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 ReactionsDirections:

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 ReactionsLi + 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

ElectrolytesElectrolytes: Solutes that dissociate in

solvents.

Non-electrolytes: Solutes that do NOT dissociate in solvents.

Chem II: 9/3/13Objectives:

• 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: 9/4/13Objectives:

• 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: 9/5/13Objectives:• 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 Ag(NO3) HCl H(OH)

Cu (copper II)

Mg

Zn

Ca

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) Pb(NO3)2 CaCl2

Na2(CO3)

Na3(PO4)

Na(OH)

Na2(SO4)

NaCl

Solubility: Dissolving

InsolubleSoluble

Salt added to water

• The degree substances dissolve (physically mix) with one another. • Like dissolves like.

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: 9.13Infinite 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

ElectrolytesElectrolytes: Solutes that dissociate in

solvents.

Non-electrolytes: Solutes that do NOT dissociate in solvents.

Net Ionic EquationsPurpose:

• Determines which ions actually react in a solution.

Na2(CO3) + Ag(NO3) Na(NO3) + Ag2(CO3)

Net Ionic EquationsSpectator Ions: Do not participate in the

reaction. “Watch the reaction only.”

Chem II: 9/6/13Objectives:• 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: 9/9/13Due:

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 Calculations1. 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: 9/10/13Objectives:• 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 LabBackground:

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: 9.11Infinite 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 Reactions1. 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 EquationsThe 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: 9.13Infinite 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: 9.16Infinite 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: MixturesSection: 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 Soluble in water ? (aqueous)

Dissociates in water?

C6H12O6

Mg(OH)2

Al(ClO3)3

H3(PO4)

Ba(CO3)

Bell Ringer: MixturesSection: 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. ColloidsSuspensions:

Colloids:

Tyndall EffectWhen 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

www.chem.wisc.edu 

Strong Acid: HCl Weak Acid: H(NO2)

Strong Acids/Bases: Dissociates 100% in solution.Wead Acids/Bases: Dissocates less than 5% in solution.

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 BasesPredict 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: 9.17Objectives:• 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 BasesLook 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:

• NH3 ammonia

• NH4(OH) ammonium hydroxide

Weak Acids:

• HC2H3O2(acetic acid)

• HF (hydrofluoric acid) • HCN (hydrocyanic acid)

• HNO2 (nitrous acid)

• H2(CO3) (carbonic acid)

Oxidation Numbers