Determine the molecular geometry for the following molecule: FSSF.

• A. Tetrahedral
• B. Bent
• C. Trigonal Planar
• D. Trigonal Pyramidal

Answer: (B)

Verified step by step guidance

1. Step 1: Draw the Lewis structure of FSSF. Count the total valence electrons from each atom: Fluorine (F) has 7 valence electrons, and Sulfur (S) has 6 valence electrons. Add them up for all atoms in the molecule.
2. Step 2: Determine the central atom, which is usually the least electronegative atom that can form multiple bonds. In FSSF, sulfur atoms are central, and fluorine atoms are terminal.
3. Step 3: Arrange the atoms and electrons to satisfy the octet rule for each atom, placing bonding pairs between atoms and distributing remaining electrons as lone pairs on atoms, especially on sulfur and fluorine.
4. Step 4: Count the number of bonding pairs and lone pairs around the central sulfur atom that you are analyzing for molecular geometry. Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the shape based on electron pair repulsions.
5. Step 5: Based on the number of bonding pairs and lone pairs, determine the molecular geometry. For example, if there are two bonding pairs and one or more lone pairs on the central atom, the shape is bent. Confirm this matches the correct answer.