Question

select the lewis structure that most accurately represents sulfur difluoride (sf₂). refer to a periodic table.

Explanation:

Step1: Determine valence electrons

Sulfur (S) has 6 valence electrons, and each fluorine (F) has 7. For \( SF_2 \), total valence electrons: \( 6 + 2\times7 = 20 \).

Step2: Analyze bonding and lone pairs

• Sulfur is the central atom. It forms single bonds with two F atoms (2 electrons each, total 4).
• Remaining electrons: \( 20 - 4 = 16 \). These form lone pairs: S has \( \frac{6 - 2}{2}= 2 \) lone pairs (4 electrons), each F has \( \frac{7 - 1}{2}= 3 \) lone pairs (6 electrons each, total \( 2\times6 = 12 \)).
• The structure with S as central, single bonds to two F (each with 3 lone pairs) and S with 2 lone pairs matches the second option (top - right: \( \ddot{F}-S-\ddot{F} \) with S having two lone pairs and each F having three lone pairs).

Answer:

The Lewis structure in the top - right box (the one with central S, single bonds to two F atoms, each F with three lone pairs, and S with two lone pairs: \( \ddot{F}-S-\ddot{F} \) with S having two lone pairs)