Answer to Question 1
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Answer to Question 2
Ionic solid:
Any two of brittle; crystalline; high melting point; hard.
The forces are electrostatic attractions, forming a network of ions. The strength and three-dimensional nature of ionic bonds determine these properties.
Molecular solid:
Any two of soft; low melting point; crystalline.
The forces are London dispersion, hydrogen bonds, or dipole forces, usually in two dimensions. These are relatively weak compared to ionic bonds, and thus molecular solids are not as sturdy as ionic compounds.
Covalent network:
Any two of very hard; very high melting point; crystalline.
The atoms in a covalent network are held together by covalent bonds in all directions. This combination makes the network very strong.
Metal or alloy:
Any two of shiny; ductile; malleable; conductors of heat and electricity; crystalline.
The atoms in a metal or alloy are held together by the electrostatic attraction of all the nuclei for the freely moving electrons. The stationary nuclei determine the crystalline structure, and the freedom of movement of the electrons contributes to the other properties.
Amorphous solid:
Any two of noncrystalline, no sharp melting point, possibly fluid, rounded instead of sharp edges when shattered.
These properties are accounted for by the fact that the interparticle forces in amorphous solids vary greatly, but are not usually very strong.
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