Download PIB - Unit 6 - Chemical Reactions - Student

Instructor Lesson Plan – (PIB/HH Chemistry)
Unit 6: Chemical Reactions
Instructor:
Ditkowsky
Introductory Resources:
Addison-Wesley v.5 - Chapter 8
Addison-Wesley v.4 - Chapter 7
Advanced Resources:
Brown v.4 - Chapter 3
Zumdahl v.3 - Chapter 3
Zumdahl v.5 - Chapter 3
Main Idea Summary:
 A chemical reaction can be concisely represented by a chemical equation.
 The substances that undergo a chemical reaction are the reactants. The new substances
formed are the products.
 Special symbols are written after formulas in equations to show a substance’s state. The
designations for solid, liquid, or gas, are (s), (l), and (g), respectively. A substance dissolved
in water is designated (aq).
 A catalyst is a substance that increases reaction rate without being used up by the reaction. If
a catalyst is used, its formula is written above the arrow.
 In accordance with the law of conservation of mass, a chemical equation must be balanced.
In balancing an equation, coefficients are used so the same number of atoms of each element
are on each side of the equation.
 In a synthesis reaction, there is always a single product.
 A decomposition reaction involves the breakdown of a single reactant.
 In a single replacement reaction, the reactants and products are an element and a compound.
The activity series of metals can be used to predict whether single replacement reactions will
take place.
 A double replacement reaction involves the exchange of cations between two compounds.
This reaction generally takes place between two ionic compounds in aqueous solution. The
solubility rules can be used to predict whether double replacement reactions will take place,
and what product will be insoluble in water.
 A combustion reaction always involves oxygen. The products of the complete combustion of
a hydrocarbon are carbon dioxide and water.
 A complete ionic equation shows all dissolved ionic compounds as their free ions. A netionic equation shows only the ions that take part in the actual reaction, and not the spectator
ions, ions that do not participate in the reaction.
HW6A: Outline Chapter 8. Add notes from the supplementary text below.
Supplementary Text:
A chemical reaction is the process by which one or more substances are changed into one or
more different substances. The original substances are called REACTANTS and the resulting
substances are called PRODUCTS. According to the Law of CONSERVATION OF MASS, the
total mass of the reactants are equal to the total mass of the products.
A chemical EQUATION represents with symbols and formulas, the identities and relative
amounts of reactants and products in a chemical reaction.
The following are indications of a chemical reaction:
1. Evolution of heat and light. A change in matter that releases energy as both heat and
light is strong evidence that a chemical reaction has occurred. However, some physical changes
also release either heat or light.
2. Production of a gas. The evolution of gas bubbles when two substances are mixed is
often evidence of a chemical reaction.
3. Formation of a precipitate. Many chemical reactions take place between aqueous
substances. If a solid appears after two solutions are mixed, a reaction has likely occurred. The
solid in this case is called a PRECIPITATE.
Characteristics of Chemical Equations.
1. The equation must represent known facts.
2. The equation must contain the correct formulas for the reactants and products.
3. The law of conservation of mass must be satisfied. Atoms are neither created nor destroyed in
ordinary chemical reactions. To equalize numbers of atoms coefficients are added when
necessary. COEFFICIENTS are small whole number ratios that appear in front of a formula in a
chemical equation.
Word and Formula Equations
It is often helpful to begin with a word equation which describes the reactants and products. This
qualitative description helps you to write a formula equation. A word equation has the general
format of reactant  product; where the  means yield, reacs to formt, or forms. A formula
equation represents the reactants and products of a chemical reaction using symbols/formulas.
Once a formula equation is written, it can be balanced by adjusting the coefficients.
Word Equation: Solid carbon reacts with steam to make carbon dioxide and hydrogen gas.
Formula Equation: C(s) + H2O(g)  CO2(g) + H2(g)
Balanced Chemical Equation: 1 C(s) + 2 H2O(g)  1 CO2(g) + 2 H2(g)
(Reactants: 1C, 4H, 2 O)(products 1C, 2 O, 4 H) matter is
conserved!
Types of Chemical Reactions
There are five major types of reactions:
1. Composition or Synthesis
2. Decomposition
3. Single Replacement or Single Displacement
4. Double Replacement or Double Displacement or Metathesis
5. Combustion
____________________________________________________________________
Synthesis or Composition reactions have the general form A + B  AB
Examples of synthesis reactions include the addition of oxygen to another atom:
ex: 2 Mg + O2 2 MgO
S8 + 8 O2  8 SO2
4 Fe + 3 O2  2 Fe2O3
Both metals and nonmetals can combine with oxygen in synthesis reactions.
Another type of synthesis reaction involves the reaction of metals with halogens. This is another
type of reaction that can also occur with nonmetals.
ex: 2 Na + Cl2  2 NaCl
U + 3 F2  UF6
Ca + Cl2  CaCl2
O2 + F2  OF2
In both cases above, two elements are combining. It is also possible for two compounds to
combine, or a compound and an element.
ex: CaO + H2O  Ca(OH)2
SO2 + H2O  H2SO3
2 H2SO3+ O2  2 H2SO4
CaO + SO2  CaSO3
___________________________________________________________________
Decomposition reactions have the general form AB  A + B
The simplest type of decomposition reaction involves a binary compound (bi = two)
decomposing to its elements:
ex:
2 H2O  2 H2 + O2
(electrolysis)
2 NaCl  2 Na + Cl2 (also done using electrolysis)
2 HgO  2 Hg + O2
CaS
 Ca + S
There are patterns of decomposition reactions which make it very easy to predict what products
you will get in a given decomposition reaction. Substances which are low energy are formed
often, for example, water and carbon dioxide are frequently products of chemical reactions.
Decomposition of Carbonates: MnCO3
Carbonates decompose to form the metal oxide and carbon dioxide.
ex: CaCO3  CaO + CO2
Na2CO3  Na2O + CO2
Decomposition of Metal Hydroxides: Mn(OH)m
Metal hydroxides decompose to form metal oxides and water.
ex: Ca(OH)2  CaO + H2O
2 NaOH  Na2O + H2O
Decomposition of Metal Chlorates: Mn(ClO3)m
Metal chlorates decompose to form chorides and oxygen.
ex:
Ca(ClO3)2  CaCl2 + 3 O2
2 NaClO3  2 NaCl + 3 O2
Decomposition of Acids: HXOn
Certain acids decompose into nonmetal oxides and water. (Carbonic Acid decomposes
like both an acid and a carbonate)
ex:
H2CO3  CO2 + H2O
H2SO4  SO3 + H2O
_________________________________________________________________
Single Replacement Reactions have the general form A + BC  AC + B or
A + BC  BA + C
In this type of reaction, the more active element can replace a less active element in a compound.
