Question

select the lewis structure that most accurately represents sulfur hexafluoride (sf₆). refer to a periodic table.

Explanation:

Step1: Determine valence electrons

Sulfur (S) is in group 16, so it has 6 valence electrons. Fluorine (F) is in group 17, so each F has 7 valence electrons. For \( SF_6 \), total valence electrons: \( 6 + 6\times7 = 6 + 42 = 48 \).

Step2: Analyze bonding and octets

Fluorine follows the octet rule (needs 8 electrons, 7 valence + 1 from bond). Sulfur can expand its octet (has empty d - orbitals). In \( SF_6 \), S is bonded to 6 F atoms. Each F - S bond is a single bond (since F only needs 1 more electron to complete octet, and S can form 6 single bonds here).

Looking at the structures:

• The first and third structures have a central F (incorrect, central atom should be S).
• The fourth structure has double bonds, but F doesn't form double bonds (it only needs 1 bond to complete octet).
• The second structure has S as the central atom, bonded to 6 F atoms (each single bond), and each F has 3 lone pairs (completing octet), and S has 6 bonding pairs (no lone pairs, which is allowed as S expands its octet here).

Answer:

The Lewis structure with S as the central atom, bonded to 6 F atoms (each with 3 lone pairs) (the second structure in the given options).