The following figure represents the emission spectrum of a hydrogenlike ion (Z is not 1 but has one electron) in the gas phase. All the lines result from the electronic If the wavelength of line C is 27.1 nm, calculate the wavelength of line A and the 21d ionization energy (ionization energy if electron is at n=2). hint: calculate Z first using 27.1 nm -m.Z´e* | 1 8h Eo 1 AE=E,-E,=hv=D - 2 2 2 n n Continuum- B A

The following figure represents the emission spectrum of a hydrogenlike ion (Z is not 1 but has one electron) in the gas phase. All the lines result from the electronic If the wavelength of line C is 27.1 nm, calculate the wavelength of line A and the 21d ionization energy (ionization energy if electron is at n=2). hint: calculate Z first using 27.1 nm -m.Z´e* | 1 8h Eo 1 AE=E,-E,=hv=D - 2 2 2 n n Continuum- B 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 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.
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?
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 = ?)?
In the photoelectric effect, electrons are ejected from a metal surface when light strikes it. A certain minimum energy, Emin, is required to eject an electron. Any energy absorbed beyond that minimum gives kinetic energy to the electron. It is found that when light at a wavelength of 540 nm falls on a cesium surface, an electron is ejected with a kinetic energy of 2.601020J. When the wavelength is 400 nm, the kinetic energy is 1.541019J. (a) Calculate Emin for cesium in joules. (b) Calculate the longest wavelength, in nanometers, that will eject electrons from cesium.
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).
Imagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and mi quantum numbers are unchanged from those of our world. Write the quantum numbers for the first two shells (i.e., n = 1 and n = 2).
Potassium atoms in a flame emit light as they undergo transitions from one energy level to another that is 4.91019J lower in energy. Calculate the wavelength of light emitted and, by referring to Figure 4.3, predict the color visible in the flame.