Difference between revisions of "Calcium"

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== Description ==
 
== Description ==
  
A soft, white, metallic element. Calcium occurs naturally in the earth's crust at concentrations of 3.64%, which makes it the 5th most abundant element in the earth's crust. The pure material was first isolated by Sir Humphrey Davy in 1808. Calcium is found as salts, such as [http://cameo.mfa.org/materials/fullrecord.asp?name=calcium%20carbonate calcium carbonate] ([http://cameo.mfa.org/materials/fullrecord.asp?name=limestone limestone], [http://cameo.mfa.org/materials/fullrecord.asp?name=marble marble], [http://cameo.mfa.org/materials/fullrecord.asp?name=chalk chalk], etc) and [http://cameo.mfa.org/materials/fullrecord.asp?name=calcium%20sulfate calcium sulfate] ([http://cameo.mfa.org/materials/fullrecord.asp?name=gypsum gypsum]). It is an essential component in plants and animals. As a metal, calcium is harder than [http://cameo.mfa.org/materials/fullrecord.asp?name=sodium sodium] but softer than [http://cameo.mfa.org/materials/fullrecord.asp?name=aluminum aluminum] or [http://cameo.mfa.org/materials/fullrecord.asp?name=magnesium magnesium]. It tarnishes on exposure to air. Metallic calcium is used in smelting metals as a getter to absorb [http://cameo.mfa.org/materials/fullrecord.asp?name=oxygen oxygen], [http://cameo.mfa.org/materials/fullrecord.asp?name=carbon%20dioxide carbon dioxide], and [http://cameo.mfa.org/materials/fullrecord.asp?name=sulfur%20dioxide sulfur] gases.
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A soft, white, metallic element. Calcium occurs naturally in the earth's crust at concentrations of 3.64%, which makes it the 5th most abundant element in the earth's crust. The pure material was first isolated by Sir Humphrey Davy in 1808. Calcium is found as salts, such as [[calcium carbonate]] ([[limestone]], [[marble]], [[chalk]], etc) and [[calcium sulfate]] ([[gypsum]]). It is an essential component in plants and animals. As a metal, calcium is harder than [[sodium]] but softer than [[aluminum]] or [[magnesium]]. It tarnishes on exposure to air. Metallic calcium is used in smelting metals as a getter to absorb [[oxygen]], [[carbon dioxide]], and [[sulfur dioxide|sulfur] gases.
  
 
== Synonyms and Related Terms ==
 
== Synonyms and Related Terms ==

Revision as of 14:09, 9 January 2014

Calcium carbonate

Description

A soft, white, metallic element. Calcium occurs naturally in the earth's crust at concentrations of 3.64%, which makes it the 5th most abundant element in the earth's crust. The pure material was first isolated by Sir Humphrey Davy in 1808. Calcium is found as salts, such as calcium carbonate (limestone, marble, chalk, etc) and calcium sulfate (gypsum). It is an essential component in plants and animals. As a metal, calcium is harder than sodium but softer than aluminum or magnesium. It tarnishes on exposure to air. Metallic calcium is used in smelting metals as a getter to absorb oxygen, carbon dioxide, and [[sulfur dioxide|sulfur] gases.

Synonyms and Related Terms

Ca; calix (Lat.); calcio (It., Esp.); Cálcio (Port.); Kalcium (Sven.)

Other Properties

Flame color is yellow-red. Reacts violently with water, alcohols and dilute acids to evolve hydrogen. Dissolves in ammonium hydroxide to form a blue solution.

Composition Ca (atomic no. 20)
CAS 7440-70-2
Melting Point 850
Density 1.54
Molecular Weight atomic wt = 40.078
Boiling Point 1480

Hazards and Safety

Powder ignites in air.

LINK: International Chemical Safety Card

Additional Information

Web Elements: Website

Authority

  • G.S.Brady, Materials Handbook, McGraw-Hill Book Co., New York, 1971 Comment: p. 138
  • Richard S. Lewis, Hawley's Condensed Chemical Dictionary, Van Nostrand Reinhold, New York, 10th ed., 1993
  • Van Nostrand's Scientific Encyclopedia, Douglas M. Considine (ed.), Van Nostrand Reinhold, New York, 1976
  • The Merck Index, Martha Windholz (ed.), Merck Research Labs, Rahway NJ, 10th edition, 1983 Comment: entry 1613
  • The American Heritage Dictionary or Encarta, via Microsoft Bookshelf 98, Microsoft Corp., 1998
  • Chemical & Engineering News, American Chemical Society, Washington DC, 81 (36) , Sept. 8, 2003 Comment: Sture Forsen, p. 66.

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