Reactions in Aqueous Solutions, Predicting Products and Classifying Types of Chemical Reactions

Reactions in Aqueous Reactions in Aqueous Solutions, Predicting Solutions, Predicting

Products and Classifying Products and Classifying Types of Chemical Types of Chemical

ReactionsReactions

I. Predicting Whether a Reaction I. Predicting Whether a Reaction Will OccurWill Occur

A. Four Driving ForcesA. Four Driving Forces1.1. Formation of a solid (precipitate)Formation of a solid (precipitate)

2.2. Formation of waterFormation of water

3.3. Transfer of electronsTransfer of electrons

4.4. Formation of a gasFormation of a gas

B. If a driving force occurs the reaction B. If a driving force occurs the reaction will take place.will take place.

1. Soluble solid1. Soluble solid – readily dissolves in – readily dissolves in water water

2. Insoluble2. Insoluble and and slightly solubleslightly soluble solid solid – a solid where such a tiny amount – a solid where such a tiny amount dissolves in water that it is dissolves in water that it is undetectable to the naked eyeundetectable to the naked eye

3.3. Solubility is temperature dependent Solubility is temperature dependent

State is aqueous - (aq)

State is solid - (s)

Predicting States of Predicting States of SubstancesSubstances

States of reactants can be manipulated

Solubility RulesSolubility Rules (on snoopy sheet)(on snoopy sheet)

Ex. Predict whether the Ex. Predict whether the following following substances are substances are soluble or insoluble.soluble or insoluble.

AgNO3

Al(OH)3

Cu3PO4

Li2CO3

ZnSO4

(aq)

(aq)

(aq)

(s)

(s)

Solubility RulesMainly water soluble (aq)All nitrates are soluble.All acetates are soluble.All chlorates are soluble.All chlorides are soluble except AgCl, Hg2Cl2,

and PbCl2All bromides are soluble except AgBr, Hg2Br2,

PbBr2, and HgBr2

All iodides are soluble except AgI, Hg2I2, PbI2, and HgI2

All sulfates are soluble except CaSO4, SrSO4, BaSO4, PbSO4, Hg2SO4, and Ag2SO4

Mainly water insoluble (s)All sulfides are insoluble except those of 1A

and 2A elements and (NH4)2SAll carbonates are insoluble except those of

1A and (NH4)2CO3

All phosphates are insoluble except those of 1A and (NH4)3PO4

All hydroxides are insoluble except those of 1A, Ba(OH)2, Sr(OH)2 and Ca(OH)2

Learning CheckLearning Check

Try these: Determine if the following Try these: Determine if the following are AQUEOUS or SOLIDare AQUEOUS or SOLID

1. lead (II) nitrate1. lead (II) nitrate

2. potassium sulfide2. potassium sulfide

3. barium hydroxide3. barium hydroxide

4. ammonium carbonate4. ammonium carbonate Turn to your neighbor and compare Turn to your neighbor and compare

answersanswers

When a soluble ionic salt dissolves in water When a soluble ionic salt dissolves in water the ions separate and a hydration shell is the ions separate and a hydration shell is formed around each ion formed around each ion (Dissociation)(Dissociation)

Ex. Ba(NOEx. Ba(NO33))22 in water – in water –

Ba(NO3)2 (aq) Ba+2(aq) + 2 NO3

-1(aq)

Al(C2H3O2)3 (aq) Al+3(aq) + 3 C2H3O2

-1(aq)

Al2(CO3)3 (s) Al2(CO3)3 (s) or No RXN

Aluminum acetate

Aluminum carbonate

Draw a beaker of dissociated sodium chloride; Draw a beaker of dissociated sodium chloride; a beaker of dissociated Aluminum nitrate; a beaker of dissociated Aluminum nitrate;

and a beaker of silver chloride.and a beaker of silver chloride.

Na+1

Na+1

Na+1

Na+1

Cl-1

Cl-1Cl-1

Cl-1

Cl-1Na+1

Cl-1

Na+1 = sodium ion

= chloride ion

Al+3

Al+3

NO3-1

NO3-1

NO3-1

NO3-1

NO3-1

NO3-1

Al+3

NO3-1

= aluminum ion

= nitrate ion

Cl-1

Ag+1 Cl-1Cl-1

Cl-1Ag+1

Ag+1

Ag+1

Cl-1

Ag+1 = silver ion

= chloride ion

Special RulesSpecial Rules

1. Acids are aqueous

2. Most metal oxides are solids

3. Most non-metal oxides are gases

Learning checkLearning check

Write a dissociation equation for Write a dissociation equation for aluminum sulfatealuminum sulfate

Draw a beaker of dissociated Draw a beaker of dissociated aluminum sulfatealuminum sulfate

Check with your neighborCheck with your neighbor

III. Types of ReactionsIII. Types of Reactions

Double Displacement: Double Displacement:

