Why Is the Enthalpy of Formation for NaCl Less Negative Than for KCl?

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The discussion centers on the enthalpy of formation (ΔHf) for NaCl being less negative than that for KCl, despite the expectation that Na+, being smaller than K+, would create stronger electrostatic attractions with Cl-. Participants express confusion over this observation, as stronger attractions should theoretically lead to a more negative ΔHf for NaCl. The conversation also touches on the contrasting behavior observed with fluorine compounds, where the reasoning appears consistent. The need for clarification on the underlying principles affecting these enthalpy values is emphasized. Understanding the factors influencing ionic bonding and lattice energy is crucial for resolving this discrepancy.
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Homework Statement


In my book it is given that ΔHffor NaCl is less negative than that for KCl.
I'm not able to understand that...I think that electrostatic attractions between Na+ and Cl- will be stronger than K+ & Cl- as Na has smaller size than K...in its formation more energy should be released and ΔHffor NaCl should be more negative.

I also noticed that in case of F my reasoning seems correct.


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please reply someone...thanks
 

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