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About Calcium

Calcium Bohr

Calcium is the fifth most abundant element by mass in the earth’s crust, where it is found as a component of many common minerals. Calcium carbonate is one of the most common compounds of calcium, found widely as the primary component of limestone. For millennia, humans have used limestone directly as a building material, and additionally to produce lime, which itself was widely used in building materials such as mortar. As a chemical agent, lime found historic uses in arenas such as agriculture, tanning, and glassmaking. Other widely known and used calcium minerals include marble, a type of rock resulting from the metamorphosis of limestone, and gypsum, which is composed of calcium sulfate. Though calcium is ubiquitous in these mineral forms, the metallic form is so highly reactive that it is not found in nature, and was not produced chemically until 1808. Sir Humphry Davy accomplished the production of a calcium-mercury amalgam through electrolysis of lime in the presence of mercury oxide, and from this was able to distill pure calcium metal, which he named from the latin “calc”, meaning lime.

Calcium mineral products are still widely used in building materials, as they have been for centuries. Limestone is no longer favored as a structural material due to its tendency to be eroded by acid rain, but the crushed stone is frequently used as a base material in road building. Marble, long used both to build structures and as a sculpture medium, remains in use for these and other applications. Calcium hydroxide, often termed “builder’s lime”, is a major component of many mortars, plaster, and stucco, while calcium oxide, or quicklime, is essential for the making of cement. Gypsum is also often found in both plaster and cement, but is most notable for use as gypsum board, known more commonly as drywall.

Calcium and calcium compounds are incredibly important as chemical agents. In steel refining, calcium oxide is used as a flux to remove impurities, a use that accounts for almost a third of lime consumption. Calcium hydroxide is widely used in mining and metallurgy, both as an active agent in extracting metals from their ores and as a means to neutralize acids produced by the ores or used in their processing. Calcium hydroxide also finds use in water treatment, as well as in flue gas desulfurization, where it reacts with gaseous sulfur pollutants, preventing their release into the air. Incidentally, this use results in the production of synthetic calcium sulfate, which can be used in the manufacture of gypsum products such as drywall. Lime is additionally important in processing wood pulp into paper, refining sugar, making glass, and producing a number of other important industrial chemicals. Additionally, hydrated lime is used in drilling fluid for oil and gas drilling, and serves as a source of both calcium and alkalinity, important for removing soluble carbonate ions and controlling corrosion.

Calcium plays many essential roles in biological systems, and its compounds are therefore have important agricultural and medical uses. Agricultural lime consists of pulverized limestone, and is added to soil as a source of calcium and magnesium for plants, as well as to neutralize acidic soils. Calcium carbonate is used as an antacid, a calcium supplement, and as a phosphate binder in the treatment of patients with renal failure. As a safe and relatively inert compound, it also is used as a filler in tablets and other forms of pharmaceuticals. Additionally, hydroxyapatite, the form of calcium found in bones, is often used to coat medical implants in order to promote integration of the implant with existing bone.

There are many other calcium compounds that play important roles in industry. Calcium hypochlorite is a common bleaching agent. Calcium phosphate is used in the production of fertilizer. Calcium carbide was once used in carbide lamps, but today is mostly important for production of acetylene, from which PVC is mate, and in steelmaking. Calcium phosphide is found in pyrotechnic applications such as fireworks, flares, and incindiery bombs. Calcium chloride is a dessicant and deicing agent, while calcium silicate is used as an alternative to asbestos for high-temperature insulation.

Heating calcium-rich limestones decomposes the carbonate, producing calcium oxide, or quicklime. The addition of water to quicklime produces calcium hydroxide, which is often termed slaked or hydrated lime. Most industrial calcium products use one of these as raw material, with the exception of those products that require the use of gypsum. Gypsum may be mined, or may be recovered from industrial processes where it accumulates as a byproduct. Calcium metal has comparatively few uses, but when needed is produced by mixing calcium oxide with fine particles of aluminum, and then heating the mixture in a vacuum.

