Final answer:
A carbon atom typically forms four covalent bonds, as it has four valence electrons that it can share with other atoms to achieve a stable octet.
Step-by-step explanation:
A carbon atom typically forms four covalent bonds. This is due to carbon having four electrons in its valence shell, and it needs to attain a full octet for stability. Through covalent bonding, carbon can achieve this by sharing its four valence electrons with other atoms.
For example, in a molecule of carbon dioxide (O=C=O), one carbon atom forms two double covalent bonds with two oxygen atoms, utilizing four electrons, two from carbon and two from each oxygen, to create the stable molecule.
Moreover, the valence electron configuration of carbon is 2s²2p², which indicates the presence of four valence electrons available for bonding. This allows carbon to form various types of bonds, including single, double, and even triple bonds, as long as the total number of covalent bonds amounts to four.