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(Figure 1) is an energy-level diagram for a quantum system. What wavelengths appear in the system's emission spectrum? Express your answers in nanometers separated by commas.

(Figure 1) is an energy-level diagram for a quantum system. What wavelengths appear in the system's emission spectrum? Express your answers in nanometers separated by commas.

College Physics
College Physics
11th Edition
ISBN:9781305952300
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
Chapter1: Units, Trigonometry. And Vectors
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(Figure 1) is an energy-level diagram for a quantum system. What wavelengths appear in the system's emission spectrum?

Express your answers in nanometers separated by commas.
The image illustrates the energy levels of an electron within an atom. The energy levels are denoted by 'n', which signifies the principal quantum number. There are three energy levels displayed, each with a corresponding energy value (E) measured in electron volts (eV). 1. The first energy level (n = 1) is labeled as \( E_1 = 0.0 \) eV. This represents the ground state, which is the lowest energy state of the electron in the atom. 2. The second energy level (n = 2) is labeled as \( E_2 = 1.5 \) eV. This is an excited state where the electron has higher energy compared to the ground state. 3. The third energy level (n = 3) is labeled as \( E_3 = 4.0 \) eV. This is another higher excited state with even more energy than the second level. These values indicate the discrete energy states that electrons can occupy within the atom, following the principles of quantum mechanics. Electrons can transition between these states by absorbing or emitting energy in the form of photons.
Transcribed Image Text:The image illustrates the energy levels of an electron within an atom. The energy levels are denoted by 'n', which signifies the principal quantum number. There are three energy levels displayed, each with a corresponding energy value (E) measured in electron volts (eV). 1. The first energy level (n = 1) is labeled as \( E_1 = 0.0 \) eV. This represents the ground state, which is the lowest energy state of the electron in the atom. 2. The second energy level (n = 2) is labeled as \( E_2 = 1.5 \) eV. This is an excited state where the electron has higher energy compared to the ground state. 3. The third energy level (n = 3) is labeled as \( E_3 = 4.0 \) eV. This is another higher excited state with even more energy than the second level. These values indicate the discrete energy states that electrons can occupy within the atom, following the principles of quantum mechanics. Electrons can transition between these states by absorbing or emitting energy in the form of photons.
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