Solved: CHEMISTRY Question for NEET

NEET CHEMISTRYEasy

Identify the incorrect statement among the following:

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

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

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 90°

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

Methane (CH₄): The central carbon atom is $sp^3$ hybridised with 0 lone pairs. The molecule has a regular tetrahedral geometry with a bond angle of 109.5° .
Ammonia (NH₃): The central nitrogen atom is $sp^3$ hybridised but possesses 1 lone pair. According to VSEPR theory, the repulsion between the lone pair and bond pairs ( $lp-bp$ ) is greater than between bond pairs ( $bp-bp$ ), causing the bond angle to decrease from 109.5° to 107° .
Water (H₂O): The central oxygen atom is $sp^3$ hybridised with 2 lone pairs. The repulsive interaction follows the order $lp-lp > lp-bp > bp-bp$ . The presence of two lone pairs squeezes the bond angle further to 104.5° .
Verification of Statements:

Option A: States H₂O angle (104.5°) > CH₄ angle (109.5°). This is Incorrect.
Option B: States CH₄ angle (109.5°) > NH₃ angle (107°). This is Correct.
Option C: All angles (109.5°, 107°, 104.5°) are > 90°. This is Correct.
Option D: States H₂O angle (104.5°) < NH₃ angle (107°). This is Correct.

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