s-Block ElementsHard
Question
Going down in II A group, following properties decrease :
Options
A.solubility of sulphates in H2O
B.hydration energy
C.thermal stability of carbonates
D.ionic radius in water.
Solution
(A) The sulphates of the alkaline earth metals are all white solid and stable to heat. BeSO4 and MgSO4 are readily soluble in water; the solubility decreases from CaSO4 to BaSO4. The greater hydration enthalpies of Be2+ and Mg2+ ions overcome the lattice enthalpy factor and therefore their sulphates are soluble in water.
(B) Hydration energy of alkaline earth metal ions decrease with increase in ionic size down the group and the order is, Be2+ > Mg2+ > Ca2+ > Sr2+ > Ba2+.
(C) The thermal stability of oxy-acid salts of alkaline earth metals generally increases down the group with increasing metallic character, i.e. electropositive character.
(D) Hydration energy of alkaline earth metal ions decrease with increase in ionic size down the group so the order of their ionic radius in water is, Be2+ < Mg2+ < Ca2+ < Sr2+ < Ba2+.
(B) Hydration energy of alkaline earth metal ions decrease with increase in ionic size down the group and the order is, Be2+ > Mg2+ > Ca2+ > Sr2+ > Ba2+.
(C) The thermal stability of oxy-acid salts of alkaline earth metals generally increases down the group with increasing metallic character, i.e. electropositive character.
(D) Hydration energy of alkaline earth metal ions decrease with increase in ionic size down the group so the order of their ionic radius in water is, Be2+ < Mg2+ < Ca2+ < Sr2+ < Ba2+.
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