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Chemical Reactions Academic Chemistry

Summary: Chemical reactions require the use of the law of conservation of mass to write, predict, balance,

understand, and differentiate among oxidation-reduction (synthesis, decomposition, and single-replacement), precipitation (double-replacement), and acid-base reactions (neutralization). Objectives: Use the law of conservation of mass to write and balance chemical equations

Understand and differentiate among acid-base reactions and oxidation-reduction reactions

Vocabulary: atoms, molecules, compounds, acid, base, polyatomic ions, oxidation number, coefficient,

subscript, catalyst, reactant, product, aqueous, precipitate, synthesis, decomposition, single-replacement, double-replacement, oxidation-reduction, combustion, neutralization, endothermic, exothermic

Memorize: Provided: Periodic table

CHECKLIST: How to be successful in OTHS Academic Chemistry

Pay attention and take notes in class Ask questions in class on material that is not clear Work every page in the practice packet for the unit Check answers to the practice packet online at http://othschem.weebly.com/ Come to tutorials with any chemistry teacher Do the online homework and check solutions once they become available Always do the practice test for every test & ask good questions on review day Keep up with the calendar for the class/be aware of approaching quizzes, tests, & other deadlines Use videos posted on website as a quick and convenient tutorial Read the chapter in the book

Name___________________ Per. _____

Balancing Equations Worksheet #1 1. ___ C2H4 + ___ O2 ___ CO2 + ___ H2O 2. ___ AlBr3 + ___ Cl2 ___ AlCl3 + ___ Br2 3. ___ Br2 + ___ FeI3 ___ FeBr3 + ___ I2 4. ___ BF3 + ___ H2O ___ B2O3 + ___ HF 5. ___ P4O10 + ___ KOH ___ K3PO4 + ___ H2O 6. ___ Pb(NO3)2 ___ PbO + ___ NO2 + ___ O2 7. ___ SnCl4 + ___ Na ___ NaCl + ___ Sn 8. ___ C3H8 + ___ O2 ___ CO2 + ___ H2O 9. ___ Ca(OH)2 + ___ HNO3 ___ Ca(NO3)2 + ___ H2O 10. ___ Fe + ___ H2O ___ Fe3O4 + ___ H2 11. ___ HCl + ___ BaCO3 ___ BaCl2 + ___ H2O + ___ CO2 12. ___ PbCO3 + ___ HNO3 ___ Pb(NO3)2 + ___ H2O + ___ CO2 13. ___ P4O10 + ___ H2O ___ H3PO4 14. ___ XeF2 + ___ H2O ___ Xe + ___ O2 + ___ HF

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Name________________________ Per____

Balancing Equations Worksheet #2

1. ___Pb(NO3)2 + ___K2CrO4 ___PbCrO4 + ___KNO3 2. ___MnO2 + ___HCl ___MnCl2 + ___H2O + ___Cl2 3. ___K + ___H2O ___KOH + ___H2 4. ___BaO2 ___BaO + ___O2 5. ___Zn(OH)2 + ___H3PO4 ___Zn3(PO4)2 + ___H2O 6. ___Fe(NO3)3 + ___LiOH ___Fe(OH)3 + ___LiNO3 7. ___CS2 + ___Cl2 ___CCl4 + ___S2Cl2

8. ___CH4 + ___Br2 ___CH3Br + ___HBr 9. ___Ba(CN)2 + ___H2SO4 ___BaSO4 + ___HCN 10. ___(NH4)2Cr2O7 ___Cr2O3 + ___H2O + ___N2 11. ___Al + ___CuSO4 ___Al2(SO4)3 + ___Cu 12. ___F2 + ___KCl ___KF + ___Cl2 13. ___BaCl2 + ___H3PO4 ___Ba3(PO4)2 + ___HCl 14. ___CdCl2 + ___H2S ___CdS + ___HCl

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Name______________________________ Per. _____

