Why is the enthalpy change of hydration always exothermic?

Write equation to represent the hydration of a sodium ion.

Write equation to represent the hydration of a chloride ion.

Draw diagram to show four water molecules hydrating a magnesium ion. Show the dipole on each water molecule.

Draw diagram to show two water molecules hydrating a bromide ion. Show the dipole on each water molecule.

Explain why the value of $∆{\mathrm{H}}_{\mathrm{hyd}}^{⊝}$ for magnesium ions is much more exothermic than $∆{\mathrm{H}}_{\mathrm{hyd}}^{⊝}$ for potassium ions.

Name the change associated with the equation below:

$\mathrm{KBr}\left(\mathrm{s}\right) + \mathrm{aq} \to \mathrm{KBr}\left(\mathrm{aq}\right)$ (for $1 \mathrm{mole}$ of $\mathrm{KBr}$)

Name the change associated with the equation below:

${\mathrm{K}}^{+}\left(\mathrm{g}\right) + \mathrm{aq}\to {\mathrm{K}}^{+} \left(\mathrm{aq}\right)$ (for $1 \mathrm{mole}$ of ${\mathrm{K}}^{+}$ ions)

Name the change associated with the equation below:

${\mathrm{K}}^{+} \left(\mathrm{g}\right) + {\mathrm{Br}}^{-} \left(\mathrm{g}\right) \to \mathrm{KBr}\left(\mathrm{s}\right)$ (for $1 \mathrm{mole}$ of $\mathrm{KBr}$)