1. Chemical Reactions

2. Chemical Reactions Objectives
1.Classify and name compounds in chemical reactions
2.Describe chemical reactions in word and chemical equations.
3.Balance chemical equations based on the Law of Conservation of Mass.
4.Identify and classify types of chemical reactions and energy changes involved.
5.Predict products and energy changes in a chemical reaction.
6.Identify and test factors that affect the rate of chemical reactions.

3. Chemical Reactions What is a chemical reaction?
Use your background knowledge to explain what a chemical reaction is.
Think about chemical changes you have observed in your surroundings.
Think about chemical changes on an atomic level.

4. Chemical Reactions
Substances chemically interact to form different substances.
A substance can be an element or a compound.
Chemical bonds are broken and created.
Example:
Iron chemically reacts with Oxygen to produce Iron(II) Oxide

5. Chemical Equations Fe + O2 ------> FeO Reactants:
Starting substances.
Chemically interact with one another.
Usually located to the left of the arrow.
Products:
Ending substances.
Substances formed from the chemical reaction.
Usually located to the right of the arrow.

6. Chemical Equations
Fe(s) + O2 (g) > FeO (s)
(s)= substance in solid state
(g)= substancein gaseous state
(l)= substance in liquid state
(aq)= substance dissovled in water.
(aqueous solution)

7. Chemical Reactions
Fe(s) + O2 (g) > FeO (s)
Are atoms destroyed or created during a chemical reaction?
No, they are just rearranged to produce new substances.

8. Law of Conservation Of Mass
Matter is not created or destroyed.
Matter is just rearranged.
(mass of reactants = mass of products)
That is why it is important to balance chemical equations.

9. Conservation of Mass Lab
Observe the conservation of mass lab, to understand why it is important to balance chemical equations.

10. Balancing Chemical Equations
2Fe(s) + O2 (g) > 2FeO (s)
Balancing Chemical Equations:
Add coefficients in front of substances, do NOT change subscripts.
2. First balance elements that only appear once on each side of the equation.

11. Balancing Chemical Equations

12. Chemical Reactions Bell Ringer
1. N2 (g) H2(g) > NH3(g)
What is the chemical name of one of the reactants?
b. What is the chemical name of the product?
c. What state of matter is all the substances in this reaction?
d. Balance the chemical equation if needed.

13. Type of Anion
Name of Acid
Monatomic anion
(-ide ending)
hydro + stem + ic
Polyatomic anion
(-ite ending)
stem + ous
(-ate ending)
stem + ic

14. Balancing Chemical Equations

15. Types of Chemical Reactions
1. Synthesis (A+ B ----> AB)
2. Decomposition (AB------> A + B)
3. Single Replacement (A+ BC ---> B + AC)
4. Double Replacement (AB + CD ---> CB + AD)
5. Combustion (CxHx + O > CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)

16. Chemical Reactions Objectives
Identify and classify types of chemical reactions.
2. Identify energy changes involved with chemical reactions.
3. Predict products and energy changes in a chemical reaction.

17. Synthesis (Combination) Reaction
2 or more substances chemically combine to form a single substance.
A + B ---> AB + energy
Energy released into surroundings is more than energy absorbed by the system.
( Energy of surroundings > Energy of system)

18. Decomposition Reaction
A compound breaks down into simpler substances.
AB + energy ----> A B
Energy of system > Energy of surroundings
Why?

19. Single Replacement Reaction
An element replaces another element in a compound.
A + BC > B + AC + energy
Energy of surroundings > Energy of system

20. Double Replacement Reaction
Exchange of cations between two compounds.
AB + CD + energy ----> CB AD + more energy
Energy of Surrounding > Energy of System

21. Combustion Reaction
Fuel (hydrocarbons) reacts with oxygen to produce predictable substances and energy.
CxHx + O > CO2 + H2O + ENERGY
Energy of Surroundings > Energy of System

22. Neutralization Acid and Base react to produce predictable products.
Changes the pH to 7 (neutral).
Acid + Base > H2O + Salt
Salt: An ionic compound.
The cation comes from the base and the anion from the acid.

23. Class Reminders: Acid Rain Article (15pts.)
Balance Chemical Equations Worksheet (10pts.)
(balance and classify equations)
Word Equation Worksheet (10pts.)
*3rd Quarter Ends: March 8th*

24. Chemical Reaction Lab Purpose:
Perform and observe types of chemical reactions.
Determine reactants and predict products.
Classify chemical reactions.
Balance chemical reactions.
Write a formal lab report

25. Chemical Equations to Lab
Reaction
Chemical Equation 1 2 3 4 5 6 7 8

26. Types of Chemical Reactions
1. Synthesis (A+ B ----> AB)
2. Decomposition (AB------> A + B)
3. Single Replacement (A+ BC ---> B + AC)
4. Double Replacement (AB + CD ---> CB + AD)
5. Combustion (CxHx + O > CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)

27. Chemical Equations to Lab
Just need to check and see if they are balanced.
Mg O >
Mg HCl >
(NH4)2(CO3) > NH CO H2O
Ca(CO3) + HCl > CaCl H2O CO2
Zn CuCl >
CuCl Na3(PO4) >
HCl Na(OH) > H2O + NaCl
C2H6O O >

28. Chemical Reaction Review
What are the coefficients that will balance the chemical equation below?
AlCl3 + Na(OH) ----> Al(OH)3 + NaCl
1,3,1,3
3,1,3,1
1,1,1,3
1,3,3,1
What type of chemical reaction is in question 1?
Predict the product and balance if needed:
Ba (s) + O2 (g) >

29. Balancing and Classifying Chemical Reactions

30. Chemical Equations to Lab
Just need to check and see if they are balanced.
Mg O > MgO
Mg HCl > MgCl + H2
(NH4)2(CO3) > NH CO H2O
Ca(CO3) + HCl > CaCl H2O CO2
Zn CuCl > ZnCl2 + Cu
CuCl Na3(PO4) > Cu3(PO4)2 + NaCl
HCl Na(OH) > H2O + NaCl
C2H6O O > CO2 + H2O

31. Conclusion Needs to include the following:
Identify and explain the types of reactions obsvd. ?
Which reaction(s) did you like the best and why?
Based on data section explain which reactions were exothermic and endothermic.
What did you learn from this lab?

