Which of the following has the strongest bond | vedclass

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(A) The strength of an ionic bond is determined by the lattice energy,which is inversely proportional to the interionic distance $(r_+ + r_-)$.$CsF$ c

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$CsF$

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(A) The strength of an ionic bond is determined by the lattice energy,which is inversely proportional to the interionic distance $(r_+ + r_-)$.$CsF$ consists of $Cs^+$ and $F^-$ ions,while $NaCl$ consists of $Na^+$ and $Cl^-$ ions.The ionic radius of $F^-$ is significantly smaller than that of $Cl^-$.Although $Cs^+$ is larger than $Na^+$,the small size of the $F^-$ ion leads to a shorter interionic distance in $CsF$ compared to $NaCl$.Furthermore,the lattice energy is higher for $CsF$ due to the high charge density of the fluoride ion,making the $Cs-F$ bond stronger in terms of lattice stability.

Which of the following has the strongest bond?

Similar Questions

Elements $X$ and $Y$ have $2$ and $6$ electrons in their valence shells,respectively. If they combine,what will be the possible formula of the compound formed?

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:
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When metals combine with non-metals,the metal atom tends to:

Assertion $(A)$: Higher lattice enthalpy leads to greater stability of ionic compounds.
Reason $(R)$: Lattice enthalpy is a direct measure of the electrostatic forces of repulsion among the constituent ions in an ionic solid.
The correct answer is

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