Lecture #16 - Chemistry 2A-c W2009 (Ch9-49)145 Bohr's Model...

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1 Chemistry 2A Chemistry 2A -c W2009 c W2009 (Ch9 (Ch9 -49)145 49)145 Bohr's Model of the Hydrogen Atom This model is limited to hydrogen and hydrogen like atoms (atoms with one electon). n = 1, 2, 3, 4… Shell K, L, M, N… Quantim Mechanics or Wave Mechanics Wave Equation (1929) Erwin Schrödinger Schrödinger Equation: H Ψ( n, l, m l ) = E Ψ( n, l, m l ) H = Hamiltonian (mathematical operator) Ψ( n, l , m l ) = wave function, where (n, l , m l ) is a set of 3 quantum #s. Probability of finding an e -1 in the atom: ⏐Ψ( n, l , m l ) 2 E((n, l , m l ) = Eigen-energy (depends on 3 quantum #s) Radial Angular e -
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2 Chemistry 2A Chemistry 2A -c W2009 c W2009 (Ch9 (Ch9 -50)146 50)146 Atomic wavefunctions are governed by 4 Quantum numbers (n, l , m l , m s ) n = principal quantum number: n = 1, 2, 3, . . . , integer Main energy level. A maximum of 2(n) 2 electrons. l = azimuthal or orbital angular momentum quantum number: l = 0, 1, 2, 3, 4, …, n-1 sub-shell: s p d f g,… Characterize orbital shapes. Allowed values are (0 to n-1) m l = magnetic quantum number: Allowed values: - l , - l+ 1, …, 0, …, l -1, l There are 2 l +1 values Orientation of orbitals in space m s = electron spin quantum number Allowed values: m s =+1/2 ( α , spin up) and m s =-1/2 ( β , spin down)
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This note was uploaded on 02/25/2009 for the course CHEM chem 2a taught by Professor Ng during the Winter '09 term at UC Davis.

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Lecture #16 - Chemistry 2A-c W2009 (Ch9-49)145 Bohr's Model...

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