Calcium
Calcium is the chemical element with atomic number 20; it has an atomic mass of 40.078 atomic mass units (amu). The chemical symbol for calcium is Ca. Calcium is a soft gray alkaline earth metal, and is the fifth most abundant element by mass in the Earth's crust; moreover, it is the fifth most abundant dissolved ion in seawater both in terms of number of atoms and mass, after sodium, chloride, Magnesium, and sulfate.[1]
Calcium an is essential nutrient for almost all living organisms, with vital roles in cellular metabolism, especially with regard to movement of the calcium ion Ca++ into and out of the cytoplasm functions as a signal for many cellular processes. As a chief component needed in mineralization of bones and shells, calcium is the most abundant metal by mass in a large number of faunal species, especially vertebrates, testudines and mollusca.
| Previous Element: Potassium Next Element: Scandium |
| |
| Physical Properties | ||
|---|---|---|
| Color | Silvery-white | |
| Phase at Room Temp. | solid | |
| Density (g/cm3) | 1.55 | |
| Hardness (Mohs) | 1.5 | |
|
Melting Point (K) |
1112.2 | |
|
Boiling Point (K) |
1767 | |
| Heat of Fusion (kJ/mol) | 9.3 | |
| Heat of Vaporization (kJ/mol) | 151 | |
| Heat of Atomization (kJ/mol) | 178 | |
| Thermal Conductivity (J/m sec K) | 201 | |
| Electrical Conductivity (1/mohm cm) | 255.754 | |
| Source | Calcite (oxide) | |
| Atomic Properties | ||
| Electron Configuration | [Ar]4s2 | |
|
Number of Isotopes |
22 (6 natural) | |
| Electron Affinity (kJ/mol) | --- | |
| First Ionization Energy (kJ/mol) | 589.8 | |
| Second Ionization Energy (kJ/mol) | 1145.4 | |
| Third Ionization Energy (kJ/mol) | 4911.8 | |
| Electronegativity | 1 | |
| Polarizability (Å3) | 22.8 | |
| Atomic Weight | 40.08 | |
| Atomic Volume (cm3/mol) | 25.9 | |
| Ionic Radius2- (pm) | --- | |
| Ionic Radius1- (pm) | --- | |
| Atomic Radius (pm) | 197 | |
| Ionic Radius1+ (pm) | --- | |
| Ionic Radius2+ (pm) | 114 | |
| Ionic Radius3+ (pm) | --- | |
| Common Oxidation Numbers | +2 | |
| Other Oxid. Numbers | --- | |
| Abundance | ||
| In Earth's Crust (mg/kg) | 4.15×104 | |
| In Earth's Ocean (mg/L) | 4.12×102 | |
| In Human Body (%) | 1.43% | |
| Regulatory / Health | ||
| CAS Number | 7440-70-2 | |
| OSHA Permissible Exposure Limit (PEL) | No limits | |
| OSHA PEL Vacated 1989 | No limits | |
|
NIOSH Recommended Exposure Limit (REL) |
No limits | |
|
Sources: |
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Contents
Natural occurrence
Elemental calcium is not abundant in the biotic environment on Earth. As a solid calcium occurs chiefly in coral reefs, sedimentary rock, especially in limestone and in the specific minerals calcite, dolomite and gypsum. Some of the most dramatic occurrences are in limestones, where stalactites and stalagmites are formed in underground caverns under favorable conditions of pH, temperature and ionic concentration of calcium. Calcium is additionally found in certain igneous and metamorphic rocks: principally in the silicates:[2] plagioclase, amphiboles, pyroxenes, garnet and some serpentine rocks. In addition to terrestrial mining, certain countries routine mine coral reefs for construction materials; China is the largest such nation that mines corals. This practise is obviously quite deleterious to coral reefs.(Kimura et al, 2008) as reportedby the Global Coral Reef Monitoring Network and Reef and Rainforest Research Center, Australia.
Biogeochemical cycles u
Calcium is a key link between tectonics, climate and the carbon cycle. Since mountain block uplift exposes calcium bearing strata to chemical weathering, significant release occurs of Ca++ into surface waters. Much of this dissolved calcium ultimately is transported tothe oceans, where it reacts with dissolved carbon ioxide to produce limestone. Certain quantities of this limestone precipitates to the sea floor where it is incorporated into new rock strata. Dissolved carbon dioxide, together with carbonate and bicarbonate ions, are termed dissolved inorganic carbon.
The actual reaction is more complex, involving bicarbonate ion (HCO3-), which is produced when carbon dioxide ionizes in pH levels found in oceans.
Ca++ + 2 HCO3- → CaCO3 (limestone) + CO2 + H2O
Note that at pH levels of the oceans, most of the CO2 produced in this reaction is immediately converted back into HCO3-. The reaction thus results in a net transport ofcarbon dioxide from the ocean or atmosphere into the lithosphere.[3] This cycling is a significant sink for carbon dioxide, and provides an important negative feedback loop for carbon dioxide additions to the atmosphere, and thus a key mitigation measure to potential global warming.
Isotopes
There are four stable calcium isotopes (40Ca, 42Ca, 43Ca, 44Ca); in addition,[4] 46Ca and 48Ca are radioactive, but possess extremely long half-lives. Furthermore radioactive 41Ca also is produced in the uppermost meter of the Earth crust by neutron activation of 40Ca; moreover, 41Cahas the long half-life of 103,000 years. 41Ca is received much attention in stellar studies because it decays to 41K, a critical indicator of solar-system anomalies.
