1. Chemical Reactions

2. Chemical Reactions Study Guide Chpt. 9.4 Acids and Bases Chpt. 11: Balancing, Classifying, and Predicting Chemical Reactions Chpt. 18.1: Reaction Rates

3. 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.

4. Chemical Reaction Pre-Test 1.What is a chemical reaction? 2.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: Iron chemically reacts with Oxygen to produce Iron(II) Oxide a.Express the word equation as a chemical equation. b.Give an example of a reactant and a product from this reaction. c.Balance the chemical equation if needed. d.Circle the type of chemical reaction you think this represents.: synthesis, decomposition, replacement, neutralization, combustion

5. Chemical Reaction Iron chemically reacts with Oxygen to produce Iron(II) Oxide

6. 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.

7. Pre-AP Chemistry (2/14) Due: Acid Rain Article w/qts. Ingredients Assignment for partial credit Objectives: Acid/Base Nomenclature Quiz Balance Chemical Equations Homework: Balancing Chemical Equations worksheet (Do even problems on front and back.)

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: Iron chemically reacts with Oxygen to produce Iron(II) Oxide

9. Chemical Equations Fe + O 2 ------> 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. Chemical Equations Fe (s) + O 2 (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. Chemical Reactions Fe (s) + O 2 (g) ------> FeO (s) Are atoms destroyed or created during a chemical reaction? No, they are just rearranged to produce new substances.

12. Chemical Reactions Infinite Campus Update: Acid/Base Nomenclature Quiz (15pts.) Cu and Zn Alloy Lab(10pts.) Ingredients Assignment (20 pts.) Acid Nomenclature worksheet (10pts.) Objectives: Establish and balance chemical equations

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. Balancing Chemical Equations a. K + MgCl 2 ---------> KCl + Mg b. Ag 2 O ---------> Ag + O 2 c. CH 4 + O 2 -------> CO 2 + H 2 O

15. Chemical Reactions (2/19) Objectives: Balance chemical equations Validate the Law of Conservation of Mass

16. Chemical Equations

17. Balancing Chemical Equations Dihydrogen monoxide + sodium (hydrogen carbonate) ---> carbon dioxide + sodium hydroxide + dihydrogen monoxide a.convert to chemical equation b.Balance equation if needed.

18. 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.

19. 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

20. Open vs. Closed System http://www.chem.umass.edu/people/botch/Chem122S08/Chapters/Ch6/InternalE.html

21. 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).

22. States of Matter Abbreviations Fe (s) + O 2 (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)

23. Chemical Equations 1.magnesium chloride + fluorine yields magnesium fluoride + chlorine 2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

24. 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).

25. Pre-AP Chemistry (2/25) Reminder: Quiz over balancing chemical equations. Objective: Validate the Law of Conservation of Mass (Design, perform, and analyze chemical reaction between Alka Seltzer and tap water). Formal Lab report due on March 6 th (typed)

26. Chemical Equations 1.magnesium chloride + fluorine yields magnesium fluoride + chlorine 2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

27. 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)

28. Open vs. Closed System http://www.chem.umass.edu/people/botch/Chem122S08/Chapters/Ch6/InternalE.html

29. Chemical Reactions Bell Ringer 1. N 2 (g) + H 2 (g) --------> NH 3 (g) a.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.

30. Law of Conservation of Mass Lab Team #Open SystemClosed System 1 2 3 4 5 6 7 8

31. Pre-AP Chemistry (2/27) Objectives: Discuss lab results and format of lab report Discuss types of reactions. Classify chemical reactions. Review balancing equations quiz Homework: Balancing and classifying chemical reactions

32. 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 (C x H x + O 2 ----> CO 2 + H 2 O) 6. Neutralization (Acid + Base--> H 2 O + Salt) (type of double replacement reaction)

33. Chemical Reactions Objectives 1.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.

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

35. Decomposition Reaction A compound breaks down into simpler substances. RS + energy ----> R + S Energy of system > Energy of surroundings Why? Breaking more bonds then creating bonds.

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

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

38. Combustion Reaction Fuel (hydrocarbons) reacts with oxygen to produce predictable substances and energy. C x H x (O x ) + O 2 ----> CO 2 + H 2 O + ENERGY Energy of Surroundings > Energy of System

39. Neutralization An acid and a base react to produce predictable products. Changes the pH to 7 (neutral). Acid + Base -------> H 2 O + Salt Salt: The cation comes from the base and the anion from the acid. Ex. Na(OH) + HCl  NaCl + H 2 O

40. Pre-AP Chemistry (2/28) Objectives: Balance and classify chemical reactions. Classify chemical reactions as either exothermic or endothermic. Clarify format of lab report. Homework: Work on Formal Lab Report Chemical Reactions Lab: Read background/procedures and answer pre-lab qts.

