Arrange the following in increasing order of their covalent character.
(A) ${CaF}_{2}$
(B) ${CaCl}_{2}$
(C) ${CaBr}_{2}$
(D) ${CaI}_{2}$
Choose the correct answer from the options given below.

Question

Arrange the following in increasing order of their covalent character. (A) CaF 2 (B) CaCl 2 (C) CaBr 2 (D) CaI 2 Choose the correct answer from the options given below.

TestHub · Accepted Answer

Cation is same in all case while anions are different.
According to Fajan's rule, Larger the anion, less is the effective nuclear charge that holds the valence electron of the ion in place. Since the last electron is loosely bound in large anions, it can easily be polarised by a cation, thereby making the compound more covalent.
Hence, the larger the size of the anion, greater is the covalent character of the ionic bond.
${CaF}_{2} < {CaCl}_{2} < {CaBr}_{2} < {CaI}_{2}$

CHEM_REMOVED - CHEMICAL BONDING Question with Solution | TestHub

Options:

Doubts & Discussion