Ninety seven percent of naturally occurring calcium is in the form of 40Ca, which is one of the daughter products of 40K decay, along with the daughter 40Ar. While potassium-argon dating has been widely employed extensively in the earth sciences field, the utility of this dating technique is limited due to the minute quantities of argon gas that are required to be measured; in practical terms the technique is useful where long geological time scales are involved (e.g. the order of 100,000 years);[5] moreover, as measurement techniques steadily improve, the utility is rising.
Notable properties
Calcium possesses the lightest density of all the alkali earth metals. It is chemically reactive and is so soft that it can be cut with a knife, although it is somewhat harder than lead. As a metal it is silvery in appearance; to produce the metallic form, one usually utilizes electrolysis upon a fused salt like calcium chloride. When exposed to the air in its metallic form, a coating is quickly formed as a whitish gray oxide and nitride coating. Unlike Magnesium, it is difficult to ignite; however, upon combustion it manifests a brilliant brick-red high intensity luminence. As a metal, calcium reacts with water, rapidly producing hydrogen gas, but exuding little heat. If the metal has been powdered, the reaction with water is more robust,due to theconsiderablygreater surface area.
Calcium has a higher electrical resistivity than copper or aluminium. Calcium actually has an electrical conductivity about forty percent that of copper; however, its conductivity under normal atmospheric conditions is usually limited by its chemical reactivity with air.
Ionic solutions of calcium salts are generally colorless. Many calcium salts are not soluble in water. When in solution, the calcium ion to the human taste varies with its anion, being reported variously as moderately salty, sour or mineral like. It has been demonstrated that many fauna can taste calcium, and use this sense to detect the mineral in salt licks.[6]
Example compounds
Calcium phosphate leads to the formation of calcium hydroxylapatite, the mineral portion of human and animal bones and dentin.[6] The mineral portion of some corals can also be transformed into hydroxylapatite.
Calcium hydroxide (slaked lime), employed in numerous chemical refinery processes, is produced from applying heat to limestone at temperatures above 825 °C, following by hydration. When lime is mixed with sand, it hardens into a mortar and is converted into plaster after carbon dioxide uptake. Mixed with other compounds, lime forms an component of Portland cement. Calcium carbonate, one of the common compounds of calcium, can be heated to form quicklime (CaO). After hydration, quicklime is converted to slaked lime (Ca(OH)2), which is a cheap commodity utilized widely in the chemical manufacturing industry.[7] Chalk and marble are other alternative forms of calcium carbonate; chalk is a commonly occurring natural substance, notably in western Europe at places like the cliffs of Dover and in the Orkney Islands, Scotland.
Other notable calcium compounds are calcium sulfate, calcium chloride, calcium sulfide, calcium carbide and calcium hypochlorite.
Faunal metabolism
Calcium is the most abundant mineral not only in the human body but for many other faunal species. A human adult body has about one kilogram of calcium, 99 percent of which is stored in bones as calcium phosphate. Human extracellular fluid holds around 22.5 mmol, almost half of which is within blood plasma. About 500 mmol of calcium is exchanged between bone and the extracellular fluid within a complete daily cycle.[8] Hypocalcaemia in humans is the condition of deficient calcium concentration in blood plasma; this deficit circumstance is one in which less than 90 milligramsl/liter or ionized calcium concentration less than 45 milligrams/liter). This condition is an electrolyte imbalance that can lead to osteoporosis;[9] it is important to note that it is the ionized calcium which is key to metabolic regulation. Conversely, elevated blood calcium levels, known as hypercalcaemia, can lead to adverse health effects including heart arhythmia, depression and peptic ulcers.
Hypocalcaemia is also studied in depth for dairy cows, other domestic animals and fauna in the wild. In the case of dairy cows the condition is linked to inferior milk production and other disease issues.[10]
Citation
C. Michael Hogan (2013). Calcium. Retrieved from http://editors.eol.org/eoearth/wiki/calcium
== References ==- ↑ A.G.Dickson and C. Goyet. 1994. Handbook of method for the analysis of the various parameters of the carbon dioxide system in sea water. Publisher: ORNL/CDIAC
- ↑ Harvey Blatt, Robert J.Tracy and Brent E.Owens. 2006. Petrology: igneous, sedimentary, and metamorphic. Macmillan. 530 pages
- ↑ Richard Zeebe. 2006. [[Marine carbonate chemistry. National Council for Science and the Environment]]
- ↑ H.G. Attendorn and Robert Bowen. 1998. Isotopes in the Earth Sciences, Springer. 668 pages
- ↑ Kevin Greene. 1996. Archaeology, an introduction: the history, principles, and methods. Routledge. 208 pages
- ↑ M.G.Tordoff. 2001. Calcium: Taste, Intake, and Appetite. Physiological Reviews. vol. 81, issue 4, page 1567
- ↑ Joon Bu Park and Roderic S. Lakes. 2007. Biomaterials: an introduction, Springer. 561 pages
- ↑ W.J.Marshall. 1995. Clinical Chemistry, third edition. Mosby Publishers, London.UK
- ↑ Maurice Edward Shils and Moshe Shike. 2006. Modern nutrition in health and disease. Lippincott Williams & Wilkins. 2069 pages
- ↑ U.S. National Research Council, Subcommittee on Dairy Cattle Nutrition. 2001. Nutrient requirements of dairy cattle. National Academies Press. 381 pages
