Single Choice

______ cation and ______ anion favour least covalent character.

ASmall,large
BLarge,small
Correct Answer
CLarge,large
DSmall,small

Solution

According to Fajan's rules of polarization, small the size of anion, more easily it will be polarized and hence, the compound will be least covalent. Large the size of cation, more will be it's polarizing power and hence, compound will be least covalent.

Hence option B is the correct answer.

SIMILAR QUESTIONS

Chemical Bonding

Polarisation is the distortion of the shape of anion by an adjacently placed cation. Which of the following statement is correct?

Chemical Bonding

Which of the following has been arranged in order of increasing covalent character?

Chemical Bonding

Polarising action of $$Cd^{2+}$$ an anions is stronger than that of $$Ca^{2+}$$ because:

Chemical Bonding

Which compound among the following has more covalent character ?

Chemical Bonding

Amongst $$LiCl$$, $$RbCl$$, $$BeCl_2$$ and $$MgCl_2$$, the compounds with the greatest and the least ionic character, respectively are:

Chemical Bonding

Among the following, the maximum covalent character is shown by which compound?

Chemical Bonding

Among the following which one has the highest cation to anion size ratio?

Chemical Bonding

Arrange the below molecules in order of increasing ionic character.$$LiF$$ $$, \ \displaystyle K_{2}O $$, $$ \displaystyle N_{2} $$, $$ \displaystyle SO_{2} $$ and $$ \displaystyle ClF_{3} $$

Chemical Bonding

The correct order of the increasing covalent character of the following is:

Chemical Bonding

The bond length in $$LiF$$ will be:

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