1

Unit 8

Chemical Reactions Textbook Chapter 8!!!

Name: ______________________ Period: ___

Monday Tuesday Wednesday Thursday Friday

January 4 5 6 7 8

Student Holiday / Teacher Work Day

Day 1: Nomenclature Review Law of Conservation of Mass Lab HW: pg 5

Day 2: Writing Chem Rxn

HW: pg 8

Day 3: Balancing Reactions

HW: pg 10 - 11

Day 4: Redox HW: pg 14

11 12 13 14 15

Day 5: Types of Redox HW: pg 17

Day 6: Single Replacement Reactions HW: pg 21

Day 7: Single Replacement Continued Chalk Lab Hwk: pg 24

Day 8: Double Replacement HW: pg 27

Compound

Formation Lab

18 19 20 21 22

Celebrate No School MLK

Review STUDY GUIDE DUE (pg 30-33)

Test: Chemical Reactions

2

Day 1: Nomenclature Review!!!!!!!!!!

Before naming/writing any formula,

Identify the type of compound.

Ionic Metal and a Nonmetal

If Ionic: Does the metal need roman numerals in the name?

If Ionic: Does the compound have a Polyatomic Ion?

• Molecular Only Nonmetals (Use Prefixes in the name)

Ionic Compounds

Ionic bonds are formed between a metal and a nonmetal OR a cation + anion. Naming ionic compounds

* First name the cation and then the anion. (metal) (nonmetal)

* Change the ending of the anion to –ide. Example:

MgCl2

magnesium chloride

A polyatomic ion are groups of atoms that behave as one unit. They are treated like single ions in formulas, but use parenthesis ( ) when more than one is used in a formula.

Ba(OH)2 Barium hydroxide CaSO4 Calcium sulfate (NH4)3P Ammonium phosphide

Covalent Compounds

To name a covalent compound, name the first element, then name the second one and change its ending to -ide. Use prefixes to show how many atoms of each element you have.

P2O5 diphosphorus pentoxide CCl4 carbon tetrachloride To write the formula of a covalent compound, simply translate the prefixes and element names. Dinitrogen dioxide N2O2 Diphosphorus heptoxide P2O7

Prefixes used for naming

Covalent Compounds

3

Let’s Practice NomenclatureWrite the formula for the following compounds.

1. Fe3+ and NO3-

2. sodium oxide

3. dinitrogen trioxide

4. iron(III) chloride

5. calcium nitrate

Name the following compounds.

6. HgO

7. LiBr

8. SO2

9. Zn3(PO3)2

10. CoCO3

Law of Conservation of Mass Experiment

Problems:

1. How can the law of conservation of mass be verified?

2. How can we determine if a chemical change occurred?

Background:

Antoine Lavoisier formulated the Law of Conservation of Mass, which states that matter cannot be created or

destroyed. During a chemical reaction, the bonds of the reactants are broken, and the atoms are rearranged to

form new substances. Because matter must be conserved, the mass of the products, must be the same as the mass

of the reactants. In this lab you will verify the law of conservation of mass using the following reaction.

2NaOH (aq) + CuSO4 ---- Na2SO4 (aq) + Cu(OH)2 (s)

Pre-Lab Questions:

1. 2S (s) + 3O2 (g) 2SO3

In the above reaction, 2.6g of S reacts with 2.0g O2. How many grams of SO3 are recovered.

2. 2HCl + Mg MgCl2 + H2

In the above reaction, 5.0g of HCl react with 2.0g Mg. 3.0g of MgCl2 are recovered, how many grams of H2

were lost.

3. What are the four indications of a chemical change?

a.

b.

c.

d

4

Procedure:

1. Pour 10.0 ml of CuSO4 into a plastic measuring cup and label it.

2. Pour 10.0 ml of NaOH into a second plastic cup and label it. Carefully put each solution on the balance and

record the mass in the data table.

3. Pour the NaOH into the CuSO4. Use the stirring rod to mix the solutions. Describe what happens in your

qualitative observation section.

4. Put both containers (including the empty NaOH cup!) back on the balance and record the new mass. Did

the mass change? Record your answer in the observation section. Dispose of chemicals as teacher directs.

Data Table 1:

Procedure Mass

Mass of cup 1

Mass of cup 1 and NaOH

Mass of NaOH

Mass of cup 2

Mass of cup 2 and CuSO4

Mass of CuSO4

Mass of cup 1 and 2 after mixing

Calculations:

Calculate the total mass of the reactants. (Add 3. And 6. From data table) _____________g

Post-Lab Questions:

1. The mass before the reaction is calculated above. The mass after the reaction is 7. in your data table. Do

your values for the total mass before and after each reaction verify the Law of Conservation of Mass?

