Select the correct order with respect to increasing ionic character of the given compounds:

B e C l_{2} < M g C l_{2} < C a C l_{2} < B a C l_{2}

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B e C l_{2} < M g C l_{2} < B a C l_{2} < C a C l_{2}

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B e C l_{2} < B a C l_{2} < M g C l_{2} < C a C l_{2}

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B a C l_{2} < C a C l_{2} < M g C l_{2} < B e C l_{2}

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Solution

The correct option is A $B e C l_{2} < M g C l_{2} < C a C l_{2} < B a C l_{2}$
We know that as we move down the group in case of alkaline earth metals, electronegativity decreases, while the ionic character of halides increases.
Due to very small size and high electronegativity of $B e$ , it forms halides which are mainly covalent.
Hence, the correct order with respect to increasing ionic character of compounds is as follows:
$B e C l_{2} < C a C l_{2} < M g C l_{2} < B a C l_{2}$

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