Schaum's Outline of College Physics, Twelfth Edition (Schaum's Outlines)
12th Edition
ISBN: 9781259587399
Author: Eugene Hecht
Publisher: McGraw-Hill Education
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Chapter 43, Problem 20SP
To determine
The wavelength of the emitted photon when the hydrogen atom drops from the first excited state to the ground state.
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The two nuclei in the carbon monoxide (CO) molecules are 0.1128 nm apart. The mass of the carbon atom is 1.993x10-26 kg. The mass of the oxygen atom is 2.656x10-26 kg.What is the wavelength of the photon emitted in the transition from first excited state to the ground state? (Give your answer in mm.) [answer is not 1.291]
Unexcited hydrogen atoms are bombarded with electrons that have been accelerated through
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[06/04, 2:13 PM] +91 93814 04108: The minimum amount of energy required to energize a particle from its ground state to first excited state is 1*10^4 eV. One photon source P1 corresponding to X ray wavelength 1nm and another photon source p2 corresponding to visible light wavelength 500 nm are available. As a physicist, which one of these photons would you choose for energizing the atom?
[06/04, 2:14 PM] +91 93814 04108: Draw a neat diagram to show the procedure and show your calculations in detail.
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Schaum's Outline of College Physics, Twelfth Edition (Schaum's Outlines)
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- A hydrogen atom is excited from its ground state to the n4 state. The atom subsequently emits three photons, one of which has a wavelength of 657 mm What are the wavelengths of the other two photons? Express your answers in nanometers. Enter your answers in ascending order separated by comma. [5] ΑΣΦΑ 1873,122 Submit Previous Answers Request Answer Provide Feedback X Incorrect: Try Again: 19 attempts remaining → 99+ a neverw ? SURMIEY amarrow_forward(v):A hydrogen atom makes a transition from a bound state (Energy of the bound state = 0.11 eV) to a state with excitation energy (= 10.2 eV). Calculate the energy of the photon emitted.arrow_forwardCalculate the wavelength of the photon emitted when a particle of mass 1.0 x 10-27 g, in a potential box of length 6.0 Å, goes from the = 5 to the = 4 level. [5]arrow_forward
- It requires 3.69 x 10-19 J of energy to eject an electron from potassium metal. Calculate the minimum frequency of light necessary to do this [E=hv]. Write the units of frequency.arrow_forward(2.13) Selection rules in hydrogen Hydrogen atoms are excited (by a pulse of laser light that drives a multi-photon process) to a spe- cific configuration and the subsequent spontaneous emission is resolved using a spectrograph. Infra- red and visible spectral lines are detected only at the wavelengths 4.05 um, 1.87 µm and 0.656 µm. Explain these observations and give the values of n and l for the configurations involved in these transitions.arrow_forwardA hydrogen atom is in its ground state (n, = 1) when a photon impinges upon it. The atom absorbs the photon, which has precisely the energy required to raise the atom to the n, = 3 state. (a) What was the photon's energy (in eV)? 12.089 ev (b) Later, the atom returns to the ground state, emitting one or more photons in the process. Which of the following energies describes photons that might be emitted thus? (Select all that apply.) O 13.6 ev O 1.89 eV V 12.1 eV O 10.2 ev There are two ways a hydrogen atom in the n, = 3 state can end up in the ground state. In the first, all of the energy goes into one photon and the electron moves directly into the ground state. (What would be the energy of that photon?) In the other, the electron "descends" in two stages, each accompanied by the emission of a photon. (What would be the energies of those two photons?)arrow_forward
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