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Question

Fluorine exhibits only -1 oxidation state while iodine exhibits oxidation states of -1, + 1, + 3, +5 and + 7. This is due to :


A
flourine being a gas
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B
available d-orbitals in iodine
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C
non-availability of d-orbitals in iodine
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D
none of the above.
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Solution

The correct option is C available $$d$$-orbitals in iodine
Due to absence of d-orbitals, $$F$$ can not expand its valency but $$I$$ can expand its valency (as shown in the figure) and therefore, exhibts variable oxidation states.
165373_171966_ans.gif

Chemistry

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