Final answer:
From the options provided, Chlorine (Cl) cannot expand its valence shell as it follows the octet rule, while Phosphorus (P) and Sulfur (S) are both capable of expanding their valence shells because they have available d orbitals in the third period. Hydrogen (H) follows the duet rule and cannot expand its valence shell.
Step-by-step explanation:
The atoms that can expand their valence shell when bonding include elements in the third period of the periodic table or higher, as they have empty d orbitals that can be utilized. Specifically, from the options provided:
- B) Chlorine (Cl) cannot expand its valance shell as it is from the second period and follows the octet rule.
- C) Phosphorus (P) can expand its valence shell because it is in the third period and has d orbitals that can accommodate extra electrons.
- D) Sulfur (S) can also expand its valence shell due to the presence of d orbitals in the third period.
However, A) Hydrogen (H) cannot expand its valence shell as it only requires two electrons in its 1s subshell to be stable, following the duet rule rather than the octet rule.