Which of the following statements correctly describes the Lewis dot structure of the SF5Cl molecule?

• A. Sulfur is surrounded by four electron pairs, with three fluorine atoms and one chlorine atom bonded to it.
• B. Sulfur is surrounded by five electron pairs, with four fluorine atoms and one chlorine atom bonded to it.
• C. Sulfur is surrounded by six electron pairs, with five fluorine atoms and one chlorine atom bonded to it.
• D. Sulfur is surrounded by six electron pairs, with four fluorine atoms and two chlorine atoms bonded to it.

Answer: (C)

Verified step by step guidance

1. Step 1: Identify the central atom and the total number of valence electrons. Sulfur (S) is the central atom. Sulfur has 6 valence electrons, each fluorine (F) has 7 valence electrons, and chlorine (Cl) has 7 valence electrons. For SF5Cl, calculate the total valence electrons by adding these contributions.
2. Step 2: Determine the number of atoms bonded to sulfur. The formula SF5Cl indicates sulfur is bonded to 5 fluorine atoms and 1 chlorine atom, making a total of 6 atoms bonded to sulfur.
3. Step 3: Use the total valence electrons to draw the Lewis structure. Each bond between sulfur and a halogen atom (F or Cl) represents a pair of shared electrons. Assign bonding pairs accordingly and then distribute remaining electrons as lone pairs to satisfy the octet rule where possible.
4. Step 4: Count the electron pairs around sulfur. Since sulfur is bonded to 6 atoms, it will have 6 bonding pairs. Check if sulfur can expand its octet to accommodate these bonds, which it can because it is in period 3 and has d orbitals available.
5. Step 5: Conclude the correct description. Sulfur is surrounded by six electron pairs (all bonding pairs) with five fluorine atoms and one chlorine atom bonded to it, matching the statement that sulfur has six electron pairs with five fluorines and one chlorine bonded.