reactions in aqueous solutions, predicting products and classifying types of chemical reactions
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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
Learning checkLearning check
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
Check with your neighborCheck with your neighbor
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.
Learning checkLearning check
Try these single displacement Try these single displacement reactions:reactions:
3. copper + silver nitrate3. copper + silver nitrate
4. bromine + sodium chloride4. bromine + sodium chloride
Check with your neighborCheck with your neighbor
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.
General Equation:General Equation:
Example:Example:
2. Decomposition of a base into a metal-oxide and water.2. Decomposition of a base into a metal-oxide and water.
General Equation:General Equation:
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)
A is metal/cation, B is nonmetal/anion
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)
A is metal/cation, B is nonmetal/anion
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
Learning checkLearning check
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
Check with your neighborCheck with your neighbor
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.
General Equation:General Equation:
Example:Example:
2.2. Combining a metal-oxide and water to produce a Combining a metal-oxide and water to produce a base.base.
General Equation:General Equation:
Example:Example:
A is metal/cation, B is nonmetal/anion
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)
A is metal/cation, B is nonmetal/anion
Learning checkLearning check
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
Check with your neighborCheck with your neighbor
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
Learning checkLearning check
Try these combustion reactions:Try these combustion reactions:12. C12. C88HH1818 + oxygen + oxygen
13. C13. C22HH22 + oxygen + oxygen
Check with your neighborCheck with your neighbor
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
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