Question

Sodium metal and sodium chloride are both solid at room temperature. Using details of their bonding and structure, explain why as a solid, sodium metal conducts electricity whereas sodium chloride does not.

a. Sodium metal has a metallic lattice allowing free electron movement.
b. Sodium chloride has covalent bonds restricting electron flow.
c. Sodium metal forms an ionic lattice facilitating electron mobility.
d. Sodium chloride has a crystalline structure preventing electrical conduction.

Answer 1

Sodium metal conducts electricity due to its metallic lattice structure, while sodium chloride does not due to its ionic lattice structure.

Step-by-step explanation:

Sodium metal and sodium chloride are both solid at room temperature. However, sodium metal conducts electricity while sodium chloride does not. This is because sodium metal has a metallic lattice structure, which allows for the movement of free electrons. On the other hand, sodium chloride has an ionic lattice structure, where the positively charged sodium ions and negatively charged chloride ions are held together by strong electrostatic attractions. As a result, the ions in sodium chloride cannot move freely and the solid cannot conduct electricity.