VSEPR theory examples

📚 Quick Study Guide

• ⚛️ VSEPR theory (Valence Shell Electron Pair Repulsion) predicts the geometry of molecules based on minimizing the repulsion between electron pairs around a central atom.
• 🌐 Electron pairs can be bonding pairs (shared in a covalent bond) or lone pairs (non-bonding).
• 📐 The basic geometries are linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral.
• ✍️ To determine the shape: Count the number of bonding pairs and lone pairs around the central atom.
• 💡 Use the following table to determine molecular geometry based on electron pair geometry and number of lone pairs:

🧪 Practice Quiz

1. Which of the following molecules is linear according to VSEPR theory?
   1. $H_2O$
   2. $CO_2$
   3. $NH_3$
   4. $BF_3$
2. What is the molecular geometry of $SF_4$?
   1. Tetrahedral
   2. See-saw
   3. Square planar
   4. Trigonal pyramidal
3. What is the bond angle in a tetrahedral molecule?
   1. 90°
   2. 109.5°
   3. 120°
   4. 180°
4. Which of the following molecules has a trigonal pyramidal shape?
   1. $BF_3$
   2. $CH_4$
   3. $NH_3$
   4. $H_2O$
5. What is the molecular geometry of $XeF_4$?
   1. Tetrahedral
   2. Square pyramidal
   3. Square planar
   4. See-saw
6. How many lone pairs are present on the central atom in $H_2O$?
   1. 0
   2. 1
   3. 2
   4. 3
7. What is the electron pair geometry of $PCl_5$?
   1. Tetrahedral
   2. Octahedral
   3. Trigonal bipyramidal
   4. Trigonal planar