Answer:
The \[L{{i}^{+}}\]on being smaller in
size exerts a strong polarising action and distorts the electron cloud of the nearby
oxygen atoms of the large sized \[CO_{3}^{2-}\]ion. It results in weakening of
the C-O bond and strengthening of Li-O bond. This ultimately facilitates the
decomposition of \[L{{i}_{2}}C{{O}_{3}}\] into \[L{{i}_{2}}O\] and\[C{{O}_{2}}\]
at lower temperature. The lattice energy of \[L{{i}_{2}}O\]is higher than the
lattice energy of\[L{{i}_{2}}C{{O}_{3}}\]. This also favours the decomposition
of\[L{{i}_{2}}C{{O}_{3}}\]. \[N{{a}^{+}}\]ion being bigger in size is not
capable of exerting polarizing action on oxygen atoms of carbonate ions. Thus,\[N{{a}_{2}}C{{O}_{3}}\]is
a stable compound.
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