College Physics: A Strategic Approach (4th Edition)
4th Edition
ISBN: 9780134609034
Author: Randall D. Knight (Professor Emeritus), Brian Jones, Stuart Field
Publisher: PEARSON
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Question
Chapter 29, Problem 5CQ
To determine
Number of spectral lines seen in the emission spectrum and absorption spectrum.
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An atom has its electron in the energy level at - 1.2 eV. It absorbs a photon, which promotes the election to the -0.4 eV level. What is the wavelength (in meter) of this photon.
Round off the answer to 2 decimal places with scientific representation.
What type of spectrum is observed in the light from the sun and other stars?
a continuous spectrum consisting of all colors.
an emission spectrum.
an absorption spectrum consisting of dark lines in a continuous bright background.
an atomic spectrum of hydrogen.
A transition of an electron in a hydrogen atom takes place from n= 1 to n= infinity.
What is the end result of this transition?
What is the wavelength of the light required for this transition?
What will the result be if light with a shorter wavelength than that used in question 2 be?
Chapter 29 Solutions
College Physics: A Strategic Approach (4th Edition)
Ch. 29 - Prob. 1CQCh. 29 - Prob. 2CQCh. 29 - Prob. 3CQCh. 29 - Prob. 4CQCh. 29 - Prob. 5CQCh. 29 - Prob. 6CQCh. 29 - Prob. 7CQCh. 29 - Prob. 8CQCh. 29 - Prob. 9CQCh. 29 - Prob. 10CQ
Ch. 29 - Prob. 11CQCh. 29 - Prob. 12CQCh. 29 - Prob. 13CQCh. 29 - Prob. 14CQCh. 29 - Prob. 15CQCh. 29 - Prob. 16CQCh. 29 - Prob. 17CQCh. 29 - Prob. 18CQCh. 29 - Prob. 20CQCh. 29 - Prob. 21CQCh. 29 - Prob. 22CQCh. 29 - Prob. 23CQCh. 29 - Prob. 24CQCh. 29 - Prob. 25CQCh. 29 - Prob. 27MCQCh. 29 - Prob. 28MCQCh. 29 - Prob. 29MCQCh. 29 - Prob. 30MCQCh. 29 - Prob. 31MCQCh. 29 - Prob. 32MCQCh. 29 - Prob. 1PCh. 29 - Prob. 2PCh. 29 - Prob. 3PCh. 29 - Prob. 4PCh. 29 - Prob. 5PCh. 29 - Prob. 6PCh. 29 - Prob. 7PCh. 29 - Prob. 8PCh. 29 - Prob. 9PCh. 29 - Prob. 10PCh. 29 - Prob. 11PCh. 29 - Prob. 12PCh. 29 - Prob. 13PCh. 29 - Prob. 14PCh. 29 - Prob. 15PCh. 29 - Prob. 16PCh. 29 - Prob. 17PCh. 29 - Prob. 18PCh. 29 - Prob. 19PCh. 29 - Prob. 20PCh. 29 - Prob. 21PCh. 29 - Prob. 22PCh. 29 - Prob. 23PCh. 29 - Prob. 24PCh. 29 - Prob. 25PCh. 29 - Prob. 27PCh. 29 - Prob. 28PCh. 29 - Prob. 29PCh. 29 - Prob. 30PCh. 29 - Prob. 31PCh. 29 - Prob. 32PCh. 29 - Prob. 33PCh. 29 - Prob. 34PCh. 29 - Prob. 35PCh. 29 - Prob. 36PCh. 29 - Prob. 37PCh. 29 - Prob. 39PCh. 29 - Prob. 40PCh. 29 - Prob. 41PCh. 29 - Prob. 42PCh. 29 - Prob. 43PCh. 29 - Prob. 45PCh. 29 - Prob. 46PCh. 29 - Prob. 47PCh. 29 - Prob. 48PCh. 29 - Prob. 49PCh. 29 - Prob. 50PCh. 29 - Prob. 51PCh. 29 - Prob. 52GPCh. 29 - Prob. 53GPCh. 29 - Prob. 54GPCh. 29 - Prob. 55GPCh. 29 - Prob. 56GPCh. 29 - Prob. 57GPCh. 29 - Prob. 58GPCh. 29 - Prob. 59GPCh. 29 - Prob. 60GPCh. 29 - Prob. 61GPCh. 29 - Prob. 62GPCh. 29 - Prob. 63GPCh. 29 - Prob. 64GPCh. 29 - Prob. 65GPCh. 29 - Prob. 66GPCh. 29 - Prob. 67GPCh. 29 - Prob. 69GPCh. 29 - Prob. 70MSPPCh. 29 - Prob. 71MSPPCh. 29 - Prob. 72MSPPCh. 29 - Prob. 73MSPPCh. 29 - Prob. 74MSPPCh. 29 - Prob. 75MSPPCh. 29 - Prob. 77MSPP
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- Describe how the hydrogen atom might absorb a photon of energy less than 13.6 eV. Describe a process by which a 9.8-eV photon might be absorbed. What about a 15.2-eV photon?arrow_forwardAn electron is in the n=5 state of a hydrogen (Bohr) atom. As it de-excites to the ground state, how many emission lines are possible? Show these on an energy level diagram. Which emission line has the shortest wavelength? Which emission line has the longest wavelength? (You do not need to actually find these wavelengths.)arrow_forwardWhat is an emission spectrum? Use the Bohr model to explain why the emission spectrum of the hydrogen atom consists of distinct lines at specific wavelengths.arrow_forward
- What lines would be missing for hydrogen in an absorption spectrum? What wavelengths are missing for hydrogen in an emission spectrum?arrow_forwardWhat is the wavelength of the light emitted when hydrogen atoms go from n = 9 to n = 3? Please give your answer in nanometers.arrow_forwardWhat is the energy of the photon that is emitted by the hydrogen atom when it makes a transition from the n = 7 to the n = 2 energy level? Enter this energy measured in electron Volts (eV).arrow_forward
- Consider 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_forwardWhy don’t we see hydrogen Balmer lines in the spectra of stars with temperatures of 45,000 K? a. There is no hydrogen in stars this hot. b. The stars are hot enough that most of the hydrogen is ionized and the atoms cannot absorb energy. c. These stars are so cool that nearly all of the electrons in the hydrogen atom are in the ground state. d. Stars of this temperature are too cool to produce an absorption spectrum. e. Stars of this temperature are too hot to produce an absorption spectrum.arrow_forwardThe 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 You are correct. Your receipt no. is 162-5156 ? Previous Tries What wavelengths appear in the atom's absorption spectrum? (Enter your wavelengths in the order of smallest to largest.)arrow_forward
- A photon has a frequency 4873935 Hz. Calculate its energy in Joules. Answer in Scientific Notation. Round your answer to 2 significant figures.arrow_forwardWhich produces a shorter wavelength of light: an electron jumping from a hydrogen atom’s 6th energy level to its 2nd energy level, or one jumping from the 3rd to the 2nd energy level? Explain your answer.arrow_forwardThe energy levels for a Bohr atom are shown below. Use this diagram to solve problems 7 and 8. 0 eV -2.5 eV -4.0 eV -7.0 eV -12.5 eV 7. What amount of energy is needed for an electron to jump from n = 1 to n = 4? 8. What is the wavelength of the photon needed to make this happen? Is it emission or absorption?arrow_forward
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