This energy diagram shows the allowed energy levels of an electrpn in a certain atom. (Note: the SI prefix 'zepto' means 10 can find the meaning of any SI prefix in the ALEKS Data tab.) 1400- 1200- 1000. energy (zJ) 800- 600 400- 200 0 C If the electron makes the transition shown by the red arrow, from B to A, calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits B -A Use this diagram to complete the table below. B nm 10 X S . You Submit

This energy diagram shows the allowed energy levels of an electrpn in a certain atom. (Note: the SI prefix 'zepto' means 10 can find the meaning of any SI prefix in the ALEKS Data tab.) 1400- 1200- 1000. energy (zJ) 800- 600 400- 200 0 C If the electron makes the transition shown by the red arrow, from B to A, calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits B -A Use this diagram to complete the table below. B nm 10 X S . You Submit

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 84E: Tbe relative orbital levels for the hydrogen atom can be represented as Draw the relative orbital...

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Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff, using the spectroscope they invented in 1859. The name came from the Latin caesius ("sky blue") because of the prominent blue line observed for this element at 455.5 nm. Calculate the frequency and energy of a photon of this light.
6.27 Refer w the data and energy-Ievel diagram shown in Problem 6.26, and find the wavelength of light that would be emitted when a hydrogen atom undergoes the transition from the state labeled as n = 4 to the state labeled as n = 2. Express your answer in nm.
The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?
The energy of a photon is 3.05 1019 J. What is the wavelength of the corresponding light? What is the color of this light?
The green line in the atomic spectrum of thallium has a wavelength of 535 nm. Calculate the energy of a photon of this light.
The colors of the visible spectrum and the wavelengths corresponding to the colors are given in Figure 5.2. (a) Which colors of light involve photons with less energy per photon than yellow light? (b) Which color of visible light has photons of greater energy, green or violet? (c) Which color of light has the greater frequency, blue or green?
6.28 A neon atom cmi light at many wavelengths, two of which are at 616.4 and 638.3 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) If a transition between the two higher energy states could be observed, what would be the frequency of the light?
Selenium atoms have a particular transition that emits light of frequency 1.53 1015 Hz. (Hz is the abbreviation for hertz, which is equivalent to the unit/s, or s1.) Is this light in the visible spectrum? If so, what is the color of the light? (See Figure 7.5.)
What are the allowed values for each of the four quantum numbers: n, l, ml, and ms?
6.85 The visible lines in the hydrogen atom emission spectrum arise from transitions with a final state with n = 2. In what spectral region should we expect to find transitions that have a final state of n = 1 ? Explain your reasoning using an energy level diagram similar to the one in Problem 6.26.
Tbe relative orbital levels for the hydrogen atom can be represented as Draw the relative orbital energy levels for atoms with more than one electron and explain your answer. Also explain bow the following radial probability distributions support your answer.