Which of the following elements typically forms a Lewis structure with two lone pairs of electrons?

• A. Germanium (Ge)
• B. Sulfur (S)
• C. Iodine (I)
• D. Calcium (Ca)

Answer: (B)

Verified step by step guidance

1. Understand the concept of Lewis structures: Lewis structures are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.
2. Identify the typical electron configuration for each element: Sulfur (S) is in group 16 of the periodic table, which means it has six valence electrons. Germanium (Ge) is in group 14, Iodine (I) is in group 17, and Calcium (Ca) is in group 2.
3. Determine the number of lone pairs: Elements in group 16, like Sulfur, typically form two lone pairs because they have six valence electrons and often form two bonds, using four electrons for bonding and leaving four electrons as two lone pairs.
4. Consider the bonding preferences: Sulfur often forms two bonds, such as in H₂S, where it uses two electrons for bonding and retains four electrons as two lone pairs.
5. Compare with other elements: Germanium typically forms four bonds with no lone pairs, Iodine can form one bond with three lone pairs, and Calcium typically forms two bonds with no lone pairs as it loses its two valence electrons.