How many single bonds are present in the Lewis dot structure of germanium disulfide (GeS2)?

• A. 3
• B. 2
• C. 1
• D. 0

Answer: (B)

Verified step by step guidance

1. Identify the central atom and the surrounding atoms in the molecule GeS2. Germanium (Ge) is the central atom, and sulfur (S) atoms are the surrounding atoms.
2. Determine the total number of valence electrons available for bonding. Germanium is in group 14 and has 4 valence electrons, and each sulfur atom is in group 16 with 6 valence electrons. So, total valence electrons = 4 (Ge) + 2 × 6 (S) = 16 electrons.
3. Draw a skeletal structure with Ge in the center bonded to two S atoms. Connect Ge to each S with a single bond initially, which uses 2 electrons per bond.
4. Complete the octets of the sulfur atoms by adding lone pairs around each sulfur atom until they have 8 electrons total (including bonding electrons).
5. Check if the central atom (Ge) has a complete octet. If not, consider forming double bonds by sharing lone pairs from sulfur atoms with germanium. In GeS2, each Ge-S bond is a double bond, so there are no single bonds present.