Collision Theory
Kinetic energy and temperature
- The kinetic theory developed in the 18th century out of a need to explain how it is that gases exert pressure inside a container
- Theories about gas particles and movement were extended to include all states of matter
- The kinetic theory of matter accounts for the properties of solids, liquids and gases in terms of the interactions of particles and their relative energies
For more information on kinetic theory, see our revision note on The Kinetic Molecular Theory
- Kinetic energy refers to the energy associated with movement or motion. It is determined by the mass,m, and velocity, v, of the substance according to the kinetic energy formula:
KE = ½mv2
- As the kinetic energy of the particles at the same temperature is equal, this means there is an inverse relationship between mass and velocity
- This is why substances with a lower mass diffuse more quickly than those with greater mass at the same temperature
- Particles in a substance have a range of kinetic energies due to their random motion
- The distribution of kinetic energy is shown in the Maxwell-Boltzmann energy distribution curve
Maxwell-Boltzmann distribution curve
The Maxwell-Boltzmann energy distribution curve shows the distribution of kinetic energy of particles in a sample
- The area under the curve gives the total number of particles
- The average kinetic energy of the particles is directly proportional to the temperature of the system in Kelvin
What is collision theory?
- Collision theory explains how chemical reactions occur
- When reactants come together the kinetic energy they possess means their particles will collide and some of these collisions will result in chemical bonds being broken and some new bonds being formed
- The rate of a chemical reaction depends on how often a reaction from a collision occurs, this is influenced by the following four factors:
- Collision frequency
- Collision energy
- Activation energy
- Collision geometry
Collision frequency
- If a chemical reaction is to take place between two particles, they must first collide
- The number of collisions between particles per unit time in a system is known as the collision frequency
- The collision frequency of a given system can be altered by:
- Changing the concentration of the reactants
- Changing the total pressure
- Changing the temperature
- Changing the surface area of the reacting particles
Collision energy
- Not all collisions result in a chemical reaction
- Most collisions just result in the colliding particles bouncing off each other
- Collisions which do not result in a reaction are known as unsuccessful collisions
- Unsuccessful collisions happen when the colliding species do not have enough energy to break the necessary bonds
- If they do not have sufficient energy, the collision will not result in a chemical reaction
- If they have sufficient energy, they will react, and the collision will be successful
- The combined energy of the colliding particles is known as the collision energy
Collision energy
Collision energy is the combined energy of two colliding particles
Activation Energy
- The minimum energy the colliding particles need in order to react is known as the activation energy
- If the collision energy of the colliding particles is less than the activation energy, the collision will be unsuccessful
- If the collision energy is equal to or greater than the activation energy, the collision will be successful, and a reaction will take place
- The activation energy can be changed by the addition of a catalyst
Collision Geometry
- Particles have to have the right orientation when they collide for the reaction to be successful
- This is particularly the case with large molecules with complex shapes
Collision geometry
Orientation becomes increasingly important in large complex biomolecules such as proteins and carbohydrates where active sites (reactive part of the molecule) can only be accessed in one orientation
- Most collisions do not result in a reaction because they do not reach the activation energy rather than not having the correct collision geometry
- Ultimately, the rate of reaction depends on the number of successful collisions that happen per unit time
- A successful collision is where the particles collide in the correct orientation and with sufficient energy for a chemical reaction to occur
- An unsuccessful collision is when particles collide in the wrong orientation or when they don’t have enough energy and bounce off each other without causing a chemical reaction
Successful and unsuccessful collisions
Diagram (A) shows an ineffective collision due to the particles not having enough energy whereas (B) shows an effective collision where the particles have the correct orientation and enough energy for a chemical reaction to take place