Explain in complete sentences.

2. What indicators of a chemical change were observed? Which indicators were not observed?

5

Day 1: Homework

Na + CuS → Na2S + 2 Cu

1. In the above chemical reaction; you reacted 25.0g Na with 15.5g CuS. What is the total mass of your

products?

2. The reaction for the burning of 15.0 g of ethanol (CH3CH2OH) looks like this:

2 CH3CH2OH (l) + 7 O2 (g) 4 CO2 (g)+ 6 H2O (l)

The mass of the products is 30.0g. How much oxygen was consumed in the reaction?

3. A solid has a mass of 35 g. When it is mixed with a solution, a chemical reaction occurs. If the final total

mass of products is 85 g, what was the mass of the solution that the solid was mixed with?

4. The word equation for the following reaction is as follows:

vinegar + baking soda → sodium acetate + water + carbon dioxide

The chemical equation for the reaction is:

C2H3O2H + NaHCO3 → NaC2H3O2 + H2O + CO2

Use the data table below to find the answers to the three ?.

Mass of Weigh Boat 2.0 g

Mass of Weigh Boat and baking soda (NaHCO3) 17.0g

Mass of Baking soda ?

Mass of graduated cycliner 50.0g

Mass of Weigh Boat and vinegar (C2H3O2H) 100.0g

Mass of vinegar (C2H3O2H) ?

Mass of NaC2H3O2 40.0g

Mass of H2O 15.0g

Mass of CO2 ?

5. A full, unopened bottle of Dr. Pepper® has a mass of 1,250.0 grams. After opening the bottle

(but before taking a sip!)- the beverage now weighs 1050.0 grams. In your own words, explain why

the soda seemed to have lost mass.

6

Day 2:

Nomenclature Review: Write the formulas for the compounds below.

aluminum oxide ___________

nitrogen trioxide ___________

copper(II) nitrate ___________

sodium carbonate ________

lead(IV) oxide ________

So now let’s write some chemical equations!

Summary: • When 1 or more _______________ are reacted to produce totally new compounds that have

_________________ chemical and physical _______________than they did before.

• A chemical reaction is represented by writing a _______________ _________________

– Using chemical formulas, symbols, and ________________________.

• An equation represents the identities and relative amounts of what are called _______________ and

products in a chemical reaction.

– ________________ are the substances you start with in the reaction.

- ________________ are the results of the reaction.

_____________ __________ _________ _____________

• To know for certain a chemical rxn has taken place requires ___________ that 1 or more substances have

__________________ _________________.

• Absolute proof of such a change can only be provided by chemically ___________________ ___

_____________________.

EVIDENCE OF CHEMICAL CHANGE

1. _____________________ This is usually indicated by bubbles. Bubbles don’t always mean a gas is being

produced (Air bubbles, bubbles when something boils).

2.______________________________This is called a precipitate (ppt). If 2 liquids are combined and a solid

substance suddenly appears, this means that a new substance has been formed.

3. ______________________ When a different color or odor appears suddenly, this means a new substance

with new properties has formed.

4. ___________________________________ If a substance becomes warmer in temperature even though no

heat is being added, that is a clue that a chemical change is occurring. Substances can also get lower in

temperature due to a chemical change.

7

Writing and Balancing Chemical Reactions: Common Symbols in Reactions

Symbol Meaning

Separates Reactant from Reactant

or

Separates Product from Product

“Yields” (indicates result of reaction)

Separates Reactants from Products

solid

pure liquid

gas

dissolved in water or in solution

heat is added to the reaction

A catalyst is added to the reaction.

A gas is produced.

A solid is produced.

Common Substances in Chemical Reactions

Name Formula(s) to memorize

Diatomic Elements

Water

Ammonia

Key Words Used in Describing Chemical Reactions

Words used to separate reactants from

other reactants.

Words used to separate reactants from

products.

Class Practice

For each of the following examples write the correct chemical formulas and symbols. 1. When heated, solid tungsten metal reacts with oxygen gas to produce solid tungsten (VI) oxide.

2. Solutions of sodium iodide and lead (II) nitrate are mixed and form the precipitate, lead (II) iodide and

aqueous sodium nitrate.

3. When heated, solid aluminum oxide decomposes to form aluminum metal and oxygen gas.

8

Day 2: Homework Directions: For each item in Column A, write the letter of the matching item in the word bank. Each

choice in Column B may be used once, more than once, not at all.

