4. Consider only the four following quantum levels for the H atoms (n=4, n=3, n=2, andn=1). The emission spectrum of an excited H atom will consist of transitionsbetween these levels.a. How many emission lines are possible, considering only the four quantumlevels above?eeob,b. Photons of the lowest energy will be emitted in a transition from the levelwith n=to the level with n=mevie erilanc. The emission line having the shortest wavelength corresponds to atransition from the level with n=to the level with n=

For the maximum energy or shortest wavelength we should follow formula . E=(1/n12-1/n22)

4. Consider only the four following quantum levels for the H atoms (n=4, n=3, n=2, and n=1). The emission spectrum of an excited H atom will consist of transitions between these levels. a. How many emission lines are possible, considering only the four quantum levels above? Deeob, b. Photons of the lowest energy will be emitted in a transition from the level with n= to the level with n= bspe no eonslelees boshorluenu be c. The emission line having the shortest wavelength corresponds to a transition from the level with n= to the level with n= oute

4. Consider only the four following quantum levels for the H atoms (n=4, n=3, n=2, and n=1). The emission spectrum of an excited H atom will consist of transitions between these levels. a. How many emission lines are possible, considering only the four quantum levels above? Deeob, b. Photons of the lowest energy will be emitted in a transition from the level with n= to the level with n= bspe no eonslelees boshorluenu be c. The emission line having the shortest wavelength corresponds to a transition from the level with n= to the level with n= oute

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4.Make a prediction using your model. If an electron were to emit a photon and move from the n=3 level to the n=1 level, what wavelength of light would it emit? (Hint: use the Ryberg equation) Would this be a bigger energy What would be the energy change for this transition? change or a smaller energy change that the transition from the n=3 to the n=2 transition? Would you be able to see this energy change (will it be visible light?) What part of the electromagnetic spectrum should you look in to find these photons, the ultraviolet or the infrared?
5. An electron in a hydrogen atom makes a transition from ann= 2 orbital to an n = 5 orbital. a. For this electron transition, is energy being absorbed or released? Circle one. ABSORBED RELEASED b. Calculate the energy difference for this transition and the wavelength (in nanometers) of the photon involved in this transition.
1. Sodium vapor lamps are used to illuminate streets and highways. The very bright light emitted by these lamps is actually due to two closely spaced emission lines in the visible region of the electromagnetic spectrum. One of these lines has a wavelength of 5.890 × 10-7 m, and the other line has a wavelength of 5.896 X 10 m. a. What are the wavelengths of these radiations in centimeters? b. Calculate the frequencies of these radiations. c. In what region of the visible spectrum do these lines appear?
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What is wrong with the following set of quantum numbers? n = 2, l = 1, ml = -2, ms = +1/2 A. ml must be greater than or equal to l. B. l must be greater than or equal to n. C. l has a maximum value of n–1. D. ms must be 0 or 1. E. ml only has values equal to -l,0,+l
Molybdenum metal must absorb radiation with a minimum frequency of 1.09 × 1015 s before it can eject an electron from its surface via the photoelectric effect. а. What is the minimum energy required to eject an electron? b. What wavelength of radiation will provide a photon of this energy? c. If molybdenum is irradiated with light of wavelength of 120 nm, what is the maximum possible kinetic energy of the emitted electrons? 6.626xx0 66 X10
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Consider the energy level diagram below for a particular atom. What is the wavelength of a photon absorbed, in units of nm, that excites an electron from energy level E to energy level E4? -1.00x10-19 J E4 -4.00x10-19 J E3 -10.00x10-19 J E2 -16.00x10-19 J - E1 -
t t ot pt pt pt 1 pt 1 pt 1 pt 1 pt 1 pt 1 pt nent An advertising sign gives off blue light and yellow light. a. Which light has higher-energy photons? Oblue Oyellow blue - 570 nm Oyellow-490 nm blue - 490 nm yellow - 570 nm b. One of the colors has a wavelength of 570 nm, and the other has a wavelength of 490 nm. Which color has which wavelength? (Select all that apply.) c. Which light has the higher frequency? O blue Oyellow Submit Answer Try Another Version [References] 10 item attempts remaining the new Term Cengage Learning Cengage Technical Support Previous