Chemical Bonding & Molecular Structure I VSEPR Theory (Part-1) II NEET II JEE II Concise notes 👇👇

#VSERP # shapes #chemicalbondingandmolecularstructure Concise Notes: Here are the basic concepts from VSEPR theory (Valence Shell Electron Pair Repulsion theory) that are important for the NEET exam: 🔹 1. What is VSEPR Theory? Developed to predict the 3D shapes of molecules based on electron pair repulsions. The shape of a molecule depends on the repulsions between electron pairs (bonded and lone pairs) around the central atom. 🔹 2. Key Postulates of VSEPR Theory Electron pairs (bond pairs and lone pairs) around a central atom repel each other and try to stay as far apart as possible. Lone pair–lone pair .... lone pair–bond pair.....bond pair–bond pair in terms of repulsive strength. The shape of a molecule is determined by minimizing these repulsions. 🔹 3. Types of Electron Pairs Bond pairs: Shared between two atoms. Lone pairs: Not shared; remain on the central atom. 🔹 5. Influence of Lone Pairs Lone pairs distort shapes and reduce bond angles due to stronger repulsion. More lone pairs = more deviation from ideal geometry. 🔹 6. Multiple Bonds Double/triple bonds count as one region of electron density, not multiple. 🔹 7. Limitations Doesn’t explain bond length, bond strength, or exact angles—just predicts shape. ✅ Tips for NEET Memorize common shapes and angles. Practice drawing Lewis structures to determine electron pairs. Be careful with lone pairs—they affect geometry significantly.