Final answer:
During the formation of a bond, orbitals synchronize their phases by combining to form bonding and antibonding molecular orbitals. In-phase combinations form bonding orbitals that stabilize a molecule, while out-of-phase combinations form antibonding orbitals that make a molecule less stable. The interaction between atomic orbitals is greatest when they have the same energy.
Step-by-step explanation:
The synchronization of phases in the formation of a bond occurs through the combination of atomic orbitals to form molecular orbitals.
When two atomic orbitals combine, two types of molecular orbitals are formed: bonding and antibonding orbitals. Bonding orbitals are formed by the in-phase combination of atomic orbitals, while antibonding orbitals result from the out-of-phase combination.
For example, when two p orbitals combine in a side-by-side overlap, they form two π molecular orbitals. The out-of-phase combination results in an antibonding molecular orbital with two nodal planes, while the in-phase combination forms a bonding orbital with a node along the internuclear axis and lobes above and below the axis.
The synchronization of phases in the formation of a bond is important because electrons in bonding orbitals stabilize a molecule, while electrons in antibonding orbitals make a molecule less stable. The interaction between atomic orbitals is greatest when they have the same energy.