Single Choice

Unlike other halogens, Fluoride, does not show higher oxidation states because

Ait is highly electronegative
Bit has no $$d-$$ orbitals and it has only 1 unpaired electron.
Correct Answer
Cits atomic radius is very small
Dthe $$F^-$$ ion is stable and isoelectronic with neon

Solution

Unlike other halogens, Fluoride does not show higher oxidation states because it has no $$d-$$ orbitals and it has only 1 unpaired electron.

Hence, Option "B" is the correct answer.

SIMILAR QUESTIONS

p - block Elements

Among the following which is the strongest oxidizing agent?

p - block Elements

Assertion: Fluorine exists only in $$-1$$ oxidation state. Reason: Fluorine has $$2s^22p^5$$ configuration

p - block Elements

The non-metal that does not exhibit positive oxidation state is:

p - block Elements

Which of the following halogens doesn't exhibit positive oxidation state in its compounds?

p - block Elements

Which of the following increasing order is not correct as mentioned in the property with it?

p - block Elements

Which halogen does not show variable oxidation state?

p - block Elements

In the conversion $${Br}_{2}\rightarrow Br{O}_{3}^{-}$$, the oxidation state of bromine changes from

p - block Elements

The oxidation number of chlorine in $$HOCl$$

p - block Elements

Oxidation state of chlorine in perchloric acid is

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