What is the molecular geometry of SF2? up-side-down bent tetrahedral linear
The Correct Answer and Explanation is:
The correct molecular geometry of SF₂ (sulfur difluoride) is bent.
Explanation:
Sulfur difluoride (SF₂) is a covalent compound made of one sulfur atom and two fluorine atoms. To determine its molecular geometry, we apply Valence Shell Electron Pair Repulsion (VSEPR) theory, which helps predict molecular shape based on electron pair repulsion.
- Step 1: Count valence electrons
- Sulfur (S) has 6 valence electrons.
- Each fluorine (F) has 7 valence electrons.
- Total valence electrons = 6 (from S) + 2 × 7 (from 2 F atoms) = 20 electrons.
- Step 2: Draw Lewis structure
- Place sulfur in the center.
- Attach two fluorine atoms with single bonds. Each S–F bond uses 2 electrons, so 4 electrons are used.
- Distribute the remaining 16 electrons to satisfy the octets. Each fluorine gets 6 electrons to complete its octet.
- After fluorines are satisfied, 4 electrons remain, which go to sulfur as two lone pairs.
- Step 3: Determine electron domains around sulfur
Sulfur has:- 2 bonding pairs (from S–F bonds)
- 2 lone pairs
Total = 4 electron domains
- Step 4: Determine molecular geometry
- With 4 domains, the electron geometry is tetrahedral.
- However, because two of the domains are lone pairs, the actual molecular geometry is bent.
The lone pairs repel more strongly than bonding pairs, forcing the fluorine atoms to move closer together. This results in a bond angle of less than 109.5°, typically around 98° for SF₂.
Common Misconceptions:
- It is not linear because there are lone pairs on sulfur.
- It is not a perfect tetrahedron due to lone pair repulsion.
- It may appear “upside-down bent” visually, but the correct term is simply bent.
Therefore, bent is the scientifically accurate and accepted name for SF₂’s molecular geometry.
