Final answer:
The carbon atoms in an alkane are connected by single covalent bonds, using sp³ hybrid orbitals for bonding, leading to a zigzag molecular shape.
Step-by-step explanation:
The type of covalent bond that occurs between the carbon atoms of an alkane is a single covalent bond. Alkanes are classified as saturated hydrocarbons because they consist entirely of single bonds and have the maximum number of hydrogen atoms per carbon atom. Each carbon atom in an alkane employs sp³ hybrid orbitals to form four covalent bonds, either with other carbon atoms or with hydrogen atoms. The bond angles around the carbon atoms in alkanes are approximately 109.5°, due to sp³ hybridization, resulting in a zigzag structural shape in longer alkanes.
When depicting alkanes, scientists often use Lewis structures, which do not display the true geometric shape but indicate the bonding relationships. For comprehension, structural formulas such as the ball-and-stick and space-filling models demonstrate the actual geometry of the molecules. As the length of the carbon chain in an alkane increases, so does the boiling point, which is attributed to the enhanced strength of the intermolecular attractive forces.