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Many bond angles can be explained by either electronegativity or size arguments. Molecules with larger difference in electronegativity values between central and outer atoms have smaller bond angles. As the size of outer atom increases, the angle increases. The size of central atom can also be used to determine the bond angles in the series.
Consider the following molecules:
(I) \( \mathrm{H}_{2} \mathrm{O} \quad \) (II) \( \mathrm{H}_{2} \mathrm{~S} \)
(III) \( \mathrm{H}_{2} \mathrm{Se} \quad \) (IV) \( \mathrm{H}_{2} \mathrm{Te} \)
Arrange these molecules in increasing order of bond angle:
(a) I \( \) II \( \) III \( \) IV
(b) IV \( \) III \( \) II \( \) I
(c) I \( \) II \( \) IV \( \) III
(d) II \( \) IV \( \) III \( \) I
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