nt BACK PRINTER VERSION FULL SCREEN CALCULATOR SPECTROSCOPY AND REACTIVITY TO4/S06 The energy levels the electron can occupy in the Bet ion can be calculated using the energy level equation. A Be emitted a photon with a frequency of 9.86 x 105 Hz. What is the value of the level n for the new energy? ion with an electron in the n 4.00 level Speed of Light c 3.00x108 m/s Planck's Constant h 6.63x1034 J S Rydberg's Constant RH=2.18x1o-18J Avogadro's No. NA 6.02x1023mol1 Energy Level Eqn En(J)-RH(Z2/n2) Z=nuclear charge =quantum number exact number, no tolerance

nt BACK PRINTER VERSION FULL SCREEN CALCULATOR SPECTROSCOPY AND REACTIVITY TO4/S06 The energy levels the electron can occupy in the Bet ion can be calculated using the energy level equation. A Be emitted a photon with a frequency of 9.86 x 105 Hz. What is the value of the level n for the new energy? ion with an electron in the n 4.00 level Speed of Light c 3.00x108 m/s Planck's Constant h 6.63x1034 J S Rydberg's Constant RH=2.18x1o-18J Avogadro's No. NA 6.02x1023mol1 Energy Level Eqn En(J)-RH(Z2/n2) Z=nuclear charge =quantum number exact number, no tolerance

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter6: Electronic Structure And The Periodic Table

Section: Chapter Questions

Problem 80QAP: In the photoelectric effect, electrons are ejected from a metal surface when light strikes it. A...

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6.27 Refer w the data and energy-Ievel diagram shown in Problem 6.26, and find the wavelength of light that would be emitted when a hydrogen atom undergoes the transition from the state labeled as n = 4 to the state labeled as n = 2. Express your answer in nm.
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 = ?)?
Calculate En for n=1,2,3, and 4 (R H=2.1801018J). Make a one-dimensional graph showing energy, at different values of n, increasing vertically. On this graph, indicate by vertical arrows transitions in the (a) Lyman series (nlo=1) (b) Balmer series (nlo=2).
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.
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.
Tbe relative orbital levels for the hydrogen atom can be represented as Draw the relative orbital energy levels for atoms with more than one electron and explain your answer. Also explain bow the following radial probability distributions support your answer.
As the weapons officer aboard the Srarship Chemistry, it is your duty to configure a photon torpedo to remove an electron from the outer hull of an enemy vessel. You know that the work function (the binding energy of the electron) of the hull of the enemy ship is 7.52 1019 J. a. What wavelength does your photon torpedo need to be to eject an electron? b. You find an extra photon torpedo with a wavelength of 259 nm and fire it at the enemy vessel. Does this photon torpedo do any damage to the ship (does it eject an electron)? c. If the hull of the enemy vessel is made of the element with an electron configura tion of [Ar]4s13d10, what metal is this?
6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?
Sketch the major features (number of peaks and relative intensities for the peaks) of the expected photoelectron spectrum for atoms of nitrogen.

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