Which of the following statement (s) is/are correct for group II metals 

The lattice energy and hydration energy deo·ease down the group

$Be{F}_2$ has a high hydration energy whereas salts

${\mathrm{MgF}}_2,{\mathrm{CaF}}_2,{\mathrm{SrF}}_2$ and $Ba{F}_2$ are insoluble because for these, the hydration energy is not able to compensate the lattice energy.

$BeC{l}_2$ is covalent hence insoluble in water. While ${\mathrm{MgCl}}_2,{\mathrm{CaCl}}_2,{\mathrm{SrCl}}_2$ and $BaC{l}_2$ are ionic and are soluble in water though their solubility decreases down the group. 

$BeS{O}_4$ is soluble due to the high hydration energy of 

$B{e}^{2+}$ whereas hydration energy decreases down the group and the hydration energy is not able to compensate for the high lattice energy.