Classify each of the following solids as metallic, network covalent, ionic or molecular substances.

a.) it is insoluble in water, melts above 500c, and does not conduct electricity as a solid

b.) it dissolves in water, but does not conduct electricity as an aqueous solution or as a solid

c.) it dissolves in water, melts above 100c, and conducts electricity when present in an aqueous solution

A) Network covalent

B) Molecular

C) Ionic

Explanation:

A) Network covalent

This compouds are characterized by having atoms bonded each other by covalent union like a network that extends to all the structure (macromolecule).  They have high melting points and low conductivity. A good example of this is diamond.

B) Metallic and network covalent compounds are insoluble in water. Also, ionic compounds that are soluble in water dissociate and conduct electricity.

So, in this case we are talking about a molecular substance in particular, a polar substance.

C) Ionic

This substances dissolved in water conduct electricity. Also they have high boiling points

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c. electrical charges of ionic bonds.