WPHS ChemistryUnit 4

Chemical Reactions

Bergmann-Sams

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Chemistry: Unit 4 Outline: Chemical ReactionsAssignment Only in

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Podcast 4.1: Converting Word Equations into Formulaic EquationsWorksheet 4.1: Converting Word Equations into Formulaic EquationsPodcast 4.2: Balancing Chemical EquationsWorksheet 4.2: Balancing Chemical EquationsPodcast 4.3: Reaction Types OverviewWorksheet 4.3: Reaction Types OverviewLab: Types of Reactions Lab XPodcast 4.4: Predicting Single Replacement ReactionsWorksheet 4.4: Predicting Single Replacement ReactionsLab: Activity Series of a Metal XPodcast 4.5: Predicting Double Replacement ReactionsWorksheet 4.5: Predicting Double Replacement ReactionsLab: Small Scale Double Replacement XPodcast 4.6: Complete Ion and Net Ionic EquationsWorksheet 4.6: Complete Ion and Net Ionic EquationsPodcast 4.7: Mixed Types of ReactionsWorksheet 4.7: Mixed Types of ReactionsDemo: Light your teacher on FIRE!!! XUnit 4 Review (Review)Unit 4 VocabularyUnit 4 Exam X

Unit 4 Vocabulary

word equation chemical equation skeleton equation Catalyst Combination Reactions Decomposition Reaction Single Replacement Reaction Double Replacement Reaction precipitate Combustion Reaction Ion Ionic and Net Ionic Equations

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Cut out the following 2 tables and put them in the back of your composition book. These are reference tables that you will use throughout the year.

Activity of Metals SeriesMetal Ion FormedLithium: Li Li+

Potassium: K K+

Barium: Ba Ba2+

Calcium: Ca Ca2+

Sodium: Na Na+

Magnesium: Mg Mg2+

Aluminum: Al Al3+

Manganese: Mn Mn2+

Zinc: Zn Zn2+

Chromium: Cr Cr3+

Iron: Fe Fe3+

Cadmium: Cd Cd2+

Cobalt: Co Co2+

Nickel: Ni Ni2+

Tin: Sn Sn2+

Lead: Pb Pb2+

Hydrogen: H 2H+

Copper: Cu Cu2+

Silver: Ag Ag+

Mercury: Hg Hg2+

Platinum: Pt Pt2+

Gold: Au Au3+

Solubility TableKey: (s) = solid, (aq)= aqueous: soluble in water, H2O = water formed (NE)= does not exist,

Acetate

Brom

ide

Carbonate

Chlorate

Chloride

Chrom

ate

Hydroxide

Iodide

Nitrate

Oxide

Phophate

Sulfate

Sulfide

Aluminum (aq) (aq) NE (aq) (aq) NE (s) (aq) (aq) (s) (s) (aq) (s)Ammonium (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) NE (aq) (aq) (aq)Barium (aq) (aq) (s) (aq) (aq) (s) (s) (aq) (aq) (aq) (s) (s) (s)Calcium (aq) (aq) (s) (aq) (aq) (aq) (s) (aq) (aq) (s) (s) (s) (s)Copper II (aq) (aq) (s) (aq) (aq) NE (s) (aq) (aq) (s) (s) (aq) (s)Hydrogen (aq) (aq) Gas (aq) (aq) NE H2O (aq) (aq) NE (s) (aq) (s)Iron II (aq) (aq) (s) (aq) (aq) NE (s) (aq) (aq) (s) (s) (aq) (s)Iron III (aq) (aq) NE (aq) (aq) (s) (s) (aq) (aq) (s) (s) (aq) (s)Lead II (aq) (s) (s) (aq) (s) (s) (s) (s) (aq) (s) (s) (s) (s)Magnesium (aq) (aq) (s) (aq) (aq) (aq) (s) (aq) (aq) (s) (s) (aq) (s)Manganese II (aq) (aq) (s) (aq) (aq) NE (s) (aq) (aq) (s) (s) (aq) (s)Mercury II (aq) (aq) NE (aq) (aq) (s) (s) (aq) (aq) (s) (s) (aq) (s)Potassium (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq)Silver I (aq) (s) (s) (aq) (s) (s) (s) (s) (aq) (s) (s) (aq) (s)Sodium (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq)Strontium (aq) (aq) (s) (aq) (aq) (s) (aq) (aq) (aq) (aq) (s) (aq) (aq)Tin II (aq) (aq) NE (aq) (aq) (s) (s) (aq) (aq) (s) (s) (aq) (s)Tin IV (aq) (aq) NE NE (aq) (aq) (s) (aq) (aq) (s) NE (aq) (s)Zinc II (aq) (aq) (s) (aq) (aq) (s) (s) (aq) (aq) (s) (s) (aq) (s)

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Types of Reactions Lab

Purpose: To observe the different types of reactions: single replacement, synthesis, decomposition, combustion, double replacement.

