Question

Why does Fluorine exhibit only -1 oxidation state?

• A. It is a halogen
• B. It is a non-metal
• C. It is small in size
• D. It has no d orbitals

Answer 1

The Correct Option is D

Fluorine exhibits only a -1 oxidation state because it is the most electronegative element.
It readily gains one electron to achieve a stable electron configuration, resulting in a -1 charge in compounds.
The reason fluorine always exhibits this oxidation state is that it has no d orbitals available for bonding. As a result, it cannot expand its valence shell to accommodate positive oxidation states, which is possible for elements with available d orbitals.

Thus, Option D: It has no d orbitals is the correct explanation.

Answer 2

Fluorine exhibits only the -1 oxidation state because it is highly electronegative and lacks d orbitals, preventing it from adopting positive oxidation states. Its strong pull on electrons keeps it stable in the -1 state.