Loose Leaf For Explorations: Introduction To Astronomy
9th Edition
ISBN: 9781260432145
Author: Thomas T Arny, Stephen E Schneider Professor
Publisher: McGraw-Hill Education
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Chapter 4, Problem 9QFR
To determine
Difference between the emission and absorption.
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Why is it impossible for a gas composed of atoms that all have their electrons in the ground state to produce an
emission line?
The following image is an energy level diagram for a simple
atom, where E1
0.00 ev, E2 = 1.34 ev, and E3
3.95 ev.
%3D
n=3
E3=?
n=2
E,=?
n=1
- Ez=?
What wavelengths appear in the atom's emission spectrum?
(Enter your wavelengths in the order of smallest to largest.)
3.14x10-7 m 4.75×10-7 m 9.25x10-7 m
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Your receipt no. is 162-5156 ?
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What wavelengths appear in the atom's absorption spectrum?
(Enter your wavelengths in the order of smallest to largest.)
What are the two longest wavelengths in the absorption spectrum of sodium? What are the transitions?
Chapter 4 Solutions
Loose Leaf For Explorations: Introduction To Astronomy
Ch. 4 - Prob. 1QFRCh. 4 - Prob. 2QFRCh. 4 - Prob. 3QFRCh. 4 - Prob. 4QFRCh. 4 - Prob. 5QFRCh. 4 - Describe the Kelvin temperature scale.Ch. 4 - Prob. 7QFRCh. 4 - Prob. 8QFRCh. 4 - Prob. 9QFRCh. 4 - Prob. 10QFR
Ch. 4 - Prob. 11QFRCh. 4 - Prob. 12QFRCh. 4 - Prob. 1TQCh. 4 - Prob. 2TQCh. 4 - Prob. 3TQCh. 4 - Prob. 4TQCh. 4 - (4.3/4.4/4.5) Given that water absorbs microwaves...Ch. 4 - Prob. 6TQCh. 4 - Prob. 7TQCh. 4 - Prob. 8TQCh. 4 - Prob. 9TQCh. 4 - Prob. 10TQCh. 4 - (4.1) Use the Suns distance of 150 million...Ch. 4 - (4.1) Suppose you are operating a...Ch. 4 - Prob. 3PCh. 4 - Prob. 4PCh. 4 - Prob. 5PCh. 4 - Prob. 6PCh. 4 - Prob. 7PCh. 4 - Prob. 8PCh. 4 - (4. 6) Calculate the Doppler shift for blue light...Ch. 4 - Prob. 10PCh. 4 - (4.2) Which kind of light travels fastest? (a)...Ch. 4 - Prob. 2TYCh. 4 - Prob. 3TYCh. 4 - Prob. 4TYCh. 4 - Prob. 5TYCh. 4 - Prob. 6TYCh. 4 - Prob. 7TYCh. 4 - Prob. 8TYCh. 4 - What is Galilean relativity? Give an example of...Ch. 4 - Prob. 2EQFRCh. 4 - Prob. 3EQFRCh. 4 - Prob. 4EQFRCh. 4 - What is meant by panspermia?Ch. 4 - Prob. 6EQFRCh. 4 - Prob. 7EQFRCh. 4 - Prob. 1ETQCh. 4 - Prob. 2ETQCh. 4 - Prob. 3ETQCh. 4 - Prob. 1EPCh. 4 - Mercury orbits the Sun at speeds ranging from 59...Ch. 4 - Prob. 3EPCh. 4 - Prob. 1ETYCh. 4 - The Miller-Urey experiment demonstrated that (a)...Ch. 4 - Prob. 3ETYCh. 4 - Prob. 4ETYCh. 4 - Prob. 5ETY
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- How do the allowed orbits for electrons in atoms differ from the allowed orbits for planets around the sun?arrow_forwardIf the average temperature of the surface of the Sun is roughly 5780 Kelvin, the radiation emitted from the Sun should peak in the electromagnetic spectrum. part of the « < Question 26 of 32 » A Moving to another question will save this response. O 10:05 hp %23 24 & backspa %D 9. 4. 6. 1 2 { r y W e k S d f b C 2Narrow_forwardAn electron for a hydrogen atom absorbed enough energy to move to the third energy level and immediately returned to ground state, emitting the energy it absorbed. A second hydrogen atom had its electron absorb the same amount of energy but, instead of returning directly to ground state, it moved to the second energy level and then to ground state. What can be said of the energy emitted by these two electrons that took different paths?arrow_forward
- The energy levels of a hypothetical atom are shown here. Which of the following photons can an electron sitting in the -4eV energy level absorb? (select two answers) -0.2 ev -0.4 ev -1.8 ev 4 ev A photon with 2.5 eV of energy A photon with 3.8 eV of energy A photon with 0.4 ev of energy A photon with 1.8 ev of energy A photon with 2.2 ev of energyarrow_forwardBased on Bohr’s atomic model, how many visible wavelengths of the helium emission spectrum end at energy level n=4? What about the absorption spectrum?arrow_forwardConsider the Bohr model of the atom. Suppose an electron in a hydrogen atom transitions from the n=3 level to the n=5 level. 1) CALCULATE the energy (ΔE) for this transition. 2) Does this transition involve the absorption or emission of a photon of light? How do you know?arrow_forward
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- The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. n = 4 4.2 ev v G Color Wavelength Frequency Photon energy violet 380-450 nm 668-789 THz 2.75-3.26 eV n= 3 2.4 ev blue 450-495 nm 606-668 THz 2.50-2.75 ev n = 2 2.0 ev green 495-570 nm 526-606 THz 2.17-2.50 ev yellow 570-590 nm 508-526 THz 2.10-2.17 ev orange 590-620 nm 484-508 THz 2.00-2.10 ev red 620-750 nm 400-484 THz 1.65-2.00 ev n=1 O ev Part A Initially, electrons are in both the ground and first excited state (n=1 and n=2). A beam of light hits the gas. This beam is a continuous spectrum of yellow/green light (from 495 nm to 590 nm) How many absorption line/s will there be in the spectra? 2 Submit Previous Answers v Correct Part B Calculate the wavelength of the absorption lines. Separate answers by a comma. 1, 518,565 nm Part C After absorption of the yellow/green light, how many emission lines are possible? ? Submit Request Answerarrow_forwardIf a hydrogen atom undergoes a transition from n = 1 (E = 4.17 x 10-19 J) to n = 3 (E = 8.62 x 10-19 J), what is the wavelength of the photo absorbed?arrow_forwardWhen a photoconductor is exposed to light a. less current flows through it b.its resistance increases c.it becomes less conductive d.it becomes more conductive e.it acts like an insulatorarrow_forward
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