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The order of decreasing ionisation enthalpy in alkali metals is
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$\mathrm{Li}>\mathrm{Na}>\mathrm{K}>\mathrm{Rb}$
$\mathrm{Li}>\mathrm{Na}>\mathrm{K}>\mathrm{Rb}$
On moving down the group from Li to Rb, increased atomic radii makes the removal of electron easier. Thus, the order of decreasing ionization enthalpy will be: $\mathrm{Li}>\mathrm{Na}>\mathrm{K}>\mathrm{Rb}$
Also, LiF exhibit very high lattice energy.
Also, LiF exhibit very high lattice energy.
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