Collision Theory

• What must particles always do?

  Collide

  • Collide in the right direction
  • Need to be facing each other the right way
  • Collide with at least minimum amount of kinetic energy
• What's the minimum amount of energy also known as?

  Activation energy - particles need this much energy for bonds to break
• How d we get reactions with high activation energies?

  Give particles extra energy by heating them
• Reaction Profile Diagram

  
• Molecules don't all have the same amount of energy
• What does a Maxwell Boltzmann Distribution show us?

  Number of molecules with different kinds of kinetic energy

  
• What happens when we increase the temperature?

  Particles have more kinetic energy and will move faster

  Meaning they will have at least the activation energy and be able to react
• If temperature increases what will happen to the Maxwell-Boltzmann distribution curve?

  It's move to the right

  
• What affe ts the reaction rate?

  Concentration

  Pressure

  Catalysts
• What does increasing the concentration do to reaction rates?


  Increase conc of reactants there's more particles in a given volume of solution so the particles will collide more frequently

  More collisions = more chances to react
• What does increasing the pressure do to reaction rates?

  Reactants = gases for this to increase pressure

  More particles in a given volume of gas and this increases the frequency of successful collisions
• What do catalysts do to reaction rates?

  Lower the activation energy by providing a different way for the bonds to be broken and remade

  If activation energy is lower - particles have enough energy to react