32. Predicting Products in a Chemical Reaction
Ca N > ?
b. Cu2S > ?
NaBr + F > ?
CH O >

33. Balancing and Classifying Equations Quiz
Types of Chemical Reactions 1. Synthesis 2. Decomposition 3. Single Replacement 4. Double Replacement 5. Combustion 6. Neutralization

34. Predicting Products Check my webpage for correct chemical formulas
prior to balancing.

35. Predicting Single Replacement Reactions
An Activity Series can help us predict if a single replacement reaction will take place.

36. Activity Series Lab Hypothesis
CuCl2(aq)
Ag(NO3)
HCl (aq)
dH(OH) (l)
Copper (s)
Magnesium (s)
Zinc (s)
Calcium (s)

37. Activity Series Lab
Complete conclusion
Complete Post Lab Questions

38. Activity Series Lab
Using the Activity Series Table, predict whether the following single replacement reactions would occur:
Li + MgCl
b. Hg + Na3P
c. Pb + HF

39. Predicting Single Replacement Reactions
An Activity Series can help us predict if a single replacement reaction will take place.

40. Activity Series Lab
Complete conclusion
Complete Post Lab Questions

41. Chemical Reaction Study Guide Changes
Vocabulary words: Thermochemistry
10. HgO + energy > Hg + O2
11. Fe + F > FeF3 + energy
CH4 + O > CO2 + H2O + energy
K(OH) + H3(PO4) >
18. Omit last word equation. 

42. Chemical Reaction Review
What are the coefficients that will balance the chemical equation below?
AlCl3 + Na(OH) ----> Al(OH)3 + NaCl
1,3,1,3
3,1,3,1
1,1,1,3
1,3,3,1
What type of chemical reaction is in question 1?
Predict the product and balance if needed:
BaS + Mg >

43. Thermochemistry Energy changes that occur within reactions.
Endothermic Reactions
Exothermic Reactions

44. Exothermic Reaction Energy absorbed < Energy released.
The chemical reaction becomes cooler and its surroundings gets warmer.
Energy is on the product side.
C8H O > CO2 + H2O + energy

45. Endothermic Reactions
Energy absorbed > Energy released
Chemical reaction gets warmer and its surroundings gets cooler.
Energy is on the reactant side.
Ex. Photosynthesis

46. Chemical Reaction Energy Diagram

47. Chemical Reaction Energy Diagram
Activation Energy (Ea): The amount of kinetic energy
needed to be absorbed from the surroundings for the
chemical reaction to occur.
H : The amount of kinetic energy released into the
into the surroundings.

48. Chemical Reaction Energy Diagram Exothermic Reaction

49. Chemical Reaction Energy Diagram Endothermic Reaction
Activation
Energy

50. Chemical Reactions Objectives
1.Classify and name compounds in chemical reactions
2.Describe chemical reactions in word and chemical equations.
3.Balance chemical equations based on the Law of Conservation of Mass.
4.Identify and classify types of chemical reactions and energy changes involved.
5.Predict products and energy changes in a chemical reaction.
6.Identify and test factors that affect the rate of chemical reactions. (Chpt. 18.1)

51. Chemical Reaction Rates
Assignment:
Read Section: in textbook (pg. 540)

52. Chemical Reactions Rates
Reaction Rates = how fast the reactants chemically change into the products.
Collision Theory: Reactant particles will react to form products when they collide and exchange enough kinetic energy with one another.

53. Rates of Chemical Reactions
What are factors that can affect the rates of reactions?

54. Rates of Chemical Reactions
What are factors that can affect the rates of reactions?
Temperature
Concentration of Reactants
Surface Area of Reactants
Catalysts
Inhibitors

55. Temperature of Reaction
What if we increase the temperature of a reaction?
What if we decrease the temperature of a reaction?

56. Concentration Increase concentration of reactants?
Decrease concentration of reactants?

57. Surface Area Increase surface area of reactants?
Decrease surface area of reactants?

58. Catalysts
Catalysts speed up reactions, but they are not apart of the chemical reaction.
Ex. Enzymes keep your body temperature around 37oC (98 oF) by speeding up important biological reactions.

59. Catalyst and Energy Change

60. Inhibitors Inhibitors slow down a chemical reaction.
Inhibitors bind to a catalyst and prevent it from speeding up a reaction.
Ex. Preservation of food. Antioxidants prevent foods from becoming stale or moldy.

61. Soln. A Concentration vs. Avg. Reaction Times7 6 9
9.4 5 3
4.0 A2
6.4
9.76
9.5 8
15.2 A3
4.8 12
13.4
22.6 A4
8.9 15
15.0
19.1 14
24.3

62. Activation Energy
Activation energy = minimum energy colliding reactants must have for a reaction to occur. (Energy hump.)

63. Catalyst and Energy Change