Question

Why is the oxidation state of o2- more likely than o6+ please explain ?

Answer 1

Answer: Because more energy is required to form $O^{6+}$ ion.

Explanation:

Oxygen is the 8th element of the periodic table which belongs to Group 16.

The electronic configuration of the element is: $1s^22s^22p^4$

The number of valence electrons are 6 which is not a stable electronic configuration.

To attain stable electronic configuration, this element will either loose 6 electrons to form $O^{6+}$ ion or gain 2 electrons to form $O^{2-}$ ion.

The loosing of 6 electrons require a huge amount of energy and is an unfavorable reaction. Hence, this element will gain 2 electrons easily and form $O^{2-}$ ion.

This element is considered as a non-metal because it gains electron to attain stable electronic configuration.