Column A

_____1. The new substances that are formed in a chemical reaction

_____2. A chemical reaction that involves one or more substances change into new substances

_____3. Shows the relationship between the reactants and products in a chemical reaction

_____4. States the mass is neither created nor destroyed during a chemical reaction

_____5. The starting substances in a chemical reaction

_____6. The substances appearing on the left side of the arrow

_____7. The substances appearing on the right side of the arrow

Word Bank

a. Chemical Change

b. Reactants

c. Products

d. Chemical Equation

e. Law of Conservation of Mass

Directions: For the following problems, write the chemical equation for each reaction. Answer the question

using the equation and the Law of Conservation of Mass. Show all work on your paper.

8. In a laboratory, 178.8g of water is separated in hydrogen gas and oxygen gas. The hydrogen gas has a

mass of 20.0g. What is the mass of oxygen gas produced?

9. When calcium is placed in water, it reacts to form calcium hydroxide and hydrogen gas. A student reacts

2.3g of calcium reacts with 13.8g of water. After the reaction is completed, the student determines

that a total of 1.2g of hydrogen gas was produced. How much calcium hydroxide was produced in this

reaction?

Directions: Answer questions #10-14 based on the reaction below.

H2SO4(aq) + Na2CO3(s) CO2(g) + Na2SO4(aq) + H2O(l)

10. What are the reactants in this chemical reaction?

11. What is the physical state of water in this chemical reaction?

12. What is the physical state of sodium carbonate in this chemical reaction?

13. What sign of a chemical change is demonstrated by this reaction?

14. What does (aq) mean?

9

Day 3: Review / BALANCING CHEMICAL EQUATIONS

Cr2O3 ___________

PO2 ___________

AlCl3 ___________

AgNO3 ___________

S2O5 ___________

_________________ _________________: He is the father of modern chemistry, and first described the “Law

of Conservation of Mass.”

Antoine Lavoisier found that the mass of the reactants and the products are ___________, even when the states

of matter change. Matter is neither created nor destroyed.

________________________________: The number of each type of atom on the reactants side of the

chemical equation MUST be equal to the number of each type of atom on the products side of the equation.

___________________________: Represents the number of units of each substance taking part in the reaction.

__________________ __________________ __________________: The same number of atoms of each

element on both sides of the equation.

Four Steps to Balance Equations:

1.

2.

3.

4.

Is this chemical equation balanced?

N2 + H2 NH3

Guided Practice: Balance these equations:

1. H2 + O2 H2O

2. Mg + HCl H2 + MgCl2

3. Na + HCl NaCl + H2

**How many of each element do we have? Are both sides equal?

10

Day 3 Homework Writing and Balancing Chemical Equations

1. ____N2 + ____O2 ____ NO2

2. Magnesium Nitrate + Calcium Hydroxide Calcium Nitrate + Magnesium Hydroxide **use polyatomic Ion list.

3. _____ H2 + _____ Cl2 _____ HCl

4. Magnesium Chloride + Sodium Iodide Magnesium Iodide + Sodium Chloride

5. _____ HgO _____ Hg + _____ O2

6. ____ Ca + _____ H2O _____ Ca(OH)2 + _____ H2

7. ____C + ____O2 ____CO

8. _____ Na2O2 + _____ H2SO4 _____ Na2SO4 + _____ H2O2

9. Sulfuric Acid(H2SO4) Sulfur Trioxide + Water

11

10. _____HCl + _____Mg _____MgCl2 + _____H2

11. _____ Al (s) + _____ O2 (g) _____ Al2O3

12. _____Ag2O (s) _____ Ag + _____O2

13. _____ S (s) + _____ O2 (g) _____ SO3

14. _____ N2O5 (g) + _____H2O (l) _____ HNO3

15. ______ CaO (s) + _____H2O (l) _____Ca(OH)2

16. ______ H2O2 (l) _______H2 + _____O2

17. ________CH4 + _____ O2 ____ H2O + ____ CO2

18. ____ SrF2 + ____ Na2SO4 ____ SrSO4 + ____ NaF

19. ____ Pb(NO3)2 + ____ K2CrO4 ____ PbCrO4 + ____ KNO3

20. ____ K2SO4 + _____ BaCl2 _____ KCl + ____ BaSO4

21. ____ KOH + ____ H2SO4 ____ K2SO4 + ___ H2O

22. ____ Fe + _____ H2SO4 ____ Fe2(SO4)3 + ____ H2

12

Day 4: Oxidation-Reduction Reactions (Redox Reactions) Reaction Types are put into three categories:

All of the reaction types we’ve discussed can be placed into one of 3 categories:

*Acid-Base (Neutralization)

*Precipitate

*Oxidation-reduction ( Redox) In this unit we will be looking at Precipitate and Redox.

