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Why is Li2CO3decomposed at a lower temperature whereas Na2CO3at higher temperature?

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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...
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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.

Therefore, lithium carbonate decomposes at a low temperature while a stable sodium carbonate decomposes at a high temperature.

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Lattice energy and extent of polarization get higher as the ion becomes smaller. Lithium has a smaller size than sodium, so lithium polarizes the carbonate ion at a greater area which takes less energy to decomposed, while sodium requires more energy which makes it more stable.
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Find the oxidation state of sodium in Na2O2.
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