Molecular compounds

Definition

Molecular compounds consist of molecules formed by atoms of two or more different nonmetals sharing electrons through covalent bonds. They typically have low melting and boiling points compared to ionic compounds.

5 Must Know Facts For Your Next Test

1. Molecular compounds are generally poor conductors of electricity in any state due to the lack of free ions.
2. They often exist as gases, liquids, or low-melting solids at room temperature.
3. The smallest unit of a molecular compound is a molecule, which retains all the chemical properties of the compound.
4. Common examples include water ($H_2O$), carbon dioxide ($CO_2$), and methane ($CH_4$).
5. Lewis structures and VSEPR theory are commonly used to predict the shape and bonding in molecular compounds.

Review Questions

• What type of bond forms between atoms in a molecular compound?
• Why do molecular compounds generally have lower melting and boiling points than ionic compounds?
• Provide an example of a molecular compound and describe its physical state at room temperature.

Related terms

Covalent Bond:

A chemical bond formed when two atoms share one or more pairs of electrons.

Ionic Compound: A compound composed of positive and negative ions held together by electrostatic forces known as ionic bonds.

Lewis Structure:

A diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons that may exist in the molecule.