Textbook Question
Write the electron configurations for the following ions, anddetermine which have noble-gas configurations:(a) Ti2+(b) Br-(c) Mg2+(d) Po2-(e) Pt2+(f) V3+
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 Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 6, Problem 44a
The hydrogen atom can absorb light of wavelength 1094 nm. (a) In what region of the electromagnetic spectrum is this absorption found?
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Identify the given wavelength of light absorbed by the hydrogen atom, which is 1094 nm.
Convert the wavelength from nanometers to meters for standard unit consistency. Use the conversion factor: 1 nm = 1 x 10-9 m.
Recall the regions of the electromagnetic spectrum and their corresponding wavelength ranges. The main regions include radio, microwave, infrared, visible, ultraviolet, X-rays, and gamma rays.
Determine which region the wavelength of 1094 nm falls into by comparing it to the known wavelength ranges of the electromagnetic spectrum. For example, the infrared region typically ranges from about 700 nm to 1 mm.
Conclude that the absorption of light by the hydrogen atom at 1094 nm falls within the infrared 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 various regions such as radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays. Understanding where a specific wavelength falls within this spectrum is crucial for identifying its properties and interactions with matter.
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Electromagnetic Spectrum
Wavelength and Energy Relationship
The energy of electromagnetic radiation is inversely related to its wavelength, described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. Shorter wavelengths correspond to higher energy photons, while longer wavelengths correspond to lower energy. This relationship is essential for determining the energy associated with the absorption of light by atoms.
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00:31Frequency-Wavelength Relationship
Infrared Region
The infrared region of the electromagnetic spectrum typically ranges from about 700 nm to 1 mm in wavelength. The absorption of light at 1094 nm indicates that this wavelength falls within the infrared range. This region is significant in various applications, including thermal imaging and spectroscopy, as it relates to molecular vibrations and transitions.
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Related Practice
Textbook Question
One of the emission lines of the hydrogen atom has a wavelength of 94.974 nm. (a) In what region of the electromagnetic spectrum is this emission found?
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Textbook Question
One of the emission lines of the hydrogen atom has a wavelength of 94.974 nm. (b) Determine the initial and final values of n associated with this emission.
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Textbook Question
Order the following transitions in the hydrogen atom from smallest to largest frequency of light absorbed: n = 3 to n = 7, n = 4 to n = 8, n = 2 to n = 5, and n = 1 to n = 3.
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Textbook Question
The Lyman series of emission lines of the hydrogen atom are those for which nf = 1. (b) Calculate the wavelengths of the first three lines in the Lyman series—those for which ni = 2, 3, and 4.
Textbook Question
The hydrogen atom can absorb light of wavelength 1094 nm. (b) Determine the final value of n associated with this absorption.