Discussion
The repulsive interaction between different types of electron pairs increases in the order of
Answer: A
The order of increasing repulsion is bond pair - bond pair < lone pair - bond pair < lone pair - lone pair.
This is the core rule of VSEPR theory. A lone pair is held by only one nucleus, so its electron cloud is broader and sits closer to the central atom than a bonding pair, which is drawn out between two nuclei. Lone pairs therefore repel more strongly, and two lone pairs repel each other most of all.
That is why the H-O-H angle in water (about 104.5°) and the H-N-H angle in ammonia (about 107°) are smaller than the tetrahedral 109.5° of methane. The other three options put bond pair - bond pair repulsion above a repulsion involving a lone pair, which reverses the rule.
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