Quantum Numbers

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Quantum Numbers

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The University of Vermont
Phys 012 - Elementary Physics
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Lecture 35 Outline of Last Lecture I. When an electron goes from a higher (ni) to lower (nf) energy state, light of wavelength λ is emitted. a. 1/λ = R(1/nf2 – 1/ni2) i. R = Rydberg constant = 1.097 x 107 m-1 b. Balmer series: series of wavelengths emitted by hydrogen within the visible spectrum, where nf = 2. II. Bohr modified planetary model a. Electrons do not continuously emit radiation. b. We have “stationary states.” c. Radiation is emitted by electrons when moving to a smaller orbit (lower energy). d. Energy emitted by electron = Ei – Ef = hf = hc/λ e. Angular momentum is also quantized: L = nħ = rmev III. Energy Level Diagram for Hydrogen Outline of Current Lecture IV. Quantum Numbers a. Principal Quantum Number (n) i. n = 1, 2, 3, … ∞ ii. determines total energy of atom iii. All states with the same principal quantum number are said to form a shell. n Name 1 k 2 L 3 m b. Orbital Quantum Number (l) i. l = 0, 1, 2, 3, … (n-1) ii. gives us the total angular momentum of an electron in its orbital Physics 012 1st Edition

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