Name ______
WPHS Chemistry
Unit 4
Chemical Reactions
Bergmann-Sams
Chemistry: Unit 4 Outline: Chemical Reactions
Assignment / WB Page Number / Score / Out ofPodcast 4.1 (CB 1-3) / Online /
Worksheet A / pg 7-9 /
Podcast 4.2 (CB 5-9) / Online /
Demo: Types of Reactions / In Class /
Worksheet B
/ Pg 10-12 / Lab: Small Scale Single Replacement / Pg 4 / 100
Podcast 4.3 (CB 11-13) / Online /
Worksheet C / Pg 13-15 /
Lab: Small Scale Double Replacement / Pg 5-6 / 100
Podcast 4.4 (CB 15-17) / Online /
Worksheet D / Pg 16 /
Technology Lab / Teacher Handout / 100
Worksheet E (Review) / Pg 17-20 /
Unit 4 Exam / In Class / 100
(You must score 85/100 on all assignments with a number to move to the next unit. For those assignments with a check, you need to do it to the satisfaction of your teacher)Unit 4 Chemical Reactions: Composition Book Outline
8-1: Describing Chemical Change
1 / Converting Word Equations into Formulaic Equations (pg 203-206)Question: Answer the following question
- What is the difference between a word equation and a chemical equation
- Catalyst
3 / Balancing Chemical Equations (pg 207-211)
Read the section and: “Balancing Chemical Equations” and come up with an analogy like the bicycle and write the balanced chemical equation.
Leave the rest of the page blank
8-2: Types of Chemical Equations
5 / Reaction Types (pgs 212-216)Define: Combination Reactions, Decomposition Reaction, Single Replacement Reaction, Double Replacement Reaction, Combustion Reaction Do one at a time with the examples underneath each
List: Two examples of eachtype (written with formulas—not words)
7 / Predicting Single Replacement Reactions
Copy: Table 8.2 on page 217
9 / Predicting Single Replacement Reactions
Leave blank for teacher notes
11 / Predicting and Writing Double Replacement Reactions
Leave blank for teacher notes
13 / Predicting and Writing Double Replacement Reactions
Leave blank for teacher notes
8-3: Reactions in Aqueous Solutions
15 / Ionic and Net Ionic Equations (pg 225-228)Leave blank for teacher notes
17 / Ionic and Net Ionic Equations (pg 225-228)
Leave blank for teacher notes
Activity Series of Metals Lab
Purpose: To observe an activity series of different metals.
Procedure:
- Using the well plates, select a row of wells for each solution listed in the data table. Make sure that you write down which letter and number your wells are for each solution. There should be three wells for each solution (one of the three for each of the metals).
- Put five drops of each solution in the wells chosen for that solution.
- Put one piece of magnesium in one of the wells for each solution. For example, you should have a well of copper sulfate with magnesium in it, a well of magnesium sulfate with magnesium in it, and a well of sodium chloride with magnesium in it, a well of zinc sulfate with magnesium in it and a well of silver nitrate with magnesium in it.
- Repeat step 3 with copper instead of magnesium.
- Repeat step 3 with zinc instead of magnesium.
- After l minute has passed, make observations of both the metal strips and the solutions. Put these observations in a data table in your comp book that looks like the one below. Label this data table as 1 minute.
- After 5 total minutes have passed, take another set of observations. Make another data table like the one below and label it 5 minutes.
- After 15 total minutes have passed, take another set of observations. Again, make another data table and label it 15 minutes.
Data Table:
CuSO4 / MgSO4 / NaCl / ZnCl2 / AgNO3Cu metal
Mg metal
Zn metal
Analysis Questions: (as always with labs, these questions should be written in complete sentences)
- Why doesn’t the metal react with the same metal solution?
- In which wells did the appearance of the metal change? Be sure to tell your teacher what both of the reactants of the well were.
- Write a balanced equation for each visible reaction between a metal and it’s solution. Be sure to identify what types of reactions these are.
- Based on the results of your experiment construct your own activity series for the five metals. Put the most active metal first and the least active metal last. Be sure to include your reasoning for your rankings.
- In a short summary paragraph, describe and explain the patterns that you see in your reaction table.
