Final answer:
Solids with good electrical conductivity usually have metallic bonding, making them capable of efficiently conducting heat and electricity due to a 'sea' of delocalized electrons. Metals like iron, copper, and aluminum exemplify this with their malleability, ductility, and variable melting points depending on electron configurations.
Step-by-step explanation:
The statement that solids with good electrical conductivity have metallic bonding, and thus the correct option is True, is generally accurate. Metallic solids are composed of metal atoms that are held together by a unique type of intermolecular interaction known as metallic bonding. This bonding is characterized by a 'sea' of delocalized valence electrons that are shared among all the atoms in the metal.
These free-moving electrons allow for the efficient transfer of heat and electricity. Metallic solids can be malleable, ductile, and exhibit a shiny luster. Their melting points can vary widely depending on the strength of the metallic bonding, which is influenced by the electron configuration of the metal atoms involved.
For example, we might consider the metals iron, copper, and aluminum—all of which are known for their good electrical and thermal conductivity due to the presence of metallic bonding. Gradient in melting points among these metals can be explained by different electron configurations and varying strengths of metallic bonds.