Question

1 mark for review which of the following correctly indicates whether the solid represented by the particulate model shown above conducts electricity and explains why or why not? a it conducts electricity because it is made of positive and negative ions. b it conducts electricity because it is made of particles of different sizes. c it does not conduct electricity because its ions cannot move freely within the solid. d it does not conduct electricity because there are small spaces between the particles.

Explanation:

Step1: Recall the condition for electrical conductivity

For a substance to conduct electricity, there must be free - moving charged particles. In ionic solids, the ions are in fixed positions in the lattice structure.

Step2: Analyze each option

• Option A: Just having positive and negative ions is not sufficient. The ions must be able to move. In a solid ionic lattice, ions are fixed, so this is incorrect.
• Option B: Particle size has no relation to electrical conductivity in this context. Electrical conductivity in ionic substances depends on ion mobility, not particle size. So this is incorrect.
• Option C: In an ionic solid, the ions are held in a fixed lattice structure. They cannot move freely. Since electrical conductivity requires the movement of charged particles (in this case, ions), an ionic solid does not conduct electricity. This is correct.
• Option D: The presence of small spaces between particles is not the reason for lack of electrical conductivity. The key is the absence of free - moving ions. So this is incorrect.

Answer:

C. It does not conduct electricity because its ions cannot move freely within the solid.