Physics 012 1st Edition Lecture 35 Outline of Last Lecture I. When an electron goes from a higher (ni) to lower (nf) energy state, light of wavelength λis emitted.a. 1/λ = R(1/nf2 – 1/ni2)i. R = Rydberg constant = 1.097 x 107 m-1b. Balmer series: series of wavelengths emitted by hydrogen within the visible spectrum, where nf = 2.II. Bohr modified planetary modela. 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/λe. Angular momentum is also quantized: L = nħ = rmevIII. Energy Level Diagram for HydrogenOutline of Current Lecture IV. Quantum Numbersa. Principal Quantum Number (n)i. n = 1, 2, 3, … ∞ii. determines total energy of atomiii. All states with the same principal quantum number are said to form a shell.n Name1 k2 L3 mThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.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 orbitaliii. All states with the same value for l form a sub shelll Name1 s2 p3 d4 f5 gc. Magnetic Quantum Number (ml)i. ml = -l, (-l+1), … 0 … l, (l+1)ii. gives us component of angular momentum along the direction of an applied magnetic fieldiii. ex) Lz = mlħ; If l = 2 then ml = -2, -1, 0, 1, 2; Lz = ħ√(6); and Lz = -2ħ, -ħ, 0, ħ,2ħ.d. Spin Quantum Number (ms)i. Can either be up (+1/2) or down (-1/2).V. Pauli Exclusion Principala. No two electrons in an atom can be in the same quantum state (all the same quantum numbers).b. Allowed quantum states for electrons up to n = 3:k L mn 1 2 3l 0 0 1 0 1 2ml0 0 -1 0 1 0 -1 0 1 -2 -1 0 1 2ms c. number of electrons in an energy state =
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