The topic is about collision

2. 1. A chemical change that occurs when
two or more substances combine to
form a
new substance.
a. Activation Energy
b. Chemical Kinetics
c. Chemical Reaction
d. Product

3. 2. The measure of how fast is the
change in the concentration of the
reactants or products in a chemical
reaction.
a. Activation Energy
b. Activation Rate
c. Chemical Reaction
d. Concentration

4. 3. The substance that enter into and is
altered in the course of a chemical
reaction.
a. Catalyst
b. Enzyme
c. Product
d. Reactant

5. 4. The measure of how fast is the
change in the concentration of the
reactants or products in a chemical
reaction.
a. Activation Energy
b. Activation Rate
c. Chemical Reaction
d. Concentration

6. 5. The measure of how fast or slow a
reaction happens.
a. Activation Energy
b. Collision theory
c. Particle Size
d. Rate of Reaction

7. 6. How does a catalyst work in
speeding up a reaction?
a. It lowers the activation energy.
b. It provides more energy.
c. It creates more reactants.
d. It increases the temperature.

8. 7. What is an enzyme?
a. An inorganic substance added to
food for better digestion.
b. An organic molecule that dissolves
nutrients in the body.
c. A biomolecule that releases energy
during chemical reactions.
d. A biomolecule that serves as
catalyst in biological system

9. 8. A substance that increases the rate
of a reaction without being used up
during the reaction is called a
a. catalyst
c. product
b. reactant
d. solute

10. 9. The minimum amount of energy
needed for colliding particles to react
is called the
a. chemical energy
c. kinetic energy
b. activation energy
d. potential energy

11. 10. Catalysts permit reactions to
proceed along a ___________energy
path.
a. higher
c. restricted
b. lower
d. Stabler

15. It explains why some chemical
reactions are faster while others are
slow.
COLLISION
THEORY

16. • effectively collide
• with sufficient energy
• proper orientation.
“rate of a chemical reaction is proportional to the
number of successful collisions between the molecules
of the reactants. The more often reactant molecules
collide effectively, the more often they react with one
another and the faster the reaction rate”

17. Activation Energy- the minimum amount of energy
used to initiate a chemical reaction. If the reactant
particles do not possess the required activation energy
when they collide, they simply bounce off each other
without reacting.

18. (1) surface area/particle size of
the reactants
(2) concentration of the
reactants
(3) temperature,
(4) the presence of catalysts.

21. Guide Questions:
1. Which reaction is faster? Why?
2. How does the surface area/ particle size affect the reaction
rate?
Reaction Condition
Time the tablet was fully
dissolved
Observations
Whole effervescent tablet in a
cup of water
Broken into parts effervescent
tablet in a cup of water
powdered effervescent tablet in a
cup of water

22. In collision theory, as more
particles collide the frequency of collision
also increases and more likely results to a
faster reaction rate. The reaction becomes
faster as particles get smaller.

25. Guide Questions:
1. Which reaction is faster? Why?
2. Explain what could be occurring at the molecular level in each example. (How
are the molecules moving or acting?)
3.Why substances with high concentrations react faster than substances with low
concentrations?
Concentration Total Time Reaction Observations

26. The pure vinegar has more concentration than the vinegar solution
which makes the reaction rate faster. The rates of many reactions depend
on the concentrations of the reactants. Reaction rates usually increase
when the concentration of one or more of the reactants increases.
Increasing the concentration means more reactant particles are in a given
space (volume) which increases the likelihood of collisions between them.
The increased frequency of collisions results in a faster reaction rate.
For a chemical reaction to occur, a certain number of energized
molecules must be equal to or greater than the activation energy. As the
concentration increases, the number of molecules with the minimum
energy required also increases, and thus the reaction rate increases.

