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Arrange the following molecules in increasing order of their bond angles: H2S, NH3, BF3 and SiH4.

1. H2S < NH3 < SiH4 < BF3
2. NH3 < H2S < SiH4 < BF3
3. H2S < SiH4 < NH3 < BF3
4. H2S < NH3 < BF3 < SiH4

Correct answer: H2S < NH3 < SiH4 < BF3

Solution

The bond angles increase with the presence of lone pairs and the hybridization of the central atom. H2S has the smallest angle due to its bent shape and lone pairs, followed by NH3 with a larger angle due to one lone pair, SiH4 with a tetrahedral shape and no lone pairs, and finally BF3 with a trigonal planar shape, which has the largest bond angle.

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