CHEMISTRY-CP, PERIOD 6
CHAPTER 11—CHEMICAL REACTIONS AND EQUATIONS
DAILY PLANNER
DAY
2
CLASSWORK
HOMEWORK
Introduction to Reactions Activity (5 Pts)
HW1: Worksheet A
What is a chemical reaction?
Word Equations
Formula Equations
3
Vocabulary Quiz (20 Points)
HW2: Worksheet B
Exothermic/Endothermic
Balancing Equations
4
Daily Quiz
HW3: Worksheet C
Synthesis/Decomposition/Combustion Reactions
5
Daily Quiz
HW4: Worksheet D
Single Replacement Reactions
6
Daily Quiz
HW5: Worksheet E
Single Replacement/Activity Series Lab (20 Points)
Double-Replacement Reactions
7
Daily Quiz
HW6: Worksheet F
Net Ionic Equations
8
Double Replacement Reactions Lab (30 Points)
Study for Chapter Test
Finish Daily Quiz (25 Points)
Homework & Extra Credit Due (50 Point +)
Chapter Review Game
9
10
Review Chapter Material
Chapter 11 Test (100 Points)
Study for Chapter Test
Finish Today’s Lab
Dec. 22
Homework Grades:
A(50/50) = 6/6 Homeworks Complete
B (45/50) = 5/6 Homeworks Complete
C (40/50) = 4/5 Homeworks Complete
D (35/50) = 3.5/5 Homeworks Complete
E (30/50) = 3/6 Homeworks Complete
F (0/50) = Less than 3/6 Homeworks Complete
Extra Credit:
5 Points: Worksheet G--Balancing Review
6 Points: Text p. 351 #1-12
7 Points: Worksheet H—Midterm Review
7 Points: Create a poster illustrating the following:
1) The 3 things necessary for a fire to burn
2) What the letters A, B, C, and D refer to in classifying fires
3) The difference between “combustible” and “flammable”
4) 2 methods of combating a fire and why it is an effective method
Top Pair for Chapter 10
Alyssa Guthrie and Haley Warner
Total Possible Points This Chapter: 250 + 25 Possible Extra Credit Points
Important Dates:
Interim Progress Reports due December 16
WORKSHEET A
A. For each statement, write YES if evidence of a chemical reaction is present. Write NO if there is no evidence of a chemical reaction.
_______________________________ 1. A piece of ice melts.
_______________________________ 2. Drain cleaner is mixed with water and the solution becomes warm.
_______________________________ 3. Molten candle wax solidifies.
_______________________________ 4. Green leaves turn yellow and red as the seasons change.
_______________________________ 5. Baking powder produces a gas that makes a cake rise.
Identify the reactants and products in each of the following reactions. Then, write the word equation for the chemical reaction.
7. An automobile engine can be powered by the combustion of methane gas, CH4, and oxygen gas, O2, which produces carbon dioxide and water.
When the methane ignites, the products of the reaction expand violently, driving the pistons of the engine and eventually the wheels of the car.
a) What are the reactants in the above process?______________________________________
b) What are the products in the above process?_______________________________________
c) Write the word equation for the above process.
_______________________________________________________________________
d) Write the formula equation for the above process.
_______________________________________________________________________
8. Dinitrogen tetroxide gas decomposes into nitrogen dioxide gas.
a) What are the reactants in the above process?______________________________________
b) What are the products in the above process?_______________________________________
c) Write the word equation for the above process.
_______________________________________________________________________
d) Write the formula equation for the above process.
_______________________________________________________________________
9. Hydrogen gas and iodine gas combine in a reversible reaction to form hydrogen iodide gas.
a) What are the reactants in the above process?______________________________________
b) What are the products in the above process?_______________________________________
c) Write the word equation for the above process.
_______________________________________________________________________
d) Write the formula equation for the above process.
_______________________________________________________________________
10. Chlorine dissolved in an aqueous solution of calcium iodide can react to replace the iodine in calcium iodide to form iodine and calcium chloride.
a) What are the reactants in the above process?______________________________________
b) What are the products in the above process?_______________________________________
c) Write the word equation for the above process.
_______________________________________________________________________
d) Write the formula equation for the above process.
_______________________________________________________________________
WORKSHEET B
A.
Identify whether each reaction described below is endothermic or exothermic. In the blank, write EN for endothermic or EX for exothermic.
______ 1) A piece of coal placed in a furnace gives off heat and light before turning to ash.
______ 2) When ammonium chloride mixes with water, the solution formed feels cold.
______ 3) 3NO2(g) + H2O(l)  2HNO3(aq) + NO(g) + 144 kJ
______ 4) N2(g) + 3H2(g) + 13.2 kJ  2NH3(g)
______ 5)
Balance the following chemical equations. If it is already balanced, write the word “balanced” underneath the equation.
CaCl2

