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Oxygen differs from the other elements of the group. Compounds of oxygen with metals are more ionic in nature and hydrogen
\( \mathrm{P} \) bonding is more important for oxygen compounds. Oxygen is

W never more than divalent because when it has formed two covalent bonds, there are no low energy orbitals which can be used to form further bonds. However, the elements S, Se, Te and Po have empty d-orbitals which may be used for bonding, and they can form four or six bonds by unpairing electrons. The higher oxidation states become less stable on descending the group.
The bond between \( \mathrm{S} \) and \( \mathrm{O} \), or \( \mathrm{Se} \) and \( \mathrm{O} \), are much shorter than might be expected for a single bond owing to \( \mathrm{p} \pi-\mathrm{d} \pi \) interaction between the p-orbital of oxygen and \( \mathrm{d} \) - orbital of \( \mathrm{S} \) or \( \mathrm{Se} \).
Which one of the following orders represents the correct order for the properties indicated against them?
(a) \( \mathrm{H}_{2} \mathrm{O}\mathrm{H}_{2} \mathrm{~S}\mathrm{H}_{2} \mathrm{Se}\mathrm{H}_{2} \mathrm{Te} \) - acidic character
(b) \( \mathrm{H}_{2} \mathrm{O}\mathrm{H}_{2} \mathrm{~S}\mathrm{H}_{2} \mathrm{Se}\mathrm{H}_{2} \mathrm{Te} \) - thermal stability
(c) \( \mathrm{H}_{2} \mathrm{~S}\mathrm{H}_{2} \mathrm{Se}\mathrm{H}_{2} \mathrm{Te}\mathrm{H}_{2} \mathrm{O} \) - reducing character
(d) \( \mathrm{H}_{2} \mathrm{~S}\mathrm{H}_{2} \mathrm{Se}\mathrm{H}_{2} \mathrm{O}\mathrm{H}_{2} \mathrm{Te} \)-boiling point
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