Here's a breakdown of the key characteristics:

* Binary: The compound is composed of only two elements.

* Molecular: The elements are held together by covalent bonds, where atoms share electrons.

* Nonmetals: Both elements involved are classified as nonmetals. This is a key distinction from ionic compounds, which are formed from a metal and a nonmetal.

Examples of binary molecular compounds:

* Carbon dioxide (CO₂): Carbon and oxygen are both nonmetals.

* Water (H₂O): Hydrogen and oxygen are both nonmetals.

* Ammonia (NH₃): Nitrogen and hydrogen are both nonmetals.

* Methane (CH₄): Carbon and hydrogen are both nonmetals.

Key features of binary molecular compounds:

* Low melting and boiling points: Compared to ionic compounds, they have weaker intermolecular forces.

* Often gases or liquids at room temperature: Their weak bonds make them more likely to exist in these phases.

* Poor conductors of electricity: Covalent bonds do not readily allow for the movement of charge.

Note: While the vast majority of binary molecular compounds are formed from two nonmetals, there are exceptions. Some compounds with a metalloid (like boron) and a nonmetal can also be classified as molecular compounds.