9. The energy of an electron in a one dimensional particle in a box is given by E, =n'h'/8m,a. The mass of an electron is 9.1094 x 10 31 kg. If a is taken as the average length of a carbon-carbon bond, the energy needed to excite an electron from the n=1 (ground) state to the n=2 (1ª excited) state corresponds to light of wavelength 17.0 nm. Assuming that an electron in a bond is approximated by the particle-in-a- box model, calculate the average length of a carbon-carbon bond, i.e. "a".

9. The energy of an electron in a one dimensional particle in a box is given by E, =n'h'/8m,a. The mass of an electron is 9.1094 x 10 31 kg. If a is taken as the average length of a carbon-carbon bond, the energy needed to excite an electron from the n=1 (ground) state to the n=2 (1ª excited) state corresponds to light of wavelength 17.0 nm. Assuming that an electron in a bond is approximated by the particle-in-a- box model, calculate the average length of a carbon-carbon bond, i.e. "a".

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 161CP: The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase....

See similar textbooks

Similar questions

The Lyman series of spectral lines for the H atom, in the ultraviolet region, arises from transitions from higher levels to n = 1. Calculate the frequency and wavelength of the least energetic line in this series.
Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of electromagnetic radiation that can completely remove (ionize) the electron from the H atom is 1460 nm. What is the initial excited state for the electron (n = ?)?
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.
This laser emits green light with a wavelength of 533 nm. (a) What is the energy, in joules, of one photon of light at this wavelength? (b) If a particular laser produces 1.00 watt (W) of power (1 W = 1 J/s), how many photons are produced each second by the laser?
The most prominent line in the emission spectrum of aluminum is at 396.15nm. What is the frequency of this line? What is the energy of one photon with this wavelength? Of 1.00 mol of these photons?
In a FranckHertz experiment on sodium atoms, the first excitation threshold occurs at 2.103 eV. Calculate the wavelength of emitted light expected just above this threshold. (Note: Sodium vapor lamps used in street lighting emit spectral lines with wavelengths 5891.8 and 5889.9 Å.)
6.9 If a string of decorative lights includes bulbs with wave-lengths of 480, 580, and 700 mm, what are the frequencies of the lights? Use Figure 6.6 to determine which colors are in the set.
The wave function for the 2pz, orbital in the hydrogen atom is 2pl=142(za0)3/2e/2cos where a0 is the value for the radius of the first Bohr orbit in meters (5.29 | 1011), is Z(r/a0), r is the value for the distance from the nucleus in meters, and is an angle. Calculate the value of 2pz2 at r = a0 for = 0 (z axis) and for = 90 (xy plane).
6.17 The laser in most supermarket barcode scanners operates at a wavelength of 632.8 nm. What is the energy of a single photon emitted by such a laser? What is the energy of one mole of these photons?
Show that the value of the Rydberg constant per photon, 2.179 1018 J, is equivalent to 1312 kJ/mol photons.