Simple molecular compounds are made up of only a few atoms held together by covalent bonds. An example of a simple molecular compound is carbon dioxide (CO₂), which consists of one carbon atom bonded to two oxygen atoms. Despite the strong covalent bonds within a simple molecule, the intermolecular forces between these molecules are weak.
Properties of Simple Molecular Compounds
Simple molecular compounds have several distinctive properties:
- Low melting and boiling points: These compounds require little energy to break the weak intermolecular forces.
- Lack of conductivity: Simple molecular compounds do not conduct electricity due to the absence of free electrons or an overall charge.
- Examples of simple molecules include hydrogen, ammonia, methane, and pure water. They all have strong covalent bonds within their atoms but much weaker intermolecular forces between molecules.
When these substances melt or boil, it is the weak intermolecular forces that break, rather than the strong covalent bonds. As a result, simple molecular substances exist as gases, liquids, or solids with low melting and boiling points at room temperature.
Intermolecular Forces in Simple Molecules
The weak intermolecular forces within simple molecular compounds are responsible for their low melting and boiling points. It is the breaking of these forces that allows simple molecular substances to transition from one state to another.
Examples of Intermolecular Forces
Examples of simple molecular compounds with weak intermolecular forces include carbon dioxide, water, ammonia, and methane. These substances exhibit low melting and boiling points due to the weak attractions between their molecules.
In summary, simple molecular compounds are characterized by their strong covalent bonds and weak intermolecular forces, resulting in low melting and boiling points and a lack of electrical conductivity. These properties make them exist as gases, liquids, or solids with low melting and boiling points at room temperature.
