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
1 댓글
검증된 단계별 안내
1
Begin by understanding the properties of different types of solids. Ionic solids are typically hard and have high melting points, but they conduct electricity when molten or dissolved in water. Metallic solids conduct electricity due to the presence of free electrons.
Consider molecular solids, which are generally softer and have lower melting points compared to ionic and covalent network solids. They do not conduct electricity because they lack free-moving charged particles.
Covalent network solids are characterized by their hardness and high melting points due to the strong covalent bonds throughout the structure. They do not conduct electricity because they lack free electrons or ions.
Analyze the given properties of Compound A: it is hard, does not conduct electricity, and has a high melting point of 1400ºC. These properties align with those of covalent network solids.
Conclude that Compound A is most likely a covalent network solid, as it matches the described characteristics of hardness, non-conductivity, and high melting point.