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's consistent -1 oxidation state can be attributed to its electronic configuration and the absence of d orbitals. Being the most electronegative element, fluorine seeks to gain an electron to fill its valence shell, achieving a stable octet configuration.

Fluorine has the electronic configuration: \(1s^2 2s^2 2p^5\). Its outermost shell requires just one more electron to complete the p orbital. The absence of d orbitals in fluorine implies it cannot expand its valence shell, unlike other elements which can utilize d orbitals to form different oxidation states.

Thus, fluorine only shows an oxidation state of -1, as it cannot share or lose electrons to form higher positive oxidation states, a consequence of lacking d orbitals.

Factors	Impact on Oxidation State
Electronegativity	High
d Orbitals	Absent
Size	Small

Answer 2

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.