Domanda del libro di testo
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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TOC.tableOfContents
- 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: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 6, Problema 38a,c
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.
Guida verificata passo dopo passo1
Identify the initial and final energy levels of the electron in the hydrogen atom. Here, the electron transitions from n = 2 to n = 3.
Recall that when an electron moves to a higher energy level (higher n value), it absorbs energy. Conversely, when it moves to a lower energy level, it emits energy.
Since the electron is moving from n = 2 to n = 3, it is transitioning to a higher energy level.
Conclude that energy is absorbed during this transition because the electron is moving to a higher energy state.
Remember that the energy difference between levels can be calculated using the Rydberg formula, but the key concept here is the direction of the transition (lower to higher energy level).
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Energy Levels in Hydrogen
In a hydrogen atom, electrons occupy specific energy levels, denoted by quantum numbers (n). The energy associated with each level increases with n, meaning that higher levels are further from the nucleus and have more energy. Understanding these levels is crucial for determining whether energy is absorbed or emitted during electronic transitions.
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01:22
Hydrogenation Reactions
Absorption and Emission of Energy
When an electron transitions from a lower energy level (n = 2) to a higher energy level (n = 3), it must absorb energy, typically in the form of a photon. Conversely, when an electron falls from a higher level to a lower one, energy is emitted. This principle is fundamental in understanding how atoms interact with light and other forms of energy.
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01:51Emission Spectra
Photon Energy and the Rydberg Formula
The energy of a photon is related to its frequency and wavelength, described by the equation E = hν, where E is energy, h is Planck's constant, and ν is frequency. The Rydberg formula can be used to calculate the wavelengths of emitted or absorbed light during electronic transitions in hydrogen, providing a quantitative understanding of these processes.
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01:40Photon Energy Formulas
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