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Oxygen differs from the other elements o...

Oxygen differs from the other elements of the group. Compounds of oxygen with metals are more ionic in nature and hydrogen bonding is more important for oxygen compounds. Oxygen is never more than divalent beacasue when it hs formed two covalent bonds, there are no low energy orbitals which can be used for 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 decending the group.
The bond between S and O, or Se and O, are much shorter than might be expected for a single bond owing to `rho pi - dpi` interaction between the p- orbital of oxygen and d- orbital of S or Se.
Which one of the following orders represents the correct order for the properties indicated against them?

A

`H_(2)O lt H_(2)S lt H_(2)Se lt H_(2)Te -` acidic character

B

`H_(2)O lt H_(2)S lt H_(2)Se lt H_(2)Te` - thermal stability

C

`H_(2)S gt H_(2)Se lt H_(2)Te lt H_(2)O -` reducing character

D

`H_(2)S lt H_(2)Se lt H_(2)O lt H_(2)Te -` boiling point

Text Solution

Verified by Experts

The correct Answer is:
A
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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 bonding is more important for oxygen compounds. Oxygen is never more than divalent beacasue when it hs formed two covalent bonds, there are no low energy orbitals which can be used for 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 decending the group. The bond between S and O, or Se and O, are much shorter than might be expected for a single bond owing to rho pi - dpi interaction between the p- orbital of oxygen and d- orbital of S or Se. Which of the following statemet is incorrect ?

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