This reaction is what I call the “home-wrecker reaction” because, we start with an element (a
single) and a compound (a married couple). When the reaction is complete, the “marriage” has
been broken up, and a new married couple and a newly (divorced) single exist.
ex: 2 K
+ H2O 
2 KOH +
H2
Mr. Potassium meets Mr. and Mrs. Hydrogen-hydroxide (water). Hydrogen gets jealous and
walks out. Mr. Potassium consoles Ms. Hydroxide and they marry.
There are a few specific subcategories which may help you remember what to do for this type of
prediction.
Replacement of a metal in a compound by another metal
ex: 2 Al + 3 Pb(NO3)2  3 Pb + 2 Al(NO3)3
Replacement of hydrogen in water by another metal
ex: 2 Na + 2 H2O → 2 NaOH + H2
3 Fe + 4 H2O → Fe3O2 + 4 H2
Replacement of Hydrogen in an Acid by a Metal
ex: Mg + 2 HCl → H2 + MgCl2
Replacement of Halogens
ex:
Cl2 + 2 KBr → 2 KCl + Br2
F2 + 2 NaCl → 2 NaF + Cl2
Note that in this case, since it is the anion which is being replaced, it is always placed
second in the formula.
To tell whether a reaction will occur, you must consult the activity series.
Activity of metals
Activity of
Halogen
nonmetals
Li (most active)
F2
Rb
Cl2
K
Br2
Ba
I2
Sr
Ca
Na
Above this line, these react with cold water replacing hydrogen. They
also react spontaneously with elemental oxygen to produce oxides.
Mg
Al
Mn
Zn
Cr
Fe
Cd
Above this line, these react with steam (not cold water) and acids,
replacing hydrogen. These react with oxygen, forming oxides.
Co
Ni
Sn
Pb
Above this line, these do not react with water, they react with acids,
replacing hydrogen. These react with oxygen forming oxides.
H2
Sb
Bi
Cu
Hg
Above this line, these can react with oxygen to form oxides.
Ag
Pt
Au
Double Replacement Reactions have the general form AX + BY → AY + BX
A and B represent metals (cations). X and Y represent nonmetals or polyatomic cations.
I like to call this reaction the Prom Date reaction. A couple goes to prom and argue. At the end
of the evening the couple separates. Two couples leave with each other’s date. If two people
who went to prom together dance with each other’s date at prom, that is within acceptable
behavior. Only when the couples break apart during the evening and remain broken up when
Prom is over, only then do we consider that a reaction occurs. Just as it is accepted that during
prom, individuals mingle and have a good time; in solution, the ions in a double replacement
reaction float around in water, briefly interacting with other ions. When the reaction forms a
precipitate, those ions are effectively removed from the solution. Reactions occur when collisions
occur, solids are tethered, and can’t collide with enough force to react. (Like when two
individuals pair up and spend the rest of the evening gazing soulfully into each other’s eyes and
don’t notice the rest of the crowd). Another type of successful double replacement reaction
occurs when a gas is formed. Since the gas is a vapor, those molecules are removed from the
reaction.
Formation of a Precipitate:
ex: 2 KI (aq) + Pb(NO3)2 (aq) → PbI2 (s) + 2 KNO3 (aq)
In this reaction, K+, I-, Pb2+ and NO31- are in aqueous solution. When they mix, the Pb2+and I1stick together to form solid PbI2. The solid PbI2 falls to the bottom of the solution and remains
there. The K+ and NO31- continue to have collisions and break apart.
Formation of a Gas:
ex: FeS (s) + 2 HCl (aq) → H2S (g) + FeCl2 (aq)
Formation of Water:
ex: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
This type of reaction is also called a neutralization reaction, or an acid-base reaction. When an
acid reacts with a base, the products are a salt (cation-anion) and water.
Combustion Reaction
When a hydrocarbon reacts with water, lots of heat is generated along with carbon dioxide and
water. This is the process our body uses to process sugars, fats and carbohydrates. Our body
uses enzymes to control the reactions so we can use the energy generated. In most combustion
reactions, in addition to heat, light is also produced. Combustion requires an initial input of
energy. Enzymes reduce the initial amount of energy and slow the reaction so we can use the
energy to power our bodies. In the case of hydrocarbons in cars or gas stoves, the gas doesn’t
ignite until a spark is applied to the gas vapor. Once ignited, boatloads of energy are given off in
the form of heat and light.
ex: 2 H2 + O2 → 2 H2O
C3H8 + O2 → 3 CO2 + 4 H2O
Worksheet 6.1 – Variety
NAME _______________________
Put numbers in the blanks to balance the following equations. Learn to recognize the
distinguishing features of each reaction type.
SYNTHESIS (also known as COMBINATION):
___S + ___O2 → ___SO2
___S + ___O2 → ___SO3
___P + ___O2 → ___P2O5
DECOMPOSITION:
___KClO3 → ___KCl + ___O2
___H2O2 → ___H2O + ___O2
___NaNO3 → ___NaNO2 + ___O2
SINGLE REPLACEMENT (also known as DISPLACEMENT):
___Na + ___H2O → ___NaOH + ___H2
___Zn + ___NaOH → ___Na2ZnO2 + ___H2
___Zn + ___HCl → ___ZnCl2 + ___H2
DOUBLE REPLACEMENT (also known as METATHESIS):
___Fe(OH)3 + ___H2SO4 → ___Fe2(SO4)3 + ___H2O
___MgCl2 + ___NaOH → ___Mg(OH)2 + ___NaCl
___AgNO3 + ___H2S → ___Ag2S + ___HNO3
COMBUSTION:
___C3H8 + ___O2 → ___CO2 + ___H2O
___C6H14 + ___O2 → ___CO2 + ___H2O
___C9H20 + ___O2 → ___CO2 + ___H2O
Laboratory Activity 6A – Synthesis
1. Wear Goggles
2. Observe a strip of magnesium ribbon. Write down any and all observed physical properties.
3. Use the sparklighter to ignite the Bunsen burner.
4. Use the crucible tongs to hold the magnesium ribbon in the Bunsen burner flame. Caution:
DO NOT look directly at the chemical reaction, because it may cause damage to your eyes
and permanently harm your vision. Remove the magnesium from the flame.
