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6. explain the relative conductivities of the different solutions of a) iodine, b) graphite, c) sodium chloride
Accepted Answer
Here's a breakdown of the relative conductivities of the solutions you mentioned:
a) Iodine (I₂)
Poor conductor: Iodine is a nonpolar covalent molecule and does not dissociate into ions when dissolved in water. Since the movement of ions is the basis of electrical conductivity in solutions, iodine solutions are poor conductors.
b) Graphite
Good conductor: Graphite is a form of carbon with a layered structure. Within each layer, electrons are delocalized, allowing for free movement of charge. This makes graphite a good electrical conductor, even in solid form. Graphite can be dispersed in certain solvents, but this dispersion would not significantly alter its conductive properties.
c) Sodium Chloride (NaCl)
Excellent conductor: Sodium chloride is an ionic compound that readily dissociates into Na+ and Cl- ions when dissolved in water. The presence of these freely moving ions makes sodium chloride solutions excellent electrical conductors.
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