29. Guide Questions:
1. In which glass of water does the effervescent tablet dissolved faster? Why?
2. What happens to the reactant molecules as you increase the temperature of the
reaction?
3. How does the temperature affect the reaction rate?
Temperature of
water
Time the tablet was
fully dissolved
Observations
Hot water
Cold water

30. The effervescent tablet dissolved faster in hot water than in
cold water. Therefore, the reaction rate is directly proportional to the
temperature. The reaction becomes faster as the temperature gets
higher.
Increasing the temperature of the reactants increases the
kinetic energy that it possesses causing the particles to move faster.
As they move faster, the frequency of collision between them
increases. This gives the reactants enough energy to overcome the
activation energy thus making the reaction faster.

31. Factors Affecting the Rate of Reaction
1. Activation Energy- The activation energy refers to the
minimum energy required for a reaction to take place.
2. Temperature refers to the average kinetic energy of the
particles in an object. As a rule of thumb, a rise in temperature
of 10C doubles the reaction rate. The rate of a chemical reaction
increases with increasing temperature.
3. The rate of a chemical reaction is affected by the concentration
of reacting substances. The term concentration refers to the
number of particles present in a given volume of solution.
4. Surface area is the measure of how much exposed area a solid
object has, expressed in square units. In a reaction between a
solid and a liquid, the more finely divided a solid is, the faster is
the rate of reaction

34. Guide Questions:
1. How will you compare the rate at which bubbles
were produced?
2. What happened to the test tube added with
manganese dioxide? What do you call the manganese
dioxide?
3. What is a catalyst? How does it affect the reaction
rate?

35. The effervescent tablet dissolved faster in hot water than in
cold water. Therefore, the reaction rate is directly proportional to the
temperature. The reaction becomes faster as the temperature gets
higher.
Increasing the temperature of the reactants increases the
kinetic energy that it possesses causing the particles to move faster.
As they move faster, the frequency of collision between them
increases. This gives the reactants enough energy to overcome the
activation energy thus making the reaction faster.

36. • Catalysis: the increase in the rate of a chemical reaction by
lowering its activation energy.
• Transition state: an intermediate state during a chemical
reaction that has a higher energy than the reactants or the
products.
• Maxwell-Boltzmann Distribution: a probability distribution
used for describing the speeds of various particles within a
stationary container at a specific temperature. The distribution is
often represented with a graph, with the y-axis defined as the
number of molecules and the x-axis defined as the speed.

38. 1. The substance that enter into and is
altered in the course of a chemical
reaction.
a. Catalyst
b. Enzyme
c. Product
d. Reactant

39. 2. The measure of how fast is the
change in the concentration of the
reactants or products in a chemical
reaction.
a. Activation Energy
b. Activation Rate
c. Chemical Reaction
d. Concentration

40. 3. The measure of how fast is the
change in the concentration of the
reactants or products in a chemical
reaction.
a. Activation Energy
b. Activation Rate
c. Chemical Reaction
d. Concentration

41. 4. A chemical change that occurs when
two or more substances combine to
form a
new substance.
a. Activation Energy
b. Chemical Kinetics
c. Chemical Reaction
d. Product

42. 5. What is an enzyme?
a. An inorganic substance added to
food for better digestion.
b. An organic molecule that dissolves
nutrients in the body.
c. A biomolecule that releases energy
during chemical reactions.
d. A biomolecule that serves as
catalyst in biological system

43. 6. How does a catalyst work in
speeding up a reaction?
a. It lowers the activation energy.
b. It provides more energy.
c. It creates more reactants.
d. It increases the temperature.

44. 7. The measure of how fast or slow a
reaction happens.
a. Activation Energy
b. Collision theory
c. Particle Size
d. Rate of Reaction

45. 8. The minimum amount of energy
needed for colliding particles to react
is called the
a. chemical energy
b. activation energy
c. kinetic energy
d. potential energy

46. 9. Catalysts permit reactions to
proceed along a ___________energy
path.
a. higher
c. restricted
b. lower
d. Stabler

47. 8. A substance that increases the rate
of a reaction without being used up
during
the reaction is called a
a. catalyst
b. reactant
c. product
d. solute