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Compounds

High Purity (99.999%) Calcium (Ca) Sputtering Target High Purity (99.999%) Calcium Oxide (CaO) Powder Calcium's primary commercial application is as a reducing agent in the production of other metals. In iron and steel production it is added to the melt to remove oxygen, sulfur and carbon. Calcium is also used in small doses in alloys of copper and beryllium. Various calcium compounds have wide application in food, pharmaceutical and cosmetics. It is also used in dietary supplements because it has been shown to improve bone and dental health. Calcium is available as metal and compounds with purities from 99% to 99.999% (ACS grade to ultra-high purity). Oxides tend to be insoluble. Fluorides are another insoluble form for uses in which oxygen is undesirable such as metallurgy, chemical and physical vapor deposition and in some optical coatings. Calcium is also available in soluble forms including chlorides, nitrates and acetates. These compounds can be manufactured as solutions at specified stoichiometries.

Calcium Properties

Calcium (Ca) atomic and molecular weight, atomic number and elemental symbolCalcium is a Block S, Group 2, Period 4 element. The number of electrons in each of Calcium's shells is 2, 8, 8, 2 and its electron configuration is [Ar] 4s2. Calcium Bohr Model Elemental CalciumThe calcium atom has a radius of 197.pm and its Van der Waals radius is 231.pm. In its elemental form, CAS 7440-70-2, calcium has a dull gray-silver appearance. Calcium is a reactive, soft metal that is a member of the alkaline earth elements. It is found in the minerals dolomite, gypsum, plagioclases, amphiboles, pyroxenes and garnets. Calcium was discovered and first isolated by Sir Humphrey Davy in 1808. The name calcium originates from the Latin word 'calics' meaning lime.

Symbol: Ca
Atomic Number: 20
Atomic Weight: 40.078
Element Category: alkaline earth metal
Group, Period, Block: 2, 4, s
Color: silvery white/ gray
Other Names: Cálcio, Kalcium
Melting Point: 842 °C, 1547.6 °F, 1115.15 K
Boiling Point: 1484 °C, 2703.2 °F, 1757.15 K
Density: 1.55 g/cm3
Liquid Density @ Melting Point: 1.378 g/cm3
Density @ 20°C: 1.55 g/cm3
Density of Solid: 1550 kg·m3
Specific Heat: 0.156 Cal/g/K @ 25°C
Superconductivity Temperature: N/A
Triple Point: N/A
Critical Point: N/A
Heat of Fusion (kJ·mol-1): 9.33
Heat of Vaporization (kJ·mol-1): 150.6
Heat of Atomization (kJ·mol-1): 177.74
Thermal Conductivity: 2.01 W/cm/K @ 298.2 K
Thermal Expansion: (25 °C) 22.3 µm·m-1·K-1
Electrical Resistivity: 3.91 µΩ·cm @ 0 °C
Tensile Strength: N/A
Molar Heat Capacity: 25.929 J·mol-1·K-1
Young's Modulus: 20 GPa
Shear Modulus: 7.4 GPa
Bulk Modulus: 17 GPa
Poisson Ratio: 0.31
Mohs Hardness: 1.75
Vickers Hardness: N/A
Brinell Hardness: 167 MPa
Speed of Sound: (20 °C) 3810 m·s-1
Pauling Electronegativity: 1
Sanderson Electronegativity: 0.95
Allred Rochow Electronegativity: 1.04
Mulliken-Jaffe Electronegativity: 1.08 (sp orbital)
Allen Electronegativity: 1.034
Pauling Electropositivity: 3
Reflectivity (%): N/A
Refractive Index: N/A
Electrons: 20
Protons: 20
Neutrons: 20
Electron Configuration: [Ar] 4s2
Atomic Radius: 197 pm
Atomic Radius, non-bonded (Å): 2.31
Covalent Radius: 176±10 pm
Covalent Radius (Å): 1.74
Van der Waals Radius: 231 pm
Oxidation States: 2, 1 (strongly basic oxide)
Phase: Solid
Crystal Structure: face-centered cubic
Magnetic Ordering: diamagnetic
Electron Affinity (kJ·mol-1) 2.368
1st Ionization Energy: 589.83 kJ·mol-1
2nd Ionization Energy: 1145.46 kJ·mol-1
3rd Ionization Energy: 4912.40 kJ·mol-1
CAS Number: 7440-70-2
EC Number: 231-179-5
MDL Number: MFCD00085314
Beilstein Number: 4241647
SMILES Identifier: [Ca]
InChI Identifier: InChI=1S/Ca
InChI Key: OYPRJOBELJOOCE-UHFFFAOYSA-N
PubChem CID: 5460341
ChemSpider ID: 4573905
Abundance
Earth - Total: 1.54%
Mercury - Total: 1.18%
Venus - Total:  1.61% 
Earth - Seawater (Oceans), ppb by weight: 4220
Earth - Seawater (Oceans), ppb by atoms: 650
Earth -  Crust (Crustal Rocks), ppb by weight: 50000000
Earth -  Crust (Crustal Rocks), ppb by atoms: 26000000
Sun - Total, ppb by weight: 70000
Sun - Total, ppb by atoms: 2000
Stream, ppb by weight: 1500
Stream, ppb by atoms: 38
Meterorite (Carbonaceous), ppb by weight: 11000000
Meterorite (Carbonaceous), ppb by atoms: 5200000
Typical Human Body, ppb by weight: 14000000
Typical Human Body, ppb by atom: 2200000
Universe, ppb by weight: 70000
Universe, ppb by atom: 2000
Discovered By: Humphry Davy
Discovery Date: 1808
First Isolation: Humphry Davy (1808)