5. When the magnesium oxide has cooled, observe its properties.
6. Clean up your equipment and return it to your teacher.
7. Write a balanced equation explaining what happened in lab, causing the transformation of
magnesium into magnesium oxide.
Laboratory Activity 6B – Decomposition
1. Wear Goggles.
2. Put a small quantity of copper (II) sulfate pentahydrate into a crucible. Record the
appearance of the substance.
3. Place the crucible on a wire triangle on a ring-stand with the cap balanced above the crucible
(so hot air can escape).
4.
Place the Bunsen burner below the crucible and use an igniter to light the burner.
5.
Record observations. Do you see an moisture forming? Is the color changing?
6.
Allow the crucible to cool before removing it with metal tongs.
7.
Clean all equipment and return it to the cart.
Data:
Reactant (observations)
A.
B.
During the reaction
(observations)
Products (observations
Conclusions for Reactions A and B:
Write a paragraph explaining what happened in the experiment and how you know that this
happened. Make sure that your paragraph includes two balanced chemical equations.
Using worksheet 6.1, write a procedure for a similar experiment.
State Goals/Benchmark/Standard: 11A.4a-c, 13A.4a, 12C.4a, 12D.4b
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY TWO: Laboratory Activity 8A, Laboratory Activity 8B
Students will perform these extremely simple experiments. The first experiment uses Bunsen
burners to combine oxygen and magnesium in a synthesis reaction to form magnesium oxide.
The second reaction will use a battery to conduct a decomposition reaction. Important ideas to
consider are that energy must be provided to conduct a decomposition reaction, the idea here that
decomposition is always endothermic. Also, students should be able to generate balanced
reaction equations for this simple reaction.
Students should become adept at identifying and master the balancing of Synthesis and
Decomposition Reactions. Synthesis reactions are reactions in which two reactants yield one
product. Decomposition reactions are endothermic reactions in which one reactant yields two
products.
General Case:
Synthesis:
Decomposition:
A + B  AB
AB  A + B
ASSIGNMENT:
Worksheet 6.2
Worksheet 6.2 – Synthesis and Decomposition
NAME _______________________
Put numbers in the blanks to balance the following equations. Learn to recognize the
distinguishing features of each reaction type. Write the word equation below each reaction.
SYNTHESIS (also known as COMBINATION):
1. ___Ca + ___N2 → ___Ca3N2
Word equation: ____ moles Calcium react with ____ moles of nitrogen to form ___ moles of
calcium nitride.
2. ___N2 + ___O2 → ___NO2
Word equation:
3. ___Cu + ___S → ___Cu2S
Word equation:
4. ___Na + ___O2 → ___Na2O
Word equation:
5. ___Al + ___N2 → ___AlN
Word equation:
6. ___Hg + ___I2 → ___HgI2
Word equation:
7. ___Fe + ___O2 → ___Fe2O3
Word equation:
8. ___NO + ___O2 → ___NO2
Word equation:
9. ___H2 + ___Cl2 → ___HCl
Worksheet 6.2 continued:
DECOMPOSITION:
10. ___HgO → ___Hg + ___O2
Word equation: ____ moles of mercury (II) oxide decompose to form ____ moles of mercury
and ___ moles of oxygen.
11. ___CaCO3 → ___CaO + ___CO2
Word equation:
12. ___CuSO4∙5H2O → ___CuSO4 + ___H2O
Word equation:
13. ___NH4NO3 → ___N2O + ___H2O
Word equation:
14. ___BaO2 → ___BaO + ___O2
Word equation:
15. ___NO2 → ___N2 + ___O2
Word equation:
16. ___H2O → ___H2 + ___O2
Word equation:
17. ___NH3 → ___N2 + ___H2
Word equation:
18. ___NCl3 → ___N2 + ___Cl2
Word equation:
State Goals/Benchmark/Standard: 12C.4b, 12D.4b
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY THREE: Activity Series, Practice with Single Replacement Equations
Students must learn about Single Replacement reactions. In a single replacement reaction, the
atoms of an element replace the atoms of a second element in a compound. Metals replace
metals. Nonmetals replace nonmetals.
DEMONSTRATION: Sodium in Water
The teacher will drop a small piece of sodium into a plastic container filled with water. This
demonstration MUST be done in the fume hood. The sodium replaces the hydrogen in water,
yielding hydrogen gas and sodium hydroxide. Students should be told that for the purposes of
Single Replacement and Double Replacement, it might help them if they view water as a
hydrogen ion bonded to a hydroxide ion, or HOH, instead of H2O.
Whether one metal will replace another metal from a compound can be determined by the
relative reactivity of the two metals. The Activity Series lists metals in order of decreasing
reactivity. A reactive solo metal will replace any bonded metal found below it in the activity
series. By contrast, a solo metal of lesser reactivity will not replace a bonded metal found above
it in the table. Students must not only learn to balance single replacement reactions, but must
also factor reactivity into any single replacement reactions they encounter, noting whether or not
a single replacement reaction will occur.
General Case:
Single Replacement: AX + B  BX + A
Students are also taught of the memory aid, HONClBrIF, the list of diatomic elements. Most
other elements are monatomic in nature. This fact will help students later on, when they are
attempting to predict the products of a reaction, knowing only the reactants.
ASSIGNMENT:
Worksheet 6.3
Prepare Laboratory Activity 6C for use in class
Activity Series of Metals:
Lithium
(highest reactivity)
Cesium
Rubidium
Potassium
Barium
Strontium
Calcium
Sodium
Magnesium
Aluminum
Manganese
Zinc
Chromium
Iron
Cadmium
Cobalt
Nickel
Tin
Lead
Hydrogen
Copper
Silver
Mercury
Platinum
Gold
(lowest reactivity)
Metals from Lithium to Sodium will replace Hydrogen from acids and water; from Magnesium to Lead they will
replace Hydrogen from acids only.
