The correct option is 2 and 3 only.
Explanation
Carbon compounds are predominantly characterized by covalent bonding. Unlike ionic compounds, which are formed by the transfer of electrons and held together by strong electrostatic forces, carbon compounds are formed by the sharing of electrons between atoms.
Statement-wise Analysis:
- Statement 1 is Incorrect.
Carbon compounds generally possess lower melting and boiling points compared to ionic compounds. While the covalent bonds within the molecules are strong, the intermolecular forces of attraction (such as Van der Waals forces) between the molecules are relatively weak. In contrast, ionic compounds are held together by strong electrostatic forces between ions, requiring significantly more energy to break.
- Statement 2 is Correct.
Carbon compounds are largely non-conductors of electricity. Since the bonding involves the sharing of electrons, there are no free ions or free electrons available to conduct electricity in the molten state or in solution. (Note: Graphite is a specific allotrope of carbon that conducts electricity, but typical organic carbon compounds do not).
- Statement 3 is Correct.
Carbon has a tetravalent nature (four valence electrons). It cannot energetically sustain the loss or gain of four electrons to form ionic bonds (C4+ or C4-). Therefore, it attains stability by sharing its valence electrons with other atoms, forming covalent bonds.
Key Takeaway:
Typical carbon compounds are covalent in nature, resulting in weak intermolecular forces (low melting/boiling points) and an absence of free charge carriers (poor electrical conductivity).