Calcium
2007 Schools Wikipedia Selection. Related subjects: Chemical elements
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| General | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
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| Name, Symbol, Number | calcium, Ca, 20 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Chemical series | alkaline earth metals | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Group, Period, Block | 2, 4, s | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Appearance | silvery white |
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| Atomic mass | 40.078 (4) g/mol | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Electron configuration | [Ar] 4s2 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Electrons per shell | 2, 8, 8, 2 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Physical properties | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Phase | solid | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Density (near r.t.) | 1.55 g·cm−3 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Liquid density at m.p. | 1.378 g·cm−3 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Melting point | 1115 K (842 ° C, 1548 ° F) |
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| Boiling point | 1757 K (1484 ° C, 2703 ° F) |
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| Heat of fusion | 8.54 kJ·mol−1 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Heat of vaporization | 154.7 kJ·mol−1 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Heat capacity | (25 °C) 25.929 J·mol−1·K−1 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
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| Atomic properties | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Crystal structure | cubic face centered | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Oxidation states | 2 (strongly basic oxide) |
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| Electronegativity | 1.00 (Pauling scale) | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Ionization energies ( more) |
1st: 589.8 kJ·mol−1 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| 2nd: 1145.4 kJ·mol−1 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| 3rd: 4912.4 kJ·mol−1 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Atomic radius | 180 pm | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Atomic radius (calc.) | 194 pm | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Covalent radius | 174 pm | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Miscellaneous | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Magnetic ordering | paramagnetic | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Electrical resistivity | (20 °C) 33.6 nΩ·m | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Thermal conductivity | (300 K) 201 W·m−1·K−1 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Thermal expansion | (25 °C) 22.3 µm·m−1·K−1 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Speed of sound (thin rod) | (20 °C) 3810 m/s | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Young's modulus | 20 GPa | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Shear modulus | 7.4 GPa | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Bulk modulus | 17 GPa | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Poisson ratio | 0.31 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Mohs hardness | 1.75 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Brinell hardness | 167 MPa | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| CAS registry number | 7440-70-2 | |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| Selected isotopes | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
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Calcium ( IPA: /ˈkalsiəm/) is the chemical element in the periodic table that has the symbol Ca and atomic number 20. It has an atomic mass of 40.078. Calcium is a soft grey alkaline earth metal, and is the fifth most abundant element in the Earth's crust. It is essential for living organisms, particularly in cell physiology, and is the most common metal in many animals. It may be used as a reducing agent in the extraction of thorium, zirconium and uranium.
Notable characteristics
Calcium is a rather soft, gray, metallic element that can be extracted by electrolysis from calcium fluoride. It burns with a yellow-red flame and forms a white nitride coating when exposed to air. It reacts with water, displacing hydrogen and forming calcium hydroxide.
Calcium is essential in muscle contraction, oocyte activation, bones and tooth structure, blood clotting, nerve impulse transmission, regulating heartbeat, and fluid balance within cells. In the U.S., between about 50% and 75% of adults do not get sufficient calcium in their diet. Adults need between 1,000 and 1,300 mg of calcium in their daily diet.
The most abundant isotope, 40Ca, has a nucleus of 20 protons and 20 neutrons. Its electron configuration is: 2 electrons in the K shell (principal quantum number 1), 8 in the L shell (principal quantum number 2), 8 in the M shell (principal quantum number 3), and 2 in the N shell (principal quantum number 4). The outer shell is the valence shell, with 2 electrons in the lone 4s orbital, the 3d orbitals being empty.
Occurrence
Calcium is not naturally found in its elemental state. Calcium is found mostly in soil systems as limestone, gypsum and fluorite. Stalagmites and stalactites contain calcium carbonate. Being an essential macromineral in the human diet, soil conservation practices often consider the sustainable equilibrium of calcium concentrations in the earth.
Applications
Uses include:
- as a reducing agent in the extraction of other metals, such as uranium, zirconium, and thorium.
- as a deoxidizer, desulfurizer, or decarbonizer for various ferrous and nonferrous alloys.
- as an alloying agent used in the production of aluminium, beryllium, copper, lead, and magnesium alloys.
- in the making of cements and mortars to be used in construction.
History
Calcium (Latin calcis, meaning "lime") was known as early as the first century when the Ancient Romans prepared lime as calcium oxide. It was not actually isolated until 1808 in England when Sir Humphry Davy electrolyzed a mixture of lime and mercuric oxide. Davy was trying to isolate calcium and when he heard that Berzelius and Pontin prepared calcium amalgam by electrolyzing lime in mercury, he tried it himself. He worked with electrolysis throughout his life and also discovered/isolated magnesium, strontium and barium.
Compounds
Calcium, combined with phosphate to form hydroxylapatite, is the mineral portion of human and animal bones and teeth. The mineral portion of some corals can also be transformed into hydroxylapatite.
