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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:Among the following H atom transitions, which would emit a photon of light with
the longest wavelength?
A) n = 4 to n = 2
B) n = 6 to n = 3
C) n = 6 to n = 4
D) n = 5 to n = 2
E) n = 3 to n = 1
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- Select each set of quantum numbers that are acceptable. A) n = 1, t=0, m₂ = −1, m² = -1/2 B) n = 4, l= 2, m₂ = −2, m₂ = +½/2 C) n = 3, t= 3, m₂ = 0, ms=-½ D n=2, l=1, me = -1, ms = + ½ E) n = 4, l = 3, me = +3, ms = +½arrow_forwardSa 1 points An electron completes a transition from the n = 1 energy level where it has energy E1 =-2.18 x 10-18 Joules to the n=3 energy level where it has energy E3-2.42 x 10-19 Joules by absorbing 1018 Joules (essentially the difference between these two values). Calculate the wavelength (A) of a photon that would need to be absorbed to cause the n=1 to n 3 transition. energy E= 1.94 X hc where Plank's constant h 6.626 x 1034JSarrow_forwardWhich wavelength corresponds to the transition of an electron in a hydrogen atom from n = 2 to n = 1? a) 182 nm c) 724 nm e) 122 nm b) 91.2 nm d) 812 nmarrow_forward
- Which of the following atomic electron transitions in a hydrogen atom would emit a photon of light with the longest wavelength (λ)? Group of answer choices n = 2 to n = 1 n = 6 to n = 5 n = 6 to n = 7 n = 3 to n = 2 n = 3 to n = 1arrow_forwardIn the H atom, which transition produces a photon with the lowest energy? n=2 --> n=1 n=6 --> n=1 n=3 --> n=1 n=4 --> n=1arrow_forwardWhich of the following electron transitions in a hydrogen atom would emit a photon with the highest frequency? Group of answer choices n = 5 → n = 3 n = 3 → n = 2 n = 1 → n = 6 n = 3 → n = 1 n = 2 → n = 1arrow_forward
- which energy level transition for a hydrogen atom would emit the photon with the lowest frequecy n=4 to n=1 n=5 to n=1 n=2 to n=3 n=5 to n=4arrow_forwardIdentify the type of electromagnetic radiation that would be observed or required for each transition. If visible light, indicate the color. a) n=3 to n=1 b) n= 3 to n=2 c) n=4 to n=2 d) n=5 to n=2 e) n=4 to n=3arrow_forwardWhich of the following atomic electron transitions would emit a photon of light with the longest wavelength (λ)? Group of answer choices (1) n = 4 to n = 5 (2) n = 3 to n = 1 (3) n = 2 to n = 1 (4) n = 5 to n = 4 (5) n = 3 to n = 2arrow_forward
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