The solutions of some molecular compounds are good conductors of electricity. explain how this can be true when ions are required to conduct electricity

Explanation:

Ionic compounds are compounds that have cations and anions.

A polar molecule is one that is neutral, that is, it does not have a net charge. But it has an internal distribution of charges that form a partially positive region and a partially negative region.

Given that "the like dissolves the like" and that water is a polar molecule, it is possible to say that water is good for dissolving ions and polar molecules, but bad for dissolving non-polar molecules.

Water molecules are polar, with positive partial charges on hydrogen, a partial negative charge on oxygen and a general angular structure. Its distribution of charges is due to the greater electronegativity of oxygen with respect to hydrogen, which makes the shared electrons of the O-H bonds more attracted by the O atom than by the H atom.

As an ionic compound mixes in water, charged water molecules break up the charged compound molecules, which combine into a weaker ionic bond. Then the compound dissociates in water in cations and anions. The positively charged ions are surrounded by the negative partial oxygen charges of the water molecules, while the negatively charged ions are surrounded by the ends of the positively charged hydrogen. Given this, it can be said that the intermolecular forces that are acting in this case are the ion-dipole forces (intermolecular force that occurs when the ions of a substance interact with the dipoles of a polar covalent molecule). This allows the ionic compound to dissolve easily in water.

These dissolved ions are the ones that will conduct the electricity. Because the electric current is transported by means of ions in solution, the conductivity increases when the ion concentration increases.

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