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Question
Assertion :Oxygen is never more than divalent,as in H2O2. Reason: S, Se and Te can form four or six bonds,as in SF6.
Assertion :Oxygen is never more than divalent,as in H2O2. Reason: S, Se and Te can form four or six bonds,as in SF6.
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Solution
The correct option is B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion,
Oxygen, being highly electronegative, is never more than divalent, as in H2O2
S, Se and Te can form four or six bonds as in SF6. With decrease in the electronegativity on moving down the group, the importance of +4 and +6 oxidation states increases in comparison to +2 oxidation state.
In other words, the valence shell of oxygen contains only s and p electrons. It does not contain d orbitals. Hence, it cannot expand its valency beyond 2. Whereas S, Se and Te have empty d orbitals and can utilize all the valence electrons to form 2,4 and 6 covalent bonds.
Hence, both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
Oxygen, being highly electronegative, is never more than divalent, as in H2O2
S, Se and Te can form four or six bonds as in SF6. With decrease in the electronegativity on moving down the group, the importance of +4 and +6 oxidation states increases in comparison to +2 oxidation state.
In other words, the valence shell of oxygen contains only s and p electrons. It does not contain d orbitals. Hence, it cannot expand its valency beyond 2. Whereas S, Se and Te have empty d orbitals and can utilize all the valence electrons to form 2,4 and 6 covalent bonds.
Hence, both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
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