How Electrons ACTUALLY Fill Orbitals (Full Masterclass) ⚡

Master Pauli’s Exclusion Principle and Hund’s Rule of Maximum Multiplicity in just 6 minutes! Learn how electrons fill degenerate orbitals, why no two electrons can have the same four quantum numbers, and avoid common exam traps in electron pairing. Perfect for Class 11, NEET, and JEE revision. 📌 Key Topics Covered in this Video: • Pauli's Exclusion Principle: Why no two electrons in an atom can have the same set of 4 quantum numbers (n, l, m_l, m_s) • Maximum capacity of an orbital: Exactly 2 electrons with opposite spins (↑↓) • Hund’s Rule of Maximum Multiplicity: Pairing in degenerate subshells (p, d, f) only starts after each orbital is singly occupied with parallel spins • Common electron configuration mistakes and how to avoid them in competitive exams 💬 Question of the Day: According to Hund's rule, how many unpaired electrons are present in a ground-state Nitrogen atom (Z = 7)? Drop your answer in the comments below! 👇 🔔 Subscribe to Raw Learning for concise, high-yield NEET Chemistry & Biology concepts and shortcuts! #PauliExclusionPrinciple #HundsRule #ElectronicConfiguration #StructureOfAtom #NEETChemistry #Class11Chemistry #AtomicStructure #NEET2027 #RawLearning