Li2CO3 is thermally unstable whereas other Group-I carbonates are stable. Predict the reason.
Correct answer: C. Li+ can effectively polarize CO3-2 ion
- A. Li is less electropositive
- B. Li has low ionization potential
- C. Li+ can effectively polarize CO3-2 ion
- D. Li+ cannot effectively polarize CO3-2 ion
Explanation
The thermal instability of lithium carbonate (Li2CO3) compared to other alkali metal carbonates due to following reasons:Size and Charge of Lithium Ion (Li^+): Lithium ions are smaller and have a higher charge density compared to other alkali metal ions. Ionic Radius of Lithium: The small ionic radius of lithium ions.Carbonate Ion StabilityHigher Basicity of Lithium Oxide: The product of lithium carbonate decomposition, lithium oxide (Li2O), is a stronger base compared to lithium carbonate. Overall, the combination of these factors leads to the greater thermal instability of lithium carbonate compared to other alkali metal carbonates.
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About Reactions of Group I Elements
Group I elements have one valence electron, so their reactivity increases down the group as ionisation energy decreases. Their reactions with water, oxygen, hydrogen and halogens produce hydroxides, oxides, hydrides and halides, while the behaviour of lithium differs from the heavier metals because of its small ionic size.
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