Name:___________________________Period:__________________________

Chemistry Unit 7 – Chemical Reactions Chemistry Daily JournalToday’s Date

What did I accomplish yesterday?

What are my goals today? What sections, activities, and labs do I want to get done today?

1

Objective Learning Opportunities Suggested Due Date

Date Completed

7.1 Identify the parts of a chemical equation.

□ Read p. 321 – 323□ Podcast 7.1 – Chemical

Reactions□ #1, p. 324 and #7, p. 329□ Catalyst Demonstrations□ Word Equations

01/26/12

7.2 Classify reactions as one of four basic types of reaction, or as a special type of reaction (Combustion, Redox, or Acid-Base)

□ Read p. 330 – 341* Especially Figure 11.10

□ Podcast 7.2A – The Basic 4 Types □ Types of Reaction Demonstrations□ # 22, 23, 25, and 27 pg. 339 □ Podcast 7.2B – Special Types□ Redox Demos□ Oxidation-Reduction Movie□ Combustion Day Demos

01/30/12

7.3 Balance Chemical Equations.

□ Read p. 324 – 327 *Especially “Rules for Writing and Balancing Equations”

□ Podcast 7.3 Balancing Equations

□ Keeping Track of Atoms □ More Balancing Problems□ #3, 4 pg. 327. #5-6 pg. 328,

#8-12 pg. 329□ Chemical Equations –

Balancing Equations

02/01/12

7.4 Predict the Products of Chemical Reactions

□ #13-14 pg. 331; #15-16 pg. 332; #17 pg. 334; #18-19 pg. 335

□ Relative Reactivities of Metals Lab

□ Predicting Products of Reactions

02/03/12

7.5 Predict Solubility in Double Replacement Reactions.

□ Read p. 342 – 344□ 11.3 Reactions in Aqueous

Solution□ Copper-to-Copper Lab

(Composition Notebook)

02/07/12

7.6 Recognize Spectator Ions in Complete Ionic Equations

□ #30-35 pg. 344.□ Net Ionic Equations

02/09/12

Unit 7 Test □ Unit 7 Test Review□ Paper/pencil OR Moodle Version

of the Unit 7 Test with 75%

02/17/12

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Mastery and Self-Evaluation

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WORD EQUATIONS: Translate the following chemical sentences into balanced chemical equations. HINT* Pay attention to diatomic elements (Br I N Cl H O F)1. Two molecules of hydrogen plus one molecule of oxygen yields two molecules

of water.

2. One molecule of nitrogen plus three molecules of hydrogen yields two molecules of ammonia (NH3)

3. Two molecules of aluminum bromide plus three molecules of chlorine yields two molecules of aluminum chloride and three molecules of bromine.

4. One molecule of hydrochloric acid plus one molecule of sodium hydroxide yields one molecule of sodium chloride plus one molecule of water.

5. One atom of Iron plus one molecule of lead (II) sulfate react forming one molecule of iron (II) sulfate plus one atom of lead.

6. Two molecules of potassium chlorate when heated produces two molecules of potassium chloride plus three molecules of oxygen.

7. One molecule of sulfuric acid decomposes to form one molecule of sulfur trioxide gas plus one molecule of water.

8. One molecule sodium oxide combines with one molecule of water to make two molecules of sodium hydroxide.

9. Two molecules of potassium iodide reacts with one molecule of bromine forming two molecules of potassium bromide plus one molecule of iodine.

10. Two molecules of sodium phosphate reacts with three molecules of calcium nitrate to produce six molecules of sodium nitrate plus one molecule of calcium phosphate.

Classifying Chemical Reactions

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Classify the following reactions as synthesis, decomposition, single replacement, or double replacement.

