3.7 Quantum Numbers: Principal (n) and Angular Momentum (l) Quantum Numbers, Shells & Subshells

Chapter 3: Quantum Theory and Electronic Structure | Lecture 7 of 10 General Chemistry: The Complete College Lecture Series This chapter covers the wave nature of light, the photoelectric effect, the Bohr model, the de Broglie wavelength, the uncertainty principle, quantum numbers, orbitals and electron configurations. This lecture introduces quantum numbers, the set of numbers that come out of the Schrödinger equation and describe where an electron can be found in an atom. We define an atomic orbital as the region that holds electrons, and then focus on the first two quantum numbers: the principal quantum number n, which tells us the shell and its size (shell 1 is closest to the nucleus, then shell 2, 3, 4 and so on, with larger shells farther away and higher in energy), and the angular momentum quantum number l, which designates the subshell and the shape of the orbital. Mastering these ideas is essential, because we use them throughout the rest of the chemistry course for electron configurations, the periodic table and bonding. These are comprehensive general chemistry lecture videos, built to help students succeed in the course, with clear step-by-step explanations, closed captions and practice quiz questions. Timestamps: 0:00 Introduction to quantum numbers 2:10 The angular quantum number and the subshell Part of: General Chemistry, Chapter 3 Keywords: quantum numbers, principal quantum number, angular momentum quantum number, shells, subshells, atomic orbital, Schrödinger equation results Related search terms: MCAT chemistry, DAT chemistry, OAT chemistry, PCAT chemistry, AP Chemistry, IB Chemistry, CLEP general chemistry, A-level chemistry, NEET chemistry, JAMB chemistry, community college chemistry, college general chemistry #GeneralChemistry #Chapter3 #QuantumNumbers #AtomicOrbitals #ElectronShells #DrKunapareddy