Single Displacement:Single Displacement:

Decomposition: Decomposition:

Synthesis:Synthesis:

Combustion:Combustion:

AB A + B

AB +YZ AZ + YB

A +YB Y + AB

A + B AB

CxHx + O2 CO2 + H2O

Reactants are: 2 compounds

Reactants are: 1 element & 1 Compound

Reactant is: 1 compound

Reactants are: 2 elements or 2 oxides

Reactants are: hydrocarbon and oxygen

IV. Predicting ProductsIV. Predicting Products

Steps for Predicting ProductsSteps for Predicting Products

1.1.Formulas & States for ReactantsFormulas & States for Reactants

2.2.Type of ReactionType of Reaction

3.3.Predict Formulas & States for Predict Formulas & States for ProductsProducts

4.4.No Reaction (if missing driving force)No Reaction (if missing driving force)

oror Balance Equation Balance Equation

IV. Predicting ProductsIV. Predicting Products

A.A. Double Displacement reactionsDouble Displacement reactions: : two compounds combine to produce two compounds combine to produce two different compounds - two different compounds - Acid-Acid-Base Base

and Precipitation Reactions. and Precipitation Reactions.

* Use solubility rules.* Use solubility rules.

General Equation: General Equation:

Example:Example:

AB + YZ AZ + YB

Lead (II) acetate + sodium chloridePb(C2H3O2)2 (aq)

+ NaCl(aq)

PbCl2 (s)+ NaC2H3O2 (aq)

2 2

Driving force = water product

Driving force = solid product

Pb+2 C2H3O2-1 Na+1 Cl-1


Try these double displacement reactions:Try these double displacement reactions:

1. sodium sulfate + lead (II) nitrate1. sodium sulfate + lead (II) nitrate

2. sulfuric acid + potassium hydroxide2. sulfuric acid + potassium hydroxide


B.Single Replacement ReactionsB.Single Replacement Reactions: : Activity Series Activity Series

Single Displacement reactionsSingle Displacement reactions: an : an element and a compound combine to element and a compound combine to form a new element and compound.form a new element and compound.

* Use the activity series.* Use the activity series.

General Equation:General Equation:

Example:Example:

A + YB Y + AB (Cation) B + AZ Z + AB (Anion)

Sodium + Lead (II) acetateNa+1 Pb+2 C2H3O2

-1

Na(s) + Pb(C2H3O2)2(aq) Pb(s) + NaC2H3O2 (aq)2 2

*If you don’t know the charge use +2

Single Replacement ReactionsSingle Replacement Reactions: : Activity Series Activity Series

Active metal elements can replace less Active metal elements can replace less active metals, active nonmetal elements active metals, active nonmetal elements can replace less active nonmetals.can replace less active nonmetals.

Use the Use the Activity seriesActivity series (snoopy sheet) to (snoopy sheet) to determine whether or not the reaction will determine whether or not the reaction will occur.occur.

Driving force is the transfer of electrons.Driving force is the transfer of electrons.


Try these single displacement Try these single displacement reactions:reactions:

3. copper + silver nitrate3. copper + silver nitrate

4. bromine + sodium chloride4. bromine + sodium chloride


C. Decomposition reactionsC. Decomposition reactions: a single compound : a single compound is broken down into more than one product. There is broken down into more than one product. There are six different types.are six different types.

1. Decomposition of a binary compound into its 1. Decomposition of a binary compound into its elements.elements.

* Usually requires heat or electricity.* Usually requires heat or electricity.


Example:Example:

2. Decomposition of a base into a metal-oxide and water.2. Decomposition of a base into a metal-oxide and water.


Example: Example:

AB A + B

Δ = heat or electricity

Sodium Chloride

NaCl(aq) +Na(s) Cl2(g)2 2

AOH AO + H2O

Sodium Hydroxide

NaOH(aq) + H2O (l)2

Base = Compound that contains hydroxide (OH-1)

A is metal/cation, B is nonmetal/anion

Na2O(s)

Metal-oxide = solid

3. Decomposition of a ternary acid into a 3. Decomposition of a ternary acid into a nonmetal-oxide and water.nonmetal-oxide and water.

General Equation:General Equation: Example:Example: 4. Decomposition of a metallic carbonate 4. Decomposition of a metallic carbonate

into a metal-oxide and carbon dioxide.into a metal-oxide and carbon dioxide.General Equation:General Equation: Example:Example:

HBO BO + H2O

sulfuric acid

H2SO4(aq) + H2O (l)

ACO3 AO + CO2

Sodium Carbonate

Na2CO3(aq) + CO2(g)

SO3(g)

nonmetal-oxide = gas

Na2O (s)


5. Decomposition of a metallic chlorate into 5. Decomposition of a metallic chlorate into a metal-chloride and oxygen gas.a metal-chloride and oxygen gas.

