1. What are the six types of chemical reactions?

2. 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 + O > CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)

3. 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 + MgCl > Double Replacement Reaction: Ex. CaCl2 + Na3(PO4) --->

4. Replacement Reactions
Single Replacement Reaction: Ex. Li + MgCl > LiCl2 + Mg Double Replacement Reaction: Ex. CaCl2 + Na3(PO4) ---> Ca3(PO4)2 + NaCl

5. 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?

6. Single Replacement Reactions
Li + MgCl >

7. 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 (?)

9. Acids and Bases dissolve and dissociate in water.

10. Ionic vs. Covalent Compounds
Most covalent compounds (exception acids), will not dissociate in solvents.
Ionic solution Covalent solution

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

13. 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 : Synthesis and Decomposition Rxtns.
Stoichiometry Enrichment Problems (3pts.)

14. 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 = g/mL)
2. Validate why the calculated volume of 6M HCl above could increase percent yield of products.
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 *

15. 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 )
Homework:
Stoichiometry Enrichment problem (3pts to test)
Synthesis and Decomposition Practice problems on webpage

16. 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.

17. 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 )
Address Chem I Exams
Homework:
Complete net ionic equations for double replacement lab.
Predicting products worksheet (webpage)
Quiz tomorrow: Activity Series and Solubility

18. Activity Series Lab Results
CuCl2
Ag(NO3)
HCl
H(OH) Cu
(copper II) Mg Zn Ca

19. 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.

21. Solubility Lab Results
Ag(NO3)
Pb(NO3)2
CaCl2
Na2(CO3)
Na3(PO4)
Na(OH)
Na2(SO4)
NaCl

23. Solubility: Dissolving
The degree substances dissolve (physically mix) with one another.
Like dissolves like.
Salt added to water
Soluble
Insoluble 23

24. Dissociation The degree a solute separates into its ions in a solvent.
Ionic compounds, acids, and bases can dissociate.
NaCl dissociated in H2O 24

25. Acids and Bases dissolve and dissociate in water.

26. 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! 

27. Ionic vs. Covalent Compounds
Most covalent compounds (exception: acids), will not dissociate in solvents.
Ionic solution Covalent solution

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

29. Net Ionic Equations Purpose:
Determines which ions actually react in a solution.
Na2(CO3) + Ag(NO3)  Na(NO3) + Ag2(CO3)

30. Net Ionic Equations
Spectator Ions: Do not participate in the reaction. “Watch the reaction only.”

31. 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 )
Homework:
Predicting Products and Net Ionic Equation Wksht. (webpage)

32. Net Ionic Equations KI + Pb(NO3)2 ----> PbI2 + K(NO3)
Balance the chemical equation and establish states of matter.
Re-write the equation emphasizing the ions in the reaction.
Cancel out spectator ions.
Re-write equation with ions that participate in the reaction.

33. Gallery Walk Activity Series Table (Single Replacement)
Solubility Table for Ionic Compounds
Establish Net Ionic Equations for Double Replacement Reactions

34. 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.

35. Chemical Reactions For each reaction: Classify type of reaction
Predict products
Balance Equations
Predict states of matter for each substance.
If double replacement, establish net ionic equation.

36. 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)

37. 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)

38. Molarity Calculations
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?

39. 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

40. Chemical Reactions: Predicting Products
Webpage Problems: *9. SO2 + H2O ---->

41. 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)

42. Chem I Review Exam

43. 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)

44. Molarity Calculations

45. 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.

46. 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)

47. Bell Ringer: Chemical Reactions
Determine if the following reactions would occur. If so, predict products, balance equation, and establish states of matter for each substance in the reaction.
Al + Sr(OH)2 ---> c. I NaCl
K + H2O > d. Cl2 + BaBr2
Classify each reaction, predict products, balance equations, and establish the state of matter for all substances in the reaction.
Pb(NO3)4 + BaI >
Mg(OH) >
SO3 + H2O >
Mn(ClO3)2
3. Establish the net ionic equation for the double replacement reaction in qts. 2.

48. Molality Wksht

49. 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) --->

50. Molarity vs. Molality Lab

51. 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! 

52. 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:

53. Bell Ringer: Mixtures Section: 12.1
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?

54. 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

55. Electronegativity and Polar Molecules

56. Solubility Table Overall very reliable (confirmed from lab).
Soluble: > 0.1M concentration of solute dissolved in solution.
Insoluble: < M concentration of solute dissolved in solution.
Slightly soluble: between M and 0.1 M of solute dissolved in solution.

57. Soluble vs. Insoluble Substance Soluble in water ? (aqueous)
Dissociates in water?
C6H12O6
Mg(OH)2
Al(ClO3)3
H3(PO4)
Ba(CO3)

59. Bell Ringer: Mixtures Section: 12.1
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.
a. What is the Tyndall Effect?
b. How is it useful to scientists?

60. Suspension vs. Colloids
Suspensions: Colloids:

61. Tyndall Effect When light is scattered by particles in a colloid,
because they are not uniformly distributed.
schools.birdville.k12.tx.us

62. Acids and Bases
Define and illustrate the difference between an acid and a base.

63. Acids and Bases dissolve and dissociate in water.

64. 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)

65. 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

66. 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

67. Strength of Acids and Bases
Predict whether or not each example below is classified as strong or weak.
HF K(OH)
Na(OH) Mg(OH)2
Ca(OH)2
H2(CO3)
H(C2H3O2)
H(NO3)
H2(SO4)
H3(PO4)

68. Chem II: 9.17
Objectives:
Distinguish between suspensions, colloids, and solutions.
Classify strong and weak acids/bases.
Identify oxidation numbers in substances.
Homework:

69. Mixtures Classify the following as a solution, suspension, or colloid.
sugar and water
soluble starch and water
clay and water
food coloring and water
sodium borate and water
cooking oil and water
gelatin and water
2% milk

70. Strength of Acids and Bases
Look over section 1 from Chpt 14 to validate if correct or not.
HCl
Na(OH)
Ca(OH)
H2(CO3)
H(C2H3O2)

71. Strong Acids and Bases

72. Weak Acids and Bases Weak Bases: Weak Acids: NH3 ammonia
NH4(OH) ammonium hydroxide
Weak Acids:
HC2H3O2(acetic acid)
HF (hydrofluoric acid)
HCN (hydrocyanic acid)
HNO2 (nitrous acid)
H2(CO3) (carbonic acid)

73. Oxidation Numbers