College Physics: A Strategic Approach (3rd Edition)
3rd Edition
ISBN: 9780321879721
Author: Randall D. Knight (Professor Emeritus), Brian Jones, Stuart Field
Publisher: PEARSON
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Chapter 29, Problem 59GP
To determine
Wavelength of the series limit of Lyman series in hydrogen.
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What is the longest - wavelength line
in nanometers in the infrared series
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1) The Lyman series of lines in the emission spectrum of hydrogen corresponds to transitions from various excited states to the n1 = 1 orbit. Calculate the wavelength (in nm) of the energy line (n = 11) in the Lyman series to five significant figures. (RH = 109677.57 cm-1). Think about where this is in the spectrum.
2) What is the wavelength, (in angstroms, A) of an electron (m = 9.11 X 10-31 kg) moving at 7.80 X 105 m/sec. (h= 6.626 X 10-34 Js)
A doubly ionized lithium atom (Li++) is one that has had two of its three electrons removed. The energy levels of the remaining single-electron ion are closely related to those of the hydrogen atom. The nuclear charge for lithium is +3e instead of just +e. How are the energy levels related to those of hydrogen? How is the radius of the ion in the ground level related to that of the hydrogen atom? Explain.
Chapter 29 Solutions
College Physics: A Strategic Approach (3rd 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. 19CQCh. 29 - Prob. 20CQCh. 29 - Prob. 21CQCh. 29 - Prob. 22CQCh. 29 - Prob. 23CQCh. 29 - Prob. 24MCQCh. 29 - Prob. 25MCQCh. 29 - Prob. 26MCQCh. 29 - Prob. 27MCQCh. 29 - Prob. 28MCQCh. 29 - Prob. 29MCQCh. 29 - Prob. 30MCQCh. 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. 21PCh. 29 - Prob. 22PCh. 29 - Prob. 23PCh. 29 - Prob. 24PCh. 29 - Prob. 25PCh. 29 - Prob. 26PCh. 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. 38PCh. 29 - Prob. 39PCh. 29 - Prob. 40PCh. 29 - Prob. 41PCh. 29 - Prob. 42PCh. 29 - Prob. 43PCh. 29 - Prob. 44GPCh. 29 - Prob. 45GPCh. 29 - Prob. 46GPCh. 29 - Prob. 47GPCh. 29 - Prob. 48GPCh. 29 - Prob. 49GPCh. 29 - Prob. 50GPCh. 29 - Prob. 51GPCh. 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. 68GPCh. 29 - Prob. 69GPCh. 29 - Prob. 70GPCh. 29 - Prob. 71GPCh. 29 - Prob. 73GPCh. 29 - Prob. 74GPCh. 29 - Prob. 75GPCh. 29 - Prob. 76MSPPCh. 29 - Prob. 77MSPPCh. 29 - Prob. 78MSPPCh. 29 - Prob. 79MSPP
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- a) Calculate the energy of the emissive transition with the lowest energy possible for the Lyman series, for a mole of hydrogen atoms. Express your answer in joules/mol. b) Is this transition in the visible spectral domain? If not, in which region is it located?arrow_forwardIn hydrogen’s characteristic spectra, each series (Lyman, Balmer, etc) has a “series limit”, where the wavelengths at one end of the series tend to “bunch up”, approaching a single limiting value. part a: Is it at the short-wavelength or the long-wavelength end of the series that this series limit occurs? part b: What is it about hydrogen’s allowed energies that leads to this phenomenon?arrow_forwardFrom the energy-level diagram for hydrogen, explain the observation that the frequency of the second Lyman-series line is the sum of the frequencies of the first Lyman-series line and the first Balmer-series line.This is an example of the empirically discovered Ritz combination principle. Use the diagram to find some other valid combinations.arrow_forward
- Tutorial Week 15 1. Find the amount of energy needed in the transition of hydrogen electrons into higher orbits (total of three), absorbing photons which have wavelengths of (1) 1005 nm (2) 1282 nm and (3) 1875 nm. 2. Determine the longest and shortest wavelengths of the Lyman series. 3. Suppose the initial amount of Cesium-137 is 1.5 kg, find the amount of Cesium-137 remain after 1000 years.arrow_forwardWhat is the average radius of the orbit of an electron in the n=2 energy level of an oxygen atom (Z=8)? Express your answer in pico-meters.arrow_forwardIf you look at it, there is an Ag atom with an atomic number of 47. Then, there are electrons from outside hitting electrons in the base shell (n=1) : a. how much energy does the electron need to bounce off? and is there any energy absorbed by the electrons? b. How much the radiation energy and wavelength produced by the transition of electrons from the L shell (n=2) to the ground shell (n=1) in filling the electron holes?arrow_forward
- It is possible that a muon be captured by a proton to form a muonic atom. A muon is identic to an electron, except when your mass, which is m = 105.7 MeV/c^2. What ia the smallest wave length for a Lyman series for this atom? Give your answer in pm.arrow_forwardlmagine an alternate universe where the mass of the electron is 2.4 times larger than in our universe.Assuming that none of the other properties of the universe are changed, what would be the wavelength of the first line (the line with the longest wavelength)in the Lyman series of the hydrogen atom? Give your answer in nm.arrow_forwardThe wavelengths of the Lyman series for hydrogen are given by = RH(1-2), = 2, 3, 4, ... 1/2 (a) Calculate the wavelengths of the first three lines in this series. nm nm nm (b) Identify the region of the electromagnetic spectrum in which these lines appear. O ultraviolet region O infrared region O x-ray region O visible light region O gamma ray regionarrow_forward
- c) The Bohr model of the atom postulated electrons orbiting around the nucleus in stable orbits. De Broglie explained what orbits could exist by postulating that electrons (and any- thing else) with momentum p have an associated wavelength λ, given by λ=h/p where h is Planck's constant. i) For an electron orbiting around a proton (the Bohr model), equating the centripetal force with the Coulomb force gives the expression v² = e²/(4πεmer). Calculate the speed of an electron orbiting at the Bohr radius, ˜Â = 0.053 nm. ii) Calculate the momenta and the de Broglie wavelengths of the electron of part (i) and of a bird (a racing pigeon) that weighs 0.350 kg and flies at 100 km per hour. iii) Compare the wavelength for the electron that you obtain in (ii) with the circumference of the orbit. Comment on this comparison. Explain briefly what it implies about the other possible orbits of the Bohr model and how the higher orbits might be predicted.arrow_forwardc) The Bohr model of the atom postulated electrons orbiting around the nucleus in stable orbits. De Broglie explained what orbits could exist by postulating that electrons (and any- thing else) with momentum p have an associated wavelength λ, given by λ = h/p where h is Planck's constant. i) For an electron orbiting around a proton (the Bohr model), equating the centripetal force with the Coulomb force gives the expression v² = e²/(4πmer). Calculate the speed of an electron orbiting at the Bohr radius, rB 0.053 nm. = ii) Calculate the momenta and the de Broglie wavelengths of the electron of part (i) and of a bird (a racing pigeon) that weighs 0.350 kg and flies at 100 km per hour. iii) Compare the wavelength for the electron that you obtain in (ii) with the circumference of the orbit. Comment on this comparison. Explain briefly what it implies about the other possible orbits of the Bohr model and how the higher orbits might be predicted.arrow_forwardA visible (violet) emission spectral line for chromium (Cr) occurs at wavelength λ = 425.435 nm. A) What is the frequency (ν) of this light?(Give correct units and answer to six significant figures.) B) What is the magnitude of the energy change associated with the emission of one mole of photons of light with this wavelength?arrow_forward
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