According to VSEPR model, molecules adopt geometries in which their valence electron pairs position themselves as far from each other as possible. The VSEPR model considers double and triple bonds to

Question

According to VSEPR model, molecules adopt geometries in which their valence 
electron pairs position themselves as far from each other as possible. The VSEPR
model considers double and triple bonds to have slightly greater repulsive 
effects than single bonds because of the repulsive effect of $\pi$-electrons. 
However the lone pair creates the maximum repulsive effect.

Prashant Kotian · Accepted Answer

Correct answer: D. Step 1: Determine the geometry of water (H2O). It is sp3 hybridized with two bonding pairs and two lone pairs, resulting in a bent shape. Step 2: Because of its asymmetrical bent geometry, the individual polar O-H bond dipoles do not cancel each other out, which gives the molecule a net non-zero dipole moment (mu > 0). Step 3: Therefore, the statement that the molecule has mu = 0 is incorrect, which corresponds to option (a).

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