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[[Category: Done 2018-12-10]]
[[File:Ca.png|200px|thumb|Figure 1. Calcium, with [[atomic number]] 20 and [[atomic weight]] of 40.078.<ref>Made internally by a member of the Energy Education team, with information from periodictable.com, Available: http://periodictable.com/Elements/001/index.html</ref>]]

<onlyinclude>'''Calcium''' is the 20th [[element]] on the [[periodic table of elements]] and it is the fifth most abundant element in the earth's crust.</onlyinclude><ref name=info>Royal Society of Chemistry Periodic Table, ''Calcium'' [Online], Available: http://www.rsc.org/periodic-table/element/20/calcium</ref> Some of its properties are listed below:<ref name=info/>

{| class="wikitable"
|-
| '''[[Atomic weight]]''' || 40.078
|-
| '''[[Density]]''' (at 0oC) || 1.54 [[gram|g]]/cm3
|-
| '''[[Boiling point]]''' || 1757 [[Kelvin|K]]
|-
| '''[[Melting point]]''' || 1115 K
|}

Calcium is an [[alkaline]] Earth [[mineral]]. It is naturally found in bones, teeth, shells, [[rock]]s, and minerals. Calcium carbonate is a naturally occurring compound that is the basis for limestone, marble, and chalk. Stalagmites and stalactites in caves form from calcium carbonate precipitating out of solution.<ref name = NBB>John Emsley, "Nature’s Building Blocks: An A-Z Guide to the Elements", Oxford University Press, New York, 2nd Edition, 2011.</ref>

==Calcium uses==
Calcium is used as a [[redox|reducing]] and/or [[alloy]]ing agent for metals<ref name=info/>. It is used primarily in the creation of steel to improve the steel's mechanical properties. Historically, calcium was used to create lime (a calcium oxide and/or hydroxide compound), which was used as a building material. Lime is still used today in substances like paints, concrete, cement, and plaster.

Calcium compounds (such as calcium carbonate or calcium magnesium pills) are often used as calcium supplements for human consumption. Calcium carbonate is also used as an antacid for indigestion<ref name=NBB/>.

==Calcium Carbonate as part of the Carbon Dioxide Cyle==
Calcium carbonate compounds (limestone, shells, etc.) are natural carbon sinks in two ways:<ref name=CCB>John W. Morse, Rolf S. Arvidson, and Andreas Lüttge. "Calcium Carbonate Formation and Dissolution". Chemical Reviews, 2007, V.107 (2), pg 342-381.</ref>
*The formation of carbonate (CO3) often involves the capture of CO2
*Calcium carbonate can react with carbon dioxide saturate water and for calcium bicarbonate (Ca(HCO3)2)

Through [[weathering]] and human activities, the calcium carbonate can be made to break down, releasing the stored carbon dioxide. Acidified solutions (e.g. acid rain) and heat (especially from human processign) are particularly good at breaking down calcium carbonate and bicarbonate into calcium oxide and carbon dioxide (and water, in the case of bicarbonate breakdown)<ref name=CCB/>.

==Isotopes==
Calcium has six [[isotope]]s found in nature:<ref name=info/>
{| class="wikitable"
|-
!Symbol!!Natural Abundance
|-
| 40Ca || 96.941%
|-
| 42Ca || 0.647%
|-
| 43Ca || 0.135%
|-
| 44Ca || 2.086%
|-
| 46Ca || 0.004%
|-
| 48Ca || 0.187%
|}

==Video==
The video below is from the University of Nottingham's [http://www.periodicvideos.com/ periodic videos project].<ref>See more videos from the University of Nottingham on different elements here: http://www.periodicvideos.com/</ref> They have created a complete suite of short videos on every element on the [[periodic table of elements]].

<html>
<iframe width="854" height="480" src="https://www.youtube.com/embed/V9fuY8_ffFg" frameborder="0" allow="autoplay; encrypted-media" allowfullscreen></iframe>
</html>

==For Further Reading==
*[[Periodic table of elements]]
*[[Carbon dioxide]]
*[[Greenhouse gas]]
*[[Metal]]
*[[Carbon capture and storage]]
*Or explore a [[Special:Random|random page]]

==References==
{{reflist}}

Calcium - Revision history

Jmdonev: 1 revision imported

2dev>Jmdonev at 21:11, 15 November 2018