Energy levels The diagram on the left shows several energy levels for a hydrogen atom. Four possible electron energy level transitions are labeled. 13.6 eV 12.8 eV 12.1 eV 10.2 eV Il II IV Oev 11. Which energy level transition would emit a photon with the largest wavelength? O Transition I O Transition II O Transition III O Transition IV

Energy levels The diagram on the left shows several energy levels for a hydrogen atom. Four possible electron energy level transitions are labeled. 13.6 eV 12.8 eV 12.1 eV 10.2 eV Il II IV Oev 11. Which energy level transition would emit a photon with the largest wavelength? O Transition I O Transition II O Transition III O Transition IV

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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1
A hypothetical atom has energy levels given in the figure below. Which figure most accurately depicts the absorption spectrum, assuming all transitions between energy levels is possible? The black vertical lines represent the absorbed wavelengths. Eo = -11.5 eV E₁ = -9.6 eV E₂ = -5.2 eV O E3 = -1.1 eV wavelength increases → wavelength increases → wavelength increases → wavelength increases → wavelength increases →
The 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?
Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108 m/s. a. 1.89/hxc b. hc/1.89 c. 1.89 x h x c d. (1.51 + 3.4)/hc e. hc/3.4
Figure below shows electron energy levels in a hydrogen atom. The arrows show four possible transitions. n = 4 n= 3 D B n= 2 E A n = 1 Which transition emits the shortest wavelength? O B O E O A
Infrared light with a wavelength of 1870 nm is emitted from hydrogen. What are the quantum numbers of the two states involved in the transition that emits this light?
Question 14 a) A narrow beam of white light is passed through a clear glass vessel containing cool hydrogen gas at a low pressure. A prism is used to disperse the light leaving the vessel. This results in a white light spectrum, crossed by a series of dark lines. Explain the origin of these dark lines and name the type of spectrum that is produced. b) Some of the atomic energy levels of hydrogen are shown in the diagram below. i. ii. iii. Energy/eV 0 -0.85 -1.51 -3.39 -13.58 n = 4 n = 3 n = 2 n = 1 Determine the ionization energy of hydrogen and express this in joules. Determine the wavelength of the light emitted when an electron falls from the n = 3 level to the n = 1 energy level. A photon of energy 10.19 eV is in collision with a hydrogen atom. What would happen to this photon?
What wavelength of light is emitted by a hydrogen atom in which an electron makes a transition from the n = 5 to the n = 2 state? Enter this wavelength expressed in nanometers to one decimal place. 1 nm = 1 x 10-9 m Assume the Bohr model.
As shown a few energy levels of the mercury atom. One valence electron is always in the 6s state; the other electron changes states. Make a table showing all of the allowed transitions in the emission spectrum. For each transition, indicatea. The wavelength, in nm.b. Whether the transition is in the infrared, the visible, or the ultraviolet spectral region.c. Whether or not the transition would be observed in the mercury absorption spectrum.
What is the frequency of the photon emitted by a hydrogen atom when its electron drops from the n = 6 to n = 4 energy level? [? ] × 10¹²] Hz Coefficient (green) Exponent (yellow) Enter
7. When an electron transitions from the third excited state to the ground state in a hydrogen atom, the energy emitted in one photon is: A. 12.7 eV B. 10.5 eV C. 3.6 eV D. 0 eV
Figure below shows electron energy levels in a hydrogen atom. The arrows show four possible transitions. n = 4 n = 3 B n = 2 E A n = 1 Which transition emits the shor wavelength? O E O A Ов