Question:
What are the products formed when \(\text{Li}_2\text{CO}_3\) undergoes decomposition?
What are the products formed when \(\text{Li}_2\text{CO}_3\) undergoes decomposition?
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Among alkali metals, only lithium carbonate decomposes easily on heating due to high polarizing power.
Updated On: Apr 26, 2026
- \(\text{Li}_2\text{O} + \text{CO}_2\)
- \(\text{LiO} + \text{CO}_2\)
- \(\text{LiC} + \text{CO}_2\)
- \(\text{Li}_2\text{O}_2 + \text{CO}\)
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The Correct Option is A
Solution and Explanation
Concept:
Alkali metal carbonates generally decompose on heating to form metal oxide and carbon dioxide. However, \(\text{Li}_2\text{CO}_3\) is less thermally stable compared to other alkali metal carbonates due to the small size and high polarizing power of \(\text{Li}^+\). Step 1: Understand thermal decomposition. On heating: \[ \text{Metal carbonate} \rightarrow \text{Metal oxide} + \text{CO}_2 \]
Step 2: Apply to lithium carbonate. \[ \text{Li}_2\text{CO}_3 \xrightarrow{\Delta} \text{Li}_2\text{O} + \text{CO}_2 \]
Step 3: Reason behind decomposition.
Step 4: Eliminate incorrect options.
Step 5: Conclusion. \[ \text{Products = Li}_2\text{O + CO}_2 \]
Alkali metal carbonates generally decompose on heating to form metal oxide and carbon dioxide. However, \(\text{Li}_2\text{CO}_3\) is less thermally stable compared to other alkali metal carbonates due to the small size and high polarizing power of \(\text{Li}^+\). Step 1: Understand thermal decomposition. On heating: \[ \text{Metal carbonate} \rightarrow \text{Metal oxide} + \text{CO}_2 \]
Step 2: Apply to lithium carbonate. \[ \text{Li}_2\text{CO}_3 \xrightarrow{\Delta} \text{Li}_2\text{O} + \text{CO}_2 \]
Step 3: Reason behind decomposition.
- \(\text{Li}^+\) has high charge density
- It polarizes the carbonate ion strongly
- This weakens the \(\text{CâO}\) bonds and promotes decomposition
Step 4: Eliminate incorrect options.
- (B) LiO does not exist as a stable compound $\times$
- (C) LiC is not a valid product $\times$
- (D) \(\text{Li}_2\text{O}_2\) forms in oxidation reactions, not here $\times$
Step 5: Conclusion. \[ \text{Products = Li}_2\text{O + CO}_2 \]
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