Consider the molecules `CH_(4),NH_(3)` and `H_(2)O` which of the given statement is false ?

Options

A. The `H-O-H` bond angle in `H_2O` is larger than the `H-C-H` bond angle in `CH_4`
B. The `H-O-H` bond angle in `H_2O` is smaller than the `H-N-H` bond angle in `NH_3`
C. The `H-C-H` bond angle in `CH_4` is larger than the `H-N-H` bond angle in `NH_3`
D. The `H-C-H` bond angle in `CH_4`, the `H-N-H` bond angle in `NH_3` and the `H-O-H` bond angle in `H_2O` are all the greater than `90^@`

Answer

A, D

Explanation

As the number of lone pair of electrons on central element increases, repulsion between those lone pair of electrons increases and therefore, bond angle decreases.
Molecules Bond angle
`CH_4` (no lone pair of electrons) `109.5^@`
`NH_3` (one lone pair of electrons ) `107.5^@`
`H_2O` (two lone pair of electrons ) `104.45^@`