"Of the alkali metal carbonates, only $L i_{2} C O_{3}$ decomposes to give $C O_{2}$ and metal oxide."
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Solution

Of the alkali metal carbonates, only $L i_{2} C O_{3}$ decomposes to give $C O_{2}$ and metal oxide.
As we move down the alkali metal group, the electropositive character increases. This causes an increase in the stability of alkali carbonates. However, lithium carbonate is not so stable to heat.
This is because lithium carbonate is covalent. Lithium ion, being very small in size, polarizes a large carbonate ion, leading to the formation of more stable lithium oxide.
$L i_{2} C O_{3} (on heating) ⟶ L i_{2} O + C O_{2}$
Therefore, lithium carbonate decomposes at a low temperature while a stable other alkali carbonate decomposes at a high temperature.

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