1. 2KClO3 → 2KCl + 3O2

2. HCl + NaOH → NaCl + H2O3. Mg + 2HCl → MgCl2 + H2

4. 2Al + NiBr2 → 2AlBr3 + 3Ni5. 4Al + 3O2 → 2Al2O3

6. 2NaCl → 2Na + Cl2

7. CaCl2 + F2→ CaF2 + Cl2

8. AgNO3 + KCl → AgCl + KNO3

9. N2 + H2→ 2NH3

10. 2H2O2 → 2H2O + O2

11. (NH4)2SO4 + Ba(NO3)2 → BaSO4 + 2NH4NO3

12. 4C + 6H2 + O2 → 2C2H6O

Match each type of chemical reaction in Column II with its description in Column I. Write the letter of the correct reaction in the space provided.Column I_____12. A precipitate, water, or a gas forms when two ionic compounds are dissolved in a solution._____13. Two or more substances combine to form another substance._____14. One element replaces another in a compound._____15. A substance breaks down into two or more simpler substances.

Column IIa. synthesis reactionb. decomposition reactionc. single replacement

reactiond. double replacement

reaction

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An Introduction to Oxidation and ReductionOxidation and Reduction Movie Questions

Reduction1) Where did the term reduction come from?

2) What are two ways (or processes) to reduce metal ions?

3) Write the definition of reduction that makes the most sense to you.

Oxidation4) Name two examples of oxidation.

5) Write the definition of oxidation that makes the most sense to you.

Redox6) What does GER LEO stand for?

7) T/F Oxidation and reduction reactions take place together most of the time.

8) In the zinc and copper example, what was being reduced and what was being oxidized?

9) What is a reducing agent?

10) What happened with the silver tree? (wait for the copper wire demonstration before answering?

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Keeping Track of AtomsBefore looking at the equations, determine the number of atoms of each element in the following compounds.

1. CaCO3 = _____Ca, _____C, _____O2. Ba(NO3)2 = ____Ba, ____N, ____O 3. 4 Mg(OH)2 = ____Mg, ____O, ____H4. 3 H2 = ____H5. (NH4)2SO4 = ____N, ____H, ____S, ____O

For each of the following, show the number of each type of atom on each side of the reaction. This is called an ATOM INVENTORY. Decide if the chemical equation is balanced or not. You do NOT need to balance these equations!

6. 2 Na + 2 H2O 2 NaOH + H2

___________ Na ______________________ H ______________________ O ___________ Balanced? Yes_____

No_____7. 4 NH3 + 6NO 5 N2 + 6 H2O

___________ N ______________________ H ______________________ O ___________ Balanced? Yes_____

No_____8. NaCl + F2 NaF + Cl2

___________ Na ______________________ Cl ______________________ F ___________ Balanced? Yes_____

No_____9. 3 NaBr + H3PO4 2 HBr + Na3PO4

___________ Na ______________________ Br ______________________ H ______________________ P ______________________ O ___________ Balanced? Yes_____

No_____

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Same thing but now practice doing your own atom inventories. DON’T GET LAZY!

10. N2H4 + N2O4 3 N2 + 4 H2O

Balanced? Yes_____ No_____

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11. 4 Ag + 4 H2S + O2 2 Ag2S + 4 H2O

Balanced? Yes_____ No_____

12. 2 Bi + 3 F2 2 BiF3

Balanced? Yes_____ No_____

13. Al + Ni(NO3)2 Al(NO3)3 + Ni

Balanced? Yes_____ No_____

14. 3 NaBH4 + 4 BF3 2 B2H6 + 3 NaBF4

Balanced? Yes_____ No_____

15. 4 C3H5(NO3)3 6 N2 + O2 + 12 CO2 + 10 H2O

Balanced? Yes_____ No_____

16. Ca10F2(PO4)6 + 7 H2SO4 2 HF + 3 Ca(H2PO4)2 + 7 CaSO4

Balanced? Yes_____

No_____Now practice writing an equation using the given information. Determine if your

written equation is balanced or not.17. Natural gas contains methane (CH4), which burns with oxygen (O2) in

the air to produce () carbon dioxide (CO2) and water (H2O)Equation:

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Balanced? Yes_____ No_____

18. When hydrobromic acid (HBr) reacts with magnesium metal (Mg), hydrogen gas (H2) and magnesium bromide (MgBr2) is produced.Equation:

Balanced? Yes_____ No_____

More Balancing ProblemsBalance the following equations with the correct coefficients to balance them. Do an atom inventory before the equation is balanced to give you an idea of a good starting point. Then do an atom inventory after it has been balanced to check your answers.

