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+
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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 44a
The hydrogen atom can absorb light of wavelength 1094 nm. (a) In what region of the electromagnetic spectrum is this absorption found?
Verified step by step guidance1
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.
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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Frequency-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
Use the de Broglie relationship to determine the wavelengths of the following objects: (a) an 85-kg person skiing at 50 km/hr (b) a 10.0-g bullet fired at 250 m/s
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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
The Lyman series of emission lines of the hydrogen atom are those for which nf = 1. (a) Determine the region of the electromagnetic spectrum in which the lines of the Lyman series are observed.
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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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