What are the six types of chemical reactions?
Types of Chemical Reactions
1. Synthesis
(A+ B ----> AB)
2. Decomposition (AB------> A + B)
3. Single Replacement (A+ BC ---> B + AC)
4. Double Replacement (AB + CD ---> CB + AD)
5. Combustion (CxHx + O2 ----> CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)
Replacement Reactions
Directions:
Predict products, balance equations, and
predict the states of matter for each
substance. (s, l, g, aq)
Single Replacement Reaction:
Ex. Li + MgCl2 ----->
Double Replacement Reaction:
Ex. CaCl2 + Na3(PO4) --->
Replacement Reactions
Single Replacement Reaction:
Ex. Li + MgCl2 -----> LiCl2 + Mg
Double Replacement Reaction:
Ex. CaCl2 + Na3(PO4) ---> Ca3(PO4)2 + NaCl
Replacement Reactions
Single Replacement Reaction:
Li (s) + MgCl2(aq) -----> LiCl2 (aq) + Mg (s)
Double Replacement Reaction:
3CaCl2(aq) + 2Na3(PO4) (aq) ---> Ca3(PO4)2 (aq) + 6NaCl (aq)
Do replacement reactions always occur?
Single Replacement Reactions
Li + MgCl2 ----->
Double Replacement Reactions
• Usually will occur because the reactants are
aqueous solutions (mobile ions able to interact
equally with other ions of opposite charge).
3CaCl2(aq) + 2Na3(PO4) (aq) ---> Ca3(PO4)2 (aq) + 6NaCl (aq)
• Can use the solubility table to determine if one of
the products of a double replacement reaction is
insoluble in solution (precipitate/solid)
3CaCl2(aq) + 2Na3(PO4) (aq) ---> Ca3(PO4)2 (?) + 6NaCl (?)
Acids and Bases dissolve and
dissociate in water.
Ionic vs. Covalent Compounds
• Most covalent compounds (exception acids),
will not dissociate in solvents.
Ionic solution
Covalent solution
Electrolytes
Electrolytes: Solutes that dissociate in
solvents.
Non-electrolytes: Solutes that do NOT
dissociate in solvents.
Chem II: 9/3/13
Objectives:
• Evaluate hypothesis for Activity Series and
Solubility Labs with peers.
• Record, analyze, and establish conclusions for
each lab.
Homework:
• Conclusion and Balance equations from labs if
needed.
• Read pgs. 276-280: Synthesis and
Decomposition Rxtns.
• Stoichiometry Enrichment Problems (3pts.)
Stoichiometry Lab: Enrichment
1.Calculate the amount of 6M HCl (in mL) needed
to sufficiently react with 2.0 grams of
Na(HCO3). (Hint: Density of 6M HCl = 1.09 g/mL)
2. Validate why the calculated volume of 6M HCl
above could increase percent yield of products.
3.Compare the calculated volume of 6M HCl with
the actual amount you added in the expt.
*Can add 3 pts. to chem I review exam  *
*Due Thursday *
Chem II: 9/4/13
Objectives:
• Complete Activity Series and Solubility Lab
• Address Chem I Exams
• Address Predicting Products in Synthesis and
Decomposition Reactions (pgs. 276-280)
Homework:
• Stoichiometry Enrichment problem (3pts to test)
• Synthesis and Decomposition Practice
problems on webpage
Replacement Reaction Labs
• Establish a purpose for each lab.
• First evaluate hypothesis on white boards.
with peers. (data table with hypothesis)
• As perform mini reactions, record data on your
lab sheet and on white board.
• Use white board to discuss results with peers
and complete conclusion section on your lab
sheet.
Waste: Use water bottle to remove waste from
spot plates into trash cans. Rinse and dry
spot plates.
Chem II: 9/5/13
Objectives:
• Analyze results from replacement reaction labs.
• Establish the net ionic equation for each reaction in
the double replacement lab.
