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

Oxygen differs from the other elements of the group. Compounds of oxyg

1.	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 gt H_(2)Se lt H_(2)O lt H_(2)Te -`"boiling point "
Answer» (A) As bond (H-E) dissociation enthaply decreases down the group, the acidic character increases from `H_(2)O` to `H_(2) Te`. (B) Order of thermal stability is `H_(2)O gt H_(2)S gt H_(2)Se gt H_(2)Te`. (C ) `H_(2)O` does not have reducing property and this character increases from `H_(2)S` to `H_(2)Te`. (D) Water has highest boiling point because of H-bonding and thus the correct order is `H_(2)S lt H_(2)Se lt H_(2)Te lt H_(2)O`.

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