CHEM 101 1nd Edition Lecture 25Outline of Last Lecture I. Einstein and the Photoelectric Effect II. Atomic Line Emission Spectra and Neils BohrIII. The Bohr Model of the AtomIV. Energy AbsorptionV. Energy CalculationsVI. Origin of Line SpectraVII. The Wave-Like Behavior of MatterOutline of Current Lecture I. Quantum MechanicsII. Quantum NumbersCurrent LectureI. Quantum Mechanicsa. Applied idea of e- behaving as a wave to the problem of electrons in atomsb. Determined Wave Equationi. Defines energy of an electron in terms of wavesii. Composed of Wave functions, Ψ1. Have radial and angular partsc. Consequences of Schrodinger’s Equationi. Only certain wave functions are allowed (quantization)ii. Quantum numbers describe approximate location of e-d. Ψ 2 is proportional to probability of finding an e - at a given pointi. Not the same for all orbitalsII. Quantum Numbersa. Wave functions, or orbitals, describe the region of space where an electron can be found & are described by three quantum numbersi. n, l, ml. b. Principle Quantum Number, ni. Defines the energy level and size of the orbitalii. n = 1, 2, 3, …c. Angular Momentum (Azimuthal) Quantum Number, li. Defines the shape of the orbitii. l = 0,1,2,3,… These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a
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