• Discuss Predicting Products in Synthesis and
Decomposition Reactions (pgs. 276-280)
• Address Chem I Exams
Homework:
• Complete net ionic equations for double replacement
lab.
• Predicting products worksheet (webpage)
• Quiz tomorrow: Activity Series and Solubility
Activity Series Lab Results
CuCl2
Cu
(copper II)
Mg
Zn
Ca
Ag(NO3) HCl
H(OH)
Activity Series Lab
• For those reactions that occurred in the
lab, use the solubility diagram to determine
if the ionic compound formed is soluble or
insoluble in solution.
Solubility Lab Results
Ag(NO3)
Na2(CO3)
Na3(PO4)
Na(OH)
Na2(SO4)
NaCl
Pb(NO3)2
CaCl2
Solubility: Dissolving
• The degree substances dissolve (physically mix)
with one another.
• Like dissolves like.
Salt added to water
Soluble
Insoluble
Dissociation
• The degree a solute separates into its ions in a
solvent.
• Ionic compounds, acids, and bases can dissociate.
NaCl dissociated in H2O
Acids and Bases dissolve and
dissociate in water.
Chem II: 9.13
Infinite Campus Update:
• Molarity vs. Molality Lab
Objectives:
• Chemical Reactions Exam
• Address solubility rules misconceptions
• Introduce Acidic and Basic Solutions
Homework:
• Enjoy the weekend! 
Ionic vs. Covalent Compounds
• Most covalent compounds (exception: acids),
will not dissociate in solvents.
Ionic solution
Covalent solution
Electrolytes
Electrolytes: Solutes that dissociate in
solvents.
Non-electrolytes: Solutes that do NOT
dissociate in solvents.
Net Ionic Equations
Purpose:
• Determines which ions actually react in
a solution.
Na2(CO3) + Ag(NO3)  Na(NO3) + Ag2(CO3)
Net Ionic Equations
Spectator Ions: Do not participate in the
reaction. “Watch the reaction only.”
Chem II: 9/6/13
Objectives:
• Gallery Walk: Activity Series, Solubility, Net Ionic
Equations
• Activity Series and Solubility Quiz
• Address Chem I Exam and Enrichment Problem
• Discuss Predicting Products in Synthesis and
Decomposition Reactions (pgs. 276-280)
Homework:
• Predicting Products and Net Ionic Equation Wksht.
(webpage)
Net Ionic Equations
KI
+ Pb(NO3)2
---->
PbI2
+
K(NO3)
1. Balance the chemical equation and establish
states of matter.
2. Re-write the equation emphasizing the ions in
the reaction.
3. Cancel out spectator ions.
4. Re-write equation with ions that participate in the
reaction.
Gallery Walk
• Activity Series Table (Single Replacement)
• Solubility Table for Ionic Compounds
• Establish Net Ionic Equations for Double
Replacement Reactions
Chem II: 9/9/13
Due:
Acitivty Series and Solubility Lab
Objectives:
• I can predict products and states of matter for
most chemical reactions.
• I can establish Net Ionic Equations for Double
Replacement Reactions.
• Address Chem I exam and stoichiometry
enrichment problem.
• Assess Activity Series/Solubility Quiz
• I can distinguish between moles and molarity.
Chemical Reactions
For each reaction:
1. Classify type of reaction
2. Predict products
3. Balance Equations
4. Predict states of matter for each substance.
5. If double replacement, establish net ionic
equation.
Synthesis Reactions
• Oxides of active metals react with water
to produce metal hydroxides.
Ex. CaO (s) + H2O(l) -----> Ca(OH)2 (s)
• Oxides of some non-metals react with
water to produce oxyacids.(containing
oxygen).
