Consider the molecules CH4, NH3 and H2O. Which of the given statements is false?

  • Option 1)

    The H - C - H bond angle in CH4, the H - N - H bond angle in NH3, and the H - O - H bond angle in H2O are all greater than 90o.

  • Option 2)

    The H - O - H bond angle in H2O is larger than the H - C - H bond angle in CH4.

  • Option 3)

    The H - O - H bond angle in H2O is smaller than the H - N - H bond angle in NH3.

  • Option 4)

    The H - C - H bond angle in CH4 is larger than the H - N - H bond angle in NH3.

 

Answers (1)

As we learnt in

VSEPR Theory -

1.  The shape of the molecule is determined by repulsions between all of the electron pair present in valence shell.

2.  Order of repulsion 

             lone \:pair-Lone\: pair> Lone\:pair-Bond\:pair> Bond\:pair-bond\:pair

3  Repulsion among the bond pair is directly proportional to the bond  order and electronegativity difference between the central atom and the other atom.

-

 From the above fugure it is clear that H—O—H bond angle in H_{2}O is smaller than H—C—H bond angles in CH_4.


Option 1)

The H - C - H bond angle in CH4, the H - N - H bond angle in NH3, and the H - O - H bond angle in H2O are all greater than 90o.

This option is incorrect

Option 2)

The H - O - H bond angle in H2O is larger than the H - C - H bond angle in CH4.

This option is correct

Option 3)

The H - O - H bond angle in H2O is smaller than the H - N - H bond angle in NH3.

This option is incorrect

Option 4)

The H - C - H bond angle in CH4 is larger than the H - N - H bond angle in NH3.

This option is incorrect

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