1. ___C + ___S8 ___CS2

C C

S S

2. ___Na + ___O2 ___Na2O2

Na Na

O O

3. ___K + ___H2O ___KOH + ___H2

K K

H H

OH OH

4. ___KOH + ___HBr ___KBr + ___H2O

K K

OH OH

H H

Br Br

5. ___Al + ___Pb(NO3)2 ___Al(NO3)3 + ___Pb

Al Al

Pb Pb

NO3 NO3

6. __CH3CH2CH2CH3+___O2___CO2+ ___H2O

C C

H H

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O O

Continue balancing the following equations. Be sure to double check your answers to make sure the reactants equal the products.

7. ___N2 + ___H2 ___NH3

8. ___Cs + ___N2 ___Cs3N

9. ___HCl + ___NaOH ___NaCl + ___H2O

10. ___Cu + ___AgNO3 ___Cu(NO3)2 + ___Ag (hint: keep the polyatomic atom together)

11. __MnO2+___HCl___MnCl2+__Cl2+ __H2O

12. ___Cl2 + ___LiI ___LiCl + ___I2

13. ___Ca(OH)2 + ___HCl ___CaCl2 + ___H2O

14. ___CH4 + ___O2 ___CO2 + ___H2O

15. ___N2 + ___O2 ___N2O5

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16. ___KOH + ___H3PO4 ___K3PO4 + ___H2O

17. __Al(NO3)3+__H2SO4 __Al2(SO4)3+__HNO3

18. __Na2SO3+__HCl__NaCl+__H2O+__SO2

19. ___(NH4)2SO4 + ___KOH ___K2SO4 + ___NH3 + ___H2O

20. ___FeS2 + ___O2 ___Fe2O3 + ___SO2

Chemical Equations: B A L A N C I N G E Q U A T I O N S

1. __ZnS + __HCl __ZnCl2 + __H2S2. __HCl + __Cr __CrCl2 + __H2

3. __Al + __Fe3O4 __Al2O3 + __Fe4. __H2 + __Br2 __HBr5. __Na2S2O3 + __I2 __NaI + __Na2S4O6

6. __LaCl3 + __Na2CO3 __La2(CO3)3 + __NaCl7. __NH4Cl + __Ba(OH)2 __BaCl2 + __NH3 + __H2O8. __Ca(OH)2 + __H3PO4 __Ca3(PO4)2 + __H2O9. __La2(CO3)3 + __H2SO4 __La2(SO4)3 + __H2O + __CO2

10. __Na2O + __(NH4)2SO4 __Na2SO4 + __H2O + __NH3

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11. __C4H10 + __O2 __CO2 + __H2O12. __C7H6O2 + __O2 __CO2 + __H2O13. __P4O10 + __H2O __H3PO4

14. __FeS2 + __O2 __Fe2O3 + __SO2

15. __NH3 + __O2 __NO + __H2O

16. __Fe + __HCl __H2 + __FeCl2

17. __PbO2 + __HCl __H2O + __PbCl2 + __Cl2

18. __Fe2O3 + __H2SO4 __Fe2(SO4)3 + __H2O19. __NO2 + __H2O __NO + __HNO3

20. __C2H6S + __O2 __CO2 + __H2O + __SO2

Complete combustion:21. C6H14 22. C2H5OH23. C3H7OH24. C6H6

25. C17H35COOH

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Related Reactivities of Metals Lab

DDATAATA T TABLEABLEMetal Cu(NO3)2

Cu2+Mg(NO3)2

Mg2+Zn(NO3)2

Zn2+AgNO3

Ag+

CuMgZnAg

Analysis Questions1. Which metal reacted with the most solutions?

2. Which metal reacted with the fewest solutions?

3. With which of the solutions (of any) would you expect silver metal to react, if it were available to be tested? Fill your prediction in on the data table.

4. List the metals (including silver) in order, placing the most reactive metal first (the one reacting with the most solutions) and the least reactive metal last (the one reacting with the fewest solutions.

1) 3)2) 4)

5. Refer to your “metal activity series” list in questions #4. Write a brief explanation of why the outside surface of a penny is made of copper instead of zinc.

