quantum-mechanics-handout - Quantum Mechanics Quantum...

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Quantum Mechanics Quantum Mechanics overview • We will see: electrons have discrete energies, not because they are in shells but because they can only have certain wavelengths • Line spectra are not due to electrons jumping from shell to shell (as in Bohr’s model)… • Instead they’re due to electrons transforming from one wavelength (waveform) to another • Each electron is a wave that can be described by a series of “quantum numbers” • There are four quantum numbers: n, l , m l , m s • Today we will be looking at the first three • The combination of these 3 defines an “orbital” Waves: standing, travelling Read pg. 199 - 200 (stop at “The theory of quantum mechanics…” –3 rd paragraph) Q1: What is the difference between standing and traveling waves? Q2 – How many wavelengths (W) are represented in each figure below? W = 1 Classifying waves: hypothetical ex. • We have used the symbol “W” to represent
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