Domanda del libro di testo
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
3571
views
3
rank
Ch.8 - The Quantum-Mechanical Model of the Atom
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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 65
An electron in a hydrogen atom is excited with electrical energy to an excited state with n = 2. The atom then emits a photon. What is the value of n for the electron after the emission?
Guida verificata passo dopo passo1
Identify the initial excited state of the electron, which is given as n = 2.
Understand that when an electron emits a photon, it transitions to a lower energy level.
Recall that the lowest energy level for a hydrogen atom is n = 1, which is the ground state.
Since the electron is initially at n = 2 and emits a photon, it will transition to the next lower energy level.
Conclude that the value of n for the electron after the emission is n = 1.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Quantum States and Energy Levels
In quantum mechanics, electrons in an atom occupy discrete energy levels, denoted by quantum numbers (n). The principal quantum number n indicates the electron's energy level, with lower values corresponding to closer proximity to the nucleus. For hydrogen, these levels are quantized, meaning an electron can only exist in specific states.
Video consigliato:
Percorso guidato
02:55
Principal Quantum Number
Photon Emission
When an electron transitions from a higher energy level to a lower one, it emits energy in the form of a photon. The energy of the emitted photon corresponds to the difference in energy between the two levels. This process is fundamental in understanding how atoms interact with light and is key to phenomena such as spectral lines.
Video consigliato:
Percorso guidato
02:02Gamma Emission
Excited State and Ground State
An excited state refers to an electron being in a higher energy level (n > 1) compared to its ground state, where n = 1. After emitting a photon, the electron returns to a lower energy level, which could be the ground state or another excited state, depending on the energy released. In this case, the electron will return to n = 1 after the emission.
Video consigliato:
Percorso guidato
01:32Ground State Electron Configurations
Pratica correlata
Domanda del libro di testo
Which combinations of n and l represent real orbitals, and which do not exist? a. 1s b. 2p c. 4s d. 2d
2102
views
1
rank
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?
1091
views
2
comments
Domanda del libro di testo
Sketch the 1s and 2p orbitals. How do the 2s and 3p orbitals differ from the 1s and 2p orbitals?
1729
views
Domanda del libro di testo
Sketch the 3d orbitals. How do the 4d orbitals differ from the 3d orbitals?
1426
views