The way compounds are structured at the atomic level can really change how well they conduct electricity. Here’s a simple breakdown of how different types of compounds behave:

1. Ionic Compounds:

   • These are made up of charged particles called ions.
   • They are good at conducting electricity when they are either dissolved in water or melted.
   • For example, table salt, known as sodium chloride (NaCl), conducts electricity well when mixed in water. Its conductivity measures about 10 mS/cm in a watery solution.

2. Covalent Compounds:

   • These types of compounds usually do not conduct electricity because they don’t have any free-moving charged particles.
   • A common example is glucose, which is a type of sugar (C₆H₁₂O₆). It has a very low conductivity of about 0.1 mS/cm because it doesn’t form ions.

3. Metallic Compounds:

   • These compounds have electrons that can move around freely, which makes them great conductors.
   • A great example is copper (Cu), which has one of the highest conductivities, measuring about 5.8 x 10^7 S/m.

In summary, how well a compound can conduct electricity depends a lot on its molecular structure. Ionic and metallic compounds are generally good conductors, while covalent compounds aren’t.