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Oxygen does not show oxidation states of...

Oxygen does not show oxidation states of `+4 " and " +6` like sulphur. Explain.

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Sulphur shows`+4 " and " +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 " and " +6` oxidation states in compounds. For more details, consult text part.
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Knowledge Check

  • Oxygen shows +2 oxidation state is

    A
    `F_(2)O`
    B
    `H_(2)O`
    C
    `K_(2)O`
    D
    `D_(2)O`

  • Oxygen shows oxidation state of -1 in the compound -

    A
    `NO_(2)`
    B
    `MnO_(2)`
    C
    `PbO_(2)`
    D
    `Na_(2)O_(2)`

  • Which halogen does not show +7 oxidation state?

    A
    Chlorine
    B
    Bromine
    C
    Iodine
    D
    Fluorine

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    Oxygen exhibits an oxidation state of - 2 while the other members of the family show oxidation states of +2, +4 " and " +6 . Explain.

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    Highest oxidation state of oxygen is

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