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CHEM103 Lecture Notes - Lecture 12: Wolfgang Pauli, Valence Electron, Covalent Bond

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emeraldmouse191

7 Feb 2019

School

University of Delaware

Department

Chemistry and Biochemistry

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Professor

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Document Summary

D orbitals - four leaf clover shaped. F orbitals - eight leaf clover shaped. Quantum numbers: zip codes for electrons in atoms. Principal q. n = n = 1, 2, 3, 4, . L = 0, 1, 2, 3, , n-1. Spin q. n = s = + (spin up) or - (spin down) Exclusion principle: no two electron in the same atom may have the same values for all four quantum number. Therefore, a maximum of two electrons may occupy any one orbital. Addresses = 1, 0, 0, + ot 1, 0, 0, - . Aufbau principle: electrons in atoms occupy the orbitals of lowest energy first. Only after these orbitals are filled will electrons occupy orbitals of higher energy. Hund"s rule: electrons in orbitals with the same energy (degenerate orbitals) tend to. Spread out occupying as many orbitals as possible before pairing up . (like people on the bus)

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Related Questions

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