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$\bullet$ (a) Use the information for neon shown in Fig. 28.26 to compute the energy difference for the $5 s-$ to- 3$p$ transition in neon. Express your result in electron volts and in joules. (b) Calculate the wavelength of a photon having this energy, and compare your result with the observed wavelength of the laser light. (c) What is the wavelength of the light from the $3 p-$ to- $-3 s$ transition in neon?

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621.2 $\mathrm{nm}$

Physics 102 Electricity and Magnetism

Physics 103

Chapter 28

Photons, Electrons, and Atoms

Electromagnetic Waves

Atomic Physics

Rutgers, The State University of New Jersey

University of Michigan - Ann Arbor

Hope College

McMaster University

Lectures

02:42

Atomic physics is the field of physics that studies atoms as an isolated system of electrons and an atomic nucleus. It is primarily concerned with the arrangement of electrons around the nucleus and the processes by which these arrangements change. The theory of quantum mechanics, a set of mathematical rules that describe the behaviour of matter and its interactions, provides a good model for the description of atomic structure and properties.

03:50

In atomic physics, the Rutherford-Bohr model or Bohr model or Bohr model of the atom was first proposed by Niels Bohr in 1913. It was the first quantum theory of the atomic structure, applying the principles of quantum mechanics to the hydrogen atom. The Rutherford-Bohr model is a planetary model in which the electron is assumed to revolve around the nucleus in circular orbits. The Rutherford-Bohr model of the atom was based on Max Planck's quantum theory of radiation, which explained the spectrum of blackbody radiation, and Albert Einstein's theory of the photoelectric effect, which explained the origin of the spectrum of line emission from atoms. The Bohr model of the atom was the first to explain the discrete spectrum of hydrogen and how the spectral lines of the hydrogen atom were split into multiple spectral lines in a phenomenon called the fine structure. It introduced the Bohr radius and the concept of quantum levels to explain the discrete nature of the spectrum of the hydrogen atom. The Bohr model of the atom had a significant influence on the development of quantum mechanics, and was instrumental in the development and validation of quantum mechanics.

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(a) Use the information fo…

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Figure 30.39 shows the ene…

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02:28

Neon gas is generally used…

01:52

Figure $\mathrm{P} 42.44$ …

03:12

A photon is emitted when a…

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Figure $\mathrm{P} 42.52$ …

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Consider a Bohr model of d…

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Find the wavelength of a p…

Okay, so I've copied over for us. The energy diagram for Neon in part a were asked about the energy change associated with the five s 23 p transition. So five of us has an energy of 20.66 TV and three p has an energy of 18.70 e v. So the gap in energy is simply 20.66 minus 18.70 this's equal toe 1.96 TV. And if we want to convert that to Jules, we simply multiply it by 1.6 times 10 to the negative 19 in part B were asked what wavelength is associated with this transition? And we know that he is equal to H C over Lambda So Lamda equals H C over E for H. We want to express it in electron volts for 0.14 times 10 to the negative 15. And the e that we use is our answer to part A. She's 1.96 and this comes out to 633 nana meters. The known value is 632.8. So this is consistent in part see where I saw it. A different transition. We now have three Peter three. Yes. So, again, we just read off the energy levels. We have 18.70 minus 16.70 gives to me. And once again, we solve for Lambda. Using Lambda is equal to H C over e same formula we had before or only now, in the denominator we're going to use to evey instead of 1.96 And in this case, lamb that comes out to 620 nanometers.

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