Question

Solve the following question with explaination.


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

(a) The H-C-H bond angle in CH4, the H-N-H bond angle
in NH3, and the H-O-H bond angle in H20 are all
greater than 90°

(b) The H-O-H bond angle in H2O is larger than the
H-C-H bond angle in CH4

(c) The H-O-H bond angle in H20 is smaller than the
H-N-H bond angle in NH3.

(d) The H-C-H bond angle in CH4, is larger than the
H-N-H bond angle in NH3.

⚠️⚠️⚠️DON'T SPAM⚠️⚠️⚠️​

Answer 1

Option B

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

Reason :

Here the molecules like CH4, H20 and NH3 are all sp ³ hybridised.

➡️And there is a slight difference in their bond angles mainly due to lone pair issue.

➡️Here mainly we consider water and methane for above question to

The bond angle of water is 104.5'

The bond angle of methane is 109.25'

Bond angle is due to bond and lone pair repulsion too, as I mentioned above.

Hence the bond angle of methane(CH4) is larger than the water. (H20)

So that. Option 2 us wrong.

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Answer 2

Answer :

Option B)

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

All the three molecules are sp³ hybridised but the bond angles are different due to the presence of lone pair. The bond angle of H2O is 104.5° due to bond pair - lone pair repulsion and the bond angle of CH4 is 109.25°.