Carbon compounds with only single bonds between carbon atoms are termed saturated, while those with double or triple bonds are referred to as unsaturated. The nature of bonding influences the properties of these compounds.

Carbon’s ability to form bonds with other carbon atoms, known as catenation, enables the formation of long chains, branched structures, or rings in carbon compounds. This property contributes to the vast diversity of carbon compounds.

Covalently bonded molecules have strong intramolecular bonds but weak intermolecular forces, resulting in low melting and boiling points. Since no charged particles are formed, these compounds are generally poor conductors of electricity.

Methane (CH₄) is formed by carbon sharing its four valence electrons with four hydrogen atoms, forming covalent bonds. The molecule lacks charged particles, contributing to its low melting and boiling points.

The electron dot structure of NH₃ shows that each hydrogen atom shares electrons with nitrogen, forming single covalent bonds and allowing all four atoms to attain stable noble gas configurations.