A) \[LiCl<BeC{{l}_{2}}<BC{{l}_{3}}<CC{{l}_{4}}\]
B) \[LiCl<BeC{{l}_{2}}>BC{{l}_{3}}>CC{{l}_{4}}\]
C) \[LiCl>BeC{{l}_{2}}<BC{{l}_{3}}<CC{{l}_{4}}\]
D) \[LiCl>BeC{{l}_{2}}>BC{{l}_{3}}>CC{{l}_{4}}\]
Correct Answer: A
Solution :
Key Idea Bond polarity \[\propto \] electronegativity difference of bonded atom If there is a large difference in electronegativity of two atoms then bonding is either ionic or polar. If there is a small difference in electronegativity of two atoms then bonding is either covalent or non-polar. As the covalent character increase with the decrease in the value of difference in electro negativities of bonded atoms. Therefore, the covalent bond character in \[LiCl,\,\,BeC{{l}_{2}},\,BC{{l}_{3}}\] and \[CC{{l}_{4}}\] in the following order \[LiCl<BeC{{l}_{2}}<BC{{l}_{3}}<CC{{l}_{4}}\] Note - High charge and small size of the cation will exert greater polarising effect on anions and therefore, covalent character increase because if polarisation is large the bonding is covalent.
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