Which of the following statements correctly describes the Lewis dot structure of the PF_6^- ion?

• A. Phosphorus is surrounded by five fluorine atoms, each forming a single bond, and phosphorus has one lone pair.
• B. Phosphorus is surrounded by six fluorine atoms, each forming a single bond, and each fluorine has two lone pairs.
• C. Phosphorus is surrounded by six fluorine atoms, each forming a single bond, and phosphorus has no lone pairs.
• D. Phosphorus is surrounded by six fluorine atoms, each forming a double bond, and phosphorus has one lone pair.

Answer: (C)

Verified step by step guidance

1. Identify the central atom and the surrounding atoms in the PF_6^- ion. Here, phosphorus (P) is the central atom, and it is surrounded by six fluorine (F) atoms.
2. Determine the total number of valence electrons available. Phosphorus has 5 valence electrons, each fluorine has 7 valence electrons, and there is an extra electron due to the negative charge, so total electrons = 5 + (6 × 7) + 1.
3. Distribute the electrons to form bonds between phosphorus and each fluorine atom. Since there are six fluorines, form six single bonds, each bond consisting of 2 electrons.
4. Assign the remaining electrons as lone pairs on the fluorine atoms to complete their octets. Each fluorine should have three lone pairs (6 electrons) after bonding.
5. Check the phosphorus atom's electron count. With six single bonds, phosphorus has 12 electrons around it, which is allowed as an expanded octet. Therefore, phosphorus has no lone pairs in this structure.