6. a. Which of the four metals mentioned in this lab activity might be an even better choice than copper for the outside of a penny? Why?

b. Why do you think that metal is not used for the coating of the outside of a penny?

7. Given your new knowledge about the relative chemical activities of these four metals:a. Which metal is most likely to be found in an uncombined or “free” state in

nature?

b. Which metal is least likely to be found chemically uncombined with other elements?

8. Reconsider the procedure for this lab.a. Would it have been possible to eliminate one or more of the metal-solution

combinations and still obtain all the information needed to create the chemical activity ratings for the metals?

b. If so, which combination(s) and why?

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Predicting Products of Reactions Based on Reaction Type

Work together with a partner to predict the products of the reactions given below. If the reaction occurs, complete the balanced equation. If it does not occur, write “NR” for “no reaction.”

PARTNER A

____________________

1. HCl + Mg→

2. H2SO4 + Zn→

3. MgCl2 + Al→

4. ZnCl2 + Al→

5. CaCl2 + Br2→

6. AlBr3 + F2→

PARTNER B

____________________

7. Na2SO4 + BaCl2→

8. HCl + AgNO3→

9. NH4Cl + Mg(OH)2→

10. NaOH + H3PO4→

11. Na2S + AlCl3→

12. Ca(NO3)2 + Ag2SO4→

Work together with a partner to predict the products of the reactions given below. If the reaction occurs, complete the balanced equation. If it does not occur, write “NR” for “no reaction.”

PARTNER A _________________

13. Mg(ClO3)2→

14. Na2CO3→

15. Na3PO4 + AlCl3→

16. Ba(NO3)2+ Na2SO4→

17. AlBr3 + Cl2→

18. Al2S3→

19. MgF2→

20. Na + N2→

21. Al + O2→

22. Li + H2O→

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PARTNER B __________________

23. MgCl2 elect .→

24. Ba(OH)2 + HCl→

25. Al(OH)3 + H2SO4 →

26. Na + HCl→

27. NaOH + Cu →

28. Zn + AlCl3→

29. Li2O →

30. K3N→

31. Rb + O2 →

32. Mg + N2→

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11.3 Reactions in Aqueous SolutionRead pages 342 – 344. Answer the following questions using complete sentences.1. What does the symbol (aq) represent?

2. What is a complete ionic equation? Give an example

3. When ions do not change on both sides of the equation what should you do?

4. Define a spectator ion

5. What is a net ionic equation? Give an example.

6. What is a precipitate?

7. What are the general rules for solubility of ionic compounds? (HINT: look at table 11.3)

8. Look at Table 11.3. Re-write these solubility rules into your own words.

9. Answer Questions 30 – 35 on page 344 on your own paper.

Steps for Solving Net Ionic Equations1. Determine for each particle if it is written as an ion or molecule2. For ions, write down the charge plus the number of ions determined from the

formula3. Write ionic equation for all substances4. Cancel out like terms

EXAMPLE:AgNO3 (aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)

1. Use your solubility rules to determine what will break into ions and what will remain as a compound. Rule number 4 says that chlorides are soluble except when paired with Silver, Lead, or Mercury

Ag+ + NO3

- + Na+ + Cl- AgCl (s) + Na+ + NO3

-

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2. Cancel out the spectator ions (the ones that don’t change on both sides)

Ag+ + Cl- AgCl (net ionic equation)

A Series of Copper ReactionsPLEASE complete the pre-lab in your lab notebook and get a stamp from your teacher BEFORE you begin this lab.

Purpose: In this experiment, you will perform a series of chemical reactions beginning with a weighed amount of copper metal. You will then recover the copper metal in the final reaction and determine the percent recovery. Since one of the basic laws of chemistry is the Law of Conservations of Mass, you should end up with the same weight of copper as you started with.Reactions:Cu + Cu(NO3)2 → Cu(OH)2 → CuO → CuCl2 → CuProcedure:

