C Solved: One reason spe X Y One reason spectrosco X y Choose all possible valu X ect.mheducation.com/flow/connect.html work i Soved 2 attempts left Check my work Be sure to answer all parts. One reason spectroscopists study excited states is to gain information about the energies of orbitals that are unoceupied in an atom's ground state. The following electron configuration represents an atom in an excited state. Identify the element and write its condensed ground-state configuration: 1s°2s²2p°3s°3p°4s*3d*4p! Element symbol: Mn Condensed ground-state configuration: [Ar]3d 4s (Remember to use square brackets, and do not forget to superseript only the electron values.) 13 of 32 Next O search LEEN

C Solved: One reason spe X Y One reason spectrosco X y Choose all possible valu X ect.mheducation.com/flow/connect.html work i Soved 2 attempts left Check my work Be sure to answer all parts. One reason spectroscopists study excited states is to gain information about the energies of orbitals that are unoceupied in an atom's ground state. The following electron configuration represents an atom in an excited state. Identify the element and write its condensed ground-state configuration: 1s°2s²2p°3s°3p°4s3d4p! Element symbol: Mn Condensed ground-state configuration: [Ar]3d 4s (Remember to use square brackets, and do not forget to superseript only the electron values.) 13 of 32 Next O search LEEN

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 55AP: The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in...

See similar textbooks

Similar questions

Construct an energy level diagram showing all orbitals for the hydrogen atom up to n=5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?
Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom).
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.
Using Table 5.2, write down the mathematical expression for the 2px wave function for an electronically excited H atom. Estimate the probability of finding the 2px electron if you look in a cubical box of volume of 0.8(pm)3 centered at a distance of 0.5001010m in the =/2 , =0 direction. Does this probability change as you change ? At what angles is the probability of finding the electron smallest and at what angles is the probability the largest? (Note that =2 is the same location as =0 , so don’t double count.)
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.)
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.
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.
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?
Use the mathematical expression for the 2pz wave function of a one-electron atom (see Table 5.2) to show that the probability of finding an electron in that orbital anywhere in the x-y plane is 0. What are the nodal planes for a dxz orbital and for a dx2y2 orbital?
Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.
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?