Collision Theory & Rate of Reaction Flashcards
Particle Theory
States that all matter is made up of partciles, atoms, molecules, or ions that ae constanlly moving
When does a reaction occurs?
When there is a successfu collison in which per exiting bonds or the reactants are broken and new bonds from to create products.
Collision Theory
States that for a successful collision to occur particles must collide with both the correct orientaion and sufficient energy
Even if particles have sufficient energy why won’t they collide correctly?
becuase a collision with the incoorect orientation will not result in a chemical reaction
Why won’t a chemical reaction occur if the particles are moving too slowly?
becuase of low kinetic energy. This means that they do not have enough energy and the collision will not result in a chemical reaction.
What is a combination reaction (combining)
Is a reaction in which 2 or more substances combine to form a signle new substance. These can also be called synthesis reactions.
Why can combing not result in an immediment chemical reaction?
Offen combining reactants together does not immediatley make them react beucase if the energy of the reactant particles is too low for a successful collisions to occur, some energy needs to be added to the system for the reaction to occur.
Activation energy (Ea)
The name given to the minimum energy required to make a reaction happen.
It is measured in kilojoules per mole (kj/mol)
Reactants that collide with the energy above the activation energy will…
react togehter, but they need to be in the correct orientation.
Energy diagrams
They show the energy within a system as a reaction progresses.
How do reactants get into a state where their bonds can break and can react to form the peoducts
They must gain energy
Activation energy on an energy diagram
The activation energy is the difference between the energy of the reactant and the maximum energy on the diagram.
What is an effective collisison?
When particles collide with suffcient energy and correct orientation
The faster the rate of effective collisions beteen molecules in a reaction the faster…
The rate of reaction.
What factors increase the rate of reaction?
-Increasing the frequency of collisions
and
-the propotion of these collisions that are effective