Single Replacement (Zinc + Hydrochloric Acid)

Synthesis (Hydrogen + Oxygen)

Decomposition (Hydrogen Peroxide (H2O2))

Combustion (Cellulose (C6H12O6) + Oxygen)

Double Replacement (Calcium Chloride + Sodium Carbonate)

Part A: Single Replacement and Synthesis

1. Place one square of Zinc into a medium test tube.2. Add 10mL of 1.0M HCl3. Cover the test tube with your thumb4. Record observations5. Write the chemical reaction for this single replacement reaction

6. Have your partner light a wood splint7. Release your thumb and immediately have your partner place the wood splint near

the mouth of the test tube.8. Record your observations9. Write the chemical reaction for this synthesis reaction (water is a product).

OBSERVATIONS and REACTIONS

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Part B: Decomposition and Combustion

1. Place 10ml of hydrogen peroxide into a medium test tube2. Add 0.2g of MnO2 (MnO2 is a catalyst and is not part of the reaction)3. Record your observations4. Write the chemical reaction for this decomposition reaction (products are water

and oxygen gas)

5. While the decomposition reaction is still occurring light a wood splint, let it burn for a few seconds and blow it out.

6. While the wood splint is still glowing (but not burning), place it into the mouth of the test tube.

7. Record your observations8. Write the chemical reaction for this combustion reaction between cellulous and

oxygen.

OBSERVATIONS and REACTIONS

Part C: Double Replacement1. Obtain 1mL of 1.0M Calcium Chloride and 1mL of 1.0M Sodium Carbonate2. Mix the two solutions in a medium test tube3. Record your observations4. Write the chemical reaction for this double replacement reaction

OBSERVATIONS and REACTIONS

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Activity Series of Metals Lab

Purpose: To observe an activity series of different metals.

Procedure: 1. 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).

2. Put five drops of each solution in the wells chosen for that solution. 3. 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.

4. Repeat step 3 with copper instead of magnesium.5. Repeat step 3 with zinc instead of magnesium.6. 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.

7. After 5 total minutes have passed, take another set of observations. Make another data table like the one below and label it 5 minutes.

8. 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 AgNO3

Cu metalMg metalZn metal

Analysis Questions: (as always with labs, these questions should be written in complete sentences)

1. Why doesn’t the metal react with the same metal solution?2. 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.3. 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.4. 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.

5. In a short summary paragraph, describe and explain the patterns that you see in your reaction table.

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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:

1. Write out each complete reaction that occurs (you must balance it)2. Write out the ionic equation for each reaction that occurs.3. 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 Na3PO4

NaCl

X X X X X XAgNO3

X X X X X XPb(NO3)2

X X X X X XNa2SO4

X X X X XBaCl2

X X X X X XNaOH

X X X X X XNa3PO4

X X X X X X

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Data Table: Write in your observations here.Chemical NaCl AgNO3 Pb(NO3)2 Na2SO4 BaCl2 NaOH Na3PO4

NaCl

AgNO3

Pb(NO3)2

Na2SO4

BaCl2

NaOH

Na3PO4

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Worksheet 4.1: Converting Word Equations to Formulaic EquationsWrite each of the following equations using chemical symbols and all other appropriate symbols. Remember to put state of matter in parenthesis and subscripted.

1. Iron is heated in the presence of solid sulfur to from solid iron III sulfide

2. Gaseous methane CH4 is reacted with oxygen gas to form carbon dioxide gas and water vapor

3. Aqueous copper II chloride is added to aqueous lead II nitrate to from solid lead II chloride and aqueous copper II nitrate

4. Chlorine gas is bubbled into aqueous sodium bromide to form aqueous sodium chloride and liquid bromine

5. Solid silver is added to aqueous gold III chloride to form solid gold and silver I chloride.

6. Gaseous ammonia(NH3) is bubble into water to form aqueous ammonium hydroxide

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Worksheet 4.2: Balancing Chemical EquationsBalance the following equations

1) __HgO __Hg + __O2

2) __HCl + __Mg __H2 + MgCl2

3) __CH4 + __O2 __CO2 + __H2O

4) __C6H12O6 + __O2 __CO2 + __H2O

5) __H2 + __O2 __H2O

6) __H2 + __N2 __NH3

7) __NO + __O2 __NO2

8) __Al2O3 __Al + __O2

9) __CaO + __H2O __Ca(OH)2

10) Hydrogen gas reacts with iodine to produce hydroiodic acid.

