Lecture10 - Chem 1P Lecture 10 Orbitals Periodic Table...

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Chem 1P Lecture 10: Orbitals & Periodic Table
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Chang Section 2.8 Where is the electron?
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Wavefunctions The electron bound to the atom looks like a standing wave.
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Electron orbits In the Bohr model of the atom, the hydrogen atom is like a planetary system with the electron in certain allowed circular orbits. " n , l , m l
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Allowed wavefunctions Each orbital is characterized by a set of quantum numbers. Principal quantum number (n): integral values (1,2,3…). Related to the size and energy of the orbital. Angular momentum quantum number ( l ): integral values from 0 to (n-1) for each value of n. Magnetic quantum number (m l ): integral values from - l to l for each value of n. " n , l , m l There are n different l -levels for each value of n There are (2 l +1) different m l -levels for each value of l
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s-orbitals s-orbitals have l = 0, there are a total of 2 l +1 = 1 s-orbitals for each n. Ψ n , 0 , m l
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p-orbitals have l = 1, there are a total of 2 l +1 = 3 p-orbitals. Ψ
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Lecture10 - Chem 1P Lecture 10 Orbitals Periodic Table...

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