Question

Is $ Ca $ metal or nonmetal?

Answer 1

Hint: The chemical element with the symbol $ Ca $ , atomic number $ 20 $ , as an alkaline earth metal, it is the fifth element and the third most abundant metal in the earth’s crust. Its atomic mass is $ 40 $ . The metal is trimorphic, harder than sodium, but softer than aluminum.

Complete answer:
Calcium is considered as a metal because it is more likely to give away its two valence electrons in the outermost shell in order to reach the configuration of Argon. It has the second lowest ionization energy in its periodic table and it is quite reactive at standard temperature and pressure. Calcium does not occur naturally in the Free State, but compounds of the elements are widely distributed.
Calcium is a very ductile silvery metal whose properties are very similar to the heavier elements in the group, strontium, barium, and radium. A calcium has twenty electrons, arranged in the electronic configuration $ [Ar]4{s^2} $ . Calcium metal melts at $ 842^\circ $ C and boils at $ 1494^\circ $ C, these values are higher than magnesium and strontium. Its density is $ 1.55g/c{m^3} $ is the lowest in its group. $ Ca{(OH)_2} + C{O_2} \to CaC{O_3} + {H_2}O $
Calcium is used as a reducing and alloying agent for metal. It is used primarily in the creation of steel to improve the steel’s mechanical properties. Calcium is used to create lime which is used as a building material, paints, concrete, cement and plaster. Calcium compounds (such as calcium carbonate or calcium magnesium pills) are often used as calcium supplements for human consumption. Calcium carbonate is used as an antacid for indigestion.
Reactions:
Reactions of calcium with halides. Calcium forms salts with halides. They have a variety of uses, but the most commonly used to chemistry students is the use of calcium chloride as a drying agent.
  $ CaC{l_2} + 2{H_2}O(l) \to CaC{l_2}.2{H_2}O $
Reaction of calcium with carbonates. Calcium carbonate is important in the formation of cave stalactites. This reaction allows calcium carbonate to be dissolved into solution as calcium bicarbonate.
 $ CaC{O_3}(s) + C{O_2}(l) + {H_2}O(l) \to Ca{(HC{O_3})_2} $
Reaction of calcium with water. Calcium metal is fairly reactive and combines with water at room temperature to produce hydrogen gas and calcium hydroxide.
 $ Ca(s) + 2{H_2}O(g) \to Ca{(OH)_2}(aq) + {H_2}(g) $
Reaction of calcium with acid. Calcium dissolves in acid to form dissociated ions of $ Ca $ and $ Cl $ along with hydrogen gas.
 $ Ca(s) + 2HCl(aq) \to C{a^{2 + }}(aq) + 2C{l^ - }(aq) + {H_2}(g) $
Reaction of calcium with oxygen. Calcium metal slowly oxidizes in air, becoming encrusted with white $ CaO $ and $ CaC{O_3} $ , which protect from attack by air. When ignited, calcium burns to give calcium oxide.
 $ 2Ca(s) + {O_2}(g) \to 2CaO(s) $

Note:
Calcium carbonate, in moderate amounts, can also be used as an antacid or a calcium supplement. Calcium nitrate is also a common fertilizer. Pure $ CaC{O_3} $ can be extracted from limestone in a series of three reaction:
 $ \bullet $ Calcination: $ CaC{O_3} \to CaO + C{O_2} $
 $ \bullet $ Slaking: $ CaO + {H_2}O \to Ca{(OH)_2} $
 $ \bullet $ Carbonation: $ Ca{(OH)_2} + C{O_2} \to CaC{O_3} + {H_2}O $