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Chapter 8: Problem 119

In your own words, define the following terms or symbols: (a) \(\lambda ;\) (b) \(\nu ;\) (c) \(h ;\) (d) \(\psi ;\) (e) principal quantum number, \(n\).

Short Answer

Expert verified
\(\lambda\) is the wavelength of a wave. \(\nu\) is the frequency of a wave. \(h\) is known as Planck's constant. \(\psi\) represents a wave function in quantum mechanics. The principal quantum number, \(n\), is the number that determines the size and energy level of an electron shell in an atom.

Step by step solution

01

Define \(\lambda\)

\(\lambda\) can be defined as the wavelength of a wave. It is the distance between two successive crests or troughs of a wave.
02

Define \(\nu\)

\(\nu\) is the frequency of a wave. It tells how many cycles of the wave can occur in a second, and is measured in Hertz (Hz, cycles per second).
03

Define \(h\)

\(h\) is known as Planck's constant. It is a fundamental constant with a value of approximately 6.626 x 10^-34 Joule seconds.
04

Define \(\psi\)

\(\psi\) represents a wave function in quantum mechanics. It describes the quantum state of a particle and the probability of finding a particle within a given region of space.
05

Define principal quantum number, \(n\)

The principal quantum number, \(n\), is the number that determines the size and energy level of an electron shell in an atom. It's a positive integer that starts from 1.

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Most popular questions from this chapter

In everyday usage, the term "quantum jump" describes a change of a very significant magnitude compared to more gradual, incremental changes; it is similar in meaning to the term "a sea change." Does quantum jump have the same meaning when applied to events at the atomic or molecular level? Explain.

Between which two orbits of the Bohr hydrogen atom must an electron fall to produce light of wavelength \(1876 \mathrm{nm} ?\)

The following electron configurations correspond to the ground states of certain elements. Name each element. (a) \([\mathrm{Rn}] 7 s^{2} 6 d^{2} ;\) (b) \([\mathrm{He}] 2 s^{2} 2 p^{2} ;\) (c) \([\mathrm{Ar}] 3 d^{3} 4 s^{2}\) (d) \([\mathrm{Kr}] 4 d^{10} 5 s^{2} 5 p^{4} ;\) (e) \([\mathrm{Xe}] 4 f^{2} 6 s^{2} 6 p^{1}\)

Explain the important distinctions between each pair of terms: (a) frequency and wavelength; (b) ultraviolet and infrared light; (c) continuous and discontinuous spectra; (d) traveling and standing waves; (e) quantum number and orbital; (f) spd f notation and orbital diagram; (g) \(s\) block and \(p\) block; (h) main group and transition element; (i) the ground state and excited state of a hydrogen atom.

What is the wavelength, in nanometers, associated with a \(1000 \mathrm{kg}\) automobile traveling at a speed of \(25 \mathrm{m} \mathrm{s}^{-1},\) that is, considering the automobile to be a matter wave? Comment on the feasibility of an experimental measurement of this wavelength.
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