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Element, Properties, Uses, Compounds

Calcium Element Information

Calcium (Ca) is the chemical element or alkaline-earth metal of Group-2 (IIA) of the periodic table. It is the essential element in the human body to building bones, to clothing blood, to contract the muscle, to beating our heart. About 90 percent of the calcium in the human body used to make our bones and teeth. Calcium is silvery-white, lustrous, and relatively hard metal than the alkali metals. The electronic configuration of calcium suggests that the metal has two s-electron available for chemical bonding.

Calcium, alkaline earth metal position on the periodic table elements

Calcium forms a face-centered cubic crystal lattice with a higher melting point than alkali metals. It posses a 4s2 valence shell electronic configuration over the previous noble gas argon. The s2 configuration leads to inclusion in Group-2 or IIA of the periodic table. Some important properties of the metal are given below the table.

Calcium element chemical symbol and periodic table properties

Properties of Calcium
Atomic number 20
Atomic weight 40.078
Electronic Configuration [Ar] 4s2
Melting point 842 °C, ​1548 °F
Boiling point 1484 °C, ​2703 °F
Density 1.55 g/cm3
Oxidation number or states +2
Ionization energy 1st – 589.8 kJ/mol
2nd – 1145.4 kJ/mol
3rd – 4912.4 kJ/mol

Occurrence and Production

Calcium is the fifth most abundant element (3.63 percent) in the earth’s crust. It is concentrated in minerals that are probably separated during the main stage of crystallization of magma. Weathering and leaching lead to the formation of minerals calcium carbonate (CaCO3) or limestone in earth soil. The very low solubility of CaCO3 is the most probable reason for the absence of a significant amount of Ca+2 ion in sea-water. Gypsum (CaSO4, 2H2O), fluorspar (CaF2) and apatite [3Ca3(PO4)2, CaF2] are important minerals of calcium.

Naturally, occurring calcium is a mixture of five stable isotopes like 40Ca, 42Ca, 43Ca, 44Ca, and 46Ca. The radioactive isotope 48Ca (half-life of about 4.3 × 1019 years) can be considered stable. It is the first lightest element that contains six naturally occurring isotopes.

Every day we lose calcium from our body through our skin, nails, hair, sweat, urine, and feces, but our body cannot produce it. Therefore, we need to eating Ca reached foods or vegetables that sustain the deficiency of calcium for our body. Dairy products (milk, yogurt, cheese) and vegetables like green leaf, beans, broccoli, brussels sprouts, collards, kale, mustard greens, etc are the sources of calcium for our daily requirements.

Calcium is produced on a commercial scale by electrolysis of fused CaCl2. Some fluorspar (CaF2) was added due to lowering the temperature for fusion. The electrolysis is carried out in a graphite pot serving as an electrode or anode. A water-cooled iron cathode hangs into the fused electrolyte. The produced metal is deposited on the cathode in the form of a rod when the electrolysis proceeds. A layer of fused electrolyte protects the metal from oxidation.

Chemical Properties and Compounds

Grup-2 elements of the periodic table are characterized by two valence electrons in an s-shell of the atoms. These two electrons are always involved together to show uniform bivalency of the metal. The properties of elements like calcium, strontium, barium, radium and their compounds are systematically and gradually changed with the increasing atomic number. Electropositive or metallic character and ionic radius increase from calcium to radium. Thermal stabilities of carbonates, nitrate, sulfates are also increased from Ca to Ra.


Calcium hydride is formed by ionic bonding due to the high electropositive character and large size of the metal. CaH2 is a high meting crystalline solid, conducting electricity in a fused state and liberate hydrogen on electrolysis. The hydride is obtained by the direct combination of hydrogen with the metal. The reaction of CaH2 with water provides a ready source of hydrogen.


All the oxides of Grup-2 elements are ionic with a high melting point but beryllium oxide is formed by covalent bonding. The tendency to form peroxide and superoxide increases with the increasing atomic number of the Group-2 elements. Calcium superoxide is formed by the reaction of metal peroxide with 30 percent hydrogen peroxide.  The oxides react with water to form hydroxides and the basic properties of Group-2 hydroxides increase from beryllium to barium.


All the crystalline halides of calcium are ionic in nature with a high melting point. CaF2 is a high meting (melting point 1418 °C) water-insoluble solid while the chloride is lower meting and water-soluble. The bromide and iodide have still lower meting and higher soluble in water and alcohol.

Uses of Calcium

Due to a strong chemical affinity for oxygen and sulfur, metallic calcium is widely used for making steel. It is an important reducing agent for the production of chromium, zirconium, thorium, and uranium. It is used as a scavenger in the steel industry to remove oxygen, sulfur, and phosphorus. Calcium is used in aluminum alloying to improve the strength of metal, to remove the nitrogen from argon, to manufacture hydrolith (CaH2).

About 90 percent of the metal in the human body used to make our bones and teeth. Metallic calcium not only plays a major structural role but also plays crucial regulatory functions like muscle construction, nerve transmission, and blood coagulation. The deficiency of calcium in the human body causes hypocalcemia, rickets, osteoporosis.