Which of the following best describes the Lewis dot structure of the neutral compound SF_3?

• A. Sulfur is the central atom, bonded to three fluorine atoms with single bonds, and has one lone pair of electrons.
• B. Sulfur is the central atom, bonded to three fluorine atoms with single bonds, and has two lone pairs of electrons.
• C. Sulfur is the central atom, bonded to three fluorine atoms with single bonds, and has no lone pairs.
• D. Sulfur is the central atom, bonded to three fluorine atoms with double bonds, and has no lone pairs.

Answer: (A)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons available for the molecule SF_3. Sulfur (S) is in group 16 and has 6 valence electrons, and each fluorine (F) atom is in group 17 with 7 valence electrons. Since there are three fluorine atoms, calculate the total valence electrons as: \$6 + 3 \times 7$.
2. Step 2: Identify the central atom, which is usually the least electronegative element. In this case, sulfur is the central atom, and the three fluorine atoms will be bonded to it.
3. Step 3: Form single bonds between the sulfur atom and each fluorine atom. Each single bond consists of 2 electrons, so subtract the electrons used in bonding from the total valence electrons.
4. Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule for the fluorine atoms first, since fluorine atoms typically complete their octet with three lone pairs.
5. Step 5: Assign any leftover electrons to the central sulfur atom as lone pairs. Then, determine the number of lone pairs on sulfur by considering the total electrons around it (bonding and nonbonding) to complete its octet or accommodate expanded octet if necessary.