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Ch.6 - Electronic Structure of Atoms
Chapter 6, Problem 39b

(b) Is this line in the visible region of the electromagnetic spectrum?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electromagnetic Spectrum

The electromagnetic spectrum encompasses all types of electromagnetic radiation, arranged by wavelength or frequency. It includes gamma rays, X-rays, ultraviolet light, visible light, infrared radiation, microwaves, and radio waves. The visible region specifically refers to the wavelengths that can be detected by the human eye, typically ranging from about 400 to 700 nanometers.
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Visible Light

Visible light is the portion of the electromagnetic spectrum that is visible to the human eye. It consists of various colors, each corresponding to a specific wavelength, with violet having the shortest wavelength and red the longest. Understanding the characteristics of visible light is essential for determining whether a specific line or wavelength falls within this range.
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Wavelength and Frequency

Wavelength and frequency are fundamental properties of electromagnetic waves. Wavelength is the distance between successive peaks of a wave, while frequency is the number of peaks that pass a point in one second. These two properties are inversely related; as wavelength increases, frequency decreases, and vice versa. This relationship is crucial for identifying whether a specific line is in the visible spectrum.
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Related Practice
Textbook Question

Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? (b) from an orbit of radius 0.846 nm to one of radius 0.212 nm

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Textbook Question

Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from n = 2 to n = 3 (c) from the n = 9 to the n = 6 state.

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Textbook Question

(a) Using Equation 6.5, calculate the energy of an electron in the hydrogen atom when n = 3 and when n = 6. Calculate the wavelength of the radiation released when an electron moves from n = 6 to n = 3.

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Textbook Question

Consider a transition of the electron in the hydrogen atom from n = 8 to n = 3. (b) Will the light be absorbed or emitted?

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Textbook Question

The visible emission lines observed by Balmer all involved nf = 2. (a) Which of the following is the best explanation of why the lines with nf = 3 are not observed in the visible portion of the spectrum: (i) Transitions to nf = 3 are not allowed to happen, (ii) transitions to nf = 3 emit photons in the infrared portion of the spectrum, (iii) transitions to nf = 3 emit photons in the ultraviolet portion of the spectrum, or (iv) transitions to nf = 3 emit photons that are at exactly the same wavelengths as those to nf = 2.

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Textbook Question

The visible emission lines observed by Balmer all involved nf = 2. (b) Calculate the wavelengths of the first three lines in the Balmer series—those for which ni = 3, 4, and 5—and identify these lines in the emission spectrum shown in Figure 6.11.

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