11-2-10 - Lecture 11 - Chapter 7 %26 Chapter 8

11-2-10 - Lecture 11 - Chapter 7 %26 Chapter 8 - Hydrogen...

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Unformatted text preview: Hydrogen Wavefunctions Orbitals Orbitals The Schrdinger equation describes the properties of an allowed electron state: A quantized energy Labeled by 3 quantum numbers Properties may be determined from the mathematical form of the wavefunction QUANTUM NUMBERS QUANTUM NUMBERS The shape, size, and energy of each orbital is a function of 3 quantum numbers: n (principal quantum number) T shell (angular momentum quantum number) T subshell m (magnetic quantum number) x P ( designates an orbital within a subshell Shells & Subshells Each shell has a number called the PRINCIPAL QUANTUM NUMBER, n The principal quantum number of the shell is the number of the period or row of the periodic table where that shell begins. Shells Shells n = 1 n = 2 n = 3 n = 4 etc. Principal Quantum Number Principal Quantum Number n = 1, 2, 3, 4, 5, 6, . . . (an integer) Determines the energy, E = - Rh/n 2 Indicates the average distance of the electron from the nucleus. The total number of nodes is n - 1 Corresponds to the Bohr orbits Size of orbital is approximately n 2 a 0 (a is the Bohr radius) Angular Momentum Angular Momentum Quantum Number Quantum Number = 0, 1, 2, 3, . . . (n-1) different possible values for a given value of n specifies the shape of the orbital Coded using letters 0 1 2 3 4 5 . . ....
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11-2-10 - Lecture 11 - Chapter 7 %26 Chapter 8 - Hydrogen...

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