A. _______________________ ( Synthesis,Decomposition and Single Replacement reactions) - In redox reactions the oxidation number for an element _________________ in a chemical reaction. __________________ Number: A number assigned to an element, based on the distribution of electrons. The same element can have very different properties in different oxidation states.

13

_________________is a reaction in which

there is the loss of electrons.

0 +1

Ex: Na Na+1 + e-

___________________is a reaction in

which there is the gain of electrons.

0 -1

Ex: Cl2 + 2e- 2Cl-

“LEO the lion says GER” “OIL RIG”

Losing of Electrons is Oxidation OR Oxidation Is Loss (of electrons)

Gaining of Electrons is Reduction Reduction Is Gain (of electrons)

Since oxidation is the _______________of electrons and reduction is the _____________ of

electrons, they must occur simultaneously.

** Any chemical process in which elements undergo changes in oxidation number is an

oxidation – reduction reaction, or redox reaction for short.**

Practice determining whether the following elements have been oxidized or reduced and label

the reaction.

14

Day 4 Homework

1. Label the following as an oxidation or reduction reaction.

Ag Ag+ + e- _______________

F2 + 2e- 2F- _______________

Cu Cu2+ + 2e- _______________

2. Complete the tables below.

15

Day 5: Types of Redox Reactions Synthesis (also called Combination or Composition)

Synthesis means “_______________ _______”

2 or more elements/simple compounds combine to form 1 compound.

General form: A + B AB

Identifying feature: only one ________________

Analogy: A boy and a girl come to the dance separately, but end up dancing together.

EX: 2 Mg + O2 2 MgO

EX: The combination of iron and sulfur to form iron (II) sulfide: Fe + S FeS

EX: Burning Charcoal: C (s) + O2 (g) CO2 (g)

2. Decomposition

Decomposition means “_______________ __________”

1 compound is broken down into 2 or more simpler elements/compounds.

General form: AB A + B

Identifying feature: only one ________________ (opposite of Synthesis!)

Analogy: A boy and a girl are a couple, but they had an argument. This resulted in the boy and the girl

staying apart for the rest of the night.

Examples: 2 NaCl 2 Na + Cl2

2 KClO3 2 KCl + 3 O2

EX: The electrolysis of water to make oxygen and hydrogen gas: 2H2O (l) 2H2 (g) + O2 (g)

3. Combustion

Also known as _________________.

Always follows the same form:

Compound containing C and H (& sometimes O) + O2 CO2 + H2O

16

Note: In a combustion reaction, the compound always burns in oxygen gas and always releases

carbon dioxide and water.

During incomplete combustion (a limited amount of O2), carbon monoxide (CO) is also produced.

Examples: CH4 + 2 O2 CO2 + 2 H2O

2 C3H6 + 9 O2 6 CO2 + 6 H2O

**Trick for balancing tough combustion reactions:**

Balance from right to left. 1. Balance the H first by placing a coefficient in front of the water. 2. If that coefficient is ODD, double it and proceed with balancing C, then O. 3. If even, leave it alone and proceed with C, O. 4. Always balance oxygen last!!!

Example:

1. _____ C7H14 + _____ O2 _____ CO2 + _____ H2O

In class practice for balancing combustion.

1. _____ C4H8 + _____ O2 _____ CO2 + _____ H2O

2. _____ C5H12 + _____ O2 _____ CO2 + _____ H2O

3. _____ C9H18 + _____ O2 _____ CO2 + _____ H2O

4. _____ C11H22 + _____ O2 _____ CO2 + _____ H2O

17

Day 5: Types of Reactions Homework Balance and Identify the following: synthesis = S

decomposition = D

combustion = C

Find Oxidized and Reduced Elements in 1., 3, and 5.

