Arrange the following sulphates of alkaline earth metals in order of decreasing thermal stability :

$B e S O_{4}, M g S O_{4}, C a S O_{4}, S r S O_{4}$

B e S O_{4} > M g S O_{4} > C a S O_{4} > S r S O_{4}

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S r S O_{4} > M g S O_{4} > C a S O_{4} > B e S O_{4}

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S r S O_{4} > C a S O_{4} > M g S O_{4} > B e S O_{4}

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S r S O_{4} > C a S O_{4} > B e S O_{4} > M g S O_{4}

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Solution

The correct option is C $S r S O_{4} > C a S O_{4} > M g S O_{4} > B e S O_{4}$
Sulphates decompose on heating to give the corresponding oxide. $M g S O_{4} Δ \to M g O + S O_{2} + \frac{1}{2} O_{2}$
The stability increases as the basic nature of the metal increases. This is clear from the increasing decomposition temperatures down the group. $S r S O_{4} > C a S O_{4} > M g S O_{4} > B e S O_{4}$ .
Hence option C is correct.

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B e S O_{4}, M g S O_{4}, C a S O_{4}, S r S O_{4}, B a S O_{4}

B e S O_{4}, M g S O_{4}, C a S O_{4}

Why are $B e S O_{4} a n d M g S O_{4}$ readily solubel in water whle $C a S O_{4}, S r S O_{4}$ are insoluble?

B e S O_{4}

M g S O_{4}

C a S O_{4}

H_{2} O ?

(1) B e S O_{4} > M g S O_{4} > C a S O_{4} > B a S O_{4}

(2) B e (O H)_{2} > M g (O H)_{2} > C a (O H)_{2} > B a (O H)_{2}

(3) L i O H < N a O H < K O H < R b O H

(4) L i_{2} C O_{3} < N a_{2} C O_{3} < K_{2} C O_{3} < R b_{2} C O_{3}

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