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Question

# Which of the following has the highest bond angle?

A

${\mathrm{H}}_{2}\mathrm{O}$

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B

${\mathrm{H}}_{2}\mathrm{S}$

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C

${\mathrm{NH}}_{3}$

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D

${\mathrm{PH}}_{3}$

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Solution

## The correct option is C ${\mathrm{NH}}_{3}$The explanation for the correct answer(C) ${\mathbf{NH}}_{\mathbf{3}}$The angle between two covalent bonds that originate from the same atom is called the Bond angle.The Bond angle decreases down the group.${\mathrm{NH}}_{3}$have $3$bonding pair and $1$lone pair. $\mathrm{N}$is more electronegative, $\mathrm{N}$attracts the shared pair of electrons. It experiences a strong repulsion due to electron-electron repulsion force.So, ${\mathrm{NH}}_{3}$has the highest bond angle.Hence, Option (C) ${\mathbf{NH}}_{\mathbf{3}}$is correct.The explanation for the incorrect answer(A) ${\mathbf{H}}_{\mathbf{2}}\mathbf{O}$Bond angle decreases down the groupThus, ${\mathrm{H}}_{2}\mathrm{O}$ has a greater bond angle than ${\mathrm{H}}_{2}\mathrm{S}$The lone pair-lone pair repulsion on oxygen is more effective.Hence, ${\mathrm{H}}_{2}\mathrm{O}$ has a lesser bond angle than${\mathrm{NH}}_{3}$.(B) ${\mathbf{H}}_{\mathbf{2}}\mathbf{S}$Bond angle decreases down the groupThus, ${\mathrm{H}}_{2}\mathrm{S}$ has a lesser bond angle than ${\mathrm{H}}_{2}\mathrm{O}$(D) ${\mathbf{PH}}_{\mathbf{3}}$$\mathrm{P}$is less electronegative than $\mathrm{N}$It cannot attract shared pair of electrons effectively.So ${\mathrm{PH}}_{3}$has a lesser bond angle than ${\mathrm{NH}}_{3}$Therefore, Option (C) ${\mathbf{NH}}_{\mathbf{3}}$is correct.

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