1241 1241 2= ΔΕ| or AE = 2 where AE is measured in eV and is the wavelength of light emitted or absorbed by an atomic electron measured in nanometers, nm. 1 eV = 1 electron Volt=1.602 X 10 - J Atomic energy level transitions. AE = || final level | - starting level || Note all the absolute values!!! AE is always positive, so 2. is always positive!! 2. Graphs A, B and C follow. All three graphs depict atomic energy level transitions. a) Calculate the wavelength of light emitted in the transition in graph A from the n= = 3 to the n=1 state. Does the atom's energy increase or decrease? b) Calculate the wavelength of light absorbed in graph A in the n=3 to n=5 transition. Does the atom's energy increase or decrease? c) Calculate the wavelength of light emitted in the transition in graph B from the n = 4 to the n = 3 state. d) Calculate the wavelength of light absorbed in graph B in the n=1 to n = 5 transition. e) Calculate the wavelength of light emitted in the transition in graph C from the 4p state to the 2p state. You will have to estimate energy values.
A) Ionization O eV 4.9 eV - 7.65 V 13,6 V n. 5 n 4 n3 second excited state first excited state n = 2 30.6 eV - 122.4 V ground state n = 1 B) B 0 -0.54 -0.85 n = nus n4 -1.51 3 E (meV) -3.40 n = 2 -13.59 n=1 C) of ISO 72 71 so 40 13 92 41 14 59 095 Dal 45 -11 30 3d 303 -2) Hydrogen levels Energy (OV) 2p Lithium energy level diagram 4- 5: Ground state 25
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