The combination of which of the following giv | vedclass

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(A) According to Fajan's rule,the covalent character in an ionic compound increases with a smaller size of the cation and a larger size of the anion.C

Vedclass · Accepted Answer

$Mg^{2+}$ and $Cl^{-}$

Vedclass · Answer

(A) According to Fajan's rule,the covalent character in an ionic compound increases with a smaller size of the cation and a larger size of the anion.Comparing the cations: $Mg^{2+}$ is smaller than $Na^{+}$ due to higher charge density.Comparing the anions: $O^{2-}$ is smaller than $Cl^{-}$ and $Br^{-}$. However,the polarizing power of $Mg^{2+}$ is significantly higher than $Na^{+}$.Among the given options,$Mg^{2+}$ and $Cl^{-}$ provides a combination where the cation has high charge and the anion is relatively large and polarizable,leading to significant covalent character. Specifically,$MgCl_2$ is more covalent than $NaCl$ or $MgO$ due to the balance of cation size and anion polarizability.

The combination of which of the following gives an ionic compound with maximum covalent character?

Similar Questions

Arrange the following in the decreasing order of their covalent character:
$(A)$ $LiCl$ $(B)$ $NaCl$ $(C)$ $KCl$ $(D)$ $CsCl$
Choose the most appropriate answer from the options given below.

Assertion : $LiCl$ is predominantly a covalent compound.
Reason : Electronegativity difference between $Li$ and $Cl$ is too small.

Define polarization.

The melting points of $(i)$ $BeCl_2$, $(ii)$ $CaCl_2$, and $(iii)$ $HgCl_2$ follow the order:

Which of the following compounds will have the least ionic character?

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