Domanda del libro di testo
The series of emission lines of the hydrogen atom for which nf = 3 is called the Paschen series. (b) Calculate the wavelengths of the first three lines in the Paschen series—those for which ni = 4, 5, and 6.
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Ch.6 - Electronic Structure of Atoms
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 6, Problema 91a
The series of emission lines of the hydrogen atom for which nf = 3 is called the Paschen series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Paschen series are observed.
Guida verificata passo dopo passo1
Identify the initial and final energy levels for the Paschen series. The final energy level \( n_f \) is 3, and the initial energy level \( n_i \) is greater than 3.
Use the Rydberg formula for hydrogen to calculate the wavelength of the emitted light: \( \frac{1}{\lambda} = R_H \left( \frac{1}{n_f^2} - \frac{1}{n_i^2} \right) \), where \( R_H \) is the Rydberg constant.
Calculate the wavelengths for transitions from higher energy levels (e.g., \( n_i = 4, 5, 6, \ldots \)) to \( n_f = 3 \).
Determine the range of wavelengths obtained from these calculations.
Identify the region of the electromagnetic spectrum corresponding to these wavelengths, which is the infrared region.
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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. Each type of radiation has distinct properties and applications, with the visible spectrum being just a small part of the entire range.
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02:53
Electromagnetic Spectrum
Hydrogen Emission Spectrum
The hydrogen emission spectrum is the spectrum of light emitted by hydrogen atoms when they transition from higher energy levels to lower ones. Each transition corresponds to a specific wavelength of light, resulting in distinct emission lines. The Paschen series specifically refers to transitions where electrons fall to the n=3 energy level, producing infrared radiation.
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01:51Emission Spectra
Paschen Series
The Paschen series is a set of spectral lines in the hydrogen emission spectrum that occurs when electrons transition to the third energy level (n=3) from higher levels (n=4, 5, 6, etc.). These transitions emit photons in the infrared region of the electromagnetic spectrum, which is not visible to the human eye but can be detected with appropriate instruments.
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02:02Activity Series Chart
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Domanda del libro di testo
Consider a transition in which the electron of a hydrogen atom is excited from n = 1 to n = ∞. (d) How are the results of parts (b) and (c) related to the plot shown in Exercise 6.88?
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