Unit 9: Chemical Equations and Reactions Chapters 8 and 19 Name Block Unit Learning Targets (L.T.): By the end of the unit, students will be able to: Chapter 8: 1. Correctly write and balance chemical reactions 2. Identify if a chemical reaction is occurring and the type of reaction taking place. 3. Use solubility rules to predict products in chemical reactions 4. Write balanced oxidation-reduction reaction equations. Vocabulary: single replacement reactions synthesis reactions combustion reactions double replacement reactions decomposition reactions precipitate subscripts reactant product Topic and Learning Targets Activities/Labs/In-class Work Homework* Balancing Equations Chemical Reactions Predicting Products Redox Reactions Notes/Discussion: Balancing Equations Practice: Balancing Equations Notes/Discussion: Types of Chemical Reactions Lab: Flaming Bubbles Lab Notes/Discussion: Predicting Products and Solubility Rules Practice: Predicting Products Quiz: Balancing Equations and Reaction Types Notes/Discussion: Redox Reactions Review Packet Part 1 Review Packet Part 2 Review Packet Part 3 Review Packet Part 4 Redox Reactions Practice: Redox Reactions Study for Test Unit Test Unit Test TBD Please note Additional homework may be added as necessary. Any changes discussed in class and written on the board should be added to homework listed above by the student and will be due as discussed in class.
Part 1: Balancing Equations 1. Explain the Law of Conservation of Mass and how it applies to balancing equations. 2. How can you determine if a chemical equation has occurred? 3. What are substances found on the left side of the equation called? 4. What are substances found on the right side of the equation called? 5. What does the arrow signify? 6. What are the symbols for different states of matter? 7. To balance an equation, what numbers do you change? 8. What is the best way to start balancing a chemical equation? In Class Examples: 1. H 2 + Cl 2 HCl 2. Mg + O 2 MgO 3. CH 4 + O 2 CO 2 + H 2 O 4. BaCl 2 + Al 2 (SO 4 ) 3 BaSO 4 + AlCl 3 5. H 2 SO 4 + NaOH Na 2 SO 4 + H 2 O 6. C 7 H 16 + O 2 CO 2 + H 2 O
Independent Practice/Homework: 1. HgO Hg + O 2 2. N 2 + H 2 NH 3 3. KMnO 4 K 2 O + MnO + O 2 4. Fe + HCl FeCl 2 + H 2 5. H 2 O 2 H 2 O + O 2 6. Al(OH) 3 + H 2 SO 4 Al 2 (SO 4 ) 3 + H 2 O 7. NaClO 3 NaCl + O2 8. BaCl 2 + K 3 PO 4 Ba 3 (PO 4 ) 2 + KCl 9. CO 2 + H 2 O C 6 H 12 O 6 + O 2 10. Na 2 O 2 + H 2 O NaOH + O 2 11. Al 2 (SO 4 ) 3 + Ca(OH) 2 Al(OH) 3 + CaSO 4 12. BaO + H 2 SO 4 BaSO 4 + H2O 13. NaOH + Cl 2 NaCl + NaClO + H 2 O
14. Na 2 O 2 + H 2 SO 4 Na 2 SO 4 + H 2 O 2 15. SiCl 4 + H 2 O H 4 SiO 4 + HCl 16. H 2 SO 4 + HI H 2 S + I 2 + H 2 O Balancing Word Equations In class examples: 1. potassium chlorate potassium chloride + oxygen 2. silver nitrate + sodium chloride silver chloride + sodium nitrate 3. When solid copper reacts with aqueous silver nitrate, the products are aqueous copper (II) nitrate and silver metal. Independent Practice/Homework: (Don t forget diatomic molecules and to balance!) 1. magnesium + oxygen magnesium oxide 2. sodium + water sodium hydroxide + hydrogen 3. potassium + chlorine potassium chloride 4. potassium hydroxide + sulfuric acid potassium sulfate + water 5. sulfuric acid + iron iron (II) sulfate + hydrogen
6. zinc + hydrogen chloride zinc (II) chloride + hydrogen 7. When isopropanol (C 3 H 8 O) burns in oxygen, carbon dioxide, water, and heat are produced. (Be sure to use symbols to indicate state) 8. When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. (Be sure to use symbols to indicate state) 9. When dissolved beryllium chloride reacts with dissolved silver nitrate in water, aqueous beryllium nitrate and silver chloride powder are made. (Be sure to use symbols to indicate state) Part 2: Types of Reactions Match the following reaction types to their general equation: Column A Column B 1. AB A + B A) Single Displacement 2. A + B AB B) Double Displacement 3. Hydrocarbon + O 2 CO 2 + H 2 O C) Synthesis 4. AX + BY AY + BX D) Decomposition 5. A + BX AX + B E) Combustion 6. Does the following equation represent a combustion reaction, a synthesis reaction, or both? Explain your answer. 2 C + O 2 2CO 2 + energy 7. Why is it incorrect to say that a compound is broken down into its component elements in a decomposition reaction?
