Single Replacement Reaction Predictions Complete1

NameDate

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Single Replacement Reactions

Introduction:

This Lab teaches the concepts of basic single replacement reactions in an inorganic solution system. The primary concept for this lab is the interaction of cations and anions in aqueous solution, using the general formula AX +B ---> BX + A, as determined by the rules of solubility and activity level of the Ionic compounds (AX) + metal cations (B) involved. The new combination of cations and anions in a chemical reaction yield products that may be a precipitate or gas. Look for a color change in the aqueous solution or the formation of a precipitate or gas. The Activity Series of the metals is an invaluable aid to predicting the products of replacement reactions.

Pre-laboratory:Read the relevant pages of your textbook and notes. (single replacement reactions)Then answer the questions that follow.1. What is a single replacement reaction? Give an algebraic example of one.2. Define aqueous ions.3. What evidence indicates that a single replacement reaction has occurred between the aqueous ionic compound and the metal?4. List the metals found in the activity series from most reactive to least reactive

Create a data table:1. For all reactions label the columns and rows by symbols 2. Six by ten table 3. Lab results label NR = no reaction, or R = reaction4. Unknown metal X for the second day of lab

Single Replacement Reactions Activity series of Metals

Single

Replacement Reaction Predictions

1. Iron (as an ion use Fe3+)

a. Nickel (ΙΙ) Chloride

i. Iron + Nickel (ΙΙ) Chloride Iron (ΙΙΙ) Chloride + Nickel

Metal Metal Ion Reactivity

LithiumPotassiumBariumStrontiumCalciumSodiumMagnesiumAluminumManganeseZincChromiumIronCadmiumCobaltNickelTinLead(Hydrogen)CopperMercurySilverPlatinumGold

Li+

K+

Ba+

Sr2+

Ca2+

Na+

Mg2+

Al3+

Mn2+

Zn2+

Cr2+, Cr3+

Fe2+, Fe3+

CdCo2+, Co3+

Ni2+, Ni3+

Sn2+, 4+

Pb2+

H+

Cu2+

Hg2+

Ag+

Pt2+

Au+, Au3+

Most Reactive

Least Reactive

ii. 2Fe (s) + 3NiCl2 (aq) 2FeCl3 (aq) + Ni (s)

b. Cobalt (ΙΙ) Chloride

i. Iron + Cobalt (ΙΙ) Chloride Iron (ΙΙΙ) Chloride + Cobalt

ii. 2Fe (s) + 3CoCl2 (aq) 2FeCl3 (aq) + 3Co (s)

c. Lead (ΙΙ) Nitrate

i. Iron + Lead (ΙΙ) Nitrate Iron (ΙΙΙ) Nitrate + Lead

ii. 2Fe (s) + 3Pb(NO3)2 (aq) 2Fe(NO3)3 (aq) + 3Co (s)

d. Calcium Chloride

i. Iron + Calcium Chloride NR

e. Aluminum Chloride

i. Iron + Aluminum Chloride NR

f. Magnesium Chloride

i. Iron + Magnesium Chloride NR

g. Iron (ΙΙΙ) Chloride

i. Iron + Iron (III) Chloride NR

h. Copper (ΙΙ) Chloride

i. Iron + Copper (ΙΙ) Chloride Iron (ΙΙΙ) Chloride + Copper

ii. 2Fe (s) + 3CuCl2 (aq) 2FeCl3 (aq) + 3Cu (s)

i. Hydrochloric Acid

i. Iron + Hydrochloric Acid Iron (ΙΙΙ) Chloride + Hydrogen

ii. 2Fe (s) + 6HCl (l) 2FeCl3 (aq) + 3H2 (g)

2. Magnesium


i. Magnesium + Nickel (ΙΙ) Chloride Magnesium Chloride + Nickel

ii. 1Mg (s) + 1NiCl2 (aq) 1MgCl2 (aq) + 1Ni (s)


i. Magnesium + Cobalt (ΙΙ) Chloride Magnesium Chloride + Cobalt

ii. 1Mg (s) + 1CoCl2 (aq) 1MgCl2 (aq) + 1Co (s)


i. Magnesium + Lead (ΙΙ) Nitrate Magnesium Nitrate + Lead

ii. 1Mg (s) + 1Pb(NO3)2 (aq) 1Mg(NO3)2 (aq) + 1Pb (s)

d. Calcium Chloride

i. Magnesium + Calcium Chloride NR


i. Magnesium + Aluminum Chloride Magnesium Chloride + Aluminum

ii. 3Mg (s) + 2AlCl3 (aq) 3MgCl2 (aq) + 2Al (s)


i. Magnesium + Magnesium Chloride NR


i. Magnesium + Iron (ΙΙ) Chloride Magnesium Chloride + Iron

ii. 3Mg (s) + 2FeCl3 (aq) 3MgCl2 (aq) + 2Fe (s)


i. Magnesium + Copper (ΙΙ) Chloride Magnesium Chloride + Copper

ii. 1Mg (s) + 1CuCl2 (aq) 1MgCl2 (aq) + 1Cu (s)


i. Magnesium + Hydrochloric Acid Magnesium Chloride + Hydrogen

ii. 1Mg (s) + 2HCl (l) 1MgCl2 (aq) + 1H2 (g)

