Question

The bond angle is the lowest in which of the following species?

• A. $H_3{O}^{+}$
• B. $N{H}_4^{+}$
• C. $F_{2}O$
• D. $BC{l}_3$

Answer 1

The correct option is C $F_{2}O$

In $F_{2}O$, there are two lone pairs and two bond pairs of electrons. Due to the lone pair - lone pair repulsions and high electronegativity of $F$, the bond angle of $F-O-F$ decreases and found to be less than ${109.5}^o$.
$H_3{O}^{+}$ has a tetrahedral geometry and is pyramidal in shape as it has one lone pair of electrons and the bond angle is around ${107}^o$.

$N{H}_4^{+}$ has a tetrahedral geometry with a bond angle of ${109.5}^o$.

$BC{l}_3$ has a trigonal planar geometry with a bond angle of ${120}^o$.