Question

In which of the following bond angle is maximum.

• A. ${\mathrm{NH}}_3$
• B. ${{\mathrm{NH}}_4}^{+}$
• C. ${\mathrm{PCl}}_3$
• D. ${\mathrm{SCl}}_2$

Answer 1

The correct option is B

${{\mathrm{NH}}_4}^{+}$

Explanation for correct option:

(b) ${{\mathrm{NH}}_4}^{+}$

• Ammonium ion, ${{\mathrm{NH}}_4}^{+}$, has theoretical tetrahedral bond angles of roughly $109.5$degrees.
• The Ammonium ion has perfect symmetry.
• Also, there are no lone pairs in Ammonium ion so, there will be no repulsion between lone pairs and bond pairs.
• The structure of Ammonium ion is as follows:

Explanation for incorrect options:

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

• Ammonia (${\mathrm{NH}}_3$) has a bond angle less than the standard$109.5°$.
• The bond angle is $107°$.
• There is one lone pair due to which the bond angle decreases.
• It is due to the pyramidal shape of Ammonia as shown below:

(c) ${\mathrm{PCl}}_3$

• Phosphorus Trichloride (${\mathrm{PCl}}_3$) also has a bond angle less than the standard$109.5°$.
• The bond angle is $100°$.
• There is one lone pair due to which the bond angle decreases.
• It is due to the Trigonal pyramidal geometry of Phosphorus Trichloride as shown below:

(d) ${\mathrm{SCl}}_2$

• In nature, Sulphur Chloride (${\mathrm{SCl}}_2$) possesses a bent molecular geometry.
• ${\mathrm{SCl}}_2$ is made up of one Sulphur atom surrounded by two Chlorine atoms.
• There are two lone pairs due to which the bond angle decreases.
• The geometry is as follows:

Hence, the correct option is (b). Ammonium ion has the maximum bond angles.