Double Replacement Lab
Use Beral Pipets to add each solution on the grid. For those that have a reaction occur, describe the reaction. For those that do not, record NVR (No visible reaction) When done you need to:
- Write out each complete reaction that occurs (you must balance it)
- Write out the ionic equation for each reaction that occurs.
- Write out the net-ionic equation for each reaction that occurs.
Put “flimsy” over the top of this page and mix all of the chemicals. Do not mix the same chemical with the same.
Chemical / NaCl / AgNO3 / Pb(NO3)2 / Na2SO4 / BaCl2 / NaOH / Na3PO4NaCl / X / X / X / X / X / X
AgNO3 / X / X / X / X / X / X
Pb(NO3)2 / X / X / X / X / X / X
Na2SO4 / X / X / X / X / X
BaCl2 / X / X / X / X / X / X
NaOH / X / X / X / X / X / X
Na3PO4 / X / X / X / X / X / X
Data Table: Write in your observations here.
Chemical / NaCl / AgNO3 / Pb(NO3)2 / Na2SO4 / BaCl2 / NaOH / Na3PO4NaCl
AgNO3
Pb(NO3)2
Na2SO4
BaCl2
NaOH
Na3PO4
Equation Worksheet A:
Balancing Chemical Equations
Balance the following equations and identify the type of reaction: (Double Replacement, Single Replacement, Combination, Decomposition, or Combustion)
1)__HgO __Hg+__O2Type: ______
2)__HCl+__Mg__H2+MgCl2 Type: ______
3)__CH4+__O2__CO2+__H2O Type: ______
4)__C6H12O6+ __O2__CO2+ __H2OType: ______
5)__H2+__O2__H2OType: ______
6)__H2+__N2__NH3Type: ______
7)__NO+__O2__NO2Type: ______
8)__Al2O3__Al+__O2Type: ______
9)__CaO+__H2O__Ca(OH)2Type: ______
10)Hydrogen gas reacts with iodine to produce hydroiodic acid.
Type: ______
11)Sulfur reacts with oxygen to produce sulfur dioxide.
Type: ______
12)Calcium acetate reacts with sodium carbonate to produce calcium carbonate and sodium acetate.
Type: ______
13)Write the chemical reaction that shows how rust forms: (Iron III oxide)
Type: ______
14)Iron combines with oxygen and water to form iron (III) hydroxide
Type: ______
15)Sulfur trioxide is bubbled through water to produce sulfuric acid
Type: ______
16)Copper metal is made by treating copper ore the following way: Copper (II) sulfide is heated with carbon and oxygen to produce copper and sulfur dioxide and carbon dioxide.
Type: ______
17)Copper-bottomed cooking pans turn black because copper combines with oxygen to form copper (II) oxide.
Type: ______
18)Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium chloride and water.
Type: ______
Equation Worksheet B: Single Replacement Reactions
A. Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R. For transition metals use the following charges:
Iron: Fe3+ / Mercury: Hg2+Lead: Pb4+ / Copper: Cu1+
- Fe + CuCl2
- Hg +Sn(SO4)2
- Ba +Ni3(PO4)2
- Pb +Au(NO3)3
- Li +HOH
- K +AgCl
- Ca +NaOH
- Cu +Fe(OH)3
- Fe +Cu(OH)2
- Lead II Chloride + Magnesium
- Barium Nitrate + Zinc
- Potassium + Tin IV Nitrate
- Copper + Silver Nitrate
- Sodium Phosphate + Potassium
- Gold + Hydrochloric acid
- Magnesium + Aluminum Hydroxide
- Iron + Copper II Sulfate
- Iron + Nickel II Iodide
- Sodium Permanganate + Calcium
- hydrochloric acid + Zinc
- Aluminum + Iron II dichromate
Equation Worksheet C: Double Replacement Reactions
Complete and Balance the following reactions. If no reaction occurs then write N.R.
