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Unformatted text preview: Chapter 5 – Periodicity and Atomic Structure Lecture 12 (CHEM 1010) Agenda: Midterm comments Review of Chapter 5 to date Energy levels Aufbau Principle Hund’s Rule Electron configuration Effective nuclear charge Atomic radii Periodicity and Atomic Structure Chapter 5 Review: Light  Light can act as both a wave and a particle Wavelength (), frequency () and amplitude Spectrum of light (visible and other types) you need to know how to convert between the three terms Minimum frequency above which electrons can be ejected from the surface of the metal Orbitals exist at discrete energy levels Each element has specific line spectra associated with their electrons and the energy levels of their electrons Review: Equations λ 1 = R n 2 1 m 2 1 E light = h ν mv h λ = π 4 h p x ≥ ∆ ∆ Review: Schrödinger’s Equation Ψ is a mathematical function describing the shape of the wave (orbital) Ψ2 is the probability of finding the electron within a given volume of space around the nucleus n – principle quantum number (n = 1, 2, 3, 4, 5…) Distance of the electron from the nucleus (energy level of the electron l angular momentum quantum number ( l = n  1) Shape of the volume of space that the electron occupies ( s , p d or f ) ml magnetic quantum number ( ml =  l to + l ) Orientation of the orbital in space ms spin quantum number: ms = + ½ or – ½ Quantum Number Challenge n l ml ms Yes/No: Why?? 2 3 2 +1/2 no 4 33 +1/2 yes 2 1 31/2 no 2 1 +1/2 no 3 2 23/2 no 6 5 4 +1/2 yes 4 2 21/2 no ml = 1 ml = 0 ml = 1 ml = 2 ml = 1 ml = 0 ml = 1 ml = 2 Existence (and energy) of electron in atom is described by its unique wave function...
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 Spring '11
 OLGA
 Atom, Atomic Radii, Electron, Electrons, Atomic orbital, Pauli exclusion principle, Principal quantum number

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