Atomic Structure Class 11 Chemistry Lecture 1 | Protons, Neutrons, Electrons & Atomic Number скачать в хорошем качестве

Atomic Structure Class 11 Chemistry Lecture 1 | Protons, Neutrons, Electrons & Atomic Number

#atomicstructureclass11 #chemistry_class_11 #education #New_first_year_chemistry Playlist with all Chemistry lectures for class 11 new book    • Class 11 chemistry new syllabus 2025 Pakis...   Chemistry Notes for Lecture Chapter 1 & Solved Exercise. https://umairkhanacademy.com/free-not... Welcome to Lecture 1 of Atomic Structure (Class 11 Chemistry, Chapter 2) 🚀 In this video, we explain the fundamental concepts of atomic structure in a simple and exam-focused way. Perfect for FSc, A-Level, and O-Level Chemistry students who want clear concepts and strong preparation. 👉 Topics covered in this lecture: Protons, Neutrons & Electrons (relative charge & mass) Atomic Number (Z) & Mass Number (A) How to calculate number of neutrons (N = A – Z) Examples with Al, Cl⁻, O²⁻, P³⁻, and S²⁻ ions Difference between neutral atoms and ions Behavior of fundamental particles in an electric field Deflection based on charge/mass ratio This is the first lecture of Atomic Structure Class 11 Chemistry Playlist, where we will also cover quantum numbers, electronic configuration, orbital shapes, Pauli’s Principle, Hund’s Rule, Aufbau Principle, spectra, periodic table trends, and more in upcoming videos. ✨ Subscribe to Umair khan academy for more Chemistry lectures, solved examples, and exam tips. #chemsolvedexercise #highAchieversChemistry #umairkhanacademy #1styearchemistry2025 #chemistry2025 #fscchemistry2025 RELATED TOPC SEARCHES FOR ATOMIC STRUCTURE 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. Explain the electronic configuration, for the formation of semiconductors like silicon.