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WEEK 6
TOPIC: METALS AND THEIR COMPONDS
CONTENTS:
- Calcium- extraction of calcium,
- Properties of calcium.
- Compounds of calcium and their uses.
PERIOD 1: CALCIUM
Calcium is too reactive to occur as free metals in nature. Instead, it occurs abundantly in the state as Calcium trioxocabonate (iv) (CaCO3), in limestone marble, chalk, aragonite, calcite and coral; as calciumtetraoxosulphate (vi) (CaSO4) in gympsum and anhydrite, as double trioxocarbonate (iv) CaCO3. MgCO3. In dolomite; as calcium fluoride CaF2, in fluorspar and as various trioxosilicates (iv). Bones and teeth contain calcium tetraoxo-sulphate (v).
Extraction of calcium
Since calcium compounds are very stable, metallic calcium is commonly extracted electronically from fused calcium chloride, a fluoride is usually added to the fused calcium chloride to lower the melting point from 850oC to about 650oC. The mixture is place in a crucible, lined on the inside with graphite which serves as the anode of the cell. The cathode consists of an iron rod which just touches the surface of the electrolyte. As electrolysis proceeds, metallic calcium collects on the cathode which is gradually reused so that an irregular of calcium is formed on it.
Chlorine is liberated at the anode.
Chemistry of the reaction: Fused calcium chloride consists of calcium and chloride ions.
At the cathode: the calcium ions receive two electrons each to become reduced to the metal.
Ca2+ + 2e– → Ca [Reduction]
At the anode: Two chloride ions give up an electron each to become atomic chlorine. The two atoms the combine to become liberated as a gaseous molecule
Cl– → Cl + e– (oxidation)
Cl + Cl → Cl2
Overall electrolytic reaction:
Ca2+(l) + 2Cl– → Ca(s) + Cl2(g)
PERIOD 2: PHYSICAL PROPERTIES
Appearance | Silv Silvery-grey solid |
Relative density | 1.55 |
Malleability and ductility | Malleable and ductile |
Tensile strength | Relatively low tensile strength |
Melting point | 85.10C |
Conductivity | Good conductor of heat and electricity. |
CHEMICAL PROPERTIES
Reaction with air: calcium is a very electropositive and reactive metal. On exposure to air, it rapidly tarnishes and loses its metallic lustre due to the formation of a white film of calcium oxide or quick lime on the surface of the metal. In the presence of atmospheric moisture and carbon (IV) oxide, some calcium hydroxide and calcium-trioxocarbonate (IV) may also be formed.
When calcium is heated in air, it burns with a brick-red flame calcium oxide.
2Ca(s) + O(g) → 2Ca(s)
TEST FOR CALCIUM IONS
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