Collision Theory VMA

Successful collision

A collision with sufficient energy and in the correct orientation

Increase rate of reaction

Can be caused due to increase in temp

increase in concentration/pressure (gas)

increase in surface area

increased temperature

particles gain energy = moves quicker = more frequent + faster collisions

increased concentration

more particles of reactant colliding between molecules = more frequent collisions

increased pressure

particles more compressed together = more frequent collisions

Increase in surface area

particles around solution have more area to work on = more frequent collisions

Activation energy

minimum amount of energy needed by particles to react

Catalyst

substance speeding up reaction

w/o being changed/used-up in reaction

The Collision Theory states that 3 conditions must be met for a collision to occur. What are the conditions?

1. Atoms must collide

2. Atoms must be in the correct orientation

3. Atoms must hit each other with enough energy.

High concentration vs. Low concentration

The higher the concentration (amount) of reactants the more likely it is that there will be a collision

Energy profile diagram

A diagram that shows the energy changes during the course of a reaction.

rate of reaction

the change in concentration/mass/colour/ of a reactant or product per unit time

Types of reactions

synthesis, decomposition, single replacement, double replacement, combustion, neutralisation