Ex. SO2(g) + H2O (l) ----> H2(SO3) (aq)
Decomposition Reactions
• Decomposition of less active metal oxides:
Ex. HgO (s) ----> Hg(l) + O2(l) (breaks into elements)
• Decomposition of metal carbonates:
Ex. Ca(CO3) --->CaO + O2 (metal oxide + CO2)
• Decomposition of metal chlorates
Ex. K(ClO3) (S) ----> KCl (S) + O2 (g) (metal chloride + O2)
• Decomposition of metal hydroxides (reverse of
synthesis)
• Decomposition of acids (reverse of synthesis)
Molarity Calculations
1. If a 3.5 L solution contains 0.5 moles
sodium chloride, what is the solution’s
molarity?
2. What is the molarity of a solution containing
5.85 g of KI dissolved in enough water to
make 0.125L of solution?
Chem II: 9/10/13
Objectives:
• I can predict products and states of matter for
most chemical reactions.
• I can establish Net Ionic Equations for Double
Replacement Reactions.
• Address Chem I exam and stoichiometry
enrichment problem.
• I can distinguish between Molarity (M)) and
Molality (m).
Homework:
Molarity vs. Molality Practice problems
Molarity vs. Molality Lab: complete conclusion
Chemical Reactions: Predicting Products
Webpage Problems:
*9. SO2 + H2O ---->
Synthesis Reactions
• Oxides of active metals react with water
to produce metal hydroxides.
Ex. CaO (s) + H2O(l) -----> Ca(OH)2 (s)
• Oxides of non-metals react with water to
produce oxyacids.
Ex. SO2(g) + H2O (l) ----> H2(SO3) (aq)
Chem I Review Exam
Stoichiometry Lab: Enrichment
Na(HCO3) + HCl  NaCl + CO2 + H2O
1.Calculate the amount of 6M HCl (in mL)
needed to sufficiently react with 2.0 grams of
Na(HCO3). (Hint: Density of 6M HCl = 1.09 g/mL)
Molarity Calculations
Molarity vs. Molality Lab
Background:
One can calculate the concentration of a
solution by molarity (M) or molality (m).
Purpose: Understand the difference between
molarity and molality through a lab
application.
Chem II: 9.11
Infinite Campus Update:
• Activity Series/Solubility Lab (30 pts.)
• Replacement Reaction Quiz (16pts.)
Objectives:
• Bell Ringer :Chemical Reactions
• Distinguish between molarity and molality
concentrations of solutions.
• Address solubility rules misconceptions
Homework:
• Complete conclusion for Molarity vs. Molality Lab
• Review chemical reaction material (exam 9.12)
Bell Ringer: Chemical Reactions
1. Determine if the following reactions would occur. If so,
predict products, balance equation, and establish states
of matter for each substance in the reaction.
a. Al + Sr(OH)2 --->
c. I2 + NaCl
b. K + H2O ---->
d. Cl2 + BaBr2
2. Classify each reaction, predict products, balance
equations, and establish the state of matter for all
substances in the reaction.
a. Pb(NO3)4 + BaI2 ----->
b. Mg(OH)2 ----->
c. SO3 + H2O ----->
d. Mn(ClO3)2
3. Establish the net ionic equation for the double
replacement reaction in qts. 2.
Molality Wksht
Net Ionic Equations
The first pair that can prove with written
evidence that this double replacement reaction
can be simplified will get a free homework
pass and gator tag. 
Al(OH)3 + H(NO3) --->
Molarity vs. Molality Lab
Chem II: 9.13
Infinite Campus Update:
• Molarity vs. Molality Lab
Objectives:
• Chemical Reactions Exam
• Address solubility rules misconceptions
• Introduce Acidic and Basic Solutions
Homework:
• Enjoy the weekend! 
Chem II: 9.16
Infinite Campus Update:
• Molarity vs. Molality Lab (12pts.)
Objectives:
• Address solubility rules misconceptions
• Distinguish between suspensions, colloids, and
solutions.
• Introduce Acidic and Basic Solutions
Homework:
Bell Ringer: Mixtures
Section: 12.1
1. a.Distinguish between homogenous mixtures
and heterogenous mixtures.
b. Give an example of each.
2. a. What is the difference between a
suspension and a colloid and give an example
of each.
b. Classify each as a homogenous or
heterogenous mixture.
