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: Identify the nature of intermolecular forces in HF, NH3, and H2S. HF and NH3 exhibit strong intermolecular hydrogen bonding, whereas H2S only exhibits weaker van der Waals forces. Step 2: Compare the hydrogen bond strengths of HF and NH3. Since fluorine is more electronegative than nitrogen, HF forms much stronger hydrogen bonds than NH3, giving HF a higher boiling point. Step 3: This results in the boiling point order: HF > NH3 > H2S, corresponding to option (a).

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