|Appearance||dull gray, silver; with a pale yellow tint|
|Standard atomic weight (Ar, standard)||40.078(4)|
|Calcium in the periodic table|
|Atomic number (Z)||20|
|Group||group 2 (alkaline earth metals)|
|Element category||alkaline earth metal|
|Electron configuration||[Ar] 4s2|
Electrons per shell
|2, 8, 8, 2|
|Phase at STP||solid|
|Melting point||1115 K (842 °C, 1548 °F)|
|Boiling point||1757 K (1484 °C, 2703 °F)|
|Density (near r.t.)||1.55 g/cm3|
|when liquid (at m.p.)||1.378 g/cm3|
|Heat of fusion||8.54 kJ/mol|
|Heat of vaporization||154.7 kJ/mol|
|Molar heat capacity||25.929 J/(mol·K)|
|Oxidation states||+1, +2 (a strongly basic oxide)|
|Electronegativity||Pauling scale: 1.00|
|Atomic radius||empirical: 197 pm|
|Covalent radius||176±10 pm|
|Van der Waals radius||231 pm|
|Spectral lines of calcium|
|Crystal structure||face-centered cubic (fcc)|
|Speed of sound thin rod||3810 m/s (at 20 °C)|
|Thermal expansion||22.3 µm/(m·K) (at 25 °C)|
|Thermal conductivity||201 W/(m·K)|
|Electrical resistivity||33.6 nΩ·m (at 20 °C)|
|Magnetic susceptibility||+40.0·10−6 cm3/mol|
|Young's modulus||20 GPa|
|Shear modulus||7.4 GPa|
|Bulk modulus||17 GPa|
|Brinell hardness||170–416 MPa|
|Discovery and first isolation||Humphry Davy (1808)|
|Main isotopes of calcium|
Calcium is a chemical element. Its symbol on the periodic table (a list of all the elements) is Ca. Its atomic number is 20. (The atomic number says where Calcium sits in the periodic table.) It has 20 protons and 20 electrons (if is an atom, see ion). The most common isotopes are Ca-40 and Ca-44. Its mass number is about 40.08. Calcium is very important in the human body, for making bones and for other purposes.
Properties[change | change source]
Physical properties[change | change source]
Calcium is a soft white-gray metal. It is a solid and is opaque. It is an alkaline earth metal. Its melting point is hotter than most other reactive metals. It is a little harder than lead. It has two allotropes. It does not conduct electricity as well as copper, but is much lighter in weight.
Chemical properties[change | change source]
It reacts with water to produce hydrogen and calcium hydroxide. It reacts with water very fast when it is powdered. When it is in a chunk, it starts reacting slowly because calcium hydroxide makes a coating that does not dissolve on the calcium. If a little acid is added to calcium hydroxide, it dissolves it, making the calcium react very fast. It burns when powdered to make a reddish flame. This makes calcium oxide. It also makes calcium nitride when heated. It can react with halogens to make calcium halides like calcium chloride with chlorine.
Calcium compounds[change | change source]
Calcium forms chemical compounds in the +2 oxidation state. Calcium compounds are colorless. Most calcium compounds are not toxic. They are needed in the human body, actually. They are unreactive as far as calcium ions go. Calcium oxide was used to make limelights, which have a flame heating calcium oxide and makes it glow very bright.
- Calcium bromate
- Calcium carbonate
- Calcium chloride
- Calcium hydroxide
- Calcium nitrate
- Calcium nitride
- Calcium oxide
- Calcium permanganate
- Calcium phosphate
- Dicalcium phosphate
- Monocalcium phosphate
Occurrence[change | change source]
In the ground[change | change source]
Calcium in cells[change | change source]
It is important to know how cells work. Many cells have calcium channels on their surface. These are openings where calcium ions can enter the cell. The cell is told to act and it opens the channels. Once in the cell calcium ions activates many proteins to do specific things. For example, when it goes into muscle cells, it makes them contract (shorten so the muscle pulls.) When it goes into nerve cells, it triggers electrical impulses that send a messages. When it goes into white blood cells it makes them fight germs.
Calcium ions are important to cells, but too many calcium ions can be bad. If a cell gets more calcium ion than it needs it can die. This is why the amount of calcium ion in cells is highly regulated. Conversely, not enough calcium ion is bad. Cells must have the right amount to function properly.
Sometimes cells are unhealthy and need to die in for the body to replace them with new, healthy cells. This keeps the whole organism healthy. Cells know when they should die and can trigger reactions to end their life cycles in many ways. When this happens it is called apoptosis, also known as a 'programmed cell death' (planned cell death.) One way cells accomplish apoptosis by taking in toxic levels of calcium ions.
Calcium is very important for the human body.
Calcium storage[change | change source]
Calcium as an element is not found in the human body, just calcium ions in the form of chemical compounds.
Calcium regulation[change | change source]
Organisms need to keep calcium ion levels very well controlled. High calcium levels are bad, and low calcium levels are bad.
The body controls this by changing
- how much calcium we get from the food we eat
- how much calcium we lose in urine
- how much calcium is put in bones
The body controls calcium levels with many hormones. Calcitonin, Parathyroid hormone (acronym PTH), and Vitamin D are the most important hormones in calcium metabolism. (Vitamin D works as a hormone but it is called a vitamin.)
Preparation[change | change source]
Uses[change | change source]
As an element[change | change source]
Calcium is used in the reduction of other metals. It can also be used to make alloys with other metals.
As chemical compounds[change | change source]
Calcium is part of calcium oxide. Calcium oxide is used to make paper, pottery, food, and to purify water (make it good to drink.) Calcium carbonate is used as a calcium supplement. Calcium permanganate can be used as a rocket propellant.
Safety[change | change source]
Calcium is toxic as an element. It reacts with water and makes a strong base, calcium hydroxide. Calcium compounds are not toxic unless the anion is toxic. Calcium permanganate is only toxic because of the permanganate, not the calcium. Like other alkaline earth metals calcium burns easily and brightly.
Related pages[change | change source]
Sources[change | change source]
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 112. ISBN 0-08-037941-9.
- Meija, J.; Coplen, T. B.; Berglund, M.; Brand, W.A.; De Bièvre, P.; Gröning, M.; Holden, N.E.; Irrgeher, J. et al. (2016). "Atomic weights of the elements 2013 (IUPAC Technical Report)". Pure and Applied Chemistry 88 (3): 265-91. doi:10.1515/pac-2015-0305. https://www.degruyter.com/downloadpdf/j/pac.2016.88.issue-3/pac-2015-0305/pac-2015-0305.xml.
- Krieck, Sven; Görls, Helmar; Westerhausen, Matthias (2010). "Mechanistic Elucidation of the Formation of the Inverse Ca(I) Sandwich Complex [(thf)3Ca(μ-C6H3-1,3,5-Ph3)Ca(thf)3] and Stability of Aryl-Substituted Phenylcalcium Complexes". Journal of the American Chemical Society 132 (35): 12492–12501. doi:10.1021/ja105534w. PMID 20718434.
- Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
- "Calcium: the essentials". WebElements. Retrieved 7 February 2016.
Other websites[change | change source]
- Calcium -Citizendium