1. CHEMICAL REACTIONS

2. KINETIC MOLECULAR THEORY
Matter is composed of tiny particles called atoms or molecules
These particles are always undergoing constant, random (Brownian) movement.

3. Collision Theory
Reactants must collide with the correct orientation and with sufficient energy.

4. Orientation – position in space

5. Effect of Collision Energy on Chemical Reactions
SUFFICIENT ENERGY = NEW PRODUCTS
INSUFFICIENT ENERGY = NO NEW PRODUCT

6. Reactions must have a minimum activation energy…if too little, no reaction.

7. A reaction takes place if the energy available is greater than the minimum activation energy.

8. Exothermic (Exogonic) Reaction = Energy of the Reactants > Energy of the Products

9. Endogonic (Endothermic) Reactions – Energy of the Reactants < Energy of the Products

10. STEPS IN CHEMICAL REACTIONS

11. 1. Bond Breaking

12. 2. Formation of Activated Complex – an intermediate product

13. 3. Formation of Product

14. FACTORS AFFECTING REACTION RATES

15. 1. Nature of Reactants
A reaction could only take place if the reactants are reactive enough to form a new product.
Ex. Neon gases are inert and will not react with oxygen while sodium metal will burn if exposed to O2 gas.

16. 2. Temperature

17. 3. Concentration of Reactants

19. Presence of catalyst or inhibitor

20. Effect of the presence of catalyst on a reaction

21. END OF TOPIC

22. Le Chatelier's Principle
If a system at equilibrium is altered in a way that disrupts the equilibrium, the system will shift in such a way as to counter the change.

23. Rates of Reaction for Reversible Reactions

24. Changes in Concentrations for a Reversible Reaction

25. Effect of Increased Concentration on Equilibrium

26. Change in Rates When Reactant Added

27. Effect of Decreased Concentration on Equilibrium

28. Change in Rates When Product Removed