1. Chemical Reactions

2. Chemical Reactions Study Guide
Chpt Acids and Bases
Chpt. 11: Balancing, Classifying, and Predicting Chemical Reactions
Chapter 17.1: Thermochemistry (pg )
Chpt. 18.1: Reaction Rates

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

4. 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.

5. 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

6. 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

7. 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)

8. 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.

9. 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)

10. 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.

11. 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.

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. Chemistry (3/4) Infinite Campus Update:
Conservation of Mass Lab (12pts.)
Balancing Chemical Equations (10pts)
Objectives:
Balancing Chemical Equation Quiz
Classifying Chemical Reactions
Discuss Law of Conservation of Mass Lab
Homework: (Due Wed.)
Balancing Chemical Equations Worksheet
Classifying Chemical Reactions Worksheets

24. 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.

25. Chemistry (3/6) Chemical Reaction Lab (pre-lab qts.)
Infinite Campus Update:
Balancing Chemical Equations Quiz (14pts.)
Due Today:
Balancing Chemical Equation Worksheet (10pts.)
Objectives:
Classifying Chemical Reactions
Identify energy changes associated with chemical reactions
Discuss Balancing Chemical Equation Quiz
Homework: (Due Wed.)
Classifying Chemical Reactions Worksheets
Chemical Reaction Lab (pre-lab qts.)

26. Chemistry (3/6) Infinite Campus Update:
Balancing Chemical Equations Quiz (14pts.)
Objectives:
Address qts. over Balancing Chemical Equation Quiz
Address qts. over Balancing and Classifying wks (homework)
Discuss Neutralization Reaction
Introduce Chemical Reaction Lab
Homework: (Due Wed.)
Chemical Reaction Lab (pre-lab qts.)

27. Chemical Reaction Lab
Purpose: To perform and observe eight chemical reactions in the lab.
Homework:
Read the introduction, background, and procedures section; then answer the pre-lab questions on the front. (1-9)

28. Balancing Chemical Equation Quiz

29. Types of Chemical Reactions
1. Synthesis (R+ S ----> RS)
2. Decomposition (RS------> R+ S)
3. Single Replacement (T+ RS ---> TS + R)
4. Double Replacement (R+S- + T+U- ---> R+U-+ T+S-)
5. Combustion (CxHx + O > CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)
(type of double replacement reaction)

30. Synthesis (Combination) Reaction
2 or more substances chemically combine to form a single substance.
R+ S ----> RS + energy
More energy is released at the end of the reaction then is needed to start the reaction.
(energy released by surroundings > energy absorbed by system)

31. Decomposition Reaction
A compound breaks down into simpler substances.
RS + energy ----> R S
More energy is required to start the reaction then is released at the end of the reaction.
(energy absorbed by system > energy released to surroundings) .

32. Single Replacement Reaction
An element replaces another element in a compound.
T+ RS ---> TS + R + energy
Usually energy of surrounding > energy of system

33. Double Replacement Reaction
Exchange of cations between two ionic compounds.
R+S- + T+U- ---> R+U-+ T+S- + energy
Usually energy of surrounding > energy of system

34. Combustion Reaction
Fuel (CHO) reacts with oxygen to produce predictable substances and energy.
CxHx(Ox) + O > CO2 + H2O + ENERGY
Always energy of surroundings > energy of system

35. Neutralization
An acid and a base react to produce predictable products.
Changes the pH to 7 (neutral).
Acid + Base > H2O + Salt(ionic compounds)
Salt: The cation comes from the base and the anion from the acid.
Ex. Na(OH) + HCl  NaCl + H2O

36. Chemistry (3/11)
Due:
Classifying and Balancing Chemical Equations wksht
Pre-lab questions(1-9) from Chemical Reaction Lab
Objectives:
Chemical Reaction Lab
Homework:
Turn in 3rd qtr. missing assignments for partial credit.
(Deadline: Wed. 3/13)

37. Chemical Equations to Lab
Write the reactants for each reaction, and then predict what type of reaction you think you are going to observe.
Mg O >
Mg HCl >
(NH4)2(CO3) >
Ca(CO3) + HCl >
Zn CuCl >
CuCl Na3(PO4) >
HCl Na(OH) >
C2H6O O >

38. Chemical Reaction Lab (3/11)
Purpose:
Predict the type of reaction for each experiment.
Perform, observe, and record data for each chemical reaction.

39. Chemistry (3/12) Infinite Campus Update:
Classifying and Balancing Chemical Rxtns. (10pts.)
Objective:
Chemical Reaction Lab
Homework:
Balancing reactions and establishing a conclusion for the lab.

40. Chemical Reaction Lab (3/12)
Purpose:
Complete chemical reaction lab.
Predict products of each reaction.
Balance each chemical reaction.

41. Chemistry (3/13) Objectives
Predict products of each reaction from the lab
Balance equations(if needed) and establish conclusion for lab.
Homework:
Complete chemical reaction lab

42. Chemical Equations to Lab
Predict the products of each reactant.
Mg O > MgO
Mg HCl >
(NH4)2(CO3) > NH CO H2O
Ca(CO3) + HCl > CaCl H2O CO2
Zn CuCl >
CuCl Na3(PO4) >
HCl Na(OH) >
C2H6O O >

43. 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

44. Conclusion A summary that includes the following:
Identify and explain which reactions from the lab were synthesis, decomposition, single replacement, double replacement, neutralization, combustion.
Based on the data section explain which reactions were exothermic and endothermic.
Which reaction(s) did you like the best and why?
What did you learn from this lab? (be specific)

45. Chemistry (3/14) Due Today: Chemical Reaction Lab Objectives:
Classifying reactions
Predicting products
Balancing chemical equations
Homework:
Predicting products and balancing equations wks.