A. Copper nitrate from Copper Weight approximately 1 gram of metallic copper to 0.01 g into a 150 ml beaker and record the mass of the copper. Place the beaker on a ring stand under the hood. CAREFULLY AND SLOWLY add 10 ml of concentrated nitric acid (HNO3). Brown nitrogen dioxide gas (NO2) will be released, leaving a blue solution of copper nitrate. The brown NO2 is HAZARDOUS. If the copper does not completely dissolve, slight warming and additional acid may be required. Cool the solution to room temperature. The balanced reaction is:

Cu + 4 HNO3 → Cu (NO3)2 + 2 NO2 + 2 H2O

B. Preparation of Copper Hydroxide Dilute the cooled copper nitrate solution from Part A with 50ml of water. Cautiously add about 30ml of 6 M NaOH to produce a precipitate of copper hydroxide. The reaction is complete when no further precipitate of copper hydroxide is formed as drops of 6 M NaOH solution are added to the surface of the liquid in the beaker. The solution should test basic with litmus paper. (Use a stirring rod to transfer a small drop of solution to the litmus paper. Base turns red litmus to blue.) Add more sodium hydroxide solution if necessary. Write the balanced equation for this reaction.

C. Preparation of Copper Hydroxide Bring the solution of copper hydroxide up to a total volume of about 100ml with distilled water. (The volume may already exceed 100ml.) Gently simmer the solution for about five minutes with constant stirring. A black precipitate of

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copper hydroxide will form as the copper hydroxide decomposes. If the precipitate does not settle, heat a bit longer. Allow the precipitate to settle and carefully decant the clear liquid being careful to lose as little of the precipitate as possible. Add about 100ml hot distilled water and repeat decantation. Write a balanced chemical reaction for this reaction.

D. Preparation of Copper Chloride Dissolve the copper by adding 15ml of 6 M hydrochloric acid (HCl) to the precipitate. Additional 1 ml amounts of HCl may be required to dissolve all the precipitate. Write a balanced chemical equation describing this process.

E. Recovery of Copper Metal Add at least 1 gram of zinc foil to the solution to replace the copper. Stir the solution to increase the reaction rate. When all the copper has been replaced, the solution will be colorless. Remove the remaining zinc foil and scrape any copper film off into the beaker. Recover the copper metal by decanting off the liquid. Wash the copper metal with 50 ml of distilled water, stir, allow to settle and decant. Repeat with another 50 ml of water. Transfer the copper to a dry, weighed, evaporating dish using as little water as possible. Allow the copper to settle and decant most of the water. Dry the copper completely in a drying oven at 80˚C Weigh the dish and dry copper metal. Write a balanced chemical equation for this final reaction and calculate the percent of copper recovered.

Safety Alerts1. All solutions contain nitric acid which is very corrosive to skin and eyes. Wash

spills off yourself with LOTS of water. Neutralize spills on the lab table with baking soda.

2. Solutions are toxic; so wash your hands before you leave the lab.3. Sodium hydroxide is a strong base and is hazardous to skin and eyes. If you get

any on yourself, wash off with large amounts of water. Neutralize spills on the counter with vinegar.

4. You will be using solutions with high concentrations of sulfuric and nitric acids and sodium hydroxide, both of which are highly damaging to skin and eyes. Be careful when handling them. If you spill any on yourself, wash off with lots of water. Neutralize sulfuric acid spills on the counter with baking soda, and neutralize potassium hydroxide spills with vinegar (dilute acetic acid).

5. When zinc dissolves in sodium hydroxide solution, hydrogen gas is produced. Make sure that no flames are present. This step should be performed in a fume hood.

6. Wear Chemical Splash Goggles and a Chemical-Resistant Apron.

Prelab Questions: Please draw safety symbols next to each step in your procedure to summarize that hazards to watch for as you complete each part of the lab. For a listing of safety symbols, please refer p. R80 in the back of your textbook. Feel free to design your own safety icon as well.

