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Chem_110_Fall_Booker_Lec5

Chem_110_Fall_Booker_Lec5 - Schrdingers Equation Beginning...

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Schrödinger’s Equation Beginning of Quantum Mechanics (Wave Mechanics) Wave Functions are solutions to Schrödinger equation H ψ = E ψ describe the electron in an atom. Square of a wave function ( ψ 2 ) provides information about location of an electron in terms of probability or electron density, also called orbitals . For hydrogen atom the allowed energies of the electron are the same as those predicted by the Bohr model; however, the Bohr model assumed a symmetrical circular orbit. Bohr model doesn’t work for other atoms Don’t confuse orbitals with orbits. 1 Electron density distribution for 1s orbital
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Shapes of Orbitals Determined by the probability ( Ψ 2 ) of finding an electron at a certain distance (r) from the nucleus Example: s orbitals 2s is than 1s Size of s orbital as n increases Shape: symmetry 2
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p and d Orbitals First p orbitals n = 2 l = 1 m l = -1, 0, 1 Two “lobes” with in between p orbitals are First d orbitals : n = 3 l = 2 m l = 3
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Representation of p and d Orbitals 4
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Subshells and Orbitals n 2 = number of states = number of orbitals in the n th shell. Subshells # of orbitals in shell? 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f Number of orbitals in each subshell 5
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Why do Energies Differ?
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