Reaction Type

1. _____ Al (s) + _____ O2 (g) _____ Al2O3 ________

Element Ox# Reactants Ox# Products Lost/Gain e- Oxid/Red

2. _____ S (s) + _____ O2 (g) _____ SO3 ________

3. _____ Cu (s) + _____ S (s) _____ Cu2S * ________

Use Cu1+

Element Ox# Reactants Ox# Products Lost/Gain e- Oxid/Red

4. _____ SO3 (g) + _____H2O (l) _____H2SO4 ________

5. _____Ag2O (s) _____ Ag + _____O2 ________

Element Ox# Reactants Ox# Products Lost/Gain e- Oxid/Red

6. _____ C6H6 + _____ O2 _____ CO2 + _____ H2O ________

7. _____ C8H18 + _____ O2 _____ CO2 + _____ H2O ________

8. _____ C6H12O6 + _____ O2 _____ CO2 + _____ H2O ________

18

Day 6: Single Replacement Single Replacement

1 element takes the place of another in a compound (“like replaces like”)

General forms: A + BC B + AC (metal replacement)

D + BC C + BD (halogen replacement)

Identifying feature: 1 element + 1 compound on each side of the arrow

Analogy: A boy and a girl are dancing, but then another boy “cuts in” and dances with the girl, leaving

the first boy alone. Or a boy and a girl are dancing, but then another girl “cuts in” and dances with the boy, leaving the first girl

alone. “Like” must replace “like”

Examples:

Metal replacement: 2 Na + CuCl2 2 NaCl + Cu

Halogen replacement: F2 + 2 KCl 2 KF + Cl2

BUT the boy/girl will not always be able to “cut in.” Sometimes the other boy/girl will not let them!

Rules for Reactions Including: Metals with Metals / Metals with Acids

We must use the _______________ ___________________ to predict whether or not the

replacement will occur.

A= Metal

B= Cation

C= Anion

19

Predicting Single Replacement Reactions

**Important Reminder: A metal can only replace another _____________________ or

_________________.**

Rule #1: Metals will replace metals that are ______________________________ than

themselves on the Activity Series. (The substances will switch partners)

A and B are metals, and X represents a negative ion.

-Will the reaction proceed? If yes, what are the products?

A + BX

A + BX

This is what it

looks like! You

can find this on

the BACK of the

Periodic Table of

the Elements.

(Higher) (Lower)

(Lower) (Higher)

You can use the activity

series to predict whether

or not certain reactions

will occur. A specific

metal can replace any

metal listed below it

that is in a compound. It

cannot replace any metal

listed above it. For

example, copper atoms

replace silver atoms in a

solution of silver nitrate.

However, if you place a

silver wire in aqueous

copper (II) nitrate, the

silver atoms will not

replace the copper. Silver

is listed below copper in

the activity series, so no

reaction occurs. The

letters NR (no reaction)

are commonly used to

indicate that a reaction

will not occur.

**This applies to the

nonmetal halogens as well.

They increase as you move

up the family.

Metals found higher up

in the activity series

means the metal is

MORE REACTIVE.

20

Using your Activity Series, predict which reactions will occur:

1. Mg(s) + AlCl3(aq)

2. FeCl2(aq) + Cu(s)

3. Sodium + Lithium Chloride

4. Silver Nitrate + Zinc

Predicting the Products (metals and metals):

1. ___Mg(s) + ____ AlCl3(aq)

2. Silver Nitrate + Zinc

3. ___Fe(s) + ___Pb(NO3)2(aq)

Rule #2: Any metal above ______________________ will react with an acid to

produce a compound + H2. Put H2 at the end of your arrow.

Example:

M= metal

X= negative ion

Using your Activity Series, predict which reactions will occur:

1. Zn + HCl

2. Cu + H2SO4

3. Calcium + Phosphoric Acid

Predicting the Products (metals and acids):

1. ____Zn + ____HCl

2. Calcium + Phosphoric Acid

21

Day 6: Homework

1. Circle any reactions that will NOT occur.

Ba + NaNO3 Fe + Pb(C2H3O2)2 KCl + Ni

Mg + HCl HBr + Au Cu + AgNO3

2. Using your activity series, determine if the reactions below will occur. If the reaction

will not occur, write no reaction. If the reaction will occur, predict the products of the

reaction and write a balanced chemical reaction.

a. ___Ag + ___Cu(NO3)2

b. ___MgCl2 + ___Ba

c. ___Zn + ___HCl

d. ___Al + ___Cu(NO3)2

e. ___Au + ____HBf _________________________________________

22

Day 7: Redox Reactions continued…

Rule #3: Any metal that is ______________________________________ will react with

water.

Helpful Hint: Think of water as ______- _______ _______.

