Which of the following statements correctly describes the Lewis dot structure of the neutral compound SiF_2?

• A. Si is the central atom with two single bonds to F atoms, and no lone pairs on Si.
• B. Si is the central atom with two double bonds to F atoms, and no lone pairs on Si.
• C. F is the central atom with single bonds to two Si atoms, and each F has three lone pairs.
• D. Si is the central atom with two single bonds to F atoms, and Si has one lone pair.

Answer: (D)

Verified step by step guidance

1. Identify the total number of valence electrons for the molecule SiF_2. Silicon (Si) has 4 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are two fluorine atoms, calculate the total as: \$4 + 2 \times 7 = 18$ valence electrons.
2. Determine the central atom. Silicon is less electronegative than fluorine, so Si will be the central atom with the two fluorine atoms bonded to it.
3. Draw single bonds between the central Si atom and each F atom. Each single bond represents 2 electrons, so 2 bonds use \$2 \times 2 = 4$ electrons.
4. Distribute the remaining electrons to satisfy the octet rule. Place lone pairs on the fluorine atoms first to complete their octets (each F needs 6 more electrons as lone pairs), then place any leftover electrons as lone pairs on the silicon atom.
5. Check the formal charges and the octet rule for each atom. The correct Lewis structure will have Si as the central atom bonded to two F atoms with single bonds, and Si will have one lone pair to complete its octet, matching the given correct answer.