46. (Chemistry 3/15) Infinite Campus:
*Chemical Reaction Lab (26pts. )-3rd qtr.*
Objectives:
Classify reactions
Predict products
Balance Chemical Equations
Homework:
Complete Predicting Products Worksheet.
Complete internet enrichment problems.
Monday: Quiz over chemical reactions. Study!

47. 3Ca + N2 --------> Ca3N2 (synthesis)
Chemical Reactions
Predict the products for each reaction and balance if needed.
3Ca N > Ca3N (synthesis)
b. Cu2S > Cu + S (decomposition)
2NaBr + F > 2NaF + Br2 (single replace)
CH O > CO H2O (combustion)
e. H2(CO3) + 2K(OH) > K2(CO3) H2O (neutralization)

48. Chemistry (3/18) Objectives:
Classifying, Balancing, Predicting Products
Activity Series Table and Single Replacement
Homework:
Activity Series Pre-Lab reading and hypothesis
Chemical Reaction Quiz (Wednesday)
Work on study guide (Test Monday)

49. Chemical Reactions: Bell Ringer
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 expressed above?
Predict the product(s) and balance if needed:
Ba (s) + O2 (g) >

50. Predicting Products

51. Predicting Products Gallery Walk
Objective:
Classify Type of Reaction
Predict Products
Balance Equation

52. Gallery Walk: Predicting Products
At each station complete the following:
Predict the type of reaction
Predict the products
Balance the chemical equation if needed

53. Chemistry (3/19) Objectives:
Activity Series Table and Single Replacement
Homework:
Activity Series Lab conclusion and post-Lab questions
Chemical Reaction Quiz (Wednesday)
Work on study guide (Test Monday)

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

56. Chemistry (3/20) Objectives: Chemical Reaction Quiz
Discuss Activity Series Lab
Discuss Endothermic and Exothermic Energy Diagrams
Homework:
Complete Activity Series Lab
Energy Changes Worksheet
Work on Study Guide

57. Activity Series Lab *After complete quiz, work on the following:
Complete conclusion and post-lab questions.

58. Chemistry (3/21) Infinite Campus Update:
Chemical Reaction Quiz (16pts.)
Due:
Activity Series Lab
Objectives:
Interpreting Activity Series Table
Interpret energy changes in chemical reactions.
Identify and test factors that affect the rate of chemical reactions.
Homework:
Work on study guide.

59. Activity Series Table *Study Guide Modification: omit qts. 18
Bell Ringer: Work on qts. 13 from study guide.

61. Thermochemistry Study of energy changes during a reaction.
Energy Review Qts:
When observing a chemical reaction what is the difference between the system and its surroundings?
Energy always flows from ____ matter to _____ matter. (cold, hot)

62. Chemistry:3/22 Infinite Campus: Chemical Reaction Quiz (16pts)
Assignments Collected:
Activity Series Lab
Objectives:
Interpret and classify energy changes in reactions
Identify and predict how factors affect the speed of a reaction.

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

64. Exothermic Reaction Energy (H) absorbed < Energy (H) released.
The chemical reaction becomes cooler and its surroundings gets warmer.
Test tube gets?
Energy is on the products side.
Examples:
combustion of fossil fuels (transportation)
C8H O > CO2 + H2O + energy
cellular respiration in living organisms
C6H12O6 + O > CO2 + H2O + energy

65. Endothermic Reactions
Energy (H) absorbed > Energy (H) released
Chemical reaction gets warmer and its surroundings gets cooler.
Test tube gets ?
Energy is on the reactants side.
Ex. Photosynthesis

66. Energy Diagram
(H)
(time)

67. Chemical Reaction Energy Diagram
Activation Energy (Ea): The minimum amount of
energy needed for the reaction to occur.
H: Energy change between reactants and products.
( H = H products – H reactants)

68. Energy Diagram
Does this represent an endothermic or exothermic reaction?
(H)
(time)

69. Energy Diagram Small activiation energy
H reactant > H product
Small activiation energy
More energy will be released in this reaction
(H)
(time)

70. Energy Diagram
Does this represent an endothermic or exothermic reaction?
Activation
Energy
(H)
(time)

71. Endothermic Energy Diagram
H reactant < H product
Large activation energy
More energy will be absorbed in this reaction
Activation
Energy

72. Thermochemistry Examples
Classify the following examples as endothermic (E) or (Ex) exothermic:
If the surroundings gets cooler and the system gets warmer.
Ice cream melting.
Melted paraffin wax is left at room temperature until it solidifies.
AlCl > Al + Cl2 + energy
A bright light is created when magnesium reacts with oxygen.
When hydrochloric acid reacts with magnesium the test tube will get warm.

73. 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.

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

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

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

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

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

79. 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.

80. Catalyst and Energy Change

81. Inhibitors
Inhibitors slow down a chemical reaction, but are not apart of the 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.

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

83. Chemical Reaction Study Guide