1. Chemical Reactions

2. Chemistry (2/25) Acid/Base Quiz
Interpreting and Balancing chemical equations
Due:
Acid/Base Nomenclature worksheet for partial credit

5. 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.

6. Chemistry (2/26) Infinite Campus Update:
Acid/Base Nomenclature Worksheet (10pts.)
Acid/Base Quiz (15pts.)
*Check infinite a lot of missing assignments!*
Objectives:
Interpreting and Balancing chemical equations
Homework:
Check for missing assignments on infinite campus
Balancing chemical equations worksheet

7. Chemical Reaction Pre-Test
What is a chemical reaction?
If matter is conserved during a chemical reaction, how is it new matter is “created”?
3. Complete the questions below on the following word equation:
Fe(s) + O2 (g) ----> FeO (s)
Give an example of a reactant from this reaction.
Give an example of a product from this reaction.
Balance the chemical equation if needed.
Circle the type of chemical reaction you think this represents.
synthesis decomposition replacement
neutralization combustion

8. 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: Fe(s) + O2 (g) ----> FeO (s)

9. 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.

10. Fe(s) + O2 (g) ------> FeO (s)
Chemical Equations
Fe(s) + O2 (g) > FeO (s)
Abbreviations for state of matter in an equation.
(s)= substance in solid state
(g)= substance in gaseous state
(l)= substance in liquid state
(aq)= substance dissovled in water.
(aqueous solution)

11. Law of Conservation of Mass
Fe(s) + O2 (g) > FeO (s)
Are atoms destroyed or created during a chemical reaction?
No, they are just rearranged to produce new substances.

12. Law of Conservation of Mass
Fe(s) + O2 (g) > FeO (s)

13. Balancing Chemical Equations
Why? Observe the Law of Conservation of Mass Rules: 1. Add coefficients in front of substances, do NOT change subscripts. 2. First balance elements that only appear once on each side of the equation. 3. Make sure coefficients are expressed in lowest terms.

14. Chemistry (2/27) Objectives:
Interpreting and Balancing chemical equations
Review acid/base quiz
Homework:
Balancing equations worksheet(due Thursday)
Law of Conservation of Mass pre-lab qts. and hypothesis
Review acids/bases nomenclature
Check for missing assignments in infinite campus
Lab:
Law of Conservation of Mass Lab: (Thursday)

15. Law of Conservation of Mass Lab
Homework:
Read through the background and procedures section.
Complete pre-lab questions and hypothesis.

16. Balancing Chemical Equations
a. K + MgCl > KCl + Mg b. Ag2O > Ag + O2 c. CH4 + O > CO2 + H2O

17. Chemical Equations

18. Chemistry (2/28) Objectives:
Interpreting and Balancing Chemical Equations
Validate the Law of Conservation of Mass with scientific evidence.
Due Today:
Balancing chemical equations worksheet (turn in tray)
Law of Conservation of Mass pre-lab qts. and hypothesis
Homework:
Balancing Chemical Equations practice problems (Fri.)
Check for missing assignments in infinite campus

19. Balancing Chemical Equations
Dihydrogen monoxide + sodium (bicarbonate) ---> carbon dioxide + sodium hydroxide + dihydrogen monoxide

20. Law of Conservation of Mass Lab
Purpose:
Validate the Law of Conservation of Mass
Lab Reminders:
Follow ALL lab procedures carefully.
Use the same balance for all measurements.

21. Acid/Base Nomenclature Quiz

23. Exit Slip: Interpret and Balance Chemical Equations
Cl2 (g) + KBr (aq) ----> KCl (aq) + Br2 (l)
Balance the equation if needed
CH4 (g) + O2 (g)  CO2(g) + H2O(g)
Balance the equation if needed.
Identify the diatomic molecule in this reaction.

24. Exit Slip: Interpret and Balance Chemical Equations
Cl2 (g) + KBr (aq) ----> KCl (aq) + Br2 (l)
Which reactant is a molecule?
What is the chemical name of the product that is an ionic compound?
What does (aq) mean?
Balance the equation if needed
CH4 (g) + O2 (g)  CO2(g) + H2O(g)
Balance the equation if needed.
Identify the diatomic molecule in this reaction.

25. Balancing Chemical Equations
Dihydrogen monoxide + sodium (bicarbonate) ---> carbon dioxide + sodium hydroxide + dihydrogen monoxide
convert to chemical equation
Balance equation if needed.

26. 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.

27. Law of Conservation of Mass Inquiry Lab
Purpose: To prove mass is conserved in chemical reactions.
Materials and Procedures: Groups will establish
Record and analyze data
Establish a conclusion

28. Open vs. Closed System

29. pre-AP Chemistry (2/20) Objectives:
Clarify misconceptions with writing and balancing chemical equations.
Validate the Law of Conservation of Mass
(Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

30. States of Matter Abbreviations
Fe(s) + O2 (g) > FeO (s)
Abbreviations for state of matter in an equation.
(s)= substance in solid state
(g)= substance in gaseous state
(l)= substance in liquid state
(aq)= substance dissovled in water.
(aqueous solution)

31. Chemical Equations
magnesium chloride + fluorine yields magnesium fluoride + chlorine
2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

