Question

determine the molecular geometry for each molecule. drag the items into the appropriate bins. pcl₃ scl₂ ch₃f cs₂ linear trigonal planar tetrahedral trigonal pyramidal bent

Explanation:

Step1: Analyze \( \text{PCl}_3 \)

Count valence electrons: P (5) + 3×Cl (7) = 26. Lewis structure: P as central, 3 Cl bonds, 1 lone pair. Electron domain: 4 (3 bonds + 1 lone pair). Molecular geometry: Trigonal Pyramidal (lone pair repels, so pyramid shape).

Step2: Analyze \( \text{SCl}_2 \)

Valence electrons: S (6) + 2×Cl (7) = 20. Lewis structure: S central, 2 Cl bonds, 2 lone pairs. Electron domain: 4 (2 bonds + 2 lone pairs). Molecular geometry: Bent (lone pairs push bonds, bent shape).

Step3: Analyze \( \text{CH}_3\text{F} \)

Valence electrons: C (4) + 3×H (1) + F (7) = 14. Lewis structure: C central, 4 single bonds (3 H, 1 F). Electron domain: 4 (4 bonds, no lone pairs). Molecular geometry: Tetrahedral (four bonded atoms, tetrahedron shape).

Step4: Analyze \( \text{CS}_2 \)

Valence electrons: C (4) + 2×S (6) = 16. Lewis structure: C central, 2 double bonds (C=S), no lone pairs. Electron domain: 2 (2 bonds, linear arrangement). Molecular geometry: Linear (two bonded atoms, straight line).

Answer:

• Linear: \( \text{CS}_2 \)
• Trigonal planar: (No molecule here)
• Tetrahedral: \( \text{CH}_3\text{F} \)
• Trigonal Pyramidal: \( \text{PCl}_3 \)
• Bent: \( \text{SCl}_2 \)