Consider the following energy levels of a hypothetical atom:  E4: −1.0 × 10-19 J E2: −10 × 10-19 J E3: −5.0 × 10-19 J E1: −15 × 10-19 J  (a) What is the wavelength of the photon needed to excite an electron from E1 to E4? (b) What is the energy  (in joules) a photon must have to excite an electron  from E2 to E3? (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.

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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 Consider the following energy levels of a hypothetical atom: 

E4: −1.0 × 10-19 J E2: −10 × 10-19 J

E3: −5.0 × 10-19 J E1: −15 × 10-19 J

 (a) What is the wavelength of the photon needed to excite an electron from E1 to E4? (b) What is the energy  (in joules) a photon must have to excite an electron  from E2 to E3? (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.

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