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Group 2 Alkaline earth metals
The elements of group II are known as the alkali earth metals.
All of these elements are reactive metals. Magnesium and calcium are abundant in the earth's crust. The
others are relatively rare.
The physical properties of the elements
Melting points and electrical conductivity:

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(b) Reactions with chlorine
All the group 2 metals react when heated in chlorine to form solid ionic chlorides.
Magnesium for example:
Mg(s) + Cl2(g) MgCl2(s)

(c) Reactions with water
Be does not react with water or steam.
Magnesium burns when heated in steam to form magnesium oxide and hydrogen.…

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Ba2+(aq) + SO42(aq) BaSO4(s) thick white precipitate formed
Sr2+(aq) + SO42(aq) SrSO4(s) thick white precipitate formed
Ca2+(aq) + SO42(aq) CaSO4(s) faint white precipitate formed
If dilute sulphuric acid or sodium sulphate is added to a solution of Mg2+ or Be2+, there is no reaction
and no precipitate is formed.

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The decomposition is a result of the polarising power of the cation.
As polarising power of the cation increases, compounds become more covalent in character and less
stable to heat.
Going down the group the cations become larger charge remains the same , so their polaring power
The smallest…


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