Domanda del libro di testo
According to the quantum-mechanical model for the hydrogen atom, which electron transition produces light with the longer wavelength: 3p → 2s or 4p → 3p?
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Ch.8 - The Quantum-Mechanical Model of the Atom
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Capitolo 8, Problema 66
Determine whether each transition in the hydrogen atom corresponds to absorption or emission of energy. a. n = 3 → n = 1 b. n = 2 → n = 4 c. n = 4 → n = 3
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1. The energy levels of an atom are quantized, meaning they are discrete rather than continuous. In the case of a hydrogen atom, these energy levels are represented by the principal quantum number 'n'. The higher the value of 'n', the higher the energy level of the electron.
2. When an electron transitions from a higher energy level to a lower energy level (i.e., 'n' decreases), energy is emitted. This is because the electron loses energy in the form of light to move to a lower energy level.
3. Conversely, when an electron transitions from a lower energy level to a higher energy level (i.e., 'n' increases), energy is absorbed. This is because the electron needs to gain energy in the form of light to move to a higher energy level.
4. Therefore, for transition a (n = 3 to n = 1), energy is emitted because 'n' decreases. For transition b (n = 2 to n = 4), energy is absorbed because 'n' increases. For transition c (n = 4 to n = 3), energy is emitted because 'n' decreases.
5. Remember, the energy of the light emitted or absorbed during these transitions corresponds to the difference in energy between the two energy levels. This can be calculated using the Rydberg formula if needed.
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Energy Levels in Atoms
In an atom, electrons occupy specific energy levels or shells, denoted by quantum numbers (n). The energy levels are quantized, meaning electrons can only exist at certain distances from the nucleus. When an electron transitions between these levels, it either absorbs or emits energy, depending on whether it moves to a higher or lower energy level.
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02:10
Atom Structure
Absorption and Emission of Energy
Absorption occurs when an electron gains energy and moves to a higher energy level (higher n value), while emission occurs when an electron loses energy and falls to a lower energy level (lower n value). The energy change associated with these transitions corresponds to the difference in energy between the two levels, often represented by the equation E = hf, where E is energy, h is Planck's constant, and f is frequency.
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01:51Emission Spectra
Quantum Transitions in Hydrogen
In the hydrogen atom, transitions between energy levels can be predicted using the Rydberg formula, which calculates the wavelengths of emitted or absorbed light. For example, a transition from n = 3 to n = 1 involves emission of energy, while a transition from n = 2 to n = 4 involves absorption. Understanding these transitions is crucial for interpreting spectral lines and the behavior of hydrogen in various energy states.
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01:05Hydrogen Compounds Example
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