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Unformatted text preview: o Solution – a series of wave functions with corresponding energies o Need quantum numbers o n, l, m l o Principle quantum number n- defines the energy level of the orbital (n=1, 2, 3, …) o Azimuthal Quantum Number l- defines the shape of the orbital (l=0,1,2,3,…n-1; l=0 s, l=1 p,l=2 d) o Magnetic Quantum Number m l – defines the orientation of the orbital (m l = -l,.,-2,-1,0,1,2,…) o n o l o m l o orbitals o 1 o o o S-orbital o 1s o 2 o o o 2s o o 1 o-1,0,1 o 2p o 3 o o 3s o o 1 o-1…1 3p o o 2 o-2…2 3d o 4 o o 4s o o 1 o-1. .1 4p o o 2 o-2…2 4d o o 3 o-3…3 4f • Look at misconceptions • Node- position where there is no electron density • M s- describes electron spin (-1/2 or +1/2) • Define electron need the four quantum numbers • For each orbital can have 2 e-• Pauli exclusion principle- no two electrons in the same atom can have the same 4 quantum numbers...
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This note was uploaded on 08/10/2010 for the course CHEM LAB 111 taught by Professor Muhammed during the Spring '10 term at Texas A&M.
- Spring '10