11) Sulfur reacts with oxygen to produce sulfur dioxide.

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12) Calcium acetate reacts with sodium carbonate to produce calcium carbonate and sodium acetate.

13) Iron combines with oxygen and water to form iron (III) hydroxide

14) Sulfur trioxide is bubbled through water to produce sulfuric acid

15) Copper-bottomed cooking pans turn black because copper combines with oxygen to form copper (II) oxide.

16) Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium chloride and water.

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Worksheet 4.3Now go back to Worksheets 4.1 and 4.2 and write down the type of each reaction

Worksheet 4.4: Predicting Single Replacement Reactions

Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R. For transition metals use the following charges:

1. Fe (s) + CuCl2(aq)

2. Hg(l) + Sn(SO4)2 (aq)

3. Ba (s) + Ni3(PO4)2 (aq)

4. Pb(s) + Au(NO3)3 (aq)

5. Li(s) + HOH(l)

6. K(s) + AgCl(s)

7. Ca(s) + NaOH(aq)

8. Cu(s) + Fe(OH)3(aq)

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9. Fe(s) + Cu(OH)2(s)

10. Lead II Chloride + Magnesium

11. Barium Nitrate + Zinc

12. Potassium + Tin IV Nitrate

13. Copper + Silver Nitrate

14. Sodium Phosphate + Potassium

15. Gold + Hydrochloric acid

16. Magnesium + Aluminum Hydroxide

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17. Iron + Copper II Sulfate

18. Iron + Nickel II Iodide

19. Sodium Permanganate + Calcium

20. hydrochloric acid + Zinc

21. Aluminum + Iron II dichromate

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Worksheet 4.5: Predicting 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

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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

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13) Solutions of copper II bromide and potassium phosphate are mixed

14) Solutions of barium acetate and zinc sulfate are mixed

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Worksheet 4.6: Complete Ion and Net Ionic EquationsFor the following reactions write the:

a. Complete Equation (Indicate states): Balanceb. Ionic Equationc. Net Ionic Equation

1. ZnCl2 (aq) + Na2S (aq) ZnS(s) + NaCl(aq)

2. (NH4)3PO4 + AgNO3

3. Magnesium Nitrate + Potassium phosphate Magnesium Phosphate (s) + Potassium Nitrate.

4. Lead II Acetate + Potassium Iodide

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Worksheet 4.7: Mixed Types of Reactions

Directions: For each of the following reactions:1) Identify the type of reaction (Single Replacement, combination, double replacement,

decomposition, or combustion)2) Complete the reaction (Put NR if no reaction takes place)3) Balance it4) Indicate states of matter for each substance (solid, liquid, gas, aqueous)

1) NaCl(aq) + AgNO3(aq)

2) Fe(s) + CuSO4(aq)

3) C4H10(g) + O2(g)

4) Ba(NO3)2(aq) + Na2SO4 (aq)

5) AgNO3(aq) + Li(s)

6) LiBr(aq) + Cu(s)

7) MgS(s) + NaOH

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8) Hg(l) + LiCl

9) Li(s) + HgCl2(aq)

10) C3H8(g) + O2(g)

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

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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

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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

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Unit 4 Review Sheet

Part A: Balance the following reactions and indicate whether they are synthesis or decomposition reactions.

1. SO3 + H2O ---> H2SO4 Type:_____________2. H2O ---> H2 + O2 Type:_____________3. HgO ---> Hg + O2 Type:_____________4. Al2O3(s) ---> Al(s) + O2(g) Type:_____________5. P + O2 ---> P2O5 Type:_____________

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. Molten sodium is reacted with chlorine gas Type: _________

2. Calcium is added to water (think of water as HOH) Type: _________

3. Aluminum chloride decomposes into its elements Type: _________

4. Potassium and Bromine are reacted Type: _________

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5. Iodine reacts with hydrogen Type: _________

Part D:

Write the molecular equation, the complete ionic equation, and the net ionic equation for each reaction.

1. Aqueous lithium phosphate reacts with aqueous calcium chloride

2. Aqueous potassium chloride reacts with aqueous lead II chlorate

3. Aqueous manganese II nitrate reacts with aqueous sodium sulfide.

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