one electron that is confined in a molecular orbital that extends over 8 adjacent carbon atoms. The electron can move freely between the 8 atoms. a) Using the one-dimensional particle-in-the-box model, calculate the energy required to promote an electron from then = 2 to the n = 5 level. The length of the box is determined by the C-C bond distance, which is 139 pm. Note: The following information may or may not be useful. n?h? En = Planck's constant = 6.626 x 10-34 J.s; Mass of Electron = 9.109 x 10-28, Rydberg constant = 1.097 x 107 m-1; Speed of Light = 2.998 x 108 m·s-1
one electron that is confined in a molecular orbital that extends over 8 adjacent carbon atoms. The electron can move freely between the 8 atoms. a) Using the one-dimensional particle-in-the-box model, calculate the energy required to promote an electron from then = 2 to the n = 5 level. The length of the box is determined by the C-C bond distance, which is 139 pm. Note: The following information may or may not be useful. n?h? En = Planck's constant = 6.626 x 10-34 J.s; Mass of Electron = 9.109 x 10-28, Rydberg constant = 1.097 x 107 m-1; Speed of Light = 2.998 x 108 m·s-1
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![2. Electrons in molecules can be found in orbitals that extend over more than one atom. Consider
one electron that is confined in a molecular orbital that extends over 8 adjacent carbon atoms.
The electron can move freely between the 8 atoms.
a) Using the one-dimensional particle-in-the-box model, calculate the energy required to
promote an electron from then = 2 to the n = 5 level. The length of the box is determined by
the C-C bond distance, which is 139 pm.
Note: The following information may or may not be useful.
n²h?
En =
8m.L?
Planck's constant = 6.626 x 10-34 J.s; Mass of Electron = 9.109 x 10-28 g;
Rydberg constant = 1.097 x 107 m-1; Speed of Light = 2.998 x 108 m·s-1
b) What frequency of light would cause this excitation?
c) Now imagine a straight chain of 2000 carbon atoms. Assume that the orbital extends over
the entire chain and repeat the calculation fr the required energy to promote an electron
from the n = 2 to n = 5 lever
d) Would you expect the energy levels to get closer or farther apart if you increased the chain
to one million carbon atoms (i.e approaching bulk properties)? Provide a brief explanation
dit](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3a1a8c69-ac20-486b-9f67-8f66504c5494%2F0f1a8182-c96e-40b6-bb09-baa4126ad0d5%2F4vzf6hy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:2. Electrons in molecules can be found in orbitals that extend over more than one atom. Consider
one electron that is confined in a molecular orbital that extends over 8 adjacent carbon atoms.
The electron can move freely between the 8 atoms.
a) Using the one-dimensional particle-in-the-box model, calculate the energy required to
promote an electron from then = 2 to the n = 5 level. The length of the box is determined by
the C-C bond distance, which is 139 pm.
Note: The following information may or may not be useful.
n²h?
En =
8m.L?
Planck's constant = 6.626 x 10-34 J.s; Mass of Electron = 9.109 x 10-28 g;
Rydberg constant = 1.097 x 107 m-1; Speed of Light = 2.998 x 108 m·s-1
b) What frequency of light would cause this excitation?
c) Now imagine a straight chain of 2000 carbon atoms. Assume that the orbital extends over
the entire chain and repeat the calculation fr the required energy to promote an electron
from the n = 2 to n = 5 lever
d) Would you expect the energy levels to get closer or farther apart if you increased the chain
to one million carbon atoms (i.e approaching bulk properties)? Provide a brief explanation
dit
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