Activity Series of Halogens:
F2
Cl2
Br2
I2
(highest reactivity)
(lowest reactivity)
Laboratory Activity 6C – Single Replacement
1. Wear Goggles.
2. Place a test tube in the test tube rack and fill it one third of the way up with 6 M
Hydrochloric acid (WARNING: Hydrochloric acid is very caustic! If you get any on you,
wash it off immediately and tell the teacher).
3. Drop the strip of Magnesium into the acid. Observe what happens. Record your
observations.
4. Cover the mouth of the test tube with the second test tube to capture any gas that is produced
in the tube.
5. Use a lit match to test the gas for flammability by putting it in the mouth of the inverted tube.
6. Rinse all glassware thoroughly before returning it.
7. Write a balanced equation for the reaction of magnesium metal with hydrochloric acid.
Remember to include symbols after each chemical formula to represent the phase of each
reactant and product. Step 5 of the lab should give a hint as to the identity of one of the
products.
Worksheet 6.3 – Single Replacement
Put numbers in the blanks to balance the following equations. Use the Activity Series to answer
the question at the right. (more reactive replaces less reactive in compounds.)
SINGLE REPLACEMENT (also known as DISPLACEMENT):
REACTION:
WILL IT OCCUR? (Yes or No)
1. ___Fe2O3 + ___Cr → ___Cr2O3 + ___Fe
________
Word equation:
2. ___Al + ___CuSO4 → ___Al2(SO4)3 + ___Cu
________
Word equation:
3. ___Ca + ___LiNO3 → ___Li + ___Ca(NO3)2
________
Word equation:
4. ___Cr
+ ___H2SO4 → ___Cr2(SO4)3 + ___H2
________
Word equation:
5. ___Zn(NO3)2 + ___Ag → ___AgNO3 + ___Zn
________
Word equation:
6. ___MgCl2 + ___K → ___KCl + ___Mg
________
Word equation:
7. ___MgCl2 + ___Ag → ___AgCl + ___Mg
________
Word equation:
8. ___Cu + ___AgNO3 → ___Ag + ___Cu(NO3)2
________
Word equation:
9. ___Mn + ___Pb(C2H3O2)4 → ___Pb + ___Mn(C2H3O2)2
________
Word equation:
10. ___PtO2 + ___H2 → ___Pt + ___H2O
Word equation:
________
Worksheet 6.3 continued:
11. ___Fe + ___CuSO4 → ___Cu + ___FeSO4
________
Word equation:
12. ___Co + ___Ba(NO3)2 → ___Ba + ___Co(NO3)2
________
Word equation:
13. ___Hg + ___Pt(OH)2 → ___Pt + ___Hg(OH)2
________
Word equation:
14. ___Al(C2H3O2)3 + ___Mg → ___Al + ___Mg(C2H3O2)2
________
Word equation:
15. ___Sr(NO3)2 + ___Na → ___NaNO3 + ___Sr
________
Word equation:
16. ___AlF3 + ___Cl2 → ___AlCl3 + ___F2
________
Word equation:
17. ___HI + ___Br2 → ___HBr + ___I2
________
Word equation:
18. ___Br2 + ___NaCl → ___NaBr + ___Cl2
________
Word equation:
19. ___ Cl2 + ___ NaBr  ___ NaCl +
Word equation:
___ Br2
________
State Goals/Benchmark/Standard: 12C.4a, 12D.4b, 11A.4a-e, 13A.4a
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY FOUR: Laboratory Activity 6C
Students will complete the Single Replacement Laboratory in the time allotted. After the lab is
done, the teacher should go over more single replacement reactions so that they are more adept at
using the Reactivity Series to identify whether or not a reaction should occur.
ASSIGNMENT:
Worksheet 6.4
Worksheet 6.4 – Double Replacement I
NAME _______________________
Put numbers in the blanks to balance the following equations.
DOUBLE REPLACEMENT (also known as METATHESIS):
REACTION:
1. ___Fe2O3 + ___AlP → ___Al2O3 + ___FeP
Word equation:
2. ___NaCl + ___K2SO4 → ___Na2SO4 + ___KCl
Word equation:
3. ___Pb(NO3)2 + ___BaCl2 → ___Ba(NO3)2 + ___PbCl2
Word equation:
4. ___Na3P + ___CaO → ___Na2O + ___Ca3P2
Word equation:
5. ___Al2O3 + ___AgCl → ___AlCl3 + ___Ag2O
Word equation:
6. ___AgCl + ___PbS → ___PbCl2 + ___Ag2S
Word equation:
7. ___Au2S3 + ___KCl → ___AuCl3 + ___K2S
Word equation:
8. ___KOH + ___Al2S3 → ___Al(OH)3 + ___K2S
Word equation:
Worksheet 6.4 continued:
9. ___AuCl3 + ___H2O → ___HCl + ___Au(OH)3
Word equation:
10. ___AgNO3 + ___CuCl2 → ___AgCl + ___Cu(NO3)2
Word equation:
11. ___CaCO3 + ___HCl → ___CaCl2 + ___H2CO3
Word equation:
12. ___BaCl2 + ___(NH4)2CO3 → ___BaCO3 + ___NH4Cl
Word equation:
State Goals/Benchmark/Standard: 12C.4b, 12D.4b
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY FIVE: Solubility Rules, Practice with Double Replacement Reactions
Double Replacement reactions occur when positive ions are exchanged between two ionically
bonded compounds. The reaction generally takes place between two ionic compounds in
aqueous solutions.
General Case:
Double Replacement:
AX + BY  BX + AY
The ions disassemble in solution, rearrange, and reform, yielding either a precipitate, a gas, or a
compound like water. Regarding the precipitate formation, one of the pairs of ions will form a
solid compound in accordance with the rules of solubility.
Students are to use the solubility rules in determining whether or not a Double Replacement
actually occurs, whether a precipitate is forms, in addition to merely balancing the equations.
It is the action of these ions, forming this solid, that drive the reaction. The other ions will do
nothing, not being directly involved in the reaction. These ions are known as spectator ions.
More will be made of this during the next day of class.
