Question

1. a sample of a hard, solid binary compound at room temperature did not conduct electricity as a pure solid but became highly conductive when dissolved in water. which of the following types of interactions is most likely found between the particles in the substance? (a) ionic bonds (b) metallic bonds (c) covalent bonds (d) hydrogen bonds

Explanation:

Ionic compounds are hard solids at room temperature. In the pure solid state, ions are fixed in the lattice structure, so there are no free - moving charge carriers, and they do not conduct electricity. When dissolved in water, the ionic lattice breaks down, and ions become free to move, enabling electrical conductivity. Covalent compounds (in the form of simple molecules) are usually gases, liquids or soft solids at room temperature (except for giant covalent structures like diamond and silicon dioxide). Metallic bonds are in metals, which are good conductors in the solid state. Hydrogen bonds are a type of intermolecular force and do not form binary compounds with the described conductivity properties.

Answer:

A. Ionic bonds