How many covalent bonds can a carbon atom form?

A carbon atom can form four covalent bonds.

This ability stems from carbon's electronic configuration. It has four valence electrons in its outermost shell. To achieve a stable octet (8 electrons in its outermost shell, similar to noble gases), carbon needs to gain, lose, or share four electrons. The most energetically favorable way for carbon to achieve this stability is by sharing electrons through covalent bonding.

Here's a breakdown:

• Valence Electrons: Carbon has four valence electrons.
• Octet Rule: Atoms tend to form bonds to achieve a full outer electron shell, typically with eight electrons (octet rule).
• Covalent Bonds: Carbon achieves its octet by sharing its four valence electrons with other atoms, forming four covalent bonds.

Examples of molecules where carbon forms four covalent bonds include:

• Methane (CH₄): Carbon forms four single bonds with four hydrogen atoms.
• Carbon Dioxide (CO₂): Carbon forms two double bonds with two oxygen atoms.
• Ethyne (C₂H₂): Each carbon forms one single bond with a hydrogen atom and one triple bond with the other carbon atom.

Therefore, the versatile bonding nature of carbon is fundamental to the vast diversity of organic compounds.