41. Bell Ringer: Classifying Reactions Classify and balance each reaction below. H 2 O + energy ---> H 2 + O 2 C 4 H 10 + O 2 ----> CO 2 + H 2 O + energy 3. Cl 2 + KBr ------> KCl + Br 2 + energy 4. K + F 2 ---> KF + energy 5. Li(OH) + H 2 (SO 4 ) ----> Li 2 (SO 4 ) + H 2 O

42. Classifying and Balancing Chemical Equations

43. Pre-AP Chemistry (3/4) Infinite Campus: Classifying and Balancing Chemical Equations(10pt) Objectives: Chemical Reaction Lab Homework: (Due Wed.) Conservation of Mass Lab Report –rough draft Predict products and balance each chemical reaction.

44. Pre-AP Chemistry (3/6) Infinite Campus: Classifying and Balancing Chemical Equations(10pt) Due: Conservation of Mass Lab Report –rough draft Objectives: Complete chemical reaction lab Predict products and balance each chemical equation. Homework: (Due Monday) Complete the lab (balance each equation) Predict products worksheet

45. Chemical Reaction Lab Purpose: Determine reactants and predict type of rxtn. Perform, observe, and record chemical reactions. Predict products and balance each chemical rxtn.

46. Chemical Equations to Lab ReactionChemical Equation 1 2 3 4 5 6 7 8

47. Pre-AP chemistry (3/11) Reminder: Rough draft: Conservation of Mass Lab report (partial credit) Objectives: Predict products and balance chemical equations. Establish conclusion from chemical reaction lab. Homework: Predict products and balance reactions worksheet Conclusion from Chemical Reaction Lab

48. Chemical Equations to Lab Just need to check and see if they are balanced. 1.Mg + O 2 ------> 2.Mg + HCl ----> 3.(NH 4 ) 2 (CO 3 ) -----> NH 3 + CO 2 + H 2 O 4.Ca(CO 3 ) + HCl ----> CaCl 2 + H 2 O + CO 2 5. Zn + CuCl 2 ----> 6.CuCl 2 + Na 3 (PO 4 ) ---> 7.HCl + Na(OH) ----> 8.C 2 H 6 O + O 2 ----->

49. Chemical Equations to Lab Just need to check and see if they are balanced. 1.Mg + O 2 ------> MgO 2.Mg + HCl ----> MgCl + H 2 3.(NH 4 ) 2 (CO 3 ) -----> NH 3 + CO 2 + H 2 O 4.Ca(CO 3 ) + HCl ----> CaCl 2 + H 2 O + CO 2 5.Zn + CuCl 2 ----> ZnCl 2 + Cu 6.CuCl 2 + Na 3 (PO 4 ) ---> Cu 3 (PO 4 ) 2 + NaCl 7.HCl + Na(OH) ----> H 2 O + NaCl 8.C 2 H 6 O + O 2 -----> CO 2 + H 2 O

50. Conclusion A summary that includes the following: Identify and explain the types of reactions obsvd. ? 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)

51. Pre-AP Chemistry (3/12) Due: Chemical Reaction Lab Objectives: Predict products in a chemical reaction. Predict when single replacement reactions will occur using the activity series table. Homework: Complete the Predicting Products worksheet Read about activity series table and complete pre-lab questions for Activity Series lab.

52. Predicting Products

53. Pre-AP Chemistry (3/13) Infinite Campus Update: Chemical Reaction Lab (26pts.) Objectives: Classifying, predicting products, and balancing chemical reactions. Homework: Read procedures for Activity Series Lab Establish hypothesis for Activity Series Lab

54. Predicting Products Assessment

55. Gallery Walk: Predicting Products At each station complete the following: a.Write the chemical formula of the reactant(s) b.Predict type of reaction c.Predict products d.Balance chemical reaction if needed

56. Pre-AP Chemistry (3/14) Infinite Campus: Chemical Reaction Lab Law of Conservation of Mass Lab rough draft Predicting Products worksheet (4 th qtr.) Objectives: Perform and record data from Activity Series Lab Establish a conclusion (compare data with your hypothesis) Homework: Complete post-lab questions

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

58. Activity Series Lab Hypothesis CuCl 2 (aq)Ag(NO 3 ) (aq) HCl (aq)dH(OH) (l) Copper (s) Magnesium (s) Zinc (s) Calcium (s)

