = |
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| Solubility = decomposes |
| Solubility = decomposes |
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|Section3={{Chembox Structure |
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| CrystalStruct = [[Cubic crystal system|Cubic]], [[Pearson symbol|cI80]] |
| CrystalStruct = [[Cubic crystal system|Cubic]], [[Pearson symbol|cI80]] |
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| SpaceGroup = Ia-3, No. 206 |
| SpaceGroup = Ia-3, No. 206 |
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|Section7={{Chembox Hazards |
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| MainHazards = |
| MainHazards = |
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| FlashPt = |
| FlashPt = |
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| AutoignitionPt = |
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| Section8 = {{Chembox Related |
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| 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]] |
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| OtherAnions = {{ubl|[[Calcium fluoride]]|[[Calcium oxide]]}} |
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| OtherCompounds = {{ubl|[[Ammonia]]|[[Calcium amide]]|[[Calcium imide]]}} |
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'''Calcium nitride''' is a red-brown, crystalline solid made up of [[calcium]] and [[nitrogen]]. Its chemical formula is [[Calcium|Ca]]<sub>3</sub>[[Nitrogen|N]]<sub>2</sub>.<ref>{{Cite book|title=Concise Encyclopedia Chemistry|author= Mary Eagleson|year= 1994|publisher=Walter de Gruyter|url= http://books.google.com/?id=Owuv-c9L_IMC&pg=PA160&lpg=PA160&dq=%22Calcium+nitride%22|isbn=3110114518}}</ref> |
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'''Calcium nitride''' is the [[inorganic compound]] with the [[chemical formula]] [[Calcium|Ca]]<sub>3</sub>[[Nitride|N]]<sub>2</sub>.<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. |
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⚫ | α-Calcium nitride |
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==Structure== |
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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: |
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⚫ | α-Calcium nitride adopts an anti-[[bixbyite]] structure, similar to [[Manganese(III) oxide|Mn<sub>2</sub>O<sub>3</sub>]], except that the positions of the ions are reversed: calcium (Ca<sup>2+</sup>) take the oxide (O<sup>2−</sup>) positions and nitride ions (N<sup>3−</sup>) the manganese (Mn<sup>3+</sup>). In this structure, Ca<sup>2+</sup> 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> |
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==Synthesis and reactions== |
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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 Ca<sub>3</sub>N<sub>2</sub>, Sr<sub>3</sub>N<sub>2</sub>, Ba<sub>3</sub>N<sub>2</sub>” in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 940-1.</ref> |
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⚫ | 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-Ca<sub>3</sub>N<sub>2</sub>) and Magnesium Nitride (Mg<sub>3</sub>N<sub>2</sub>) | 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> |
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It reacts with moisture in air to give [[ammonia]] and [[calcium hydroxide]]: |
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Like [[sodium oxide]], calcium nitride absorbs hydrogen above 350 °C: |
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This reaction also occurs in [[water]]. |
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== General references == |
== General references == |
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*{{Greenwood&Earnshaw}} |
* {{Greenwood&Earnshaw}} |
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== |
== References == |
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{{reflist}} |
{{reflist}} |
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{{Calcium compounds}} |
{{Calcium compounds}} |
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{{Nitrides}} |
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[[Category:Nitrides]] |
[[Category:Nitrides]] |
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{{inorganic-compound-stub}} |
{{inorganic-compound-stub}} |
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[[ar:نتريد الكالسيوم]] |
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[[pt:Nitreto de cálcio]] |
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[[simple:Calcium nitride]] |
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[[zh:氮化钙]] |