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Arrange the following hydrides of group 16 elements in order of increasing stability:
A) $ {H_2}S < {H_2}O < {H_2}Te > {H_2}Se $
B) $ {H_2}O < {H_2}Te < {H_2}Se < {H_2}S $
C) $ {H_2}O < {H_2}S < {H_2}Se < {H_2}Te $
D) $ {H_2}Te < {H_2}Se < {H_2}S < {H_2}O $

Last updated date: 21st Jul 2024
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Hint: The tendency of a fluid to resist breaking down under heat stress is known as thermal stability. It depends on the shape, bond lengths, bond angle, and other factors. It also depends on the electronegativity differences between the compounds.

Complete answer:
They have oxidation states of -2, +2, +4, and +6. Because of the rise in atomic size and decrease in electronegativity, the stability of the -2 oxidation state decreases down the group. Thanks to the inert pair effect, the stability of the +6 oxidation state decreases when the +4 oxidation state increases.
If the bond dissociation energy decreases, so does the stability of the group. As a result of the rise in the central atom number, the bond dissociation energy decreases down the group. As we go down the group, the bond angles steadily decrease due to a decrease in bond pair-bond pair repulsion.
If we go down the group, the size of the particles grows, lowering the effective nuclear charge and lowering stability.
Hence, the correct option is D) $ {H_2}Te < {H_2}Se < {H_2}S < {H_2}O $ .

Chemical stability is an important factor to consider when evaluating pharmaceutical properties, activity, and selectivity during drug development. It is possible that deciding how and when to research various equilibrium issues would be beneficial to a drug development programme.