Which of the following is the correct increas | vedclass

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(A) According to Fajan's rule,the polarizing power of the cation decreases as the size of the cation increases down the group. Since $Be^{2+}$ is the

Vedclass · Accepted Answer

$BeCl_2 < MgCl_2 < CaCl_2 < BaCl_2$

Vedclass · Answer

(A) According to Fajan's rule,the polarizing power of the cation decreases as the size of the cation increases down the group. Since $Be^{2+}$ is the smallest,$BeCl_2$ has the highest covalent character and lowest ionic character. As we move down the group from $Be$ to $Ba$,the size of the cation increases,which leads to a decrease in polarizing power and an increase in ionic character. Therefore,the correct increasing order of ionic character is $BeCl_2 < MgCl_2 < CaCl_2 < BaCl_2$.

Which of the following is the correct increasing order of ionic character?

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