Question

Fluorine does not show positive oxidation states because:
A.It is most electronegative elements
B.It forms only anions in ionic compounds
C.It cannot form multiple bonds
D.It shows non-bonded electron pair repulsion due to its small size.

Answer 1

Hint: Fluorine is the most electro-negative element and does not have d orbitals in its valence shell. For fluorine to exhibit a positive oxidation state, a more electronegative element has to be bonded with it, which is very difficult to make happen.

Complete answer:
Fluorine is the lightest halogen and exists at standard conditions as a highly toxic, pale yellow diatomic gas. It is the most reactive chemical element. It also has a high electron affinity. Fluorine is found in nature only in the form of its chemical compounds, except for trace amounts of the free element in fluorspar that has been subjected to radiation from radium. Not a rare element, it makes up about \[0.065\] percent of Earth’s crust.
Fluorine atoms have a small covalent radius. F is the highest electronegative element, the possibility of sharing its electron with more electronegative element than itself is not there. Its chemical activity can be attributed to its extreme ability to attract electrons (it is the most electronegative element) and to the small size of its atoms. This is the reason why fluorine does not show positive oxidation states.

Therefore the correct option is A. it is the most electronegative element.

Note:
At room temperature fluorine is a faintly yellow gas with an irritating odour. Inhalation of the gas is dangerous. Upon cooling, fluorine becomes a yellow liquid. Because fluorine is the most electronegative of the elements, atomic groupings rich in fluorine are often negatively charged.