When sulfur forms compounds such as SF6, how does it relate to the octet rule?

• A. Sulfur strictly follows the octet rule and never has more than eight electrons in its valence shell.
• B. Sulfur always forms compounds by sharing exactly eight electrons with other atoms.
• C. Sulfur loses all its valence electrons to achieve a stable configuration.
• D. Sulfur can expand its valence shell to accommodate more than eight electrons, thus violating the octet rule.

Answer: (D)

Verified step by step guidance

1. Recall the octet rule, which states that atoms tend to form bonds until they are surrounded by eight electrons in their valence shell, achieving a noble gas configuration.
2. Recognize that sulfur is in period 3 of the periodic table, meaning it has access to d orbitals in addition to s and p orbitals in its valence shell.
3. Understand that because of these available d orbitals, sulfur can expand its valence shell beyond eight electrons when forming compounds, such as SF6, where sulfur is surrounded by 12 valence electrons.
4. Note that this ability to have more than eight electrons is called an expanded octet and is common for elements in period 3 and beyond.
5. Conclude that sulfur does not strictly follow the octet rule in compounds like SF6, but instead expands its valence shell to accommodate more electrons, allowing it to form stable compounds with more than eight electrons around it.