Molecular Orbital Theory (MOT) Explained|Bond Order & MO Diagrams of He₂, N₂,O₂ | Class 11 Chemistry

📘 Class 11 Chemistry – Chapter 3: Chemical Bonding | Molecular Orbital Theory (MOT) with Examples – Helium, Nitrogen, Oxygen | New Book 2025 Welcome to this lecture on Molecular Orbital Theory (MOT), a modern theory that explains bonding, stability, and magnetic properties of molecules better than Valence Bond Theory. In this video, we introduce MOT concepts and solve detailed examples of He₂, N₂, and O₂ molecules using molecular orbital diagrams. This lesson is explained in Urdu + English for crystal clear understanding — perfect for Board Exams, MDCAT, ECAT, and NEET preparation. Molecular Orbital Theory Class 11, MOT diagrams, He₂ N₂ O₂ explained, MO diagram nitrogen, MO diagram oxygen, paramagnetism of oxygen MOT, bond order calculation MOT, Chemical Bonding Class 11, Class 11 Chemistry New Book 2025, Asim Mushtaq Ansari Chemistry, MDCAT NEET Chemistry, Stability of molecules MOT, He₂ molecule unstable, N₂ triple bond explained 🎯 Topics Covered in This Video: • Introduction to Molecular Orbital Theory (MOT). • Difference between Atomic Orbitals vs Molecular Orbitals. • Rules of MOT: Aufbau principle, Pauli’s exclusion principle, Hund’s rule. • Energy ordering of MOs • Worked-out MO diagrams & bond order calculations for: – He₂ molecule – Why it does not exist (bond order = 0). – N₂ molecule – Stable molecule with strong triple bond (bond order = 3). – O₂ molecule – Paramagnetic nature explained by unpaired electrons in π* orbitals (bond order = 2). • MOT applications: predicting stability, bond length, bond strength, and magnetic properties. 🔎 Key Examples Explained in Video 1. He₂ molecule – Total electrons = 4 → filling of σ1s and σ*1s orbitals. – Bond order = (2 – 2) ÷ 2 = 0 → molecule unstable. 2. N₂ molecule – Total electrons = 14 → filling up to σ2px, π2py, π2pz. – Bond order = (8 – 2) ÷ 2 = 3 → stable molecule with triple bond. – Explains N₂ inertness (very strong bond). 3. O₂ molecule – Total electrons = 16 → filling includes π2px, π2py with 2 unpaired electrons. – Bond order = (8 – 4) ÷ 2 = 2 → double bond. – Explains paramagnetism of O₂ (experimentally observed). 🎓 Best For: • Class 11 Chemistry Students (All Boards – Punjab, Federal, etc.) • Students following New Book 2025 syllabus • MDCAT, ECAT, NEET Aspirants • Entry Test MCQs & Conceptual Questions • Board Exams Short/Long Questions 🔗 Useful Playlists – Click to Watch 📘 📚 Full 11th Chemistry Playlist – All Chapters: 👉    • 11 Class Chemistry (New Book 2025) | 11th ...   📗 🧪 Chapter 3 – Chemical Bonding (Topic-wise Videos):    • 11 Chemistry Chapter 3  Chemical Bonding F...   📙 📝 Solved Exercises – Short Questions & MCQs: 👉    • 11th Chemistry Solved Exercises New Book 2...   #Class11Chemistry #MOT #MolecularOrbitalTheory #mot #ChemicalBonding #11ChemistryNewBook2025 #AsimMushtaqAnsari #BondOrder