General Equation:General Equation: Example:Example: 6. Decomposition of a tertiary salt into a 6. Decomposition of a tertiary salt into a

metal-oxide and a non-metal oxidemetal-oxide and a non-metal oxideGeneral Equation:General Equation: Example:Example:

AClO3 ACl + O2

Sodium Chlorate

NaClO3(aq) + O2(g)2 2

ABO AO+ BO

Sodium Phosphate

Na3PO4(aq) + P2O5(g)2 3

NaCl (aq) 3

Na2O(s)


Special SituationsSpecial Situations

Whenever HWhenever H22COCO33, H, H22SOSO33, or NH, or NH44OH is OH is a product it will decompose a product it will decompose immediately as follows:immediately as follows:

HH22COCO33 H H22O + COO + CO22

HH22SOSO33 H H22O + SOO + SO22

NHNH44OH OH H H22O + NHO + NH33


Try these decomposition reactions:Try these decomposition reactions:5. Calcium chlorate5. Calcium chlorate

6. Phosphoric acid6. Phosphoric acid

7. Barium hydroxide7. Barium hydroxide

8. Tin (IV) carbonate8. Tin (IV) carbonate


D. Synthesis reactionsD. Synthesis reactions: two substances : two substances combine to form one product. There are four combine to form one product. There are four

different types.different types. 1.1. Two elements combine to form a binary compound.Two elements combine to form a binary compound.


Example:Example:

2.2. Combining a metal-oxide and water to produce a Combining a metal-oxide and water to produce a base.base.


Example:Example:


A + B AB

Sodium + Chlorine

NaCl(aq)+Na(s) Cl2(g) 22

AO + H2O AOH

Barium oxide + water

Ba(OH)2(aq)+BaO(s) H2O(l)

3.3. Combining a nonmetal–oxide and water Combining a nonmetal–oxide and water to produce a tertiary acid.to produce a tertiary acid.

General Equation:General Equation: Example:Example: 4.4. Combining a metal-oxide and a Combining a metal-oxide and a

nonmetal-oxide to produce a tertiary salt.nonmetal-oxide to produce a tertiary salt.General Equation:General Equation: Example: Example:

BO + H2O HBO

dinitrogen pentoxide + water

HNO3(aq)+N2O5(g) H2O(l) 2

AO + BO ABO

Barium oxide + dinitrogen pentoxide

Ba(NO3)2(aq)+BaO(s) N2O5(g)



Try these synthesis reactions:Try these synthesis reactions:9. Water + magnesium oxide9. Water + magnesium oxide

10. Water + dinitrogen trioxide10. Water + dinitrogen trioxide

11. Bromine + sodium11. Bromine + sodium


E. E. Combustion reactionsCombustion reactions: Certain organic compounds : Certain organic compounds (Hydrocarbons – compound containing Carbon and (Hydrocarbons – compound containing Carbon and Hydrogen or Carbon, Hydrogen and Oxygen) burn to Hydrogen or Carbon, Hydrogen and Oxygen) burn to produce specific products. There are two types.produce specific products. There are two types.

1.1. Complete combustion – combining a hydrocarbon with Complete combustion – combining a hydrocarbon with excess oxygen to produce carbon dioxide and water.excess oxygen to produce carbon dioxide and water.

* if the equation does not indicate limited oxygen assume * if the equation does not indicate limited oxygen assume complete combustioncomplete combustion

General Equation:General Equation: Example:Example: 2.2. Incomplete combustion - combining a hydrocarbon with Incomplete combustion - combining a hydrocarbon with

limited oxygen to produce carbon monoxide and water.limited oxygen to produce carbon monoxide and water.General Equation:General Equation: Example: Example:

CxHx + O2 CO2 + H2O

CxHx + limited O2 CO + H2O

CH4(g) + limited O2(g) CO(g) +

CH4(g) + O2(g) CO2(g) + H2O(g)

H2O(g)

22

2 423


Try these combustion reactions:Try these combustion reactions:12. C12. C88HH1818 + oxygen + oxygen

13. C13. C22HH22 + oxygen + oxygen


F.F. Oxidation Reduction Oxidation Reduction reactionsreactions: (redox): (redox)

DDriving Force = Transfer of electronriving Force = Transfer of electron Always in single displacement reactionsAlways in single displacement reactions Sometimes in Synthesis and DecompositionSometimes in Synthesis and Decomposition Never in Double DisplacementNever in Double Displacement

Example: Example:

Anytime a single element is present a reaction is also classified as redox

NaCl(aq) +Na(s) Cl2(g)2 2

NaCl(aq)+Na(s) Cl2(g) 22

Zn(NO3)2(aq) + 2 Na(s) 2NaNO3(aq) + Zn(s)

decomposition & redox

synthesis & redox

single displacement & redox

Documents

Reactions in Aqueous Solutions, Predicting Products and Classifying Types of Chemical Reactions