S Block Elements

Analysis of Statement-I: Both BeSO4 and MgSO4 are readily soluble in water.
The solubility of sulfates of alkaline earth metals generally decreases down the group.
BeSO4 (Beryllium sulfate) is readily soluble in water. This is due to the very small size of the Be2+ ion, which leads to very high hydration energy. This high hydration energy more than compensates for the relatively high lattice energy, making it highly soluble.
MgSO4 (Magnesium sulfate, commonly known as Epsom salt) is also readily soluble in water. Similar to beryllium, the Mg2+ ion is relatively small, leading to significant hydration energy.
In contrast, CaSO4 (Calcium sulfate) is sparingly soluble, and SrSO4 (Strontium sulfate) and BaSO4 (Barium sulfate) are practically insoluble.
Therefore, Statement - I is correct.
Analysis of Statement - II: Among the nitrates of alkaline earth metals, only Be(NO3)2 on strong heating gives its oxide, NO2 and O2.
Alkaline earth metal nitrates decompose on strong heating to give the metal oxide, nitrogen dioxide ( NO2 ), and oxygen (O2). The general reaction is:
2M(NO3)2(s)

‌ heat ‌

‌───────▶‌

2MO(s)+4NO2(g)+O2(g)
This decomposition pattern is observed for all alkaline earth metal nitrates.
‌Be(NO3)2

‌ heat ‌

‌───────▶‌

BeO+2NO2+‌

1

2

O2
‌Mg(NO3)2

‌ heat ‌

‌───────▶‌

MgO+2NO2+‌

1

2

O2
‌Ca(NO3)2

‌ heat ‌

‌───────▶‌

CaO+2NO2+‌

1

2

O2
And similarly for Sr(NO3)2 and Ba(NO3)2.
The thermal stability of these nitrates generally increases down the group (Be(NO3)2. is the least stable, and Ba(NO3)2 is the most stable), meaning they decompose at different temperatures, but the decomposition products are the same for all of them.
The statement claims that "only Be(NO3)2 " decomposes in this manner, which is incorrect as all alkaline earth metal nitrates follow this decomposition pathway.
Therefore, Statement - II is not correct.
Conclusion:
Statement - I is correct.
Statement - II is not correct.
This matches option B.