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Fluorine exhibits an oxidation state of ...

Fluorine exhibits an oxidation state of only -1 because :

A

it can readily accept an electron

B

it is very strongly electronegative

C

it is a non-metal

D

it belongs to halogen family

Text Solution

Verified by Experts

The correct Answer is:
B
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Why sulphur exhibits even oxidation states only?

Fluorine exhibits only -1 oxidation state whereas other halogens exhibit +1, +3, +5 and +7 oxidation states. Explain.

Knowledge Check

  • Actinides exhibits oxidation state

    A
    `+3 and +4`
    B
    `+4 and 5`
    C
    `+5 and +6`
    D
    `+2` to `+7`

  • Oxygen exhibits least oxidation state in

    A
    `OF_(2)`
    B
    `KO_(2)`
    C
    `H_(2)O`
    D
    `H_(2)O_(2)`

  • Oxygen exhibits least oxidation state in

    A
    `OF_2`
    B
    `KO_2`
    C
    `H_2O`
    D
    `H_2O_2`

    • Similar Questions

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    Fluorine exhibits only -1 oxidation state whereas other halogens show +1, +3, +5 and +7 oxidation states also. Explain.

    (a) Halogens have maximum negative gain enthalpy in the respective periods of the periodic table. Why? (b) Although electron gain enthalpy of fluorine is less negative as compared to chlorine, fluorine is a stronger oxidising agent than chlorine . Why? Fluorine exhibits only-1 oxidation state, wherease other hlaogens exhibit +1,+3,+5, and +7 oxidation states also. explain.

    Fluorine exhibit only – 1 oxidation state whereas other halogens exhibit +ve oxidation states also. Explain why ?

    Account for the following observations: fluorine exhibits only -1 oxidation state whereas other halogens exhibit higher positive oxidation states also.

    Mg cannot exhibit +3 oxidation state, because its:

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