Chemistry
An element X has an electronic configuration 2, 2. The compound formed when X combines with oxygen is most likely to be:
- a compound with a low melting point.
- a gas that dissolves in water to form an electrolyte.
- a good conductor in both solid and molten state.
- an ionic solid.
Chemical Bonding
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Answer
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 O2-).
So, when X combines with oxygen, the compound formed will be of the type X2+ O2-, 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.
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