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(B) $1$. $	ext{Hydration enthalpy of } M^{+}$: As the size of the alkali metal ion increases down the group $(Li^{+} < Na^{+} < K^{+} < Rb^{+} < Cs^{

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Hydration enthalpy of $M^{+}$Ionization enthalpy of $M$Melting point of $M$decreasesdecreasesdecreases

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(B) $1$. $	ext{Hydration enthalpy of } M^{+}$: As the size of the alkali metal ion increases down the group $(Li^{+} $2$. $	ext{Ionization enthalpy of } M$: As the atomic size increases down the group,the outermost electron is further from the nucleus and more shielded,making it easier to remove. Thus,ionization enthalpy decreases.$3$. $	ext{Melting point of } M$: As the atomic size increases,the strength of the metallic bond decreases because the attraction between the nucleus and the delocalized electrons weakens. Therefore,the melting point decreases down the group.

The correct variation of the following properties of group $1$ elements $(M)$ ($Li$ to $Cs$) is:

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