Final answer:
Covalent solutes commonly have low boiling points, are poor conductors of electricity, and typically do not dissolve well in water due to the way atoms share valence electrons, forming weaker intermolecular forces compared to ionic compounds.
Step-by-step explanation:
Covalent solutes have distinct properties that are attributable to the covalent bonds holding together nonmetallic elements within them. These shared pairs of valence electrons impart characteristic physical attributes to the compounds formed. One notable property common to covalent solutes is that they have relatively low boiling points; they do not require a substantial amount of energy to separate their individual molecules because they are held together by weaker intermolecular forces compared to ionic compounds.
Being poor conductors of electricity in both solid and dissolved states is another shared property among covalent solutes. This is due to the lack of free-moving ions within these compounds. Most covalent compounds are typically poor at dissolving in water, rendering them non-electrolytes because they do not dissociate into ions when dissolved.
The formation of a covalent bond, as observed in a hydrogen molecule (H₂), occurs when two nonmetal atoms come together and their potential energy reaches a minimum at a certain interatomic distance. This bond length represents the optimal point of electron sharing and mutual nuclear attraction, resulting in structural stability and distinct covalent compound properties.