CaCO3

Al
+
O2
+
O2

SO3
1)
NaHCO3 +
2)
Al2O3
3)
S8
4)
Pb(NO3)2 +
K2CrO4 
5)
Fe
O2
+

+
NaCl
PbCrO4 +
KNO3
+
H2O
+
CO2
Fe2O3
Write balanced chemical equations for each of the following reactions. Include all appropriate symbols.
6) Solid potassium chlorate is synthesized by combination of potassium, chlorine gas, and oxygen gas.
7) Oxygen gas plus nitrogen gas produce nitrogen dioxide gas.
8) The reaction between liquid water and calcium metal produces aqueous calcium hydroxide and hydrogen gas.
9) The decomposition of solid calcium carbonate into solid calcium oxide and carbon dioxide gas.
WORKSHEET C
1. What type of reaction involves two reactants forming one product?_____________________________________________________________
2. What type of reaction involves the formation of more than one product from a single reactant?________________________________________
3. What substance is common to all combustion reactions?______________________________________________________________________
4. What is an example of a combustion reaction in the everyday world?_____________________________________________________________
5. Which of the following are decomposition reactions? Circle the letters.
a) 2NaCl  2Na + Cl2
b) 2Na + Cl2  2NaCl
c) 2H2O  2H2 + O2
d) 2H2 + O2  2H2O
e) NaOH + HCl  HOH + NaCl
6. Which of the following are synthesis reactions? Circle the letters.
a) 2NaCl  2Na + Cl2
b) 2Na + Cl2  2NaCl
c) 2H2O  2H2 + O2
d) 2H2 + O2  2H2O
e) NaOH + HCl  HOH + NaCl
7. Which of the following are combustion reactions? Circle the letters.
a) NaCl  Na + Cl2
b) H2 + O2  H2O
c) Ca + S  CaS
d) C3H8 + O2  CO2 + H2O
e) Al + O2  Al2O3
8. Predict the products for these synthesis reactions. Write a balanced chemical equation for each reaction.
a) boron + fluorine 
b)
aluminum + nitrogen 
c) iron + fluorine 
9.
(hint: iron has a positive three charge)
Predict the products for the following decomposition reactions. Write a balanced chemical equation for each reaction.
a)
magnesium bromide 
b)
cobalt(II) oxide 
c)
barium chloride 
10. Predict the product for each of the following combustion reactions. Write the complete balanced equation for each reaction.
a)
Na + O2 
b)
C2H6 + O2 
c) C8H18 + O2 
WORKSHEET D
1. A single replacement reaction starts with two reactants and ends up with two products. The uncombined element takes the place of the
combined element in the compound. Which of the following reactions are single-replacement reactions? Circle the letters.
a) NaCl  Na + Cl2
b) NaOH + HCl  HOH + NaCl
c) K + AgCl  Ag + KCl
d) Ca + S  CaS
e) Na + HCl  H2 + NaCl
2. Does the following single replacement reaction occur? Explain your answer.
3Ni + 2AuBr3  3NiBr2 + 2Au
3. In each of the following pairs, which element will replace the other in a reaction?
a) tin or sodium
b) fluorine or iodine
c) lead or silver
d) copper or nickel
4. A piece of aluminum metal is placed in aqueous KCl. Another piece of aluminum is placed in an aqueous AgNO3 solution. Explain why a
chemical reaction does or does not occur in each instance.
5. Use the activity series to write a balanced chemical equation for each of the following single-replacement reactions. If no reaction occurs, write
N.R. on the product side of the reaction.
a)
Au
+
KNO3

b)
Al
+
CuSO4

c)
Cl2
+
NaI

6. Write balanced chemical equations for the following single replacement reactions.
a) sodium + magnesium iodide  magnesium + sodium iodide
b)
lithium + gold(III) chloride  lithium chloride + gold
WORKSHEET E
MATCHING
_____ 1. Zn + 2HCl  ZnCl2 + H2
a. Synthesis
_____ 2. C + O2  CO2
b. Decomposition
_____ 3. MgCO3 + 2HCl  MgCl2 + H2CO3
c. Single-Replacement
_____ 4. 2Na + MgF2  2NaF + Mg
d. Double-Replacement
_____ 5. 2NaCl  2Na + Cl2
e. Combustion
_____ 6. 4Na + O2  2Na2O
_____ 7. Two or more substances combine to form another substance
_____ 8. One element replaces another in a compound
_____ 9. A substance breaks down into two or more simpler substances
_____ 10. A precipitate, water or a gas forms when two ionic compounds are dissolved in a solution
11. Describe what the results of a double replacement reaction would be.
12. Under what conditions does a precipitate form in a chemical reaction?
13. Predict the products for each of the following double replacement reactions. Write the complete balanced chemical equation for each reaction.
a)
Ag2SO4 +
KCl

