Multiple Choice
The emission spectrum of helium is shown below. Which emission spectrum line has the highest energy?
9. Electrons in Atoms and the Periodic Table
Emission Spectrum (Simplified)
Struggling with Introduction to Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
In a simplified model of an atomic emission spectrum, emission of light from an atom occurs when an electron does which of the following?
A
Moves from a lower-energy level to a higher-energy level by absorbing a photon
B
Is removed from the atom (ionization), emitting visible light as it leaves
C
Remains in the same energy level and emits a photon continuously
D
Moves from a higher-energy level to a lower-energy level, releasing a photon
Verified step by step guidance1
Understand that an atomic emission spectrum is produced when electrons in an atom transition between energy levels and emit light (photons).
Recall that electrons absorb energy to move from a lower energy level to a higher energy level, which is called excitation, but this process does not emit light.
Recognize that emission occurs when an electron moves from a higher energy level to a lower energy level, releasing energy in the form of a photon (light).
Note that ionization (removal of an electron) involves energy input and does not directly produce the characteristic emission spectrum lines.
Conclude that the correct description of emission in the atomic spectrum is the electron moving from a higher-energy level to a lower-energy level, releasing a photon.
1:47mWatch next
Master Emission Spectrum (Simplified) Concept 1 with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Emission Spectrum (Simplified) practice set
Problem sets built by lead tutorsExpert video explanations