Once again, students should be reminded that for Single and Double Replacement reactions,
water should be viewed as HOH, and not H2O. Also, most polyatomic ions tend to stay together
during Double Replacement reactions.
The Double Replacement Laboratory Activity should be prepared for use in class.
ASSIGNMENT:
Worksheet 6.5
Prepare Laboratory Activity 6D for use in class
Solubility Rules:
Water-Soluble Salts:
1. All salts of the chloride ion, Cl-1, bromide ion, Br-1, and iodide ion, I-1, are soluble except
those of Ag+1, Hg2+2, Pb+2, Cu+1, and Tl+1. BiI3 and SnI4 are insoluble. PbCl2 is three to five
times more soluble in hot water than in cold water.
2. All salts of the acetate ion CH3CO2-1, nitrate ion, NO3-1, chlorate ion, ClO3-1, perchlorate ion,
ClO4-1, and permanganate ion, MnO4-1, are soluble.
3. All common salts of the Group 1A cations and ammonium ion, NH4+1, are soluble.
4. All common salts of the sulfate ion, SO4-2, are soluble except those of Ba+2, Sr+2, Pb+2, and
Hg+2.
5. All Group 1A and 2A salts of the bicarbonate ion, HCO3-1, are soluble.
6. Most salts of the fluorosilicate ion, SiF6-2, thiocyanate ion, SCN-1, and thiosulfate ion, S2O3-2,
are soluble. Exceptions are the Ba+2 and Group 1A fluorosilicates, the Ag+1, Hg2+2, and Pb+2
thiocyanates, and the Ag+1 and Pb+2 thiosulfates.
Water-Insoluble Salts:
1. All common salts of the fluoride ion, F-1, are insoluble except those of Ag+1, NH4+1, and
Group 1A cations.
2. In general, all common salts of the carbonate ion, CO3-2, phosphate ion, PO4-3, borate ion,
BO3-3, arsenate ion, AsO4-3, arsenite ion, AsO3-3, cyanide ion, CN-1, ferricyanide ion,
[Fe(CN)6]-3, ferrocyanide ion, [Fe(CN)6]-4, oxalate ion C2O4-2, and the sulfite ion, SO3-2, are
insoluble, except those of NH4+1 and the Group 1A cations.
3. All common salts of the oxide ion, O-2, and the hydroxide ion, OH-1, are insoluble except
those of the Group 1A cations, Ba+2, Sr+2, and NH4+1. Ca(OH)2 is slightly soluble. Soluble
oxides produce the corresponding hydroxides in water.
4. All common salts of the sulfide ion, S-2, are insoluble except those of NH4+1 and the cations
that are isoelectronic with a noble gas.
5. Most common salts of the chromate ion, CrO4-2, are insoluble except those of NH4+1, Ca+2,
Cu+2, Mg+2, and the Group 1A cations.
6. All common salts of the silicate ion, SiO3-2 are insoluble except those of the Group 1A
cations.
Worksheet 6.5 – Double Replacement II
NAME _______________________
Put numbers in the blanks to balance the following equations. Using the Solubility Rules and a
highlighter, mark which ions typically form a precipitate. Then, predict whether or not an
insoluble product will be formed, and identify the predicted solid precipitate (or if none, the
words “no reaction”) in the blank at the right.
DOUBLE REPLACEMENT (also known as METATHESIS):
REACTION:
1. ___Pb(NO3)2 + _2_NaBr → _2_NaNO3 + ___PbBr2
________
Word equation: one mole of aqueous lead (II) nitrate reacts with 2 moles of aqueous
sodium bromide to form two moles of aqueous sodium nitrate and one mole of lead (II)
bromide precipitate.
2. ___AgHCO3 + ___NaCl → ___NaHCO3 + ___AgCl
________
Word equation:
3. ___K2SO4 + ___BaCl2 → ___BaSO4 + ___KCl
________
Word equation:
4. ___Ba(NO3)2 + ___Li2SiF6 → ___BaSiF6 + ___LiNO3
________
Word equation:
5. ___AgF + ___Ca(NO3)2 → ___AgNO3 + ___CaF2
________
Word equation:
6. ___(NH4)2CrO4 + ___Fe(NO3)3 → ___NH4NO3 + ___Fe2(CrO4)3
________
Word equation:
7. ___AgMnO4 + ___KCl → ___AgCl + ___KMnO4
Word equation:
________
Worksheet 6.5 continued:
8. ___KOH + ___Al2(SO4)3 → ___Al(OH)3 + ___K2SO4
________
Word equation:
9. ___(NH4)2S + ___SrO → ___(NH4)2O + ___SrS
________
Word equation:
10. ___AgClO4 + ___NaSCN → ___AgSCN + ___NaClO4
________
Word equation:
11. ___Na2CO3 + ___BaCl2 → ___NaCl + ___BaCO3
Word equation:
________
Laboratory Activity 6D – Double Replacement
1. Wear Goggles.
2. Observe a solution of Lead (II) Nitrate, Pb(NO3)2.
3. Fill a test tube about 1/3 of the way up with Pb(NO3)2.
4. Observe a solution of Barium Chloride, BaCl2.
5. Add an equal amount of BaCl2 to the tube.
6. Record your observations of what occurs in the tube for the next several minutes.
7. Write out a balanced equation for what occurs in the tube. Predict the identity of the
precipitate.
8. Clean up your station. Discard the contents of the tube in the solution waste container
provided by the teacher.
State Goals/Benchmark/Standard: 12C.4b, 12D.4b
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY SIX: Ionic Equations, Net Ionic Equations, Spectator Ions
The Double Replacement Reaction is driven by a precipitate formation. Two different solutions
of aqueous ions are used as reactants. Each of the aqueous solutions dissociates into ions. Then,
positive ions are exchanged, and new compounds are formed. In accordance with the solubility
rules, if one of the products formed is a solid, a precipitate is formed. If not, no reaction occurs.
Students must be taught how to correctly write out a Double Replacement reaction. There are
three ways to write the equation out.
The overall equation must be written out with subscripts designating the phase of each species
involved. (aq) stands for aqueous, meaning that the compound in question breaks up into ions
upon being put into water. (s) stands for solid, the phase of the precipitate. (l) stands for pure
liquids that might be formed, as in products such as water. (g) stands for gas, which escapes
from the reaction vessel.
