Class 11 Chemistry Chapter 2 | Aufbau Principle, Pauli’s Principle & Hund’s Rule | FSc 1st Year

#atomicstructure #chemistry_class_11 #education #New_first_year_chemistry Chapter 2 (Lec#18 -5) 1st Year Chemistry || Electronic configuration, Aufbau + Pauli + Hund's rule Playlist with all Chemistry lectures for class 11 new book    • Class 11 chemistry new syllabus 2025 Pakis...   Chemistry Notes for Lecture 4 Chapter 2 https://umairkhanacademy.com/free-not... How to draw Atomic Orbitals    • Shapes of atomic orbitals | s,p,d. | Atomi...   Welcome to Umair Khan Academy 🎓 In this lecture, Sir Umair Ali Khan explains Electronic Configuration and the fundamental rules that govern electron filling in orbitals from Class 11 Chemistry, Chapter 2: Atomic Structure. 👉 Topics covered in this lecture: Electronic Configuration – concept and notation Aufbau Principle – electrons fill lowest energy orbitals first Pauli’s Exclusion Principle – no two electrons can have the same set of quantum numbers Hund’s Rule of Maximum Multiplicity – electrons fill degenerate orbitals singly before pairing Order of increasing energy of orbitals (n + ℓ rule) Examples of electronic configurations for atoms and ions This lecture is essential for mastering atomic structure, quantum mechanics basics, and periodic table trends. Perfect for FSc, A-Level, and O-Level Chemistry students. ✨ Subscribe to Umair Khan Academy for more Chemistry lectures, solved examples, and exam tips. #AtomicOrbitals #ChemSolvedExercise #highachieverschemistry #umairkhanacademy #1styearchemistry2025 #chemistry2025 #fscchemistry2025 #فرسٹ ائر کیمسٹری If you want to purchase notes for your personal use without watermark, Send me your picture and Name. with receipt of RS. 1OO for single Chapter on following WhatsApp number. /WhatsApp no. /Jazz Cash/RAAST Id. 03099164667 Related Searches: . Describe the deflection of particles, based on mass and charge ratio. Define electronic configuration, the distribution of electrons in orbitals. What is the definition of a shell, as an electron energy level. What are sub-shells and orbitals, determining the electron location probability. Relate quantum numbers, to the electronic distribution of elements effectively. Define principal quantum number (n), describing orbital size and energy level. Calculate the maximum number of electrons in a shell, using the formula 2n squared. Define azimuthal quantum number (l), describing the shape of the orbital precisely. Describe the values of l, corresponding to s, p, d, and f orbitals easily. Calculate the number of electrons in a subshell, using the formula 2(2l plus 1). Define magnetic quantum number (m), describing orbital orientation in space. Describe degenerate orbitals, having the same energy within a subshell clearly. Define spin quantum number (s), accounting for electron rotation direction. Describe the shapes of s-orbitals, which are spherical in nature. Describe the shapes of p-orbitals, which are polar or dumbbell shaped. Describe the shapes of d-orbitals, which have complex cloverleaf shapes involved. Explain the Aufbau principle, electrons fill lowest energy orbitals first completely. Explain Pauli’s exclusion principle, forbidding identical quantum number sets for electrons. Explain Hund’s rule, regarding electron filling in degenerate orbitals singly first. Write the electronic configuration of elements and their ions, using sub-shell notation. Explain the order of increasing energy of the sub-shells, based on n plus l values. How to determine the units of rate constant, using the order of reaction formula easily. Define valence electrons, outermost electrons governing chemical properties readily. Describe how electronic configuration relates to the periodic table position. Explain the arrangement of elements, into s, p, d, and f blocks based on filling order. Describe the experimental evidences, for electronic configuration, like atomic spectra. What is atomic emission spectrum, radiation of certain wavelengths emitted when heated. What is atomic absorption spectrum, dark lines showing absorbed wavelengths from white light. Relate ionization energy, to electron energy levels, experimentally. Account for the variation in successive ionization energies, indicating shell structure clearly. Deduce the position of an element, using successive ionization energy data. Explain how ionization energy helps account for trends, across period and down group. Explain the factors influencing ionization energies, nuclear charge and shielding effect. Define free radicals, species with unpaired valence electrons easily generated. Explain the electronic configuration, for the formation of semiconductors like silicon. Describe doping, and the formation of P-type semiconductors needed. Describe doping, and the formation of N-type semiconductors needed. Explain the change in atomic radius, across a period and down a group.