3. Aluminum


i. Aluminum + Nickel (II) Chloride Aluminum Chloride + Nickel

ii. 2Al (s) + 3NiCl2 (aq) 2AlCl3 (aq) + 3Ni (s)


i. Aluminum + Cobalt (II) Chloride Aluminum Chloride + Cobalt

ii. 2Al (s) + 3CoCl2 (aq) 2AlCl3 (aq) + 3Co (s)


i. Aluminum + Lead (II) Nitrate Aluminum Nitrate + Lead

ii. 2Al (s) + 3Pb(NO3)2 (aq) 2Al(NO3)3 (aq) + 3Pb (s)

d. Calcium Chloride

i. Aluminum + Calcium Chloride Aluminum Chloride + Calcium

ii. 2Al (s) + 3CaCl2 (aq) 2AlCl3 (aq) + 3Ca (s)


i. Aluminum + Aluminum Chloride NR


i. Aluminum + Magnesium Chloride NR

g. Iron (ΙΙ) Chloride

i. Aluminum + Iron (III) Chloride Aluminum Chloride + Iron

ii. 1Al (s) + 1FeCl3 (aq) 1AlCl3 (aq) + 1Fe (s)


i. Aluminum + Copper (II) Chloride Aluminum Chloride + Copper

ii. 2Al (s) + 3CuCl3 (aq) 2AlCl3 (aq) + 3Cu (s)


i. Aluminum + Hydrochloric Acid Aluminum Chloride + Hydrogen

ii. 2Al (s) + 6HCl (l) 2AlCl3 (aq) + 3H2 (g)

4. Copper (as an ion use Cu2+)


i. Copper + Nickel (II) Chloride NR


i. Copper + Cobalt (II) Chloride NR


i. Copper + Lead (II) Nitrate NR

d. Calcium Chloride

i. Copper + Calcium Chloride NR


i. Copper + Aluminum Chloride NR


i. Copper + Magnesium Chloride NR


i. Copper + Iron (III) Chloride NR


i. Copper + Copper (II) Chloride NR


i. Copper + Hydrochloric Acid NR

5. Zinc


i. Zinc + Nickel (II) Chloride Zinc Chloride + Nickel

ii. 1Zn (s) + 1NiCl2 (aq) 1ZnCl2 (aq) + 1Ni (s)


i. Zinc + Cobalt (II) Chloride Zinc Chloride + Cobalt

ii. 1Zn (s) + 1CoCl2 (aq) 1ZnCl2 (aq) + 1Co (s)


i. Zinc + Lead (II) Nitrate Zinc Nitrate + Lead

ii. 1Zn (s) + 1Pb(NO3)2 (aq) 1Zn(NO3)2 (aq) + 1Pb (s)

d. Calcium Chloride

i. Zinc + Calcium Chloride NR


i. Zinc + Aluminum Chloride NR


i. Zinc + Magnesium Chloride NR


i. Zinc + Iron (III) Chloride Zinc Chloride + Iron

ii. 3Zn (s) + 2FeCl3 (aq) 3ZnCl2 (aq) + 2Fe (s)


i. Zinc + Copper (II) Chloride Zinc Chloride + Copper

ii. 1Zn (s) + 1CuCl2 (aq) 1ZnCl2 (aq) + 1Cu (s)


i. Zinc + Hydrochloric Acid Zinc Chloride + Hydrogen

ii. 1Zn (s) + 2HCl (l) 1ZnCl2 (aq) + 1H2 (g)

Conclusion:

Opening Paragraph

1. State purpose (single replacement lab)2. Pre-lab (predictions, activity series)3. Lab (observations)4. Unknown X

Background Paragraph

1. Introduce algebraic equation 2. Explain if there is or is not a reaction (activity series)3. Give actual example of both (explain)

Actual lab examples

1. 1 – F reactiona. Predictionb. Observation c. Why

2. 1 – Ha. Predictionb. Observation c. Why

3. Unknown Xa. State what it is b. Observationsc. Why

Closing

1. Errors made2. Science concepts learned or used

State Standards Addressed

Solving Problems

Recognize and investigate problems; formulate and propose solutions supported by reason and evidence.

Communicating

Express and interpret information and ideas.

Using Technology

Use appropriate instruments, electronic equipment, computers and networks to access information, process ideas and communicate results.

Working on Teams

Learn and contribute productively as individuals and as members of groups.

Making Connections

Recognize and apply connections of important information and ideas within and among learning areas.

STATE GOAL 11: Understand the processes of scientific inquiry and technological design to investigate questions, conduct experiments and solve problems.

11.A.5a Formulate hypotheses referencing prior research and knowledge.

11.A.5c Conduct systematic controlled experiments to test the selected hypotheses.

11.A.5e Report, display and defend the results of investigations to audiences that may include professionals and technical experts.

STATE GOAL 12: Understand the fundamental concepts, principles and interconnections of the life, physical and earth/space sciences.

12.C.4b Analyze and explain the atomic and nuclear structure of matter.

12.C.5a Analyze reactions (e.g., nuclear reactions, burning of fuel, decomposition of waste) in natural and man-made energy systems.

12.D.4b Describe the effects of electromagnetic and nuclear forces including atomic and molecular bonding, capacitance and nuclear reactions.

Single Replacement Reaction Predictions Complete1

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