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.

Carbon compounds have weak intermolecular forces, reflected in low melting and boiling points compared to ionic compounds. Their poor conductivity is attributed to the absence of ions in their bonding.

With four electrons in its outer shell, carbon aims to achieve noble gas configuration. However, gaining or losing four electrons is impractical due to the difficulty in holding or removing electrons, leading to the absence of ions in carbon compounds.

Carbon’s reactivity is driven by the quest for a filled outer shell. However, forming C⁴⁻ or C⁴⁺ ions is unfavorable due to the challenges associated with holding or removing four electrons, making such ion formation energetically impractical for carbon.