* Chlorine's Valence Electrons: Chlorine has 7 valence electrons in its outer shell (3s² 3p⁵).
* Octet Rule: Atoms tend to gain, lose, or share electrons to achieve a stable octet (8 electrons) in their outer shell.
* Chlorine's Bonding: Chlorine typically forms one covalent bond, sharing one of its valence electrons to complete its octet.
Let's break down the question and address the key concepts:
* Covalent Bonds: These involve the sharing of electron pairs between atoms.
* Degenerate Orbitals: These are orbitals within the same subshell that have the same energy level. For example, the three 2p orbitals in a given atom are degenerate.
To answer the prompt, we need to consider how chlorine's orbitals are involved in bonding:
1. Ground State: In its ground state, chlorine has one unpaired electron in a 3p orbital.
2. Hybridization: When chlorine forms a covalent bond, it doesn't actually use five orbitals. Hybridization (mixing atomic orbitals) can occur, but that's not the case with chlorine's usual bonding behavior.
3. One Covalent Bond: Chlorine typically forms only one covalent bond, using its lone unpaired electron in a 3p orbital.
Therefore, chlorine only needs one degenerate orbital (a 3p orbital) to participate in a single covalent bond.
