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(D) $1$. Solubility of alkaline earth metal hydroxides increases down the group due to the decrease in lattice energy being more significant than the

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All are correct

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(D) $1$. Solubility of alkaline earth metal hydroxides increases down the group due to the decrease in lattice energy being more significant than the decrease in hydration energy. Thus,$Be(OH)_2 $2$. Thermal stability of alkali metal hydroxides increases down the group as the electropositive character increases,making the $M-OH$ bond stronger. Thus,$LiOH $3$. Magnetic moment depends on the number of unpaired electrons. For $O_2$ (bond order $2$),the configuration is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$,having $2$ unpaired electrons. For $O_2^-$ (bond order $1.5$),the configuration has $1$ unpaired electron. Since $2 > 1$,the magnetic moment of $O_2 > O_2^-$ is correct.Therefore,all statements are correct.

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