T15. For each of the following statements, identify which quantum number (n, l, m¡ or m,) that is beingdescribed or referenced. (place answer in blank) (7 points)A)principal quantum numberB)relates to eléctron spinC)relates to the electron shellD)relates to the orientation in space for the orbitalE)relates to the shape of the orbitalF)represents a different type of orbital within a shellG)number of values for a given subshell equals 21 + 1

A) principal quantum number - - > n B) relates to electron spin - - > ms C) relates to the…

15. For each of the following statements, identify which quantum number (n, I, mj or m,) that is being described or referenced. (place answer in blank) (7 points) A) principal quantum number B) relates to electron spin relates to the electron shell D) relates to the orientation in space for the orbital E) relates to the shape of the orbital represents a different type of orbital within a shell number of values for a given subshell equals 21+ 1

15. For each of the following statements, identify which quantum number (n, I, mj or m,) that is being described or referenced. (place answer in blank) (7 points) A) principal quantum number B) relates to electron spin relates to the electron shell D) relates to the orientation in space for the orbital E) relates to the shape of the orbital represents a different type of orbital within a shell number of values for a given subshell equals 21+ 1

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 12P: The helium ion He+ is a one-electron system whose wave functions and energy levels are obtained from...

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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.
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.)
Suppose that the spin quantum number had three allowed values (ms=0,+12,12) . Give the atomic numbers of the first three noble-gas atoms in this case.
Spectroscopic studies of Li also show that Zeff(2p)=1.02 . Estimate the energy of the 2p orbital of Li. Calculate the average distance of the electron from the nucleus in the 2p orbital of Li. Comparing your results with those in Problem 13 shows that the energy values differ by about 50%, whereas the average distances are nearly equal. Explain this observation.
Explain why the wave model for radiation cannot account for the photoelectric effect.
Using a simple particle-in-a-box model for the multiple bonding in 1,2-butadiene (see Example 4.7) and the n=2 wave function for the weakest bound electron, calculate the probability of finding the electron in an 0.1 interval centered midway between the two inner carbon atoms (that is, the center is at x=2.11 , so this interval is from x1=2.06 to x2=2.16 ). Then calculate the probability of finding the electron in an 0.1 interval centered midway between an end carbon atom and the carbon atom that is double-bonded to it in the Lewis dot structure. (You may calculate the appropriate integrals or estimate the relevant areas under the curve graphically.) Then recalculate the probabilities by approximating the integral as |( x 0)|2x , where x0 is evaluated in the middle of the range from x1 to x2 . Finally, explain why you can’t approximate the integral needed for Problem 37(a) in this way.
Why isnt the electron configuration of beryllium, given as 1s22s2, considered a violation of the Pauli principle? Hint: See example 12.6.
In the Brackett series, nlo=4. (a) Calculate the wavelength in nanometers of a transition from n=6 to n=4. (b) In what spectral region are these lines formed?
The wave function of an electron in the lowest (that is, ground) state of the hydrogen atom is (r)=( 1 a 0 3 )1/2exp(r a 0 )ao=0.5291010m (a) What is the probability of finding the electron inside a sphere of volume 1.0pm2 , centered at the nucleus (1pm=1012m) ? (b) What is the probability of finding the electron in a volume of 1.0pm2 at a distance of 52.9 pm from the nucleus, in a fixed but arbitrary direction? (c) What is the probability of finding the electron in a spherical shell of 1.0 pm in thickness, at a distance of 52.9 pm from the nucleus?
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.
The helium ion He+ is a one-electron system whose wave functions and energy levels are obtained from those for H by changing the atomic number to Z=2 . Calculate the average distance of the electron from the nucleus in the 2s orbital and in the 2p orbital. Compare your results with those in Problem 11 and explain the difference.
What are the values of E, L, and Lz for an F8+ atom whose electron has the following wavefunctions, listed as n,l,ml? a 1,0,0 b 3,2,2c 2,1,1d 9,6,3.