This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the S1 prefix 'zepto' means 10 any SI prefix in the ALEKS Data tab.) 142 18 energy (23) NO. 200 -B I Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from A to B, will a photon be absorbed or emitted? 0 O absorbed O emitted 0.8 X You can find the meaning of

This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the S1 prefix 'zepto' means 10 any SI prefix in the ALEKS Data tab.) 142 18 energy (23) NO. 200 -B I Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from A to B, will a photon be absorbed or emitted? 0 O absorbed O emitted 0.8 X You can find the meaning of

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 13ALQ

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Similar questions

For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.
Suppose an atom in an excited state can return to the ground state in two steps. It first falls to an intermediate state, emitting radiation of wavelength 1 , and then to the ground state, emitting radiation of wavelength 2 . The same atom can also return to the ground state in one step, with the emission of radiation of wavelength . How are 1,2, and related? How are the frequencies of the three radiations related?
The energy needed to ionize an atom of element X when it is in its most stable state is 500kJmol1 . However, if an atom of X is in its lowest excited state, only 120kJmol1 is needed to ionize it. What is the wavelength of the radiation emitted when an atom of X undergoes a transition from the lowest excited state to the ground state?
When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
What is the difference between an atom’s ground state and an excited state?
The following is an energy-level diagram for electronic transitions in the Bohr hydrogen atom. a. Explain why the energy levels get closer together as they increase. Provide mathematical support for this. b. Verify that the colors given in the diagram are correct. Provide mathematical support.
Estimate the probability of finding an electron which is excited into the 2s orbital of the H atom, looking in a cubical box of volume 0.751036m3 centered at the nucleus. Then estimate the probability of finding the electron if you move the volume searched to a distance of 105.8 pm from the nucleus in the positive z direction. (Note that since these volumes are small, it does not matter whether the volume searched is cubical or spherical.)
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?
6.86 An excited He+ ion returns to the ground state by emitting a series of three photons, with wavelengths of 26 nm, 469 nm, and 1014 nm. The process is represented in the energy level diagram below. Which arrow (A, B, or C) in the diagram represents the 1014-nm light?
Consider the bright line spectrum of hydrogen shown in Fig. 11.10 . Which line in the spectrum represents photons with the highest energy? With the lowest energy?
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?