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Post-Lab Questions:1. Write the word equation for each of the 5 reactions.2. Write a balanced chemical equation for each of the 5 reactions.3. Write a net ionic equation for each of the 5 reactions.4. Identify the type of reaction for each of the 5 reactions

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Chemistry Lab Report RubricA Series of Copper Reactions

Name: _______________________________________

Table of Contents

Points Earned

Points

Possible

Includes the title, page numbers, and date of experiment 2Title

Capitalized appropriately, relates to the experiments, underlined at the top of the lab report 1

Problem Statement Testable and clearly stated 2

Variables Independent, Dependent, Control, at least 3 constants 6

Hypothesis States what you are doing, what you predict will happen, and

why you think that will happen. If…Then…Because 2Materials

A list of all materials used in the experiment 1Procedure

Write a complete, DETAILED procedure. 3Data

Organized table that shows the data you have collected during the experiment

- Include an appropriate title- Clearly organize and label data columns and rows- Units are clearly identified- Accuracy of data is appropriate to measuring equipment or

instruments- Data from multiple trials is clearly shown- Data and table lines are neat and presentable (USE A

RULER)

3

Analysis Calculate Percent Yield for your own trial and for the class average 2Questions:

1. Word Equations (5)2. Balanced Chemical Equations (5)3. Net Ionic Equations (5)4. Identify Reaction Type (5)

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Conclusion Written in paragraph form (minimum of 3 paragraphs) 1 Support or refute your hypothesis. Give reasons why. USE

YOUR DATA! 5 Discuss any EXPERIMENTAL error you may have had in the

experiment. 4 Discuss how to change the design to fix the errors. What further

questions or investigations does this lead to? 4Discussion/Reflection

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Discuss what you learned from this experiment and how it relates to what we are learning in class (Law of Conservation of Mass, Types of Reactions, Balancing Equations, Net Ionic Equations, etc) and applications in the real world (mining, medicine, technology, etc).

4

Total Points 60

Net Ionic Equation WorksheetWrite balanced net ionic equations for each of the following reactions. Assume all reactions occur in aqueous solution. 1. NaCl(aq) + Pb(NO3)2(aq) PbCl2(s) + NaNO3(aq)

2. Na2CO3(aq) + FeCl2(aq) FeCO3(s) + NaCl(aq)

3. Mg(OH)2(aq) + HCl(aq) MgCl2(aq) + H2O(l)

4. K2(C2O4)(aq) + CaCl2(aq) KCl(aq) + Ca(C2O4)(s)

5. (NH4)3PO4(aq) + Zn(NO3)2(aq) NH4NO3( ) + Zn3(PO4)2(

)

6. LiOH(aq) + VCl3(aq) LiCl( ) + V(OH)3( )

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7. Na2CO3(aq) + HCl(aq) NaCl( ) + CO2( ) + H2O( )

8. Mg(NO3)2(aq) + Na2CrO4(aq) NaNO3( ) + MgCrO4( )

9. FeCl3(aq) + Mg(s) MgCl2(aq) + Fe(s)

10 Zr(OH)4(s) + HNO3(aq) Zr(NO3)4( ) + H2O( )

11. Na2SO3(s) + HCl(aq) NaCl( ) + H2O( ) +

SO2(g)

12. BaBr2(aq) + Na2SO4(aq)

13. AgNO3(aq) + MgI2(aq)

14. (NH4)2C2O4(aq) + Al(ClO4)3(aq)

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15. Ni(NO3)2(aq) + NaOH(aq)

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Unit 7 – StoichiometryTest Review

1. Define AND KNOW HOW TO APPLY the following words and terms:a. Law of Conservation of Mass –

b. Chemical reaction –

c. Catalyst –

d. Coefficients –

e. Subscripts –

f. Balanced equation –

g. Skeleton equation –

h. Word equation –

i. Net ionic equation –

j. Synthesis reaction –

k. Decomposition reaction –

l. Single replacement reaction –

m. Double replacement reaction –

n. Combustion reaction –

o. Acid/Base reaction –

2. What do (s), (l), (aq), and (g) stand for in a chemical reaction?

3. The activity series of metals is utilized to predict the products for which type of reaction?

4. Looking at the solubility chart and rules, which salts will form a precipitate?

5. Write the net ionic equation for Pb(NO3)2 (aq) + NH4Cl (aq) PbCl2 (s) + NH4NO3 (aq).

6. Predict the products for C2H6 + O2

7. Predict the products for Ca + Mg(NO3)2

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8. Predict the products for H2SO4 + NaOH

9. Using the equation CS2 + O2 CO2 + SO2 a. Balance the equation. What type of reaction is this?

For those of you paying attention, you may make a 3x5 hand written note card for the test.