The ionic equation contains all of the ions involved in the reaction, and correctly identifies the
precipitate with a designation of (s). This includes two ions which are not required for the
formation of the precipitate. Since these ions are not involved in the actual precipitate formation,
they are known as spectator ions.
The net-ionic equation is similar to the ionic equation, except without the inclusion of the
spectator ions. Students must be able to write out each of these types of equations for each of the
Double Replacement Reactions they encounter.
The teacher should spend the rest of the class period helping the students understand these
equation writing techniques by rewriting the equations from Balancing Equations Worksheet #06
in all three ways.
ASSIGNMENT:
Rewrite equations from Worksheet 6.5 as “overall equations,” “ionic
equations,” and “net-ionic equations.”
Worksheet 6.6
Worksheet 6.6 – Double Replacement III
NAME _______________________
Put numbers in the blanks to balance the following equations. Using the Solubility Rules,
rewrite the equations as overall equations, ionic equations, and net-ionic equations. Be sure
to include identification of phases, like (s), (l), (g), or (aq) in the reactions.
DOUBLE REPLACEMENT (also known as METATHESIS):
REACTION:
1. ___CaCl2 + ___K2CO3 → ___CaCO3 + ___KCl
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
2. ___AgNO3 + ___FeCl3 → ___AgCl + ___Fe(NO3)3
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
3. ___Al(OH)3 + ___HC2H3O2 → ___Al(C2H3O2)3 + ___H2O
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
4. ___NaNO3 + ___K2SO3 → No Reaction (Answer the following to demonstrate why)
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
State Goals/Benchmark/Standard: 12C.4b, 12D.4b, 14A.4a-e, 13A.4a
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY SEVEN: Double Replacement Laboratory
Students will complete the laboratory activity during the class period. During any leftover time,
students should continue their work with Double Replacement Reactions.
ASSIGNMENT:
Worksheet 6.7
Prepare Laboratory Activity 6E for use in class
Laboratory Activity 6E – Combustion
1. Wear Goggles.
2. Use a dropper pipet to transfer 10 drops of Ethanol into a watch glass.
3. Drop a lit match into the watch glass and observe the flame.
4. Smother the flame by covering it with an inverted plastic cup. Observe the sides of the cup.
What compound builds up on the sides of the cup?
5. Wash and dry the glassware you used.
6. Ethanol has a formula of CH3CH2OH. Write a balanced equation for the combustion of
ethanol.
Worksheet 6.7 – Double Replacement IV
Put numbers in the blanks to balance the following equations. Using the Solubility Rules,
rewrite the equations as overall equations, ionic equations, and net-ionic equations. Be sure
to include identification of phases, like (s), (l), (g), or (aq) in the reactions.
REACTION:
1. ___Na2SO4 + ___Ba(NO3)2 → ___NaNO3 + ___BaSO4
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
2. ___CuHCO3 + ___KBr → ___CuBr + ___KHCO3
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
3. ___MgCrO4 + ___BaI2 → ___MgI2 + ___BaCrO4
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
4. ___NH4CN + ___Fe(NO3)3 → ___NH4NO3 + ___Fe(CN)3
Overall Equation:
Ionic Equation:
Net-Ionic Equation:
State Goals/Benchmark/Standard: 12C.4b, 12D.4b
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY EIGHT: Combustion Reactions
Students should be introduced to the balancing of Combustion Equations. Combustion reactions
involve the combination of a hydrocarbon, a chemical composed primarily of carbons and
hydrogens, with oxygen gas to yield carbon dioxide and water.
General Case:
Combustion:
CxHy + O2  CO2 + H2O
The best way to approach a Combustion equation is to begin by balancing Carbon. Then,
Hydrogen should be balanced next. Oxygen should be saved for last because it appears in so
many places in the reaction.
ASSIGNMENT:
Worksheet 6.8
Worksheet 6.8 – Combustion
NAME _______________________
Put numbers in the blanks to balance the following equations. Name the hydrocarbon where
indicated, you may have to draw the Lewis structure first.
COMBUSTION:
REACTION:
___C3H8 + ___O2 → ___CO2 + ___H2O
C3H8 = ___________________
___C4H10 + ___O2 → ___CO2 + ___H2O
C4H10= ___________________
___C5H12 + ___O2 → ___CO2 + ___H2O
___C7H16 + ___O2 → ___CO2 + ___H2O
___C7H14 + ___O2 → ___CO2 + ___H2O
___C9H20 + ___O2 → ___CO2 + ___H2O
___C6H14 + ___O2 → ___CO2 + ___H2O
____CH4 + ___O2 → ___CO2 + ___H2O
CH4 = ____________________
___C2H2 + ___O2 → ___CO2 + ___H2O
C2H2 = ___________________
___C2H4 + ___O2 → ___CO2 + ___H2O
C2H4 = ___________________
___C2H6 + ___O2 → ___CO2 + ___H2O
___C8H18 + ___O2 → ___CO2 + ___H2O
___C6H6 + ___O2 → ___CO2 + ___H2O
___C6H12 + ___O2 → ___CO2 + ___H2O
___C6H12O6 + ___O2 → ___CO2 + ___H2O
___C12H22O11 + ___O2 → ___CO2 + ___H2O
___C8H16 + ___O2 → ___CO2 + ___H2O
___C85H172 + ___O2 → ___CO2 + ___H2O
State Goals/Benchmark/Standard: 12C.4b, 12D.4b, 11A.4a-e, 13A.4a
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY NINE: Combustion Laboratory Activity
Students will perform the Combustion Laboratory Activity during class. If time permits,
students will do further work with identifying and balancing Combustion Equations.
ASSIGNMENT:
Worksheet 6.9
Worksheet 6.9 – Ridiculous Combustion
NAME _______________________
Put numbers in the blanks to balance the following equations.
