Question

Which of the following has highest bond angle?

• A. ${\mathrm{BBr}}_3$
• B. ${\mathrm{SO}}_2$
• C. ${\mathrm{CS}}_2$
• D. ${\mathrm{SF}}_4$

Answer 1

The correct option is C

${\mathrm{CS}}_2$

Explanation for the correct option:

(c ) ${\mathrm{CS}}_2$

• Because ${\mathrm{CS}}_2$ hybridization is sp hybridization, the carbon atom is in the centre bonding with two sulphur atoms, forming a bond angle of $180°$, making the ${\mathrm{CS}}_2$ molecule's molecular shape linear.

• Hence this option is correct

The explanation for the incorrect options:

(a) ${\mathrm{BBr}}_3$

• Because of Boron hybridization, all three have the identical bond angle of $120°$.

• ${\mathrm{CS}}_2$ has greater bond angle than ${\mathrm{BBr}}_3$
• Thus, this option is incorrect.

(b) ${\mathrm{SO}}_2$

• The sulphur dioxide molecule has a bond angle of $119°$.

• ${\mathrm{SO}}_2$ has greater bond angle than ${\mathrm{BBr}}_3$
• Thus, this option is incorrect.

(d) ${\mathrm{SF}}_4$

• ${\mathrm{SF}}_4$ has greater bond angle than ${\mathrm{BBr}}_3$
• Thus, this option is incorrect.

Hence the correct option is (c ) ${\mathrm{CS}}_2$