Questions: Choose the best Lewis structure for SF4.

Transcript text: Choose the best Lewis structure for $\mathrm{SF}_{4}$.

Solution

Solution Steps

Step 1: Determine the total number of valence electrons

Sulfur (S) has 6 valence electrons, and each Fluorine (F) has 7 valence electrons. Since there are 4 Fluorine atoms, the total number of valence electrons is: \[ 6 + (4 \times 7) = 6 + 28 = 34 \]

Step 2: Draw the skeletal structure

Place Sulfur (S) in the center and arrange the four Fluorine (F) atoms around it. Connect each Fluorine to the Sulfur with a single bond.

Step 3: Distribute the remaining electrons

Each single bond uses 2 electrons, so 4 bonds use $4 \times 2 = 8$ electrons. Subtract these from the total valence electrons: \[ 34 - 8 = 26 \] Distribute the remaining 26 electrons to complete the octets of the Fluorine atoms. Each Fluorine needs 6 more electrons to complete its octet (since each already has 2 from the bond): \[ 4 \times 6 = 24 \] This leaves 2 electrons, which are placed as a lone pair on the Sulfur atom.

Final Answer

The best Lewis structure for SF₄ is the one where Sulfur has one lone pair and forms single bonds with each of the four Fluorine atoms, each Fluorine having three lone pairs. This corresponds to the third structure in the image.

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