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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

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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

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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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That is, the circumference of the Bohr orbit, 2 r, is equal to a whole number multiple, n, of de Broglie wavelengths, Figure 28-13 illustrates this relationship In 1926, Austrian physicist Erwin Schr edinger used de Broglie s wave model to create a quantum theory of the atom based on waves This theory did not propose a simple planetary model of an atom, as Bohr s model had In particular, the radius of the electron orbit was not likened to the radius of the orbit of a planet about the Sun The Heisenberg uncertainty principle states that it is impossible to know both the position and momentum of an electron at the same time Thus, the modern quantum model of the atom predicts only the probability that an electron is in a specific region Interestingly, the quantum model predicts that the most probable distance between the electron and the nucleus for a hydrogen atom is the same as the radius predicted by the Bohr model

Figure 28-13 For an electron to have a stable orbit around the nucleus, the circumference of the orbit must be a whole-number multiple, n, of the de Broglie wavelength Note that the wholenumber multiples n 3 and n 5 are stable, whereas n 29 is not

The probability of the electron being at any specific radius can be calculated, and a three-dimensional plot can be constructed showing regions of equal probability The region in which there is a high probability of finding the electron is called the electron cloud A slice through the electron cloud for the two lowest energy states of a hydrogen atom is shown in Figure 28-14 Even though the quantum model of the atom is difficult to visualize, quantum mechanics, the study of the properties of matter using its wave properties, makes use of this model and has been extremely successful in predicting many details of atomic structure These details are very difficult to calculate precisely for all but the simplest atoms Only very sophisticated computers can make highly accurate approximations for the heavier atoms Quantum mechanics also enables the structures of many molecules to be calculated, allowing chemists to determine the arrangement of atoms in the molecules Guided by quantum mechanics, chemists have been able to create new and useful molecules that do not occur in nature Quantum mechanics also is used to analyze the details of the emission and absorption of light by atoms As a result of quantum mechanical theory, a new source of light was developed

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