COMBUSTION:
REACTION:
___C35H72 + ___O2 → ___CO2 + ___H2O
___C412H826 + ___O2 → ___CO2 + ___H2O
___C50H102 + ___O2 → ___CO2 + ___H2O
___C50H100 + ___O2 → ___CO2 + ___H2O
___C5H11OH + ___O2 → ___CO2 + ___H2O
___C8H15OH + ___O2 → ___CO2 + ___H2O
___C6000H12002 + ___O2 → ___CO2 + ___H2O
___CH3OH + ___O2 → ___CO2 + ___H2O
___HC2H3O2 + ___O2 → ___CO2 + ___H2O
___C26H54 + ___O2 → ___CO2 + ___H2O
___CH3CH2OH + ___O2 → ___CO2 + ___H2O
___C6H5COOH + ___O2 → ___CO2 + ___H2O
State Goals/Benchmark/Standard: 12C.4b, 12D.4b
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY TEN: Prediction Equations
The teacher will instruct students as to how to predict the products of chemical reactions.
Students will use the General Case scenarios to predict the outcome of equations.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
The teacher will work through the first worksheet with the students. The students will work the
second worksheet for homework.
ASSIGNMENT:
Worksheet 5.10
Worksheet 5.11
Prepare Laboratory Activity 5F for use in the class
Worksheet 6.10 – Basic Predictions
NAME _______________________
Use the General Cases to predict the products of each reaction. Balance each equation when
done. Identify each reaction type in the blank at the right.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
REACTION:
___C5H12 + ___O2 →
_________________
___Zn + ___HCl →
_________________
___Na2O →
_________________
___Li + ___Cl2 →
_________________
___Na2SO4 + ___LiCl →
_________________
___C4H10 + ___O2 →
_________________
___Al2O3 →
_________________
___Al + ___I2 →
_________________
___Zn(OH)2 + ___Al2(CO3)3 →
_________________
___FeCl3 →
_________________
Worksheet 6.11 – More Predictions
NAME _______________________
Use the General Cases to predict the products of each reaction. Balance each equation when
done. Identify each reaction type in the blank at the right.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
REACTION:
___CuCl2 + ___Na3PO4 →
_________________
___C12H26 + ___O2 →
_________________
___FeCl3 →
_________________
___K2SO4 + ___Li →
_________________
___Na + ___O2 →
_________________
___C3H8 + ___O2 →
_________________
___KMnO4 + ___Li →
_________________
___Na3P + ___Ba(OH)2 →
_________________
___H2O →
_________________
___HCl + ___Ca(OH)2 →
_________________
Laboratory Activity 6F – Predict The Products
You will react nine different chemicals together in double replacement reactions. Some of the
chemicals will react, producing a precipitate; some will not. You must use the Solubility Rules
to determine beforehand which reactions should occur and which should not. The experiment
will be used to verify your predictions.
You will react each of the following chemicals in every possible combination:
Lead (II) Nitrate
Magnesium Sulfate
Copper (II) Chloride
Sodium Chloride
Sodium Carbonate
Potassium Hydroxide
Barium Chloride
Calcium Acetate
Copper (II) Sulfate
CuSO4
KOH
CuCl2
Ca(C2H3O2)2
Na2CO3
MgSO4
BaCl2
NaCl
Pb(NO3)2
The following matrix is designed to help you keep track of the reactions. Use one drop of each
reagent in a well plate. If the results are inconclusive with only one drop, use more.
Pb(NO3)2
X
NaCl
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
X
BaCl2
MgSO4
Na2CO3
Ca(C2H3O2)2
CuCl2
KOH
CuSO4
X
State Goals/Benchmark/Standard: 12C.4b, 12D.4b
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY ELEVEN: Practice with Prediction Equations
Students will continue their work on Prediction Equations in class, with the aid of the teacher.
More problems and worksheets will be assigned.
ASSIGNMENT:
Worksheet 5.12
Worksheet 5.13
Worksheet 6.12 – Still More Predictions
NAME _______________________
Predict the products of each reaction. Balance each equation when done. Identify each reaction
type in the blank at the right.
REACTION:
___Mg + ___O2 →
_________________
___AlCl3 →
_________________
___Na + ___O2 →
_________________
___HCl + ___NaOH →
_________________
___Pb(SO4)2 + ___Al(C2H3O2)3 →
_________________
___C4H10 + ___O2 →
_________________
___H3PO4 + ___MgCO3 →
_________________
___HgCl2 + ___NaSCN →
_________________
___PtO2 + ___H2 →
_________________
___CaCO3 + ___NaCl →
_________________
___Ag + ___HNO3 →
_________________
___NCl3 →
_________________
___MgSO4∙7H2O →
_________________
Worksheet 6.13 – Yet More Predictions
NAME _______________________
Predict the products of each reaction. Balance each equation when done. Identify each reaction
type in the blank at the right.
REACTION:
___Sr + ___O2 →
________________
___Na + ___H2O →
________________
___Zn + ___HCl →
________________
___ICl →
________________
___Fe(OH)3 + ___H2SO4 →
________________
___C6H14 + ___O2 →
________________
___Au(OH)3 + ___Na2CO3 →
________________
___SrCl2 + ___NaOH →
________________
___OCl2 →
________________
___AgNO3 + ___H2SO4 →
________________
___Zn + ___O2 →
________________
___Mg(OH)2 + ___NaF →
________________
___C30H62 + ___O2 →
________________
___Mg(NO3)2 + ___H2O →
________________
___Au2S3 →
________________
___Ti(MnO4)4 + ___Fe2O3 →
________________
___MnF2 + ___O2 →
________________
___CO2 →
________________
State Goals/Benchmark/Standard: 11A.4a-e, 13A.4a
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension
DAY TWELVE: Laboratory Activity 5F
Students should spend the period working on the Prediction Laboratory Activity. For each of the
Double Replacement reactions that occurred, students should write out an Overall Equation and a
Net Ionic Equation. This should be done on a separate sheet of paper, and turned in at the end of
the lab period, if possible. If there is any time left over, the teacher should lead the class on a
review of the unit.
ASSIGNMENT:
Laboratory Equations turned in at end of period, if possible
State Goals/Benchmark/Standard:
Performance Descriptor:
Curriculum Reading Initiative:
DAY THIRTEEN: Review Balancing Equations
The teacher will lead students through a comprehensive review of the unit on Balancing
Equations and Predicting Products. Any topics that are problematic should be reviewed one
more time.
