AP Chemistry Flashcards: Kinetic Molecular Theory
Written by AP Content Team, Verified for 2026 AP Exams, Last updated: May 2026
Review key ideas with interactive flashcards. This set includes 11 cards to help you master important concepts.
How can a particulate model be used to explain gas properties?
A particulate model visually represents individual particles in random motion to explain the relationship between their movement and the macroscopic properties of the gas.
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How can a particulate model be used to explain gas properties?
A particulate model visually represents individual particles in random motion to explain the relationship between their movement and the macroscopic properties of the gas.
What is the formula relating average kinetic energy (KE) to mass (m) and average velocity (v)?
The average kinetic energy of particles is related to their average velocity by the equation KE = 1/2mv^2.
What is the Kinetic Molecular Theory (KMT)?
KMT is a model that relates the macroscopic properties of gases, such as pressure and temperature, to the motion of the individual particles that compose the gas.
What does the Maxwell-Boltzmann distribution curve show?
It graphically represents the range of particle energies and velocities within a sample at a specific temperature, showing that not all particles move at the same speed.
What is the core connection made by the Kinetic Molecular Theory?
KMT provides the connection between the microscopic motion of particles and the macroscopic properties of gases that we can observe and measure.
What is the Maxwell-Boltzmann distribution?
It is a graphical representation that describes the distribution of kinetic energies or speeds of particles in a gas at a given temperature.
According to KMT, what is the fundamental state of particles in all matter?
Particles in all states of matter are in continuous, random motion.
If two different gases are at the same temperature, what can you conclude about their particles' average kinetic energy?
If they are at the same Kelvin temperature, their particles must have the same average kinetic energy, regardless of the particles' mass.
If you increase the temperature of a gas, what happens to the average kinetic energy of its particles?
Since Kelvin temperature is proportional to average kinetic energy, increasing the temperature of the gas will increase the average kinetic energy of its particles.
What are the three frameworks mentioned for explaining the relationship between particle motion and macroscopic gas properties?
The relationship can be explained with the Kinetic Molecular Theory (KMT), a particulate model, and a graphical representation.
What is the relationship between Kelvin temperature and the particles in a substance?
The Kelvin temperature of a sample is directly proportional to the average kinetic energy of its constituent particles.