1)Na2SO4(aq) + Ba(NO3)2(aq) ---->
2)NaNO3(aq) + NH4Cl(aq) ----->
3)Pb(NO3)2(aq) + Na2CrO4(aq)
4)ZnCl2(aq) + K2CO3(aq) ---->
5)Ammonium Chloride + Silver Nitrate ------>
6)Barium Acetate + Copper II Chromate
7)Solutions of Silver Nitrate and ammonium chloride are mixed
8)Solutions of Lead II nitrate and Sodium Chloride are mixed
9)Solutions of zinc sulfate and magnesium chloride are mixed
10)Solutions of Ammonium phosphate and Zinc Chlorate are mixed
11)Solutions of Aluminum bromide and Iron II Iodide are mixed
12)Solutions of sodium sulfide and Iron II Chlorate are mixed
13)Solutions of copper II bromide and potassium phosphate are mixed
14)Solutions of barium acetate and zinc sulfate are mixed
Equation Worksheet D: Net Ionic Equation Worksheet
For the following reactions write the:
- Complete Equation (Indicate states): Balance
- Ionic Equation
- Net Ionic Equation
- ZnCl2 (aq) + Na2S (aq) ZnS(s) + NaCl(aq)
- (NH4)3PO4 + AgNO3
- Magnesium Nitrate + Potassium phosphate Magnesium Phosphate (s) + Potassium Nitrate.
- Lead II Acetate + Potassium Iodide
Equations Worksheet E: Mixed Types of Reactions
Directions: For each of the following reactions:
1)Complete the reaction (Put NR if no reaction takes place)
2)Balance it
3)Identify the type of reaction (Single Replacement, combination, double replacement, decomposition, or combustion)
4)Indicate states of matter for each reaction
1)NaCl + AgNO3
2)Fe + CuSO4
3) C4H10 + O2
4)Ba(NO3)2 + Na2SO4
5)AgNO3 + Li
6)LiBr + Cu
7)MgS + NaOH
8)Hg + LiCl
9)Li + HgCl2
10)C3H8+ O2
11)Ammonium Nitrate is added to sodium chloride
12)Lithium Chloride is added to Zinc Phosphate
13)Zinc is added to lithium chloride
14)Iron is added to a solution of silver nitrate
15)A solution of copper II sulfate is added to an iron nail
16)Octane (C8H18) is burned in air
17) A solution of Tin IV sulfate is added to a solution of ammonium hydroxide
18)Sodium hydroxide is added to hydrochloric acid
19)Calcium hydroxide is added to sulfuric acid
20)Nickel is added to hydrochloric acid
21)Strontium is added to water
22)Hydrochloric acid is added to copper metal
23)Solid bismuth is added to a solution of barium hydroxide.
24)Methanol (CH3OH) is burned in air
25)Solid gold is added to hydrochloric acid
Name: ______
Period: ______
Balancing Reactions Worksheet
Synthesis and Decomposition
Part A (Review): Balance the following reactions and indicate whether they are synthesis or decomposition reactions.
1.SO3+H2O--->H2SO4Type:______
2.H2O--->H2+O2Type:______
3.HgO--->Hg+O2Type:______
4.Al2O3(s)--->Al(s)+O2(g)Type:______
5.P+O2--->P2O5Type:______
Part B: Predict the products and indicate type (include states):
1. KBr --->Type: ______
2. Li + Cl2 --->Type: ______
3. Rb2CO3 --->Type: ______
4. NiO --->Type: ______
5. CO2 + H2O--->Type: ______
Part C: Predict the products, balance, include states, and indicate type.
1. Potassium Chlorate is heated vigorouslyType: ______
2. Molten sodium is reacted with chlorine gasType: ______
3. Calcium is added to waterType: ______
4. Zinc carbonate is heateType: ______
5. Aluminum chloride decomposes into it's elementsType: ______
6. Cesium hydroxide is heatedType: ______
7. Sulfurous Acid is heatedType: ______
8. Potassium and Bromine are reactedType: ______
9. Potassium Oxide and Carbon dioxide reactType: ______
10. Calcium chlorate is heatedType: ______
11. Sodium hydroxide is heatedType: ______
12. Iodine reacts with hydrogenType: ______
Balancing Chemical Equations Worksheet 1Name
Period
Balance the following equations:
- 2HgO 2Hg+O2
- HCl+MgH2+MgCl2
- CH4+2O2CO2+2H2O
- C6H12O6+6O26CO2+6H2O
- 2H2+O22H2O
- 2H2+Cl22HCl
- 3H2+N22NH3
- 2 NO+O22NO2
- 3Al2O34Al+2O2
- CaO+H2OCa(OH)2 already balanced
- Hydrogen gas reacts with iodine to produce hydrogen iodide.
