Multiple Choice
Which one of the following substances crystallizes in a metallic lattice?
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13. Liquids, Solids & Intermolecular Forces
Atomic, Ionic, and Molecular Solids
Multiple Choice
Compound A is hard, doesn't conduct electricity, and melts at 1400ºC. Compound A represents which of the following:
A
Ionic solid
B
Metallic solid
C
Molecular solid
D
Covalent Network solid
Verified step by step guidance1
Identify the properties of Compound A: it is hard, does not conduct electricity, and has a high melting point of 1400ºC.
Recall the characteristics of different types of solids: Ionic solids are typically hard and have high melting points but conduct electricity when molten or dissolved in water. Metallic solids conduct electricity and are malleable. Molecular solids have lower melting points and are often softer.
Consider the properties of covalent network solids: they are very hard, have high melting points, and do not conduct electricity. Examples include diamond and quartz.
Compare the properties of Compound A with those of covalent network solids: both are hard, have high melting points, and do not conduct electricity.
Conclude that based on the properties, Compound A is best described as a covalent network solid.
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