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Explain why fluorine always exhibit an o...

Explain why fluorine always exhibit an oxidation state of -1 ?

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Fluorine the most electronegative element than other halogens and cannot exhibit any positive oxidation state. Fluorine does not have d - orbital white other halogens have d - orbitals. Therefore fluorine always exhibit an oxidation state of `-1` and others in halogen family shows `+1, +3, +5 and +7` oxidation states.
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Knowledge Check

  • Alkali elements exhibit an oxidation state of __________

    A
    `+1`
    B
    `+2`
    C
    `+3`
    D
    `+4`

  • Assertion : Fluorine has an oxidation state of -1 in all its compounds. Reason : Fluorine is the most electronegative element of the periodic table.

    A
    Both assertion and reason are correct and reason is the correct explanation for assertion .
    B
    Both assertion and reason are correct but reason is not the correct explanation for assertion .
    C
    Assertion is true but reason are false.
    D
    Both assertion and reason are false.

  • Elements which generally exhibit multiple oxidation states and whose ions are usually coloured are

    A
    metalliods
    B
    transition elements
    C
    non - metals
    D
    gases

    • Similar Questions

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    Explain why d-block elements exhibit variable oxidation states?

    Name the oxometal anoins of the first series of the transition metals in which the metal exhibits the oxidation state equal to its group number.

    What do you understand by the term 'variable oxidation state ' ? Which element in a group or period exhibit variable oxidation state ?

    Which one of the following exhibits highest oxidation state ?

    Comparing Al, B, Ga and Tl , which one exhibits +1 oxidation state?

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