Health, Safety & Transportation Information for Calcium

Calcium is non-toxic and is an essential metal for living organisms. Safety data for Calcium and its compounds can vary widely depending on the form. For potential hazard information, toxicity, and road, sea and air transportation limitations, such as DOT Hazard Class, DOT Number, EU Number, NFPA Health rating and RTECS Class, please see the specific material or compound referenced in the Products tab. The below information applies to elemental (metallic) Calcium.

Safety Data
Material Safety Data Sheet MSDS
Signal Word Danger
Hazard Statements H261
Hazard Codes F
Risk Codes 15
Safety Precautions 8-24/25-43
RTECS Number N/A
Transport Information UN 1401 4.3/PG 2
WGK Germany 1
Globally Harmonized System of
Classification and Labelling (GHS)
Flame-Flammables

Calcium Isotopes

Calcium has five stable isotopes: 40Ca, 42Ca, 43Ca, 44Ca and 46Ca

Nuclide Isotopic Mass Half-Life Mode of Decay Nuclear Spin Magnetic Moment Binding Energy (MeV) Natural Abundance
(% by atom)
34Ca 34.01412(32)# <35 ns p to 33K 0+ N/A 239.19 MeV -
35Ca 35.00494(21)# 25.7(2) ms β+ to 35K; β+ + p to 34Ar 1/2+# N/A 256.59 MeV -
36Ca 35.99309(4) 102(2) ms β+ + p to 35Ar; β+ to 36K 0+ N/A 274.91 MeV -
37Ca 36.985870(24) 181.1(10) ms β+ + p to 36Ar; β+ to 37K (3/2+) N/A 290.45 MeV -
38Ca 37.976318(5) 440(8) ms EC to 38K 0+ N/A 306.91 MeV -
39Ca 38.9707197(20) 859.6(14) ms EC to 39K 3/2+ N/A 320.58 MeV -
40Ca 39.96259098(22) Observationally Stable - 0+ 0 336.11 96.941
41Ca 40.96227806(26) 1.02(7)E+5 y EC to 41K 7/2- -1.595 344.19 -
42Ca 41.95861801(27) STABLE - 0+ 0 355.99 0.647
43Ca 42.9587666(3) STABLE - 7/2- -1.31727 364.07 0.135
44Ca 43.9554818(4) STABLE - 0+ 0 374.95 2.086
45Ca 44.9561866(4) 162.67(25) d β- to 45Sc 7/2- -1.327 382.09 -
46Ca 45.9536926(24) Observationally Stable - 0+ 0 392.97 0.004
47Ca 46.9545460(24) 4.536(3) d β- to 47Sc 7/2- -1.38 400.11 -
48Ca 47.952534(4) 43(38)E+18 y - to 48Ti 0+ 0 410.05 0.187
49Ca 48.955674(4) 8.718(6) min β- to 49Sc 3/2- N/A 415.34 -
50Ca 49.957519(10) 13.9(6) s β- to 50Sc 0+ N/A 421.55 -
51Ca 50.9615(1) 10.0(8) s β- to 51Sc; β- + n to 50Sc (3/2-)# N/A 425.91 -
52Ca 51.96510(75) 4.6(3) s β- to 52Sc; β- + n to 51Sc 0+ N/A 430.26 -
53Ca 52.97005(54)# 90(15) ms β- to 53Sc; β- + n to 52Sc 3/2-# N/A 433.68 MeV
54Ca 53.97435(75)# 50# ms [>300 ns] β- + n to 53Sc; β- to 54Sc 0+ N/A 438.03 MeV
55Ca 54.98055(75)# 30# ms [>300 ns] β- to 55Sc 5/2-# N/A 440.52 MeV
56Ca 55.98557(97)# 10# ms [>300 ns] β- to 56Sc 0+ N/A 443.94 MeV
57Ca 56.99236(107)# 5# ms β- to 57Sc; β- + n to 56Sc 5/2-# N/A 445.50 MeV
Calcium Elemental Symbol

