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REMINDER: STUDY GROUP ASSIGNMENT THIS WEEK LAB THIS WEEK ELECTRON ORBITALS October 26, 2009
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Visible Spectroscopy
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Heisenberg Uncertainty Principle We can’t know both the exact location and the energy of a particlethe exact location and the energy of a particle For electrons => We know the energy, so we don’t know the location very well
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Schrödinger’s Model of Hydrogen Electrons act as standing wavesstanding waves Wave behavior is described by a wave function: ψ Certain wave functions are allowed ψ 2 describes the probability of finding the electron in a particular spot (aka, electron density)
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Here’s what a probability density looks like… (A bit simplified) …but what does it mean?
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Orbitals Each wave function describes a shape = Orbital Where an electron can be found/exist Organized into main shells and subshells Number of orbitals is different for each subshell type: s = 1 orbital p = 3 orbitals d = 5 orbitals f = 7 orbitals Size and Energy (n=1, 2, 3, … ) Size and Energy (n=1, 2, 3, … ) Shape (s, p, d, f, … ) Shape (s, p, d, f, … )
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1s ___ 1 2p ___ ___ ___ 2s ___ 2 3d ___ ___ ___ ___ ___ 3p ___ ___ ___ 3s ___ 3 ENERGY 1, 2, and 3 correspond to the major energy levels (main shells) At the same main shell level, a p orbital will be at a higher energy than an s orbital 4f ___ ___ ___ ___ ___ ___ ___ 4d ___ ___ ___ ___ ___ 4p ___ ___ ___ 4s ___ 4
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What type of orbital is this? 1. s 2. p z 3. d xy 4. d xz 10
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Which type of orbital can’t exist? 1. 1p x 2. 2p x 3. 2s 4. 3d xy 10
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NODES- Where electrons don’t go Spherical Nodes
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Hydrogen
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You too can play with hydrogen… http://homepages.ius.edu/kforinas/physlets/quantum/hydrogen.html
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Quantum # Rules There are four different quantum numbers: n, l, m l, and m s n, l, and m l are integers n cannot be zero l can be 0 to n-1 m l can be anything from –l to l Ms can be +½ or -½
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Quantum Numbers and Orbitals
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Rules for filling orbitals 1. Pauli Exclusion Principle No two electrons can have the same 4 quantum numbers An orbital has a maximum of 2 electrons of opposite spin 2. Aufbau/Build-up Principle Lower energy levels fill before higher energy levels 3. Hund’s Rule Electrons only pair after all orbitals at an energy level have 1 electron 4. Madelung’s Rule Orbitals fill in the order of the value of n + l
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Orbital Filling Order
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