Answer Sheet: Equation Balancing Card Game

1. ___ Al2C6 + ___ H2O → ___ Al(OH)3 + ___ C2H2 2. ___ Be2C + ___ H2O → ___ Be(OH)2 + ___ CH4 3. ___ NH3 + ___ O2 → ___ NO + ___ H2O 4. ___ BN + ___ F2 → ___ BF3 + ___ N2 5. ___ Sn + ___ O2 → ___ SnO 6. ___ H2 + ___ Cl2 → ___ HCl 7. ___ V2O5 + ___ Ca → ___ CaO + ___ V 8. ___ Fe3O4 + ___ H2 → ___ Fe + ___ H2O 9. ___ C + ___ SO2 → ___ CO + ___ CS2 10. ___ Na + ___ H2O → ___ NaOH + ___ H2 11. ___ NH3 + ___ O2 → ___ N2H4 + ___ H2O 12. ___ LiH + ___ AlCl3 → ___ LiAlH4 + ___ LiCl 13. ___ HBrO3 + ___ HBr → ___ H2O + ___ Br2 14. ___ N2 + ___ H2 → ___ NH3 15. ___ K2SO4 + ___ BaCl2 → ___ KCl + ___ BaSO4 16. ___ CaC2 + ___ O2 → ___ Ca + ___ CO2

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Name________________________________ Per. ____

Formula Writing/Equation Writing Practice Worksheet

1. Classify the compound as Ionic, Molecular, Acid, or Base. Write the formula for the compound. Classify Formula

a. aluminum hydroxide ______________ ___________________

b. sodium oxide ______________ ___________________

c. hydrofluoric acid ______________ ___________________

d. potassium phosphate ______________ ___________________

e. copper (I) sulfate ______________ ___________________

f. phosphorus pentabromide ______________ ___________________

2. Equation writing: Convert all chemical names to formulas and write a balanced equation. a. Solid barium reacts with oxygen gas to produce solid barium oxide.

b. Solid iron (III) oxide decomposes to form metallic iron (solid) and oxygen gas.

c. Solid iron and aqueous copper (II) sulfate react to form solid copper and aqueous iron (III) sulfate.

d. Aqueous copper (II) chloride and aqueous lead (IV) nitrate react to form aqueous copper (II) nitrate and solid lead (IV) chloride.

e. Metallic magnesium (solid) reacts with aqueous silver nitrate to form aqueous magnesium nitrate and metallic (solid) silver.

f. Aqueous sulfuric acid reacts with aqueous potassium hydroxide to form aqueous potassium sulfate and water.

g. Chlorine gas reacts with aqueous potassium bromide to form aqueous potassium chloride and liquid bromine.

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Directions: Write an example of an actual chemical reaction fitting each of the following types of reactions.

1. Synthesis: Example __________________________________________

2. Decomposition: Example __________________________________________

3. Single Replacement:

Example _____________________________________ Example _____________________________________

(Metal) (Halogen)

4. Double Replacement: Example __________________________________________

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Name Class Date

Types of Chemical Reactions

Write the type chemical reaction on the line—synthesis (combination), decomposition, combustion, single

replacement, or double replacement. Then, balance the equations using the lowest possible integers. For

questions 21 and 22, predict the products before balancing.