32. Pre-AP Chemistry (2/21) Reminder:
Quiz tomorrow over writing and balancing chemical equations. (complete extra practice problems from paper or webpage)
Objective:
Validate the Law of Conservation of Mass
(Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

33. Pre-AP Chemistry (2/22) Reminder:
Quiz today over writing and balancing chemical equations. (complete extra practice problems from paper or webpage)
Objective:
Validate the Law of Conservation of Mass
(Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

34. Chemical Equations

35. Chemical Equations
magnesium chloride + fluorine yields magnesium fluoride + chlorine
2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

36. Law of Conservation of Mass Inquiry Lab
Purpose ,Background, Hypothesis: completed
Objectives:
List materials needed for each experiment.
List procedures specific enough for someone else to repeat. (sign-off by Ms. Leeper)
Perform experiments and record data.
(record all qualitative and quantiative data)

37. Open vs. Closed System

38. 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.

39. Balancing Chemical Equations

40. 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)
*Each letter represents a substance*

41. 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.

42. 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)

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

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

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

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

47. 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.

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

49. 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

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

51. 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)

52. 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 >

53. 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) >

54. Balancing and Classifying Chemical Reactions

55. 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

56. 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?

57. Infinite Campus Update
Chemical Reaction Lab (20pts.)
Balancing Chemical Equation Wksht.(10pts.)

58. Chemical Reaction Review
1. Classify the type or reaction and balance if needed:
a. C6H12 + O > CO2 + H2O
b. LiCl > Li + Cl2
c. H2(SO3) + Al(OH) > H2O + Al2(SO3)3

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

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

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

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

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

64. Activity Series Lab
Complete conclusion
Complete Post Lab Questions

65. 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

66. Chemical Reactions Study Guide
Chpt Acids and Bases
Chpt. 11: Balancing, Classifying, and Predicting Chemical Reactions
Chpt. 18.1: Reaction Rates

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

68. Predicting Single Replacement Reactions
1. Determine which single replacement reactions below can occur using your Activity Series diagram:
K + MgCl2
Al + Li3(PO4)
Sn HCl
Ag + HCl
Pb H2(SO3)

69. 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. 

70. 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 >

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

72. 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

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

74. Chemical Reaction Review
Using the Activity Series diagram would the
following reactions take place?
a. Al + Cu(OH)
Ag + HCl
Classify the type or reaction and balance if needed:
a. C6H12 + O > CO2 + H2O
b. LiCl > Li + Cl2
c. H2(SO3) + Al(OH) > H2O + Al2(SO3)3

75. Endothermic vs. Exothermic

76. Infinite Campus Update
Chemical Reaction Lab(20pts.)
Activity Series Lab (10pts.) (1,2,4,6)
Balancing Chemical Equation Wksht.(10pts.)
Word Equation Worksheet (10pts.)

77. Infinite Campus Update
Chemical Reaction Lab(20pts.)
Balancing Chemical Equation Wksht.(10pts.)
Word Equation Worksheet (10pts.)

78. Bell Ringer: Thermochemistry
Classify as exothermic (Ex) or endothermic. (Endo)
C8H18 + O > CO2 + H2O + energy
BaBr2 + energy > Ba + Br2
2. During an experiment you observed the test tube getting cooler. Explain why this is happening including the terms system and surroundings.
Using the activity series determine which reactions will occur in nature:
Mg + FeCl2
Cu + K(OH)
Al + H2(CO3)

79. Thermochemistry Wksht
Work on question 2 on Thermochemistry wksht.

80. Chemical Reaction Energy Diagram

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

82. Chemical Reaction Energy Diagram

83. Chemical Reaction Energy Diagram
Activation
Energy

84. 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)

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

86. Chemical Reactions Rates
Reaction Rates = how fast the reactants chemically change into the products.
Collision Theory: Reactant particles will form products when reactants collide:
at the right position.
and exchange the right amount of kinetic energy.

87. Rates of Chemical Reactions
What are factors that can affect the speed of a reaction?

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

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

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

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

92. 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.

93. Catalyst and Energy Change

94. 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.

95. Soln. A Concentration vs. Avg. Reaction Times
(100%) 15 20 35 16 37 22 25 A2
(75%) 19 24 38 31 44 28 A3
(50%) 33 65 A4
(25%) 50 39 34 29 78

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

97. Chemical Reactions Study Guide
Chpt Acids and Bases
Chpt. 11: Balancing, Classifying, and Predicting Chemical Reactions
Chpt. 18.1: Reaction Rates

98. Infinite Campus Update
Classifying Chemical Reaction lab (20pts.)
Activity Series Lab (10pts.)
Starch Iodine Lab (10pts.)-due Wed.
ACT Test for Juniors: Tomorrow, March 6th
End of quarter: Thursday, March 8th

99. Chemical Reaction Study Guide

100. Catalyst and Energy Change

101. Infinite Campus Updated
Activity Series Lab (10pts)
Classifying Chemical Reaction Lab (15pts)
(Do NOT throw away-Formal Lab Report)
Starch-Iodine Reaction Lab w/graph. (15pts)
Quarter End: Tomorrow, March 8th
(All assignments by Friday).

102. Formal Lab Report Due: March 14th (next Wed.)
Written (legible) or Typed (save to flashdrive)