Using your Activity Series, predict which reactions will occur:

1. Na + H2O

2. Calcium metal is placed in water.

3. A sample of cadmium is placed in a test tube of water.

Predicting the Products (metals and water):

1. _____Na + _____ H2O

2. Calcium metal is placed in water.

Rule #4: Halogens will only replace other _________________________ that are

___________________ in the Activity Series. Halogens will NOT replace

_________________________! Use the family on the periodic table.

Using your Halogen Activity Series, predict if the following reactions will occur:

1. F2 + AlCl3

2. Chlorine gas is bubbled through a solution of sodium iodide.

3. Liquid bromine is mixed with a solution of potassium chloride.

Predicting the products (halogens):

1. ____F2 + ______ AlCl3

2. Chlorine gas is bubble through a solution of sodium iodide.

23

Experiment on the Types of Reactions (Chalk Lab)

Purpose

How do you identify the various types of reactions?

Procedure

1. Obtain a small piece of white chalk, which is basically calcium carbonate.

2. Holding the chalk with a set of tongs, heat a piece of chalk in the hottest part of the Bunsen burner for

three to five minutes.

3. While heating, add 100mL of water to a 150mL beaker.

4. Add 2-3 drops of phenolphthalein to the water. Record the initial color of the solution.

5. After heating the chalk, place the chalk into the water solution.

6. Using a stirring rod, stir the mixture in the beaker. Note any change in color of the solution.

Initial Color of the Solution Final Color of the Solution

Analysis Questions

1. When the chalk or calcium carbonate is heated, it forms solid calcium oxide and carbon dioxide gas. Write

the balanced chemical equation. Be sure to indicate the physical state of each substance and show how you can represent the heat of the Bunsen burner.

2. What type of reaction is being described in question #1?

3. In order to decompose the chalk, you relied on the combustion of methane as your source of heat. Write

the balanced chemical equation for the combustion of methane, CH4.

4. The solid calcium oxide, which is produced while the chalk is being heated, undergoes another reaction when

it is placed in the water. The solid calcium oxide reacts with water to produce aqueous calcium hydroxide.

Write the balanced chemical equation for this reaction. Be sure to include the physical states of all reactants and products.

5. What type of reaction is being described in question #4?

ANSWER IN COMPLETE SENTENCES!!

24

Day 7: Homework 1. Circle any reactions that will NOT occur.

LiCl + F2 NaF + I2

Na + H2O H2O + Fe

3. Using your activity series, determine if the reactions below will occur. If the reaction

will not occur, write no reaction. If the reaction will occur, predict the products of the

reaction and write a balanced chemical reaction.

a. ___H2O + ___Li

b. ___H2O + ___Pb _______________________________________________

c. ___H2O + ___Ca _______________________________________________

d. ___KI + ___Br2

e. ___I2 + ___NaF

f. ___LiI + ___Br2 _______________________________________________

25

Day 8: Precipitate or Double Replacement Reactions

Ions from 2 ionic compounds switch places.

General form:

AB + CD CB + AD

*A and C (the cations from each compound) switch places *

*Combine inner ions with outer ions*

Identifying feature: 2 compounds on each side of the equation

Analogy: 2 boy-girl pairs are dancing, and they switch partners.

Example: FeCl2 + Na2CO3 2 NaCl + FeCO3

How to determine if a substance is

soluble?

You will use this chart

A soluble compound An insoluble compound

26

Determine if the following compounds are soluble or insoluble

by using the solubility table.

A) Sr(NO3)2 ( )

B) AgOH ( )

C) PbCl2 ( )

D) Na3PO4 ( )

Predicting the Products of Double Replacement Reactions

A is a solid that forms when two solutions are mixed.

NaCl(aq) + AgNO3 (aq) AgCl(s) + NaNO3(aq)

TIPS FOR DOUBLE REPLACEMENT REACTIONS

Don’t use the activity series!

Determine if a precipitate will form.

o Precipitate will be an insoluble product!

o It should be marked as a solid (s).

If a precipitate forms, a reaction occurs.

If a precipitate does not form, then no visible reaction will occur.

General Formula AX + BY BY + AX

The ions should switch places!

Examples

CuCl2 (aq) + Na3PO4 (aq) ________________________________________

NaNO3(aq) + KCl(aq) ___________________________________________

KOH(aq) + Fe(NO3)3(aq) ________________________________________

CaCl2(aq) + (NH4)2SO4(aq) ________________________________________

27

Day 8: Precipitate Homework

1. Predict if the following compounds are soluble (aq) or insoluble (s). Label with (s) or (aq).

a. KCl ( ) e. NH4OH( )

b. K2S ( ) f. Ba(OH)2( )

c. CaS( ) g. PbS ( )

d. BaSO4( ) h. FeBr3( )

2. Determine if the following pairs of solutions will form a precipitate.

If they do form a precipitate, write the balanced reaction.

