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Quantum Numbers

Quantum Numbers. Tells the “address” of an electron – energy level, sublevel, orbital and spin. n = energy level (n = 0, 1, 2, 3, 4, 5, 6, 7) l = sublevel (s, p, d, f) m = orbitals (orientations – what axis it is on) s = spin ~ clockwise = + 1 / 2 , counterclockwise = - 1 / 2.

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Quantum Numbers

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  1. Quantum Numbers • Tells the “address” of an electron – energy level, sublevel, orbital and spin • n = energy level (n = 0, 1, 2, 3, 4, 5, 6, 7) • l= sublevel (s, p, d, f) • m = orbitals (orientations – what axis it is on) • s = spin ~ clockwise = +1/2, counterclockwise = -1/2

  2. n = energy level n = 3 n = 1 nucleus n = 2

  3. l = sublevel (s, p, d, f) s p d f

  4. m = orbital / orientation p = 3 orbitals Dumbbell Shaped Pxy, Pxz, Pyz holds 6 electrons s = 1 orbital Sphere shaped holds 2 electrons d = 5 orbitals Holds 10 electrons f = 7 orbitals Holds 14 electrons 2 electrons will fill 1 orbital

  5. s = spin counterclockwise = -1/2 Spin down clockwise = +1/2 Spin up

  6. Electron Configuration 3 Rules: 1) Aufbau Principle – Electrons enter orbitals of lowest energy first 2) Pauli Exclusion Principle – Only 2 electrons can fit in one orbital; one as spin up ( ) and one as spin down ( ) • Hund’s Rule – When electrons occupy an orbital, they must fill each orbital first before they pair up

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