H2+ I2 2HI
- Sulfur reacts with oxygen to produce sulfur dioxide.
S + O2 SO2
- Calcium acetate reacts with sodium carbonate to produce calcium carbonate and sodium acetate.
Ca(C2H3O2)2 + Na2CO3 2NaC2H3O2 +CaCO3
- Write the chemical reaction that shows how rust forms:
4Fe + 3O2 2Fe2O3
- Iron combines with oxygen and water to form iron (III) hydroxide
Fe + O2 + 6H2O 4Fe(OH)3
- Sulfur trioxide is bubbled through water to produce hydrogen sulfate
SO3+ H2O H2SO4 already balanced
- Copper metal is made by treating copper ore the following way:
- Copper (II) sulfide is heated with carbon and oxygen to produce copper and sulfur dioxide and carbon dioxide.
CuS +C + 4O2 SO2 + CO2 + Cu
Copper-bottomed cooking pans turn black because copper combines with oxygen to form copper (II) oxide.
2Cu + O2 2CuO
- Any Group I metal reacts with water to produce hydrogen gas and the metal hydroxide. Write the reaction that occurs when rubidium is dropped in water.
2Rb + 2HOH 2RbOH + H2
- Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium chloride and water.
Mg(OH)2 + 2HCl MgCl2 + 2H2O
- Limestone is dissolved by acid (Remember our carbonate lab in September?). This is why statues are dissolved by acid rain. First, the acid is formed in the atmosphere. Second, it falls on the statue and dissolves it. Write two reactions that show how this
happens. First, nitrogen dioxide reacts with water to form hydrogen nitrate. Second, hydrogen nitrate combines with calcium carbonate to form carbon dioxide and water and calcium nitrate.
4NO2+ 2H2O 4HNO3 balancing is difficult extra credit if you can
2HNO3 + CaCO3 Ca(NO3)2+ H2O+ CO2
Balancing Reactions Worksheet
Synthesis and Decomposition
Part A (Review): Balance the following reactions and indicate whether they are synthesis or decomposition reactions.
1.SO3+H2O--->H2SO4balancedType: synthesis
2.2H2O--->2H2+O2Type: decomposition
3.2HgO--->2Hg+O2Type: decomposition
4.2Al2O3(s)--->4Al(s)+3O2(g)Type: Decomposition
5.4P+5O2--->2P2O5Type: Synthesis
Part B: Predict the products and indicate type (include states):
1. 2KBr --->2K + Br2Type: decomp
2. 2Li + Cl2 --->2LiClType: synth
3. Rb2CO3 --->Rb2O + CO2Type: decomp
4. 2NiO --->2Ni + O2Type: decomp
5. CO2 + H2O--->H2CO3Type: synth
Part C: Predict the products, balance, include states, and indicate type.
1)Potassium Chlorate is heated vigorously
2KClO3 2KCl + 3O2decomposition
2) Molten sodium is reacted with chlorine gas
2Na + Cl2 2NaClsynthesis
3)Calcium is added to water
Ca + 2HOH Ca(OH)2synthesis
4)Zinc carbonate is heate
ZnCO3 ZnO + CO2decomposition
5)Aluminum chloride decomposes into it's elements
2AlCl3 2Al + 3Cl2decomposition
6) Cesium hydroxide is heated
4CsOH 2Cs2O + 2H2decomposition
7)Sulfurous Acid is heated
H2SO3 H2O + SO2decomposition
8)Potassium and Bromine are reacted
2K+ Br2 2KBrdecomposition
9. Potassium Oxide and Carbon dioxide react
K2O + CO2 K2CO3decomposition
10. Calcium chlorate is heated
Ca(ClO3)2 CaCl2 + 3O2decomposition
1)Sodium hydroxide is heated
4NaOH 2Na2O + 2H2decomposition
12. Iodine reacts with hydrogen
I2 + H2 2HIsynthesis
Single Replacement Reactions WorksheetName:
Do work on a separate sheet of paper
A. Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R.