If they do not form a precipitate, write NVR for no visible reaction.

a. AgNO3(aq) + CaCl2(aq) _____ ______

b. Pb(NO3)2(aq) + KC2H3O2(aq) ______

c. CuSO4(aq) + KOH(aq) _____ ______

d. Na3PO4(aq) + FeCl3(aq) _________

e. AlCl3 + NaOH __________________________________________

28

Day 9: Compound Formation Lab

Objectives

Predict the products of the double replacement reactions.

Identify the formation of a precipitate experimentally.

Background

In chemistry there are four signs that indicate that a chemical change has most likely taken place.

1. A Change in Color

2. Formation of a Gas (bubbles)

3. Release or Absorption of Energy (temperature change)

4. Odor

5. Formation of a Precipitate (solid)

A precipitate is a solid that is formed when two aqueous solutions are mixed. It usually separates from the mixture

by settling to the bottom of the container. Precipitates often appear to be cloudy, milky, gelatinous or grainy.

Pre-Lab Questions

1. In the following equation, circle the precipitate.

BaCl2(aq) + Na2SO4(aq) 2 NaCl(aq) + BaSO4(s)

2. Write the chemical equation for the following double replacement reactions. Predict the products of the

reactions, and using your solubility chart identify which product is the precipitate (insoluble), if there is

one. If no precipitate is formed, then write NO VISIBLE REACTION (NVR) as your product.

a. A solution of ammonium hydroxide is mixed with aqueous iron (III) chloride.

b. Ammonium hydroxide dissolved in water reacts with a solution of zinc (II) chloride.

c. Aqueous lead (II) chloride is mixed with aqueous ammonium hydroxide.

d. A solution of sodium hydroxide is mixed with aqueous zinc (II) chloride.

e. Aqueous sodium hydroxide reacts with iron (III) chloride.

29

f. A solution of lead (II) chloride is mixed with aqueous sodium hydroxide.

g. A solution of sodium iodide reacts with aqueous copper (II) chloride.

Procedure

1. Follow the directions on the Reaction Surface Chart.

2. Be sure to place all pipettes tip up to prevent contamination!

3. Record the appropriate data in your data table below.

4. To clean up, soak up your solutions using a paper towel. Dispose of the paper towel in the trash can.

5. Wash your overhead with water.

6. Dry your overhead completely!

Data

In each box, record the precipitate (insoluble, or solid, compound) produced by the reaction, and the color of the

precipitate if one is formed. Record “NVR” for no visible reaction if no precipitate is formed.

ZnCl2 FeCl3 PbCl2 NaI

NH4OH

NaOH

CuCl2

Analysis **WRITE IN COMPLETE SENTENCES**

1. If a product is soluble, why do you think we don’t see a precipitate?

2. If a product is insoluble, why do you think that a precipitate is visible?

3. Predict the products (and circle the precipitate) if a solution of sodium sulfate is mixed with calcium

nitrate. (Be sure to write the BALANCED chemical equation!)

30

CHEMICAL REACTIONS STUDY GUIDE

If completed in its entirety is +5 on Test!

Nomenclature Practice:

Write the correct formula

1. Aluminum chloride____________

2. Lead (II) nitrate_____________

3. Sulfur dioxide_______________

4. Sulfurous acid_______________

5. Copper (II) oxide_____________

6. Dinitrogen tetroxide___________

7. Calcium sulfate_______________

8. Hydrofluoric acid______________

9. Barium phosphate_____________

10. Nitric acid_________________

11. Write a balanced chemical equation for each word problem. Be sure to include all

appropriate symbols, formulas, and balancing!

a. Sodium reacts with water to form hydrogen gas and sodium hydroxide.

b. Solid lead (IV) oxide is heated, decomposing to lead metal and oxygen gas.

c. In the presence of a catalyst, nitrogen and hydrogen gases react to form gaseous

ammonia.

12. Complete the Single Replacement reactions. Then use the activity series of metals

and Halogens to determine which of the below reactions will occur. If a reaction will

occur, write the balanced equation.

a. Au(s) + KNO3(aq)

b. Zn (s) + AgNO3(aq)

What symbols represent the

following terms?

