Domanda del libro di testo
(c) What is the velocity of an electron with a de Broglie wavelength equal to (b)?
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Ch.5 - Periodicity & Electronic Structure of Atoms
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.5 - Periodicity & Electronic Structure of AtomsProblema 138b
McMurry 8th EditionCh.5 - Periodicity & Electronic Structure of AtomsProblema 138bCapitolo 5, Problema 138b
An energetically excited hydrogen atom has its electron in a 5f subshell. The electron drops down to the 3d subshell, releasing a photon in the process. (b) What wavelength of light is emitted by the process?
Guida verificata passo dopo passo1
Identify the initial and final energy levels of the electron. In this case, the electron transitions from the 5f subshell (n=5) to the 3d subshell (n=3).
Use the Rydberg formula to calculate the energy of the photon emitted during the transition: \( E = R_H \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) \), where \( R_H \) is the Rydberg constant, \( n_1 \) is the lower energy level (3), and \( n_2 \) is the higher energy level (5).
Calculate the energy difference between the two energy levels using the values of \( n_1 \) and \( n_2 \) in the Rydberg formula.
Convert the energy of the photon from joules to electron volts (eV) if necessary, using the conversion factor (1 eV = 1.602 x 10^-19 joules).
Determine the wavelength of the emitted photon using the equation \( \lambda = \frac{hc}{E} \), where \( h \) is Planck's constant, \( c \) is the speed of light, and \( E \) is the energy of the photon calculated in the previous steps.
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Energy Levels and Electron Transitions
In an atom, electrons occupy specific energy levels or subshells, which are quantized. When an electron transitions between these levels, it either absorbs or emits energy in the form of a photon. The energy difference between the initial and final states determines the wavelength of the emitted light.
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Percorso guidato
00:53
Electron Configurations Of Transition Metals Example
Photon Energy and Wavelength Relationship
The energy of a photon 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. This relationship allows us to calculate the wavelength of light emitted during electron transitions by determining the energy difference between the two subshells.
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00:31Frequency-Wavelength Relationship
Subshells and Their Energy Levels
Subshells (s, p, d, f) represent different shapes and orientations of electron clouds within an atom, with varying energy levels. In hydrogen, the 5f subshell is higher in energy than the 3d subshell. Understanding these subshells is crucial for predicting the behavior of electrons during transitions and the resulting photon emissions.
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01:02Angular Momentum Quantum Number and Subshell
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Domanda del libro di testo
An energetically excited hydrogen atom has its electron in a 5f subshell. The electron drops down to the 3d subshell, releasing a photon in the process. (c) The hydrogen atom now has a single electron in the 3d subshell. What is the energy in kJ/mol required to remove this electron?
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Domanda del libro di testo
Consider the noble gas xenon. (a) Write the electron configuration of xenon using the abbreviation of the previous noble gas.
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Domanda del libro di testo
Consider the noble gas xenon. (c) The energy required to completely remove the outermost electron from the excited xenon atom is 369 kJ/mol, almost identical to that of cesium (376 kJ/mol). Explain.
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Domanda del libro di testo
A minimum energy of 7.21⨉10-19 J is required to produce the photoelectric effect in chromium metal. (b) Light with a wavelength of 2.50⨉10-7 m falls on a piece of chromium in an evacuated glass tube. What is the minimum de Broglie wavelength of the emitted electrons? (Note that the energy of the incident light must be conserved; that is, the photon's energy must equal the sum of the energy needed to eject the electron plus the kinetic energy of the electron.)
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Domanda del libro di testo
A minimum energy of 7.21⨉10-19 J is required to produce the photoelectric effect in chromium metal. (a) What is the minimum frequency of light needed to remove an electron from chromium?
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