ASSIGNMENT:
Study for Unit Exam
Worksheet 5.14
Worksheet 6.14 – One More Time
NAME _______________________
Balance each equation when done. Identify each type of reaction in the blank at the right.
a) ___Na + ___I2 → ___NaI
____________
b) ___H2CO3 → ___H2O + ___CO2
____________
c) ___C3H8 + ___O2 → ___CO2 + ___H2O
____________
d) ___Na3PO4 + ___Zn → ___Na + ___Zn3(PO4)2
____________
e) ___LiCl + ___Pb(NO3)2 → ___PbCl2 + ___LiNO3
____________
f) ___MgSO4 + ___NaNO3 → ___Na2SO4 + ___Mg(NO3)2
____________
Which of the above reactions requires energy to proceed?
Two of the above reactions will not occur experimentally. Identify each one, and briefly explain
why the reaction will not take place.
Predict the products of the following reactions. Balance and identify the equations.
___C2H6 + ___O2 →
____________
___H2 + ___Li →
____________
___MgSO4 + ___K →
____________
___KMnO4 + ___Al(OH)3 →
____________
___MnI4 →
____________
What are the two possible ions that can be made from hydrogen atoms?
Identify the following ions:
SO4-2 __________
SO3-2 __________
HSO4-1 __________
IO3-1 __________
IO2-1 __________
HCO3-1 __________
State Goals/Benchmark/Standard: 11A.4a-e, 13A.4a
Performance Descriptor: Stage I
Curriculum Reading Initiative: Fluency, Comprehension, Writing
DAY FOURTEEN: Exam
Students have the entire period to complete the exam.
ASSIGNMENT:
Begin next unit
NAME _______________________
Practice Exam – Balancing Equations:
Balance each equation when done.
a) ___K + ___Cl2 → ___ ____________
b) ___ CO2MgS + ___NaNO3 → ___Na2S + ___
____________
c) ___C12H24 + ___O2 → ___CO2 + ___ __________
____________
d) ___Sr3PO4 + ___Al → ___Sr + ___ ____________
e) ___NaC2H3O2 + ___Pb(NO3)4 → ___Pb(C2H3O2)4 + ___ ____________
f) ___ Fe2CO3 → ___Fe2O + ___ ___________
Predict the products of the following reactions. Balance and identify the equations.
a) ___CH4 + ___O2 →
____________
b) ___MgSO4 + ___Sr →
____________
c) ___Au(MnO4)3 + ___Al(OH)3 →
____________
d) ___FeI3 →
____________
e) ___Au(SO3)3 + ___Pb(NO3)2 →
____________
Balance the following reactions by adding filling in the blanks.
a) ___H3PO4 + ___Al(OH)3 → ___ _________ + ___H2O
b) ___NH4NO3 → ___N2O + ___H2O
c) ___NO2 + ___H2O → ___HNO3 + ___NO
d) ___C12H22O11 + ___O2 → ___CO2 + ___H2O
Circle every one of the following that would replace chromium ion in CrF2.
Li
Fe
Ca
Pt
Mn
Cs
Pb
Sr
Cu
Hg
Rb
Circle every one of the following that would form a precipitate with BaCl2.
NaNO3
Pb(NO3)2
Na2SO4
LiHCO3
AgF
K2SiO3
K
NAME _______________________
Exam – Balancing Equations (Form B):
Balance each equation when done. Identify each type of reaction in the blank at the right.
a) ___N2 + ___Cl2 → ___NCl3
____________
b) ___Na2O → ___Na + ___O2
____________
c) ___C9H20 + ___O2 → ___CO2 + ___H2O
____________
d) ___Li2SO4 + ___Al → ___Li + ___Al2(SO4)3
____________
e) ___Mg(C2H3O2)2 + ___Fe(NO3)3 → ___Fe(C2H3O2)3 + ___Mg(NO3)2
f) ___Fe2S3 → ___Fe + ___S8
____________
____________
Predict the products of the following reactions. Balance and identify the equations.
a) ___Au2(SO4)3 + ___Mg(OH)2 →
____________
b) ___MgCO3 + ___Li →
____________
c) ___C6H6 + ___O2 →
____________
d) ___Mg3N2 →
____________
e) ___Al2(SO3)3 + ___Pb →
____________
Balance the following reactions by adding coefficients before reactants and products.
a) ___H3PO4 + ___NaOH → ___Na3PO4 + ___H2O
b) ___F + ___C + ___G → ___F2G2C
c) ___PbO2 + ___H2O → ___PbH4 + ___O2
d) ___C102H200O51 + ___O2 → ___CO2 + ___H2O
Circle every one of the following that would replace calcium ion in CaF2.
Li
Fe
Pt
Cs
Pb
Sr
Cu
Hg
Rb
K
Mn
Circle every one of the following that would form a precipitate with Sr(OH)2.
Na2SO4
LiHCO3
Pb(NO3)2
AgF
K2SiO3
NaNO3
Au
NAME _______________________
Exam – Balancing Equations:
Balance each equation when done. Identify each type of reaction in the blank at the right.
a) ___Na + ___Cl2 → ___NaCl
____________
b) ___C10H22 + ___O2 → ___CO2 + ___H2O
____________
c) ___Na3PO4 + ___Al → ___Na + ___AlPO4
____________
d) ___LiC2H3O2 + ___Pb(NO3)4 → ___Pb(C2H3O2)4 + ___LiNO3 ____________
Predict the products of the following reactions. Balance and identify the equations.
a) ___CH4 + ___O2 →
____________
b) ___MgSO4 + ___Sr →
____________
c) ___FeI3 →
____________
d) ___Au(SO3)3 + ___Pb(NO3)2 →
____________
Balance the following reactions by adding coefficients before reactants and products.
a) ___H3PO4 + ___Al(OH)3 → ___AlPO4 + ___H2O
b) ___NH4NO3 → ___N2O + ___H2O
c) ___NO2 + ___H2O → ___HNO3 + ___NO
d) ___C12H22O11 + ___O2 → ___CO2 + ___H2O
Circle every one of the following that would replace chromium ion in CrF2.
Li
Fe
Ca
Pt
Mn
Cs
Circle every one of the following that would form a precipitate with BaCl2.
NaNO3
Pb(NO3)2
Na2SO4
How many grams of BaCl2 are needed to make 75 mL of a 1.2 M solution?