Calcium oxide (lime) is used in many chemical refinery processes and is made by heating and carefully adding water to limestone. When lime is mixed with sand, it hardens into a mortar and is turned into plaster by carbon dioxide uptake. Mixed with other compounds, lime forms an important part of Portland cement.
When water percolates through limestone or other soluble carbonate rocks, it partially dissolves part of the rock and causes cave formation and characteristic stalactites and stalagmites and also forms hard water. Other important calcium compounds are nitrate, sulfide, chloride, carbide, cyanamide, and hypochlorite.
Isotopes
Calcium has four stable isotopes (40Ca and 42Ca through 44Ca), plus two more isotopes (46Ca and 48Ca) that have such long half-lives that for all practical purposes they can be considered stable. It also has a cosmogenic isotope, radioactive 41Ca, which has a half-life of 103,000 years. Unlike cosmogenic isotopes that are produced in the atmosphere, 41Ca is produced by neutron activation of 40Ca. Most of its production is in the upper metre or so of the soil column where the cosmogenic neutron flux is still sufficiently strong. 41Ca has received much attention in stellar studies because it decays to 41K, a critical indicator of solar-system anomalies.
97% of naturally occurring calcium is in the form of 40Ca. 40Ca is one of the daughter products of 40K decay, along with 40Ar. While K-Ar dating has been used extensively in the geological sciences, the prevalence of 40Ca in nature has impeded its use in dating. Techniques using mass spectrometry and a double spike isotope dilution have been used for K-Ca age dating.
Nutrition
Calcium is an important component of a healthy diet. A deficit can affect bone and tooth formation, while overretention can cause kidney stones. Vitamin D is needed to absorb calcium. Dairy products, such as milk and cheese, are a well-known source of calcium. However, some individuals are allergic to dairy products and even more people, particularly those of non-European descent, are lactose-intolerant, leaving them unable to consume dairy products. Fortunately, many other good sources of calcium exist. These include: seaweeds such as kelp, wakame and hijiki; nuts and seeds (like almonds and sesame); beans; amaranth; collard greens; okra; rutabaga; broccoli; kale; and fortified products such as orange juice and soy milk. Calcium has also been found to assist in the production of lymphatic fluids.
Calcium is essential for the normal growth and maintenance of bones and teeth, and calcium requirements must be met throughout life. Requirements are greatest during periods of growth, such as childhood, during pregnancy and when breast-feeding. Long-term calcium deficiency can lead to osteoporosis, in which the bone deteriorates and there is an increased risk of fractures. Adults need between 1,000 and 1,300 mg of calcium in their daily diet.
Recommended Adequate Intake by the IOM for Calcium:
Age------------------------Calcium (mg/day)
0 to 6 months--------------210
7 to 12 months-------------270
1 to 3 years---------------500
4 to 8 years---------------800
9 to 13 years-------------1300
14 to 18 years------------1300
19 to 50 years------------1000
51+ years-----------------1200
For more information about calcium in living nature, see calcium in biology and calcium metabolism.
Dietary calcium supplements
Calcium supplements are used to prevent and to treat calcium deficiencies. There are conflicting recommendations about when to take calcium supplements. However, most experts agree that no more than 500 mg should be taken at a time because the percent of calcium absorbed decreases as the amount of calcium in the supplement increases. It is recommended to spread doses throughout the day, with the last dose near bedtime. Recommended daily calcium intake varies from 1000 to 1500 mg, depending upon the stage of life.
In July 2006, a report citing research from Fred Hutchinson Cancer Research Centre in Seattle, Washington claimed that women in their 50's gained 5 pounds less in a period of 10 years by taking more than 500 mg of calcium supplements than those who did not. However, the doctor in charge of the study, Dr. Alejandro J. Gonzalez also noted it would be stretching it to suggest calcium supplements as a weight-limiting aid.
- Calcium carbonate is the most common and least expensive calcium supplement. It can be difficult to digest and causes gas in some people. Taking magnesium with it can help to prevent constipation. Calcium carbonate is 40% elemental calcium. 1000 mg will provide 400 mg of calcium. It is recommended to take this supplement with food to aid in absorption. In some calcium supplements based on calcium carbonate, vitamin D is added to aid in absorption. Vitamin D is needed for the absorption of calcium from the stomach and for the functioning of calcium in the body.
- Calcium citrate is more easily absorbed ( bioavailability is 2.5 times higher than calcium carbonate), easier to digest and less likely to cause constipation and gas than calcium carbonate. It also has a lower risk of contributing to the formation of kidney stones. Calcium citrate is about 21% elemental calcium. 1000 mg will provide 210 mg of calcium. It is more expensive than calcium carbonate and more of it must be taken to get the same amount of calcium.
- Calcium phosphate costs more than calcium carbonate, but less than calcium citrate. It is easily absorbed and is less likely to cause constipation and gas than either.
- Calcium lactate and calcium aspartate are both more easily digested, but more expensive than calcium carbonate