Experimental Evidences, Atomic Spectra & Ionization Energies for class 11 chapter 2 lecture 2

#AtomicStructure #chemistry_class_11 #education #New_first_year_chemistry Chapter 2 (Lec#13 -2) 1st Year Chemistry || Experimental Evidences for Electronic Configuration Playlist with all Chemistry lectures for class 11 new book    • Class 11 chemistry new syllabus 2025 Pakis...   Chemistry Notes for Lecture 1 Chapter 2 https://umairkhanacademy.com/free-not... Welcome to Umair Khan Academy! 🎓 In this video, Sir Umair Ali Khan explains Experimental Evidences for the Electronic Configuration of Atoms (Class 11 Chemistry, Chapter 2: Atomic Structure). 👉 Topics covered in this lecture: Bohr Model & Origin of Modern Atomic Theory Atomic Emission Spectrum & Atomic Absorption Spectrum (Hydrogen spectrum explained) How atomic spectra act as the fingerprints of elements Successive Ionization Energies – evidence for electron shells (example of Magnesium atom) First Ionization Energies of Different Elements Trends in ionization energy across periods and down groups Relation between atomic number, electron shells, and ionization energy This lecture will help you understand how atomic spectra and ionization energies provide solid evidence for the arrangement of electrons in shells and subshells. Perfect for FSc, A-Level, and O-Level Chemistry students preparing for exams. ✨ Don’t forget to subscribe to Umair Khan Academy for more Class 11 Chemistry lectures, solved examples, and exam tips. #ChemSolvedExercise #highAchieversChemistry #umairkhanacademy #1styearchemistry2025 #chemistry2025 #fscchemistry2025 Describe protons, neutrons, and electrons, in terms of relative charge and mass. Define atomic number, and proton number, representing the same concept effectively. Define mass number, and nucleon number, representing the sum of protons and neutrons. How to calculate the number of neutrons, using mass number and atomic number easily. Explain the behavior of beams of fundamental particles, in an electric field clearly. 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.