Recent Research & Development for Calcium

  • Mutual Inhibition between Catalytic Impurities of Sulfur and Those of Calcium in Coke during Carbon–Air and Carbon–CO2 Reactions. Jin Xiao, Qifan Zhong, Fachuang Li, Jindi Huang, Yanbin Zhang, and Bingjie Wang. Energy Fuels: February 3, 2015
  • Amido Analogues of Nonbent Lanthanide (II) and Calcium Metallocenes. Heterolytic Cleavage of Bond Ln–Carbazolyl Ligand Promoted by Lewis Base Coordination. Alexander N. Selikhov, Anton V. Cherkasov, Georgy K. Fukin, Alexander A. Trifonov, Iker del Rosal, and Laurent Maron. Organometallics: January 29, 2015
  • Effects of Anionic Polyacrylamide on Carbonation for the Crystallization of Precipitated Calcium Carbonate. Tai-Ju Lee, Hyoung-Jin Kim, Seok Jun Hong, and Jung Yun Park. Crystal Growth & Design: January 29, 2015
  • Analysis of the Calcium Alginate Gelation Process Using a Kenics Static Mixer. Takuro Hozumi, Seiichi Ohta, and Taichi Ito. Ind. Eng. Chem. Res.: January 28, 2015
  • Glycine-Mediated, Selective Preparation of Monodisperse Spherical Vaterite Calcium Carbonate in Various Reaction Systems. Yonghua Lai, Liangsen Chen, Weichao Bao, Yihua Ren, Yuxing Gao, Yingwu Yin, and Yufen Zhao. Crystal Growth & Design: January 26, 2015
  • Protein Arginine Deiminase 2 Binds Calcium in an Ordered Fashion: Implications for Inhibitor Design. Daniel J. Slade, Pengfei Fang, Christina J. Dreyton, Ying Zhang, Jakob Fuhrmann, Don Rempel, Benjamin D. Bax, Scott A. Coonrod, Huw D. Lewis, Min Guo, Michael L. Gross, and Paul R. Thompson. ACS Chem. Biol.: 42030
  • Composites of Eu3+-Doped Calcium Apatite Nanoparticles and Silica Particles: Comparative Study of Two Preparation Methods. Ayumu Isobe, Satoru Takeshita, and Tetsuhiko Isobe. Langmuir: January 23, 2015
  • Manganese Binding Properties of Human Calprotectin Under Conditions of High and Low Calcium: X-ray Crystallographic and Advanced EPR Spectroscopic Analysis. Derek M. Gagnon, Megan Brunjes Brophy, Sarah E. J. Bowman, Troy A. Stich, Catherine L. Drennan, R. David Britt, and Elizabeth M. Nolan. J. Am. Chem. Soc.: January 18, 2015
  • Combined Effect of Sunflower Stem Carbon–Calcium Alginate Beads for the Removal and Recovery of Chromium from Contaminated Water in Column Mode. Monika Jain, V.K. Garg, Krishna Kadirvelu, and Mika Sillanpää. Ind. Eng. Chem. Res.: January 14, 2015
  • Calcium Phosphate Flocs and the Clarification of Sugar Cane Juice from Whole of Crop Harvesting. Caroline C. D. Thai, Lalehvash Moghaddam, and William O. S. Doherty. J. Agric. Food Chem.: January 9, 2015