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Although the Bohr atomic model accurately explained the behavior of a hydrogen atom, it was unable to explain the behavior of any other atom Verify the limitations of the Bohr model by analyzing an electron transition in a neon atom Unlike a hydrogen atom, a neon atom has ten electrons One of these electrons makes a transition between the n 5 and the n 3 energy states, emitting a photon in the process 1 Assuming that the neon atom s electron can be treated as an electron in a
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2 Assuming that the neon atom s electron can be treated as an electron in a
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3 The actual wavelength of the photon emitted during the transition is 6328 nm
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The Bohr model was a major contribution to scientists understanding of the structure of the atom In addition to calculating the emission spectrum, Bohr and his students were able to calculate the ionization energy of a hydrogen atom The ionization energy of an atom is the energy needed to completely free an electron from an atom The calculated ionization value closely agreed with experimental data The Bohr model further provided an explanation of some of the chemical properties of the elements The idea that atoms have electron arrangements unique to each element is the foundation of much of our knowledge of chemical reactions and bonding Niels Bohr, whose accomplishments are commemorated in the stamps shown in Figure 28-12, was awarded a Nobel prize in 1922
Figure 28-12 Honored in these postage stamps from Denmark and Sweden, Niels Bohr s great contribution to our understanding of the atom earned him worldwide recognition and a Nobel prize
281 Section Review
9 Rutherford s Nuclear Model Summarize the structure of the atom according to Rutherford s nuclear model 10 Spectra How do the emission spectra of incandescent solids and atomic gases differ In what ways are they similar 11 Bohr Model Explain how energy is conserved when an atom absorbs a photon of light 12 Orbit Radius A helium ion behaves like a hydrogen atom The radius of the ion s lowest energy level is 00265 nm According to Bohr s model, what is the radius of the second energy level
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13 Absorption Spectrum Explain how the absorption spectrum of a gas can be determined Describe the reasons for the spectrum s appearance 14 Bohr Model Hydrogen has been detected transitioning from the 101st to the 100th energy levels What is the radiation s wavelength Where in the electromagnetic spectrum is this emission 15 Critical Thinking The nucleus of a hydrogen atom has a radius of about 15 10 15 m If you were to build a model of the hydrogen atom using a softball (r 5 cm) to represent the nucleus, where would you locate an electron in the n 1 Bohr orbit Would it be in your classroom On school property
Section 281 The Bohr Model of the Atom
282 The Quantum Model of the Atom
Objectives
Describe the shortcomings of Bohr s atomic model Describe the quantum model of the atom Explain how a laser works Describe the properties of laser light
he postulates that Bohr made could not be explained on the basis of accepted physics principles of the time For example, electromagnetic theory required that the accelerated particles radiate energy, causing the rapid collapse of the atom In addition, the idea that electron orbits have well-defined radii was in conflict with the Heisenberg uncertainty principle How could Bohr s work be put on a firm foundation
From Orbits to an Electron Cloud
The first hint to the solution of these problems was provided by Louis de Broglie Recall from 27 that de Broglie proposed that particles have wave properties, just as light has particle properties The de Broglie wavelength of a particle with momentum mv is defined as h/mv The angular momentum of a particle can be defined as mvr hr/ Thus, Bohr s required quantized angular-momentum condition, mvr nh/2 , can be written in the following way:
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