1)Fe + CuCl2
2)Hg+Sn(SO4)2
3)Ba +Ni3(PO4)2
4)F2+NaCl
5)Cl2+NH4Br
6)Pb+Au(NO3)3
7)Li+HOH
8)K+AgCl
9)Ca+NaOH
10)Cu+Fe(OH)3
11)Fe+Cu(OH)2
12)Br2+KI
B. Write the reactions and predict the products of each of the following single replacement reactions. Balance all reactions. If no reaction occurs write N.R.
13)Lead II Chloride + Magnesium
14)Barium Nitrate + Zinc
15)Potassium + Tin IV Nitrate
16)Copper + Silver Nitrate
17)Sodium Phosphate + Potassium
18)Gold + Hydrogen chloride
19)Magnesium + Aluminum Hydroxide
20)Iron + Copper II Sulfate
21)Iron + Nickel II Iodide
22)Sodium Permanganate + Calcium
23)Hydrogen Chloride + Zinc
24)Aluminum + Iron II dichromate
Name:______
Period:______
Mixed Types of Reactions
Directions: For each of the following reactions:
5)Complete the reaction (Put NR if no reaction takes place)
6)Balance it
7)Identify the type of reaction
8)(Single Replacement, combination, double replacement, decomposition, or combustion)
9)Indicate states of matter for each reaction
26)NaCl + AgNO3
27)Fe + CuSO4
28) C4H10 + O2
29)Ba(NO3)2 + Na2SO4
30)AgNO3 + Li
31)LiBr + Cu
32)MgS + NaOH
33)HG + LiCl
34)Li + HgCl2
35)C3H8+ O2
36)Ammonium Nitrate is added to sodium chloride
37)Lithium Chloride is added to Zinc Phosphate
38)Zinc is added to lithium chloride
39)Iron is added to a solution of silver nitrate
40)A solution of copper II sulfate is added to an iron nail
41)Octane (C8H18) is burned in air
42) A solution of Tin IV sulfate is added to a solution of ammonium hydroxide
43)Sodium hydroxide is added to hydrochloric acid
44)Calcium hydroxide is added to sulfuric acid
45)Nickel is added to hydrochloric acid
46)Strontium is added to water
47)Hydrochloric acid is added to copper metal
48)Solid bismuth is added to a solution of barium hydroxide.
49)A solution of potassium iodide is added to liquid bromine.
50)Methanol (CH3OH) is burned in air
51)Solid gold is added to hydrochloric acid
Ws E KEY
Types of Reactions Work Sheet
Directions: For each of the following reactions:
- Complete the reaction (Put NR if no reaction takes place)
- Balance it
- Identify the type of reaction
- (Single Replacement, combination, double replacement, decomposition, or combustion)
- Indicate states of matter for each reaction
1)Sodium chloride plus silver nitrate
NaCl(aq)+AgNO3(aq) AgCl(s) + NaNO3(aq)
Double Replacement
2)Iron plus copper II sulfate
2Fe(s) + 3CuSO4(aq) 3Cu(s) + Fe2(SO4)3(aq)
Fe(s) + CuSO4(aq) Cu(s) + FeSO4(aq)
Single Replacement
3)Butane (C4H10) burns completely in the presence of oxygen
C4H10(g) + 13/2O2(g) 4CO2(g) + 5H2O (g)
2C4H10(g) + 13O2(g) 8CO2(g) + 10H2O (g)
Combustion
4)Barium Nitrate + sodium sulfate
Ba(NO3)2(aq) + Na2SO4(aq) BaSO4 (s) + 2NaNO3(aq)
Double Replacement
5)Silver nitrate Plus Lithium
AgNO3(aq) + Li (s) - LiNO3 (aq) + Ag
Single Replacement
6)Lithium bromide plus copper
LiBr (aq) + Cu No reaction
7)Magnesium sulfide plus sodium hydroxide.
