lect_26dec1f08

lect_26dec1f08 - Outline 26 1-DEC-2008 Reviewe- Configs...

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1 Outline 26 1-DEC-2008 1. Review- e - Configs & Diagrams, Principles, Valence e - ’s (after noble gas, but not filled d or f) 2. Eff. nuclear charge, shielding, shape (figs. 8.3, 4, 5), Differences from H atom (Bohr) 3. Electron Spin Background 1. e - Configs& Orb. Diagrams (continued) Atoms & Ions, Period 4 (Transition) 4s 2 3d x , Exceptions (within ± 1)
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2 Name_______Quiz 26 TA _______ Given: Condensed e - config. [Ar] 5s 2 5p 2 1. What group? element? 2. How many valence e - ’s? 3. Complete the valence orbital diagram. Label the orbitals. __ __ __
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3 Review; Summary: “Rules to use”- 1. Number electrons is Z, atomic #. 2. Energy sequence for filling orbitals. Use PT. Use Aufbau Prinzip (building up principle) “Ground state” means lowest energy. 3. Number of electrons to put “in” orbital. Use Pauli Exclusion Principle. 4. Detailed distribution of electrons in given sub- shell set. Use Hund’s Rule.
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4 Review; Principles for writing e - distributions for “ ground state” atom. Aufbau Prinzip- Put electrons in lowest energy orbital first then in ascending energy order. 1s, 2s, 2p, 3s, 3p, 4s, 3p, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f Don’t memorize, get from Periodic Table. Pauli Exclusion Principle - No more than 2 e - s in one orbital; means no two e - ’s can have same set of four quantum #s [n, ℓ, m , m s ]. Hund’s Rule For sub-shells with more than orbital (p, d, f, g,. .) put one electron each, then double up.
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5 Configurations and Periodic Table Illustrates Building Up Order
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6 e - Configs. & Orbital Diagrams; atoms Ex: Consider orbital diagram below. a. Write electron configuration. Element?
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This note was uploaded on 02/18/2009 for the course CHEM 1A taught by Professor Okamura during the Fall '08 term at UC Riverside.

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lect_26dec1f08 - Outline 26 1-DEC-2008 Reviewe- Configs...

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