Chemical reaction

3. 100%

10. ➢ I can define collision theory and
describe how it affects the chemical
reaction; and
➢I can explain the different factors
affecting the rate of reaction.

11. What is Collision
Theory?

12. • This theory states that
For reactions to occur, molecules, atoms, or ions
must first collide. Not all collisions are successful. In
order for collisions to be effective collisions, particles
must possess the minimum amount of energy needed
for the reaction and must collide with proper
orientation.

13. There are two factors that determine whether a
reaction will occur between two particles that are
colliding:
1. Substances or particles of reactants must physically
collide with enough energy
2. Substance or particles must come into contact or
collide in the correct orientation (facing the correct
way).

14. Figure 1
Figure 2

15. Figure 3 Figure 4

16. What is a
chemical
reaction?

17. It is the process by
which the atoms of
one or more
substances are
rearranged to form
different substances.

18. When two particles collide,
sometimes a chemical reaction
can occur, which means
the bonds between two or
more particles are broken and
reformed, creating one or
more new substances.

19. The substances or particles
that enter and is changed in
the chemical reaction are
called reactants and the
substances that are formed
are called products.

20. How can you tell
when a chemical
reaction has
taken place?

22. Which is the
healthiest
banana?

23. Which is the
healthiest
banana?

25. EXOTHERMIC REACTION ENDOTHERMIC REACTION

26. EXOTHERMIC REACTION ENDOTHERMIC REACTION

27. EXOTHERMIC REACTION ENDOTHERMIC REACTION

28. EXOTHERMIC REACTION ENDOTHERMIC REACTION
release absorb

29. EXOTHERMIC REACTION ENDOTHERMIC REACTION
release absorb
Heat

30. EXOTHERMIC REACTION ENDOTHERMIC REACTION
release absorb
Heat

32. What is your observation
when it comes to the
number of molecules?
Collisions? and the
reaction rate?

33. 1. Activation energy
2. Concentration
3. Temperature
4. Surface area and particle
size
5. Catalysts
6. Inhibitor

34. 1. Activation Energy
➢refers to the
minimum energy
required for a reaction
to take place.

35. 1. Activation Energy
➢When a collision provides energy equal
to or greater than the activation energy,
product can form.
➢On the other hand, if the particles have
energy that is less than the activation
energy, the collision is not effective, and
they just bounce off each other
unchanged.

36. 2. Temperature
➢refers to how hot or cold a
certain substance is.
➢Usually, a rise in temperature
of 10 degrees C doubles the
reaction rate. The rate of a
chemical reaction increases
with increasing temperature.

37. 2. Temperature
➢ As the temperature increases,
collision between atoms and
molecules becomes faster resulting
to build up of more energy.
➢ The increased kinetic energy will
equal to or exceed the activation
energy resulting to more collisions
giving rise to a reaction.

38. 3. Concentration
➢ It refers to the number of
particles present in a given
volume of solution
➢ It may also mean a measure
of how much of the solute
is dissolved in a solvent to
form a homogeneous
mixture.

39. 3. Concentration

40. 4. Surface Area
and Particle Size
➢is the measure of how much area of an
object is exposed.
➢When two reactants are in the same
fluid phase, their particles collide more
frequently than when one or both
reactants are solids.

41. 4. Surface Area
and Particle Size
➢If the reactants are
uniformly dispersed in a
single homogeneous
solution, then the number
of collisions per unit time
depends on concentration
and temperature.

42. 4. Surface Area
and Particle Size
➢If the reaction is
heterogeneous, however,
the reactants are in two
different phases, and
collisions between the
reactants can occur only at
interfaces between phases.

43. 4. Surface Area
and Particle Size
➢If the reaction is
heterogeneous, however, the
reactants are in two different
phases, and collisions between
the reactants can occur only at
interfaces between phases.
➢The reaction rate of a
heterogeneous reaction depends
on the surface area of the more
condensed phase.

44. 5. Catalysts
➢ A catalyst is a substance that increases the rate
of a chemical reaction without itself being used
up in the reaction.
➢ A catalysts provide an alternative energy
pathway for the reaction.
➢ The different pathway lowers the activation
energy allowing more molecules to overcome
the activation energy and produce products at
a faster rate

45. 6. Inhibitor
➢is a substance that slows
down, or inhibits reaction
rates.
➢Preservatives
➢Weed killer