Final answer:
The relationship between these compounds can be determined by considering their properties and the type of elements involved. Substance A is a metallic solid, Substance B is an ionic solid, Substance C is a covalent network solid, and Substance D is a molecular solid.
Step-by-step explanation:
In order to determine the type of bond in a compound, we need to consider the properties of the compounds and the elements involved.
A) Ionic bonds occur between a metal and a nonmetal. These bonds involve the transfer of electrons from the metal atom to the nonmetal atom, resulting in ions that are attracted to each other due to their opposite charges.
B) Covalent bonds occur between two nonmetals. These bonds involve the sharing of electrons between atoms, resulting in a sharing of electron density between the atoms.
C) Metallic bonds occur between metal atoms. These bonds involve a sea of delocalized electrons that are shared among the metal atoms, resulting in a strong bond.
D) Polar bonds occur when there is an unequal sharing of electrons between two atoms due to differences in electronegativity. This creates a partial positive and partial negative charge on the atoms involved.
Using the information provided, we can classify the type of bond in each compound based on their properties:
Substance A: Malleable, ductile, conducts electricity well, and has a melting point of 1135 °C. This suggests that Substance A is a metallic solid.
Substance B: Brittle, does not conduct electricity as a solid but does when molten, and has a melting point of 2072 °C. This suggests that Substance B is an ionic solid.
Substance C: Very hard, does not conduct electricity, and has a melting point of 3440 °C. This suggests that Substance C is a covalent network solid.
Substance D: Soft, does not conduct electricity, and has a melting point of 185 °C. This suggests that Substance D is a molecular solid.