10. Using the equation Sn + HF SnF2 + H2:a. Balance the equation. What type of reaction is this?

This is a blast from the past (Unit 6) but you will have a section of the test VERY similar to this.It was found that a compound contains 22.1 % Al, 25.4 % P, and 52.5 % O

1. Determine the Empirical Formula of the Compound.

2. What is the name of this compound?

3. This compound is now reacting with Barium Chloride (BaCl2).a. Write and Balance the Chemical equation for this reaction.

b. 5.25g of your compound reacts with excess Barium Chloride. Calculate the number of molecules for the precipitate formed in this reaction.

4. In a recent experiment, you obtained 7.43 x 1021 molecules. According to your control, you should have obtained 8.00 x 1021 molecules. Determine your percent yield.

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Unit 7: Chemical Reactions TestEvaluating Your Test Results

Please have this page with you when you ask your teacher to type in the password for your test. You may write your scratchwork for the test on the back of this page.

For each question, decide whether you feel confident in your answer or are unsure about it and mark the corresponding box.

After your test has been graded, review each question and decide “What helped the most?” for questions you answered correctly and “Error Category” for questions you got wrong. Test corrections must be done before attempting a retake.

Problem #

Learning Target

Confident Unsure RightWhat helped the most?

WrongError Category

1 7.12 7.43 7.14 7.25 7.36 7.37 7.38 7.49 7.610 Unit 7

(LAB)Analyzing My Results: After your test has been corrected, identify which problems you got right and which you got wrong by putting X's in the "Right" and "Wrong" columns. Of the problems you got wrong, decide which ones were due to simple mistakes and mark the "Simple Mistake" column. For all of the remaining wrong answers, mark the "Don't Get It" column.Learning Targets #

Description of Learning Target

7.1 Identify the parts of a chemical equation.7.2 Classify reactions as one of four basic types of a special

type of reaction.7.3 Balance chemical equations.7.4 Predict the products of chemical reactions. 7.5 Predict solubility in double replacement reactions7.6 Recognize spectator ions in complete ionic equations.

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What Helped the MostFor each question you answered correctly: Why of the following do you think helped you to answer the question correctly? Include all the apply

a. Previewed the assigned reading material before coming to class

b. Attended all classesc. Reviewed last class’s notes before the

next classd. Rewrote the notese. Integrated the class notes with the

text bookf. Organized basic concepts using

charts, lists, outlines, tables, graphic organizers, etc

g. Self-tested on material to be covered on the exam

h. Practiced explaining or “teaching” concepts to a friend/ studied with friends

i. Got extra help from the instructor or tutoring session

j. Studied material regularly instead of waiting til the last minute or not studying at all

k. Ate healthy prior to the examl. Got plenty of sleep the night before

the exam

Error CategoriesType One Error: Known as the “D’oh!”These types of errors are usually followed by statements like “I can’t believe I clicked A when I wrote B on my paper!” “I don’t know why I marked C when I knew that D was the answer!” This type of error can also be followed by “I knew the answer, but I changed it at the last minute.” Usually, it is just a matter of slowing down when reading and responding to the test item.Type Two Error: Something about the questionThis category error is followed by a statement like, “I understood the concept of the question, but something about the way the question was worded confused me.” Usually when answering higher level questions, the result is not fully understood by the student who may have superficial study skills or only memorized notes. Sometimes though, the question is just not worded fairly by the teacher and it is misleading.Type Three Error: I don’t know itThis particular concept wasn’t studied well enough or was not present when the material was covered, is not reading the textbook, or didn’t pay enough attention in class to understand the concepts. Spend more time working in class and review on a daily basis rather than cramming for the test the night before (or not at all).

Test CorrectionsFor each question you missed on the test:

1. Restate the question and the correct answer.2. List the incorrect answers and explain why they cannot be correct (if multiple choice)3. Explain why you missed the question

a. Misread the question or didn’t understand what it was askingb. Used incorrect logicc. Didn’t know enough about it to answer correctl

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