8. When soap is added to hard water, solid soap scum forms. When water is added to baking powder, carbon dioxide bubbles form. When lemon juice is added to household ammonia solution, water is one of the products. Tell how you know a double-displacement reaction has occurred in each case. Write in the type of reaction for each of the following scenarios: 9. Aluminum lawn furniture becomes coated with aluminum oxide outside. 10. Chlorine gas is bubbled through calcium bromide solution. The solution turns brown. 11. Propane is a common household fuel. When burned, water and carbon dioxide form. 12. Steel wool burns, forming an iron oxide. 13. When an electric current is passed through molten potassium bromide, potassium and bromine form. 14. When solutions of sodium iodide and lead (II) nitrate are combined, a yellow solid forms. 15. Define synthesis reaction Write 3 examples of synthesis reactions found earlier in the packet. 16. Define decomposition reaction Write 3 more decomposition reactions found earlier in the packet. 17. Define single-replacement reaction a. Using variables, write the 2 ways a general single-replacement reaction can be written. b. Write 3 examples single-replacement reactions found earlier in the packet. Identify which element is being 'replaced.'
18. Define double-replacement reaction c. Write 3 examples of double replacement reactions found earlier in the packet. 19. Define combustion reaction d. What element will always be a reactant in a combustion reaction? e. What compounds will always be products in a combustion reaction containing carbon compounds as one of the reactants? (though not always products in all combustion reactions) d. Write one example of a combustion reaction found earlier in the packet. Identifying the Reaction Determine the type of chemical reaction. Choose from combustion, synthesis, decomposition, singlereplacement or double replacement. 20. Na 3 PO 4 + KOH ----> 3NaOH + K 3 PO 4 21. MgCl 2 + Li 2 CO 3 ----> MgCO 3 + 2LiCl 22. C 6 H 12 + 9O 2 ----> 6 CO 2 + 6 H 2 O 23. Pb + FeSO 4 ----> PbSO 4 + Fe 24. P 4 + 3 O 2 ----> 2 P 2 O 3 25. 2 NO 2 O 2 + N 2
26. Balance the following equations and indicate the type of reaction taking place: A) NaBr + H 3 PO 4 Na 3 PO 4 + HBr B) Ca(OH) 2 + Al 2 (SO 4 ) 3 CaSO 4 + Al(OH) 3 C) Mg + Fe 2 O 3 Fe + MgO D) C 2 H 4 + O 2 CO 2 + H 2 O E) PbSO 4 PbSO 3 + O 2 F) NH 3 + I 2 N 2 I 6 + H 2 G) H 2 O + SO 3 H 2 SO 4 H) H 2 SO 4 + NH 4 OH H 2 O + (NH 4 ) 2 SO 4 Part 3: Predict the Products Determine if the following single replacement reactions occur,write correct formulas for the products in the reactions that do occur, and balance. Write NR for reactions that do not occur. (activity series: pg 286) 1) Al + Pb(NO 3 ) 2 ---> 2) Cl 2 + NaI ---> 3) Al + CuCl 2 ---> 4) Au + HCl ---> 4) Br 2 + CaI 2 ---> 5) Mg + HCl ---> 6) Zn + H 2 SO 4 ---> 7) Zn + KI --->
Write correct formulas for the products in these double replacement reactions and balance. Assume all have an insoluble product. 1) Ca(OH) 2 + H 3 PO 4 ---> 2) K 2 CO 3 + BaCl 2 ---> 3) Cd 3 (PO 4 ) 2 + (NH 4 ) 2 S ---> 4) Co(OH) 3 + HNO 3 ---> 5) Al(OH) 3 + HC 2 H 3 O 2 ---> 6) Al 2 (SO 4 ) 3 + Ca 3 (PO 4 ) 2 ---> Practice Problems: Predict if the following substances are likely to be soluble or insoluble in water using the solubility rules 1. aluminum nitrate 2. magnesium chloride 3. rubidium sulfate 4. nickel (II) hydroxide 5. lead (II) sulfide 6. magnesium hydroxide 7. iron (III) phosphate 8. calcium carbonate Predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. Write no reaction if no precipitate is likely 1. FeCl 3 and H 3 PO 4 2. Ba(NO 3 ) 3 and Na 2 SO 4 3. KCl and FeSO 4 4. Pb(NO 3 ) 2 and HCl 5. Ca(NO 3 ) 2 and NaCl 6. (NH 4 ) 2 S and CuCl 2 Part 4: Redox Reactions: 1. What is a redox or oxidation-reduction reaction?
2. What is an oxidation? How can you tell that a substance has been oxidized? 3. What is a reduction? How can you tell that a substance has been reduced? 4. What is a half-reaction? Solve the following redox reactions in acids: 5. MnO 4 - + Fe 2+ Mn 2+ + Fe 3+ 6. Cu + NO 3 - Cu 2+ + NO (g) 7. Pb + PbO 2 + SO 4 2- PbSO 4 8. Fe(CN) 6-4 + MnO 4 - Mn 2+ + Fe 3+ + CO 2 + NO 3 - Solve the following redox reaction in bases: 9. CrI 3 + Cl 2 CrO 4 2- + IO 4 - + Cl - 10. Fe(OH) 2 + H 2 O 2 Fe(OH) - 11. Cr(OH) 3 + OCl - + OH - CrO 4 2- + Cl - + H 2 O