When we model light (EM radiation) as a particle, we call it a photon -- a packet of energy. How does this work with the model of light as a wave? To think through this, answer the following: If the intensity of a beam of light is related to the number of photons passing per second, how would you explain the intensity of light using the model of light as a wave? What feature (wavelength, frequency, amplitude, oscillation, etc.) can be a measure of intensity and why do you think so?

When we model light (EM radiation) as a particle, we call it a photon -- a packet of energy. How does this work with the model of light as a wave? To think through this, answer the following: If the intensity of a beam of light is related to the number of photons passing per second, how would you explain the intensity of light using the model of light as a wave? What feature (wavelength, frequency, amplitude, oscillation, etc.) can be a measure of intensity and why do you think so?

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

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 28P: Quantum mechanics predicts that the energy of the ground state of the H atom is 13.6eV . Insight...

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Similar questions

Suppose an atom in an excited state can return to the ground state in two steps. It first falls to an intermediate state, emitting radiation of wavelength 1 , and then to the ground state, emitting radiation of wavelength 2 . The same atom can also return to the ground state in one step, with the emission of radiation of wavelength . How are 1,2, and related? How are the frequencies of the three radiations related?
Photons are emitted in the Lyman series as hydrogen atoms undergo transitions from various excited states to the ground state. If ground-state He+ are present in the same gas (near stars, for example), can they absorb these photons? Explain.
Quantum mechanics predicts that the energy of the ground state of the H atom is 13.6eV . Insight into the magnitude of this quantity is gained by considering several methods by which it can be measured. (a) Calculate the longest wavelength of light that will ionize H atoms in their ground state. (b) Assume the atom is ionized by collision with an electron that transfers all its kinetic energy to the atom in the ionization process. Calculate the speed of the electron before the collision. Express your answer in meters per second (ms1) and miles per hour (milesh1) . (c) Calculate the temperature required to ionize a H atom in its ground state by thermal excitation. (Hint: Recall the criterion for thermal excitation of an oscillator in Planck’s theory of blackbody radiation is that hvkBT .)
In 1885, Johann Balmer, a mathematician, derived the following relation for the wavelength of lines in the visible spectrum of hydrogen =364.5 n2( n2 4) where in nanometers and n is an integer that can be 3, 4, 5, . . . Show that this relation follows from the Bohr equation and the equation using the Rydberg constant. Note that in the Balmer series, the electron is returning to the n=2 level.
The energies of macroscopic objects, as well as those of microscopic objects, are quantized, but the effects of the quantization are not seen because the difference in energy between adjacent states is so small. Apply Bohr’s quantization of angular momentum to the revolution of Earth (mass6.01024kg) , which moves with a speed of 3.0104ms1 in a circular orbit (radius1.51011m) about the sun. The sun can be treated as fixed. Calculate the value of the quantum number n for the present state of the Earthsun system. What would be the effect of an increase in n by 1?
A fellow chemistry student says that low-frequency radiation is short-wavelength radiation. You disagree. Explain why the other student is wrong.
What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon energy? What does a photon energy unit of a joule equal?
The wave function of an electron in the lowest (that is, ground) state of the hydrogen atom is (r)=( 1 a 0 3 )1/2exp(r a 0 )ao=0.5291010m (a) What is the probability of finding the electron inside a sphere of volume 1.0pm2 , centered at the nucleus (1pm=1012m) ? (b) What is the probability of finding the electron in a volume of 1.0pm2 at a distance of 52.9 pm from the nucleus, in a fixed but arbitrary direction? (c) What is the probability of finding the electron in a spherical shell of 1.0 pm in thickness, at a distance of 52.9 pm from the nucleus?
What is the wavelength of a baseball having mass 100.0g traveling at a speed of 160km/hr? What is the wavelength of an electron traveling at the same speed?
a For a pendulum having classical frequency of 1.00s1, what is the energy difference in J between quantized energy levels? b Calculate the wavelength of light that must be absorbed in order for the pendulum to go from one level to another. c Can you determine in what region of the electromagnetic spectrum such a wavelength belongs? d Comment on your results for parts a and b based on your knowledge of the state of science in early twentieth century. Why wasnt the quantum mechanical behavior of nature noticed?
Consider the bright line spectrum of hydrogen shown in Fig. 11.10 . Which line in the spectrum represents photons with the highest energy? With the lowest energy?
Use the mathematical expression for the 2pz wave function of a one-electron atom (see Table 5.2) to show that the probability of finding an electron in that orbital anywhere in the x-y plane is 0. What are the nodal planes for a dxz orbital and for a dx2y2 orbital?