MgS (s) + NaOH (aq) No reaction
8)Liquid mercury reacts with aqueous lithium chloride
Hg (l) + LiCl (aq) No Reaction
9)Solid Lithium is dropped into a solution of Mercury II chloride
2Li (s) + HgCl2(aq) 2LiCl (aq) + Hg (l)
Single Replacement
10)Propane (C3H8) is burned in the presence of air
C3H8(g) + 5O2(g) 3CO2(g) + 4H2O (g)
Combustion
11)Ammonium Nitrate is added to sodium chloride
NH4NO3(aq) + NaCl (aq) No reaction
12)Lithium Chloride is added to Zinc Phosphate
LiCl (aq) + Zn3(PO4)2(s) No reaction
13)Zinc is added to lithium chloride
Zn (s) + LiCl(aq) No reaction
14)Iron is added to a solution of silver nitrate
Fe (s) + 3AgNO3(aq) 3Ag(s) + Fe(NO3)3
Fe (s) + 2AgNO3(aq) 2Ag(s) + Fe(NO3)2
Single Replacement
15)A solution of copper II sulfate is added to an iron nail
3CuSO4(aq) + 2Fe (s) Fe2(SO4)3(aq) + 3Cu(s)
CuSO4(aq) + Fe (s) FeSO4(aq) + Cu
Single Replacement
16)Octane (C8H18) is burned in air
C8H18(g) + 12.5O2(g) 8CO2(g) + 9H2O(g)
2C8H18(g) + 25O2(g)
16CO2(g) + 18H2O(g)
combustion
17)A solution of Tin IV sulfate is added to a solution of ammonium hydroxide
Sn(SO4)2(aq) + 4NH4OH(aq)
Sn(OH)4(s) + 2(NH4)2SO4(aq)
double replacement
Or: No Reaction: Really a reaction will occur
18)Sodium hydroxide is added to hydrochloric acid
NaOH(aq) + HCl(aq) H2O(l) + NaCl(aq)
double replacement
19)Calcium hydroxide is added to sulfuric acid
Ca(OH)2(s) + H2SO4(aq)
CaSO4(s) + 2H2O(l)
double replacement
20)Nickel is added to hydrochloric acid
Ni(s) + 2HCl(aq) NiCl2(aq) + H2(g)
2Ni(s) + 6HCl(aq) 2NiCl3(aq) + 3H2(g)
Single Replacement
21)Strontium is added to water
Sr(s) + 2HOH(l) Sr(OH)2(s) + H2(g)
Single replacement
22)Hydrochloric acid is added to copper metal
HCl(aq) + Cu No reaction
23)Solid bismuth is added to a solution of barium hydroxide.
Bi(s) + Ba(OH)2(s) No reaction
24)A solution of potassium iodide is added to liquid bromine.
2KI(aq) + Br2(l) 2KBr(aq) + I2(s)
single replacement
25)Methanol (CH3OH) is burned in air
2CH3OH(g) + 3O2(g)
2CO2(g) + 4H2O(g)
combustion
26)Solid gold is added to hydrochloric acid
Au(s) + HCl(aq) no reaction
Reaction Type Worksheet
Balance and then identify each of the following reactions as: combustion, synthesis, decomposition, Single Displacement, Double Displacement.
1. Na+Cl2 NaClType: ______
2. AgNO3+ NaCl AgCl + NaNO3Type: ______
3. NH4CO3 (NH4)2O+ CO2Type: ______
3. CuSO4+ Li Li2SO4+ CuType: ______
4. C2H6 + O2 CO2 + H2OType: ______
5. Na3PO4 + CuCl2 Cu3(PO4)2 + NaClType: ______
6. AgNO3 + Zn Zn(NO3)2 + AgType: ______
7. CH3OH + O2 CO2 + H2OType: ______
8. CaO + CO2 CaCO3Type: ______
9. Pb(NO3)2 + Na2CrO4 NaNO3 + PbCrO4Type: ______
10. KClO3 KCl + O2Type: ______
11. Magnesium + Iron III Chloride Magnesium Chloride + Iron
12. Nickel II Iodide + Silver I Nitrate Silver I Iodide + Nickel II Nitrate
13. Sodium carbonate decomposes into sodium oxide and carbon dioxide
14. Butane (C4H10) reacts with oxygen to form carbon dioxide and water
15. Magnesium oxide reacts with carbon dioxide to make magnesium carbonate
16. Potassium Phosphate + Chromium III Chloride
Potassium Chloride + Chromium III Phosphate
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