Textbook Question
Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? (a) from n = 3 to n = 2 (c) an electron adds to the H+ ion and ends up in the n = 2 shell?
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Ch.6 - Electronic Structure of Atoms
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 6, Problem 39b
(b) Is this line in the visible region of the electromagnetic spectrum?
Verified step by step guidance1
Understand the electromagnetic spectrum: The electromagnetic spectrum includes all types of electromagnetic radiation, ranging from gamma rays to radio waves. The visible region is a small part of this spectrum, typically ranging from wavelengths of about 380 nm to 750 nm.
Identify the wavelength of the line in question: To determine if a line is in the visible region, you need to know its wavelength. This information is usually provided in the problem or can be calculated using other given data.
Compare the wavelength to the visible range: Once you have the wavelength, compare it to the visible range (380 nm to 750 nm). If the wavelength falls within this range, the line is in the visible region.
Consider the context of the problem: Sometimes, additional context or information is provided that can help confirm whether the line is visible. For example, if the problem involves a known visible light source, this can be a clue.
Reflect on the implications: Understanding whether a line is in the visible region can have practical implications, such as determining the color of light emitted or absorbed by a substance.
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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.
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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Visible Light Spectrum
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
(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
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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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
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
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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