Problem Solving: Solve the following problems. 1. Studies of the spectral lines of hydrogen show that the highest frequency of electromagnetic radiation emitted by a hydrogen atom is about 3.28 x 1015 Hz. a. What is the energy of one of the corresponding photons? b. Does this light fall in the infrared, visible, or ultraviolet part of the electromagnetic spectrum? Hint: the approximate short-wavelength end of the visible range is at A = 400 nm. C. How does this photon energy compare with the ionization energy of the hydrogen atom, 13.6 eV? %3D 2. A photon has an energy of 6.0eV. What is the frequency of the radiation?

Problem Solving: Solve the following problems. 1. Studies of the spectral lines of hydrogen show that the highest frequency of electromagnetic radiation emitted by a hydrogen atom is about 3.28 x 1015 Hz. a. What is the energy of one of the corresponding photons? b. Does this light fall in the infrared, visible, or ultraviolet part of the electromagnetic spectrum? Hint: the approximate short-wavelength end of the visible range is at A = 400 nm. C. How does this photon energy compare with the ionization energy of the hydrogen atom, 13.6 eV? %3D 2. A photon has an energy of 6.0eV. What is the frequency of the radiation?

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

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Determine the wavelengths of the visible emission bands in the hydrogen spectrum arising from n2= 4, 5, and 6. A. 410 nm, 386nm, 340nm B. 486nm, 434nm, 410nm C. 1100nm, 486nm, 434nm D. 486nm, 434nm, 384nm E. 1260nm, 1100nm, 486nm
A photon with an energy of 3-eV is absorbed by a certain atom. Afterwards, three photons are spontaneously emitted. Which statement correctly describes the emitted photons? a.) The emitted photons each have the same wavelengths. b.) The photons are produced by a single electron energy-level transition. c.) The sum of the emitted photon energies equals 3 eV. d.) Three photons are always emitted when a 3-eV photon is absorbed.
using the Bohr model of a hydrogen atom, consider the transition from n= 5 to n=3. what is the frequency of the photons emitted by hydrogen atoms when they undergo transitions from n =5 to n=3?
values, and get the results.) 1. Figure on the right is an energy-level diagram for a simple atom. (a) What wavelengths, in nm, appear in the atom's emission spectrum? (b) What wavelengths, in nm, appear in the atom's absorption spectrum? n = 3 E, = 4.00 eV n = 2 E, = 1.50 eV n = 1 E, = 0.00 eV
Exercises 1. An electron initially moves in first excited state, if it absorb energy with frequency 5x10 Hz. Find the momentum of this electron before and after interaction with photon energy. 2. An electron initially moving in the third orbit around the nucleus of the hydrogen atom. Find the photo energy which emitted from the electron transition to first excited orbit (using Rydberg formula). Calculate the De-Broglie wavelength of the electron in the orbit before transition. 3. Determine the De Broglie wavelength for electron moving in the third excited orbit around the nucleus of the hydrogen atom. 4. Calculate the De Broglie wavelength of an electron moving around a hydrogen atom with radius of 0.529x100 m.
Combine the equations on slide 10 to obtain the expressions for the radius of the electron orbit and the energy of the hydrogen atom given on slide 11.
a. Does a hot, thin gas emit a continuous spectrum, a bright line spectra with gaps between the lines, or a dark line spectra with all frequencies except the missing (absorbed) one? b. Why do we see dark line spectra when we look at stars? c. Both hydrogen and helium glow and absorb red. Are they the same frequency of red? d. A hot solid iron plate and a hot solid aluminum plate are the same temperature. Do the give off the same range of frequencies?
2. An electron in the n = 2 state of hydrogen remains there on the average of about 108 s, before making a transition to n = 1 state. Estimate the uncertainty in the energy of the n = 2 state. What fraction of the transition energy is this? What is the wavelength and width of this line in the spectrum of hydrogen atom? (a
1. The following graphical data was obtained for the wavefunction of a photon. The wavefunction is of the form Y(x) = Asin (Bx). a. Determine A. b. Determine B. c. Determine the wavelength,2, in meters (assume the x-axis of the graph is distance in meters). d. Determine the linear frequency, v, in s'¹. e. Determine the energy, E, of this photon in J.
Find the largest possible wavelength for electrons (m = 9.11 x 10-31kg emitted from sodium (work function is 3.68 x 10-19 J) when ultra-violet light (E = 5.90 x 10-19 J) shines on it.A. 6.39 x 10-10 mB. 8.10 x 10-10 mC. 1.04 x 10-9 mD. 1.47 x 10-9 mE. There is no maximum wavelength.
1. Show that the frequency of the photon emitted by a hydrogen atom in going from state n + 1 to n is always intermediate between the frequencies of revolution of the electron in the two orbits. 2. A µ − muon is in the n = 2 state of a muonic atom whose nucleus is a proton.Find the wavelength of the photon emitted when the muonic atom drops to its ground state. Consider nuclear motion in your calculation. Values for certain constants:h = 6.626 × 10 −34 Js, E 1 = −13.6 eV, r 1 = 5.29 × 10 −11 m, 1 eV = 1.602 × 10 −19 J.
2. Use Max Planck's quantum theory to explain the following behaviour of photoelectrons. a. Low-intensity light does not release any photoelectrons. What will happen if the light is made brighter? Explain your reasoning. b. Low-intensity light releases photoelectrons. What will happen if the light is made brighter? Explain your reasoning. c. Low-intensity light does not release any photoelectrons. What will happen if the frequency of the light is gradually increased? Explain your reasoning.