Which of the following statements correctly describes the Lewis dot structure of PSF3 (phosphorus sulfur trifluoride)?

• A. Phosphorus is the central atom, bonded to three sulfur atoms and one fluorine atom, with one lone pair on phosphorus.
• B. Sulfur is the central atom, bonded to three fluorine atoms and one phosphorus atom, with one lone pair on sulfur.
• C. Phosphorus is the central atom, bonded to one sulfur atom and three fluorine atoms, with no lone pairs on phosphorus.
• D. Fluorine is the central atom, bonded to one phosphorus atom and one sulfur atom, with two lone pairs on fluorine.

Answer: (C)

Verified step by step guidance

1. Identify the central atom in PSF3 by considering electronegativity and bonding capacity. Typically, the least electronegative atom that can form multiple bonds is the central atom. Between phosphorus (P), sulfur (S), and fluorine (F), phosphorus is less electronegative and can form more bonds, so it is usually the central atom.
2. Determine the number of valence electrons for each atom: phosphorus has 5, sulfur has 6, and fluorine has 7 valence electrons. Calculate the total valence electrons available for bonding in PSF3 by adding these values considering the number of each atom.
3. Arrange the atoms with phosphorus in the center, bonded to one sulfur atom and three fluorine atoms. Draw single bonds between phosphorus and each of these atoms initially.
4. Distribute the remaining valence electrons to satisfy the octet rule for the surrounding atoms first (fluorine and sulfur), placing lone pairs as needed. Then check the central atom phosphorus to see if it has a complete octet or if any lone pairs remain.
5. Verify the Lewis structure by counting all electrons around each atom to ensure the octet rule is satisfied (or expanded octet for phosphorus if applicable) and confirm that the structure matches the description: phosphorus bonded to one sulfur and three fluorines, with no lone pairs on phosphorus.