b)
CdBr2
Na2S

c)
Pb(NO3)2 +
NaI

d)
MgCl2
Ca(OH)2 
+
+
14. For each of the reactions in Question 13, CIRCLE any PRODUCTS that would PRECIPITATE.
15. In the following chemical reactions, circle the product that shows the reaction is a double replacement reaction.
a) AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)
b) 2NaCN(aq) + H2SO4(aq)  2HCN(g) + Na2SO4(aq)
c) Ca(OH)2(aq) + 2HCl(aq)  CaCl2(aq) + 2H2O(l)
WORKSHEET F
A. Circle the letter of each sentence that is true about ionic equations.
a)
A complete ionic equation shows only the ions involved in the reaction.
b) Spectator ions are left out of a net ionic equation.
c)
Atoms do not need to be balanced in an ionic equation.
d)
Ionic charges must be balanced in a net ionic equations.
B. Predict whether the following compounds are soluble or insoluble. Write I for insoluble and S for soluble.
a) Fe(OH)3
___________________________________________
b) NaOH
___________________________________________
c) Ca(ClO3)2
___________________________________________
d) HgSO4
___________________________________________
C. Write the complete ionic equation and the net ionic equation for the following reactions.
a)
Pb(NO3)2(aq) + KI(aq)  PbI2(s) + KNO3(aq)
Complete Ionic Equation:________________________________________________________________________________________
Net Ionic Equation:_____________________________________________________________________________________________
b)
NaOH(aq) + Fe(NO3)3(aq)  Fe(OH)3(s) + NaNO3(aq)
Complete Ionic Equation:________________________________________________________________________________________
Net Ionic Equation:_____________________________________________________________________________________________
c)
Ba(NO3)2(aq) + H3PO4(aq)  Ba3(PO4)2(s) + HNO3(aq)
Complete Ionic Equation:________________________________________________________________________________________
Net Ionic Equation:_____________________________________________________________________________________________
D. Determine whether or not a precipitate will form when the following aqueous solutions of ionic compounds are mixed. Check Yes if a precipitate
will form, check No if a precipitate will not form.
a) AgNO3 and Na2SO4
Yes
No
b) NH4Cl and Ba(NO3)2
Yes
No
c) CaCl2 and K2SO4
Yes
No
d) Pb(NO3)2 and HCl
Yes
No
WORKSHEET F—EXTRA CREDIT
Write balanced chemical equations for each of the following word equations.
1.
chlorine + sodium bromide
2.
sodium
3.
aluminum chloride + sodium hydroxide  sodium chloride + aluminum hydroxide
4.
silicon tetrachloride
5.
carbon +
6.
magnesium + hydrochloric acid

hydrogen +
7.
aluminum
iron(II) nitride

aluminum nitride
8.
magnesium
+
magnesium oxide
9.
zinc(II)sulfide + aluminum phosphide  zinc(II) phosphide + aluminum phosphide
10.
propane (C3H8) +
+
oxygen

hydrogen
+

sodium chloride

silicon +

oxygen 
oxygen 
+
bromine
sodium oxide
chlorine
methane (CH4)
carbon dioxide
magnesium chloride
+
+
water
iron
WORKSHEET H—MIDTERM REVIEW
Determine the answers to the following. When you are finished add up all of your answers. If you get
everything correct including the SUM you will earn 7 bonus points (the sum is worth 2 points).
1. The charge of an electron
__________________________________
2. The charge of a neutron
__________________________________
3. The atomic number of sodium
__________________________________
4. The mass number of a calcium atom with 24 neutrons
__________________________________
5. The oxidation number of a lithium ion
__________________________________
6. The oxidation number of an iodine ion
__________________________________
7. The charge of a cation formed by when an atom loses 2 electrons
__________________________________
8. The coefficient needed to balance this equation:
__________________________________
Mg + ___HCl  MgCl2 + H2
9. The charge of the following ion: iron(III)
__________________________________
10. The number of atoms of hydrogen in (NH4)2SO4
__________________________________
11. The number of protons in an atom of titanium
__________________________________
12. The number of electrons in an atom of tungsten
__________________________________
13. The number of neutrons in an atom with an atomic number of
__________________________________
6 and a mass number of 14
14. The charge of an ion in Group 16
__________________________________
15. The number of valence electrons in an atom of carbon
__________________________________
16. The number of electrons in Ba+2
__________________________________
17. The coefficient in front of Al in the equation:
__________________________________
Al2O3  Al + O2
18. The density of a metal with a mass of 32 g and a volume of 2 mL
__________________________________
19. The number of dots in a dot diagram of selenium
__________________________________
20. The number that the prefix hepta- stands for
__________________________________
21. The total number of atoms in Mg(OH)2
__________________________________
22. The amount of product if a reaction starts with 10 g of reactant
__________________________________
23. The subscript of phosphorus in the formula for calcium phosphide
__________________________________
24. The subscript of fluorine in the formula for oxygen difluoride
__________________________________
25. The number of valence electrons typically needed for an atom
__________________________________
to be stable.
TOTAL SUM OF ALL ANSWERS
_______________________________