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Be sure to answer all parts. Consider the following energy levels of a hypothetical atom: E4...

Be sure to answer all parts. Consider the following energy levels of a hypothetical atom: E4 −2.11 × 10−19 J E3 −5.61 × 10−19 J E2 −1.05 × 10−18 J E1 −1.85 × 10−18 J (a) What is the wavelength of the photon needed to excite an electron from E1 to E4? × 10 m (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? × 10 J (c) When an electron drops from the E3 level to the E1 level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process. × 10 m

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a)E1 to E4: Energy difference, AE =E4-B, =_2.1 1 × 10-19 J-(-1.85×10-18 J -1.639 x1018 J Planks constanth6.63x10 4 J.s Velocity of light, c 3x108 m/s Wavelength, A- (6.63×10-34 Js)×3x108 m/s) 1.639x 10J he 1 nm = 1.21×10 m ×10 = 121 nm b) E2 to E3: Energy difference, AE-E - E =-561×10-19 J-(-1.05×10-18 J = 4.89×10-19 J c)E, to El Energy difference, AE-E-E =-5.61×10-19 Jー(-1.85×10-B J = 1.289×10-18 J Planks constant ,に6.63×10-34 J. s Velocity of light, c = 3x108 m/s Wavelength, λ =-= hc(6.63x10-* J.s)x (3x10* m/s) 1.289 × 10-18 J 1.54×10-7 m

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