Whats the wavelength of a photon of light that permits a hydrogen atom to go from its energy level 3 to itsenergy level 2?434nm121.6nm486.1nmO 656.3nmWhats the wavelength of a photon that could make a hydrogen atom jump from energy level 4 to energy level2?656.3nm121.6nm102.6nm486.1nm

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Whats the wavelength of a photon of light that permits a hydrogen atom to go from its energy level 3 to its energy level 2? 434nm 121.6nm 486.1nm 656.3nm Whats the wavelength of a photon that could make a hydrogen atom jump from energy level 4 to energy level 2? 656.3nm 121.6nm 102.6nm 486.1nm

Whats the wavelength of a photon of light that permits a hydrogen atom to go from its energy level 3 to its energy level 2? 434nm 121.6nm 486.1nm 656.3nm Whats the wavelength of a photon that could make a hydrogen atom jump from energy level 4 to energy level 2? 656.3nm 121.6nm 102.6nm 486.1nm

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

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What is the energy of a photon with a wavelength of 19.3 µm? 3.43x10-29 J 1.55×1013 J 1.03x10-20 J 1.28x10-38)
QUESTION TWO PLEASE..
19. A hydrogen atom in excited energy state E24x 10" drops down to the ground state at energy level E 21.76 x 10"), giving off a photon. a. What is the energy of the emitted photon injoules? b. What is its wavelength? c. Based on the EM spectrum, what type of raciation is this?
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Example: An electron in a hydrogen atom drops from energy level E4 to energy level E2. What is the frequency of the emitted photon, and which line in the emission spectrum corresponds to this event? E6 E = -0.378 eV Step 1: Es E = -0.544 eV - E= -0.850 eV Find the energy of the photon. E E = Einitial - Efinal E3 E=-1.51 eV = (-0.850 eV) - (-3.40 eV) = 2.55 eV Step 2: Use Plank's equation for frequency. E₂ E= -3.40 eV 12 E E = hf; f = h (2.55 eV) (1.60 x 10-191 6.63 x 10-34 Js f= 6.15 x 10¹4 Hz Line 3 is in the visible part of the electromagnetic spectrum and appears to be blue. The frequency f = 6.15 x 10¹4 Hz lies within the range of the visible spectrum and is toward the violet end, so it is reasonable that light of this frequency would be visible blue light. Step 3: Find the corresponding line in the emission spectrum. Examination of the diagram shows that the electron's jump from energy level E4 to energy level E2 corresponds to Line 3 in the emission spectrum. 3 Incoming photon…
An electron at the n=5 energy level of hydrogen undergoes a transition to the n=3 energy level. What wavelength of photon does the atom emit in this process? a) 1.28 x 10^-6 m b) 2.37 x 10^-6 m c) 4.22 x 10^-7 m d) 3.04 x 10^-6 m e) 5.92 x 10^-5 m
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