1. ____ Zn + ____ H2SO4 → ____ ZnSO4 + ____ H2

2. ____ Na + ____ Br2 → ____ NaBr

3. ____ HCl + ____ NaOH → ____ NaCl + ____ H2O

4. ____ H2O2 → ____ H2O + ____ O2

5. ____ Cu + ____ AgNO3 → ____ Ag + ____ Cu(NO3)2

6. ____ C2H5OH + ____ O2 → ____ CO2 + ____ H2O

7. ____ KOH → ____ K2O + ____ H2O

8. ____ Mg + ____ H2O → ____ Mg(OH)2 + ____ H2

9. ____ AlCl3 → ____ Al + ____ Cl2

10. ____ H2 + ____ O2 → ____ H2O

11. ____ KI + ____ Pb(NO3)2 → ____ PbI2 + ____ KNO3

12. ____ P + ____ O2 → ____ P2O5

13. ____ Ca(ClO3)2 → ____ CaCl2 + ____ O2

14. ____ Fe2O3 + ____ C → ____ CO + ____ Fe

15. ____ Fe + ____ O2 → ____ Fe2O3

16. ____ Ca + ____ AlCl3 → ____ CaCl2 + ____ Al

17. ____ N2 + ____ H2 → ____ NH3

18. ____ Ba(NO3)2 + ____ Na2SO4 → ____ BaSO4 + ____ NaNO3

19. ____ C3H8 + ____ O2 → ____ CO2 + ____ H2O

20. ____ HgO → ____ Hg + ____ O2

21. ____ Na + ____ Cl2 →

22. ____ CH4 + ____ O2 →

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Name___________________________________ Per. _____

Practice Worksheet: Predicting Products Predict the products of the following equations and then balance

them.

I.

Synthesis

1. ___H2 + ___O2 2. ___Fe + ___S (use Fe+3) 3. ___Al + ___Cl2 4. ___Pb + ___O2 (use Pb2+) 5. ___ Mg + ___ Br2 II.

Decomposition

6. ___Al2S3 7. ___CaO 8. ___ LiF 9. ___ PbS2 10. ___ NaCl III. Single Replacement

Make sure to check the activity series; if the reaction does not occur, write NR for “no reaction.”

11. ___K + ___CuCl2 12. ___Na + ___Pb(NO3)2 13. ___Cl2 + ___KF 14. ___Mg + ___Li2CO3 15. ___Br2 + ___NaI (continued)

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IV.

Double Replacement

16. ___AlCl3 + ___NaOH 17. ___AgNO3 + ___KCl 18. ___Ba(NO3)2 + ___Li2SO4 The next 2 reactions are a special type of double replacement called neutralization. This occurs when an acid and a base react to form a salt + water. 19. ___ HCl + ___ KOH 20. ___ H2SO4 + ___ Ca(OH)2 V.

Combustion

21. ___CH4 + ___O2 22. ___C11H24 + ___O2 23. ___C12H22O11 + ___O2 24. ___C9H20 + ___O2 25. ___C2H6 + ___O2

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Name___________________________ Period ____ Date______

Oxidation Number Practice Based on the oxidation numbers known for the other element(s), determine the oxidation number of the underlined element. 1. Na2SO4 ______ 16. CO2 ______ 2. CaO ______ 17. CaCO3 ______ 3. K2CrO4 ______ 18. KClO4 ______ 4. Cr2O3 ______ 19. SO3 ______ 5. KIO3 ______ 20. Cu2O ______ 6. H2O ______ 21. KClO3 ______ 7. SO4

2- ______ 22. Cl2 ______

8. H3PO4 ______ 23. H2SO3 ______ 9. LiMnO4 ______ 24. Al 3+ ______ 10. Ag ______ 25. SO2 ______ 11. K2Cr2O7 ______ 26. H2SO4 ______ 12. HNO3 ______ 27. MnO2 ______ 13. ClO3

- ______ 28. NO3- ______

14. S 2- ______ 29. NaCl ______

15. CO ______ 30. Fe2O3 ______

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REDOX PRACTICE

First, indicate the type of chemical reaction (synthesis, decomposition, single replacement, or double replacement). Then, label the oxidation numbers for each element in the reaction on both the reactants and products side. Last, identify which element has been oxidized and which has been reduced.

1. 2Ag + S Ag2S Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

2. 2Na + FeCl2 2NaCl + Fe Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

3. 2AlCl3 2Al + 3Cl2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

4. Fe2O3 + 6HCl 2FeCl3 + 3H2O Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

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5. 3Mg + N2 Mg3N2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

6. 2NaBr +Cl2 2NaCl + Br2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

7. 2HgO 2Hg + O2 Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

8. 3Ca + 2AlCl3 3CaCl2 + 2Al Circle Type: S/D/SR/DR Element Ox.# Reactants side Ox.# Products side Lose/Gain e- Oxidized/Reduced

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