59. Pre-AP Chemistry 3/18) Infinite Campus Update: Activity Series Lab Chemical Reaction Quiz Objectives: Predict single replacement reactions using activity series table. Predict solubility of products in double replacement reaction. Go over chemical reaction quiz Homework: Complete Solubility Rules worksheet (due Tues.) Work on Study Guide Test (Friday, March 22 nd )

60. Pre-AP Chemistry 3/19) Infinite Campus Update: Activity Series Lab Chemical Reaction Quiz Objectives: Predict single replacement reactions using activity series table. Predict solubility of products in double replacement reaction. Go over chemical reaction quiz Homework: Work on Study Guide Test (Friday, March 22 nd )

61. Pre-AP Chemsistry (3/20)

62. Solubility Rules for Ionic Compounds myweb.bloomu.edu Ag, Ca, Hg(II)

63. Predicting Products Using Solubility Rules Ag(NO 3 )CaCl 2 Na(OH) Na 3 (PO 4 ) NaCl 1.Predict products for each double replacement reaction. 2.Determine if one of the products will be a precipitate. 3.Balance the equation if needed.

64. Predicting Products in a Chemical Reaction Predict the products and balance the equation if needed. a. Ca + N 2 --------> ? b. Cu 2 S -------> ? c. AlBr 3 + F 2 ------> ? d. CH 4 + O 2 -----> ? e. Ca(OH) 2 + H 3 (PO 4 ) ----->

65. Predicting Products in a Chemical Reaction a. 3Ca + N 2 --------> Ca 3 N 2 b. Cu 2 S -------> 2Cu + S c. 2AlBr 3 + 3F 2 ------> 2AlF 3 + 3Br 2 d. CH 4 + 2O 2 -----> CO 2 + 2H 2 O e. 3Ca(OH) 2 + 2H 3 (PO 4 ) -----> Ca 3 (PO 4 ) 2 + 6H 2 O

66. Chemical Reaction Review 1.What are the coefficients that will balance the chemical equation below? AlCl 3 + Na(OH) ----> Al(OH) 3 + NaCl a.1,3,1,3 b.3,1,3,1 c.1,1,1,3 d.1,3,3,1 2.What type of chemical reaction is in question 1? 3.Predict the product and balance if needed: Ba (s) + O 2 (g) ---------->

67. Activity Series Lab Complete conclusion Complete Post Lab Questions

68. Activity Series Lab 1.Using the Activity Series Table, predict whether the following single replacement reactions would occur: a.Li + MgCl b. Hg + Na 3 P c. Pb + HF

69. Chemical Reactions Study Guide Chpt. 9.4 Acids and Bases Chpt. 11: Balancing, Classifying, and Predicting Chemical Reactions Chpt. 18.1: Reaction Rates

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

71. Predicting Single Replacement Reactions 1. Determine which single replacement reactions below can occur using your Activity Series diagram: a.K + MgCl 2 b.Al + Li 3 (PO 4 ) c.Sn 2+ + HCl d. Ag + HCl e.Pb 4+ + H 2 (SO 3 )

72. 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)

73. Thermochemistry Energy changes that occur within reactions. Endothermic ReactionsExothermic Reactions

74. 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) C 8 H 18 + O 2 -------> CO 2 + H 2 O + energy cellular respiration in living organisms C 6 H 12 O 6 + O 2 ------> CO 2 + H 2 O + energy

75. 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

76. Energy Diagram (H) (time)

77. 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)

78. Chemical Reaction Energy Diagram Does this represent an endothermic or exothermic reaction?

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

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

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

82. Pre-AP Chemistry (3/21) Infinite Campus Update: Solubility Rules Homework (10pts.) Objectives: Interpret energy changes in chemical reactions. Identify and test factors that affect the rate of chemical reactions. Go over quiz Homework: Work on study guide. Test Friday or Monday?

83. 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.

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

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

86. Temperature of Reaction What if we increase the temperature of a reaction? Increase speed of reaction What if we decrease the temperature of a reaction? Decrease speed of reaction

87. Concentration Increase concentration of reactants? Increases speed of reaction Decrease concentration of reactants? Decreases speed of reaction

88. Surface Area Increase surface area of reactants? Increases the speed of a reaction Decrease surface area of reactants? Decreases speed of reaction

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

90. Catalyst and Energy Change

91. 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.

92. Chemical Reactions Study Guide Chpt. 9.4 Acids and Bases Chpt. 11: Balancing, Classifying, and Predicting Chemical Reactions Chpt. 18.1: Reaction Rates

93. Chemical Reaction Study Guide