Which of the following best describes why ionic compounds like potassium bromide (KBr) do NOT conduct electricity in solid form but do in molten form?

Correct option is C

​Correct option : (c),  Ionic bonds prevent ion movement in solid KBr.

Ionic compounds like potassium bromide (KBr) do not conduct electricity in solid form, but do conduct electricity in molten form because of the following reasons:

• ​In Solid Form:
  

1. ​In solid KBr, the potassium (K⁺) and bromide (Br⁻) ions are held together in a rigid, structured lattice.
2. The ions are not free to move because they are tightly bound in the solid crystal structure.
   
3. Since electrical conduction requires the movement of charged particles, the lack of mobility of the ions in solid KBr means it cannot conduct electricity.
   

• In Molten Form​:

1. ​When KBr is heated and becomes molten (liquid), the ionic lattice breaks down.
2. ions (K⁺ and Br⁻) are free to moveThe in the liquid state.
3. The mobility of these ions allows the conduction of electricity, as they can carry charge through the liquid when an external electric field is applied.

Conclusion : 

Ionic compounds like KBr do not conduct electricity in solid form because the ions are not free to move, but do conduct electricity in molten form because the ions are free to move and carry charge.​