Oxygen does not show +4 and +6 oxidation states like sulphur. Why?
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Explanation:
Sulphur shows +4 &. +6 oxidation states due to the presence of vacant 3d orbitals to which electrons can be promoted from 3s and 3p filled orbitals. Since oxygen atom does not have 2d orbitals, no electorn promotion is possible in this case. Therefore, oxygen cannot show +4 &. +6 oxidation states in compounds.
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Answer:
Oxygen is highly electronegative elements rather than remove electrons it act as a electron acceptor.
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