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Why do chlorine, bromine and iodine exhi...

Why do chlorine, bromine and iodine exhibit +3, +5 and +7 oxidation states in addition to - 1 and +1 oxidation tes?

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Cl, Br and I have only one unpaired electron in their ground state. Therefore, they exhibit an oxidation state of -1 or +1. However, they have 3, 5 and 7 unpaired electrons in their first, second and third excited states, respectively. Hence, they also exhibit the oxidation states of +3, +5 and + 7.
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Knowledge Check

  • Fe shows an oxidation state of +1 in

    A
    `Fe(CO)_5`
    B
    `[Fe(H_2O)_5NO]SO_4`
    C
    `FE_4[Fe(CN)_6]_3`
    D
    `FeCl_4^(-)`

  • Which of the following exhibits only + 3 oxidation state -

    A
    Th
    B
    Ac
    C
    Pa
    D
    U

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    Which shows only -1 oxidation state?

    Why do transition elements exhibit variable oxidation states ?

    Can lanthanum (Z = 57) exhibit + 4 oxidation state ?

    Which one does not exhibit a positive oxidation state in its compounds?

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