An element X has an electronic configuration 2, 2. The compound formed when X combines with oxygen is most likely to be:

an ionic solid.

Reason — Electronic configuration 2, 2 means the atom has 2 electrons in its outer shell. Hence, it belongs to Group 2, it is a metal with valency 2 (it tends to lose 2 electrons to form X²⁺).
Oxygen is a non-metal with valency 2 (it tends to gain 2 electrons to form O^2-).
So, when X combines with oxygen, the compound formed will be of the type X²⁺ O^2-, i.e. metal + non-metal. This is ionic in nature and will exist as an ionic solid with high melting point, conducting electricity only in molten/solution state.