A metal X loses 2 electrons and a non-metal Y gains 1 electron. Show the electron dot structure of compound formed between them. Is it ionic or covalent? Does it have high or low melting point? Will it conduct electricity in solid state or in aqueous solution and why? Will it be soluble in water?

The compound is ionic

The compound has a high melting point

The compound will conduct electricity in aqueous solution

The compound will be soluble in water

Explanation:

Now, let us consider the nature of the compound formed when a metal X looses two electrons and a non metal Y accepts one electron.

The compound formed must be ionic in nature with a  formula XY2. Ionic compounds are formed by transfer of electrons from metals to nonmetals.

The ionic substance formed is always soluble in water with a high melting point. Usually, ionic solids do not conduct electricity in the solid state because the charge carriers (ions) are tightly bound in the crystal structure while in the solid state. In aqueous solution, the ions are relatively free hence ionic substances conduct electricity in aqueous solution.

i dont know

explanation:

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).