Question

Of the following possible transitions of an electron in a hydrogen atom, which emits light of the highest energy? a. Transition from the $n=1$ to the $n=3$ level b. Transition from the $n=1$ to the $n=2$ level c. Transition from the $n=3$ to the $n=1$ level d. Transition from the $n=2$ to the $n=1$ level e. Transition from the $n=5$ to the $n=4$ level

Name: Problem 21, Chapter 7: General Chemistry
Uploaded: 2021-06-12T02:31:02-08:00
Duration: 46 s
Channel: Nicole Smina
Description: Of the following possible transitions of an electron in a hydrogen atom, which emits light of the highest energy? a. Transition from the n=1 to the n=3 level b. Transition from the n=1 to the n=2 level c. Transition from the n=3 to the n=1 level d. Transition from the n=2 to the n=1 level e. Transition from the n=5 to the n=4 level

   Of the following possible transitions of an electron in a hydrogen atom, which emits light of the highest energy?
a. Transition from the $n=1$ to the $n=3$ level
b. Transition from the $n=1$ to the $n=2$ level
c. Transition from the $n=3$ to the $n=1$ level
d. Transition from the $n=2$ to the $n=1$ level
e. Transition from the $n=5$ to the $n=4$ level

General Chemistry

Darrell Ebbing,… 9th Edition

Chapter 7, Problem 21

Instant Answer

Solved by Expert Nicole Smina

06/12/2021

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When an electron transitions from a higher energy level to a lower energy level, it emits light (energy). Show more…

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Of the following possible transitions of an electron in a hydrogen atom, which emits light of the highest energy? a. Transition from the $n=1$ to the $n=3$ level b. Transition from the $n=1$ to the $n=2$ level c. Transition from the $n=3$ to the $n=1$ level d. Transition from the $n=2$ to the $n=1$ level e. Transition from the $n=5$ to the $n=4$ level

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Key Concepts

Quantized Energy Levels

In the hydrogen atom, electrons exist in discrete energy levels rather than a continuous range. The energy associated with each level is determined primarily by the principal quantum number (n), where the energy is given by a specific formula (such as E = -13.6 eV/n²). This concept explains why electrons can only occupy specific energy states and why transitions occur between these defined levels.

Photon Emission from Electron Transitions

When an electron transitions from a higher energy level to a lower one, the energy difference between those levels is released in the form of a photon. The energy (and thus the frequency and wavelength) of the emitted photon directly corresponds to the magnitude of the energy gap between the initial and final states. Larger energy differences result in higher-energy (shorter-wavelength) photons.

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