A reaction is heated: _________

A catalyst is used: _________

A solution of: _________

A precipitate: _________

Gaseous: _________

Vapor: __________

31

c. Al(s) + H2SO4(aq)

d. MgBr2 + F2

e. Cu(s) + H2O(l)

f. Al(s) + CuSO4(aq)

g. NaCl + Br2

e. H2O + Na

13. Balance the following combustion reactions.

a. C4H8 + O2 CO2 + H2O

b. C8H18 + O2 CO2 + H2O

14. Predict the products in the following double replacement reactions. Identify the

precipitate formed when solutions of these ionic compounds are mixed. If there is NO

PRECIPITATE (no insoluble solid), write NVR!

a. CaSO4 + BaCl2

b. Al2(SO4)3 + NH4Cl

c. AgNO3 + K2 S

d. CaCl2 + Pb(NO3)2

e. Ca(NO3)2 + NaBr

32

15. Write a balanced equation and identify its type.(Combustion: C, Decomposition: D,

Synthesis: S, Double Replacement: DR, Single Displacement: SR)

And by Category ( ppt, redox)

16. Based on the oxidation numbers known for the other element(s), determine the

oxidation number of the underlined element.

a. NaSO4 _____ e. CaO _____

b. K2CrO4 _____ f. Cr2O3 _____

c. KCl _____ g. H2O _____

d. Ag _____

Balance the following

C,S,D,

SR,DR

ppt, acid-base,

redox

a. __ Hf + __ N2 __ Hf3N4

b. __ Mg + __ H2SO4 __ MgSO4

c.__ C2H6 + __ O2 __ CO2 + __ H2O

d. __Hg(NO3)2 + __ NH4OH __ Hg(OH)2 + ___ NH4NO3

e. ___H2O2 ____ H2 +____ O2

f. ____KBr + ____Cl2 ____KCl + ____ Br2

17. Half-reactions can be written to represent all —

A ) neutralization reactions.

B) fission and fusion reactions.

C) double-replacement reactions.

D) oxidation and reduction reactions.

18. In an oxidation-reduction reaction, reduction is defined as the —

A gain of protons.

B gain of electrons.

C loss of electrons.

D loss of protons.

33

22. Which half-reaction correctly represents oxidation?

A Fe(s) + 2 e- → Fe2+(aq)

B Fe(s) → Fe2+(aq) + 2 e-

C Fe2+(aq) + 2 e- → Fe(s)

D Fe2+(aq) → Fe(s) + 2 e-

Quick Nomenclature Review:

19. Which changes occur when Pt2+ is reduced?

A The Pt2+ loses electrons and its oxidation number decreases.

B The Pt2+ gains electrons and its oxidation number decreases.

C The Pt2+ gains electrons and its oxidation number increases.

D The Pt2+ loses electrons and its oxidation number increases.

20. The ionic chemical equation below is balanced.

Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)

Which equation represents the oxidation half-reaction?

A Zn(s) → Zn2+(aq) + 2 e-

B Cu2+(aq) + 2 e- → Cu(s)

C Cu2+(aq) → Cu(s) + 2 e-

D Zn(s) + 2 e- → Zn2+(aq)

21. The chemical equation below represents a redox reaction.

4 HCl + MnO2 → MnCl2 + 2 H2O + Cl2

What occurs during this reaction?

A The manganese is oxidized, and its oxidation number changes from +2 to +4.

B The manganese is reduced, and its oxidation number changes from +4 to +2.

C The manganese is oxidized, and its oxidation number changes from +4 to +2.

D The manganese is reduced, and its oxidation number changes from +2 to +4.

+1

+2 +3 +4 -3 -2 -1

34

Ionic Compounds: Name the metal unchanged, Name the nonmetal with “ide” on the end.

Ionic with multivalent metals: Name the metal unchanged and write the roman numeral for the oxidation of the metal, Name the nonmetal with “ide” on the end.

Covalent/Molecular Compounds: Use the prefixes listed below to name the compounds

1* 2 3 4 5 6 7 8 9 10

Mono- Di- Tri- Tetra- Penta- Hexa- Hepta- Octa- Nona- Deca-

Ionic Compounds with polyatomic Ions: Write both the metal and the polyatomic ions AS IS .

Acids: Use the chart below

ION TYPE ION ENDING ACID NAME BEGINNING ACID ENDING

Polyatomic -ite NO hydro- beginning -ous

-ate NO hydro- beginning -ic

Monatomic -ide hydro- beginning -ic

Roman Numeral

I

II

III

IV

V

VI

VII

VIII

Oxidation #

1+

2+

3+

4+

5+

6+

7+

8+

35