Both covalent-network solids and ionic solids can havemelting points well in excess of room temperature, and bothcan be poor conductors of electricity in their pure form.However, in other ways their properties are quite different.(a) Which type of solid is more likely to dissolve in water?(b) Which type of solid can become a considerably betterconductor of electricity via chemical substitution?

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A: Find: which of the following interface cannot be obtained? And why?

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Q: aplete the following table: Name Coordination # # of atoms in unit cell of the unit cell.

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Q: (d) In Covalent-solids and ionic-solids, whose electrical conductivity will be higher? Why?

A: Since you've posted multiple questions, we'll solve only the first question for you. If you want any…

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Crystal Structures

Solids are present all around us. They have different properties and applications. Diamond and graphite are two well-known solids. Diamond is the hardest material in the world and is used in making jewelry. Graphite on the other hand is soft. The lead of your pencil is graphite. Why are they so different in appearance and properties despite the fact they are chemically the same? Both are allotropes of carbon. The answer lies in the structure, the way constituent particles are arranged in the solids.