[References] Microwave radiation has a wavelength on the order of 1.6 cm. Calculate the frequency and the energy of a single photon of this radiation. Frequency = s-1 Energy = J Calculate the energy of an Avogadro's number of photons (called an einstein) of this radiation. Energy = Submit Answer Try Another Version 3 item attempts remaining

[References] Microwave radiation has a wavelength on the order of 1.6 cm. Calculate the frequency and the energy of a single photon of this radiation. Frequency = s-1 Energy = J Calculate the energy of an Avogadro's number of photons (called an einstein) of this radiation. Energy = Submit Answer Try Another Version 3 item attempts remaining

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

Chapter4: Introduction To Quantum Mechanics

Section: Chapter Questions

Problem 16P: The power output of a laser is measured by its wattage, that is, the number of joules of energy it...

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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.
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.)
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 power output of a laser is measured by its wattage, that is, the number of joules of energy it radiates per second (1W=1Js1) . A 10-W laser produces a beam of green light with a wavelength of 520 nm (5.2107m) . (a) Calculate the energy carried by each photon. (b) Calculate the number of photons emitted by the laser per second.
Lasers are now used for the total or partial removal of skin tattoos. A laser with a wavelenth of 755 nm is used to remove tattoos in green or blue inks. (a) How much energy (in kJ/mol) is given off by the laser? (b) Compare the energy obtained in (a) with that given off by an x-ray (=1109m).
The Doppler effect is one of the sources of the line broadening in atomic absorption spectroscopy. Atoms moving toward the light source encounter higher-frequency radiation than atoms moving away from the source. The difference in wavelength experienced by an atom moving at speed v (compared to one atrest) is / = v/c , where c is the velocity of light. Estimate the line width (in nanometers) of the lithiumline at 670.776(6707.76 Å) when the absorbing atoms are at a temperature of (a) 2000 K and (b) 3120 K.The average speed of an atom is given by v=8kT/m , where k is Boltzmann’s constant, Tis the absolute temperature, and m is its mass.
When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
Ozone in the stratosphere absorbs ultraviolet light of wavelengths shorter than 320 nm, thus filtering out the most energetic radiation from sunlight. During this absorption, an ozone molecule absorbs a photon, which breaks an oxygen-oxygen bond, yielding an oxygen molecule and an oxygen atom: O3(g)+hvO2(g)+O(g) (Here, hv denotes a photon.) Suppose a flask of ozone is irradiated with a pulse of UV light of wavelength 275 nm. Assuming that each photon of this pulse that is absorbed breaks up one ozone molecule, calculate the energy absorbed per mole of O2 produced, giving the answer in kJ/mol.
6.103 Atomic absorption spectroscopy is based on the atomic spectra of the elements being studied. It can be used to determine the impurities in a metal sample. If an element is present, light at the appropriate wavelength is absorbed. You are working with a metal stamping company and the rolled steel you use to form panels for automobile doors is failing at an alarming rate. There is some chance that the problem is unacceptably high levels of manganese in the steel. Given that the atomic spectrum of manganese has three lines near 403 nm, how could you use a spectrometer to determine the amount of manganese in the steel?