3.a. What is the Tyndall Effect?
b. How is it useful to scientists?
Solubility
“Like solvents dissolves like solutes”
• Polar solvents dissolve polar solutes.
Ex. salt water
• Non-polar solvents dissolve non-polar solutes.
Ex. oil-based paints dissolved in paint thinner.
en.wikipedia.org
Electronegativity and Polar Molecules
Solubility Table
• Overall very reliable (confirmed from lab).
• Soluble: > 0.1M concentration of solute
dissolved in solution.
• Insoluble: < 0.0001M concentration of solute
dissolved in solution.
• Slightly soluble: between 0.0001M and 0.1 M of
solute dissolved in solution.
Soluble vs. Insoluble
Substance
C6H12O6
Mg(OH)2
Al(ClO3)3
H3(PO4)
Ba(CO3)
Soluble in water ?
(aqueous)
Dissociates in water?
Bell Ringer: Mixtures
Section: 12.1
1. a.Distinguish between homogenous mixtures
and heterogenous mixtures.
b. Give an example of each.
2. a. What is the difference between a
suspension and a colloid and give an example
of each.
b. Classify each as a homogenous or
heterogenous mixture.
4. a. What is the Tyndall Effect?
b. How is it useful to scientists?
Suspension vs. Colloids
Suspensions:
Colloids:
Tyndall Effect
When light is scattered by particles in a colloid,
because they are not uniformly distributed.
schools.birdville.k12.tx.us
Acids and Bases
• Define and illustrate the difference
between an acid and a base.
Acids and Bases dissolve and
dissociate in water.
Properties of Acids
• Proton (H+) donors
• Have a pH lower than 7.
• Effects indicators ( blue litmus paper/ methyl orange)
• Taste sour
• Neutralizes bases
Ex. HCl + Na(OH) ----> NaCl + H2O
• Reacts with strong metals to produce H2 gas.
Ex. Mg + HCl ---> MgCl2 + H2(g)
Strong vs Weak Acids and Bases
Strong Acids/Bases: Dissociates 100% in solution.
Wead Acids/Bases: Dissocates less than 5% in solution.
Weak Acid: H(NO2)
Strong Acid: HCl
www.chem.wisc.edu
Properties of Bases
• Proton (H+) acceptors.
(OH)- + H+ ----> H2O
• Have a pH higher than 7.
• Effects indicators (red litmus paper/phenolphthalein)
• Taste bitter and can feel slippery
• Neutralizes acids
Ex. Mg(OH)2 + HCl ----> MgCl2 + H2O
Strength of Acids and Bases
Predict whether or not each example below is
classified as strong or weak.
1. HF
9. K(OH)
2. Na(OH)
10. Mg(OH)2
3. Ca(OH)2
4. H2(CO3)
5. H(C2H3O2)
6. H(NO3)
7. H2(SO4)
8. H3(PO4)
Chem II: 9.17
Objectives:
• Distinguish between suspensions, colloids, and
solutions.
• Classify strong and weak acids/bases.
• Identify oxidation numbers in substances.
Homework:
Mixtures
Classify the following as a solution, suspension,
or colloid.
a. sugar and water
b. soluble starch and water
c. clay and water
d. food coloring and water
e. sodium borate and water
f. cooking oil and water
g. gelatin and water
h. 2% milk
Strength of Acids and Bases
Look over section 1 from Chpt 14 to validate if
correct or not.
1. HCl
2. Na(OH)
3. Ca(OH)
4. H2(CO3)
5. H(C2H3O2)
6. H2(CO3)
Strong Acids and Bases
http://chem1180.blogspot.com
Weak Acids and Bases
Weak Bases:
Weak Acids:
• NH3 ammonia
• HC2H3O2(acetic acid)
• NH4(OH) ammonium • HF (hydrofluoric acid)
hydroxide
• HCN (hydrocyanic acid)
• HNO2 (nitrous acid)
• H2(CO3) (carbonic acid)
Oxidation Numbers