Chapter 5

Chapter 5 - Chapter 5 – Periodicity and Atomic Structure...

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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 3-3 +1/2 yes 2 1 3-1/2 no 2 1 +1/2 no 3 2 2-3/2 no 6 5 4 +1/2 yes 4 2 2-1/2 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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Chapter 5 - Chapter 5 – Periodicity and Atomic Structure...

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