Chemistry (2/25)
• Acid/Base Quiz
• Interpreting and Balancing chemical equations
Due:
• Acid/Base Nomenclature worksheet for partial credit

Chemical Reactions Objectives
1.Classify and name compounds in chemical reactions
2.Describe chemical reactions in word and chemical
equations.
3.Balance chemical equations based on the Law of
Conservation of Mass.
4.Identify and classify types of chemical reactions and energy changes involved.
5.Predict products and energy changes in a chemical reaction.
6.Identify and test factors that affect the rate of chemical reactions.

Chemistry (2/26)
Infinite Campus Update:
• Acid/Base Nomenclature Worksheet (10pts.)
• Acid/Base Quiz (15pts.)
*Check infinite a lot of missing assignments!*
Objectives:
• Interpreting and Balancing chemical equations
Homework:
• Check for missing assignments on infinite campus
• Balancing chemical equations worksheet

Chemical Reaction Pre-Test
1. What is a chemical reaction?
2. If matter is conserved during a chemical reaction, how is it new matter is “created”?
3. Complete the questions below on the following word equation:
Fe(s) + O
2
(g) ----> FeO (s) a. Give an example of a reactant from this reaction.
b. Give an example of a product from this reaction.
c.
Balance the chemical equation if needed. d. Circle the type of chemical reaction you think this represents.
synthesis decomposition replacement neutralization combustion

Chemical Reactions
• Substances chemically interact to form different substances.
• A substance can be an element or a compound.
• Chemical bonds are broken and created.
Example: Fe(s) + O
2
(g) ----> FeO (s)

Chemical Equations
Fe + O
2
------> FeO
Reactants:
• Starting substances.
• Chemically interact with one another.
• Usually located to the left of the arrow.
Products:
• Ending substances.
• Substances formed from the chemical reaction.
• Usually located to the right of the arrow.

Chemical Equations
Fe
(s)
+ O
2 (g)
------> FeO
(s)
Abbreviations for state of matter in an equation.
• (s)= substance in solid state
• (g)= substance in gaseous state
• (l)= substance in liquid state
• (aq)= substance dissovled in water.
(aqueous solution)

Law of Conservation of Mass
Fe
(s)
+ O
2 (g)
------> FeO
(s)
Are atoms destroyed or created during a chemical reaction?
No, they are just rearranged to produce new substances.

Law of Conservation of Mass
Fe
(s)
+ O
2 (g)
------> FeO
(s)

Balancing Chemical Equations
Why? Observe the Law of Conservation of Mass
Rules:
1. Add coefficients in front of substances, do NOT change subscripts.
2. First balance elements that only appear once on each side of the equation.
3. Make sure coefficients are expressed in lowest terms.

Chemistry (2/27)
Objectives:
• Interpreting and Balancing chemical equations
• Review acid/base quiz
Homework:
• Balancing equations worksheet(due Thursday)
• Law of Conservation of Mass pre-lab qts. and hypothesis
• Review acids/bases nomenclature
• Check for missing assignments in infinite campus
Lab:
Law of Conservation of Mass Lab: (Thursday)

Homework:
• Read through the background and procedures section.
• Complete pre-lab questions and hypothesis.

a. K + MgCl
2
---------> KCl + Mg b. Ag
2
O ---------> Ag + O
2 c. CH
4
+ O
2
-------> CO
2
+ H
2
O

Chemical Equations

Chemistry (2/28)
Objectives:
• Interpreting and Balancing Chemical Equations
• Validate the Law of Conservation of Mass with scientific evidence.
Due Today:
• Balancing chemical equations worksheet (turn in tray)
• Law of Conservation of Mass pre-lab qts. and hypothesis
Homework:
• Balancing Chemical Equations practice problems (Fri.)
• Check for missing assignments in infinite campus

Dihydrogen monoxide + sodium (bicarbonate) ---> carbon dioxide + sodium hydroxide + dihydrogen monoxide

Purpose:
Validate the Law of Conservation of Mass
Lab Reminders:
• Follow ALL lab procedures carefully.
• Use the same balance for all measurements.

Exit Slip:
Interpret and Balance Chemical Equations
1. Cl
2
(g) + KBr (aq) ----> KCl (aq) + Br
2
(l) a. Balance the equation if needed
2. CH
4
(g) + O
2
(g)  CO
2
(g) + H
2
O(g) a. Balance the equation if needed.
b. Identify the diatomic molecule in this reaction.

Exit Slip:
1. Cl
Interpret and Balance Chemical Equations
2
(g) + KBr (aq) ----> KCl (aq) + Br
2
(l) a. Which reactant is a molecule?
b. What is the chemical name of the product that is an ionic compound?
c. What does (aq) mean?
d. Balance the equation if needed
2. CH
4
(g) + O
2
(g)  CO
2
(g) + H
2
O(g) a. Balance the equation if needed.
b. Identify the diatomic molecule in this reaction.

Dihydrogen monoxide + sodium (bicarbonate) ---> carbon dioxide + sodium hydroxide + dihydrogen monoxide a. convert to chemical equation b. Balance equation if needed.

Law of Conservation Of Mass
• Matter is not created or destroyed.
• Matter is just rearranged.
(mass of reactants = mass of products)
That is why it is important to balance chemical equations.

Law of Conservation of Mass Inquiry Lab
• Purpose: To prove mass is conserved in chemical reactions.
• Materials and Procedures: Groups will establish
• Record and analyze data
• Establish a conclusion

http://www.chem.umass.edu/people/botch/Chem122S08/Chapters/Ch6/InternalE.html

pre-AP Chemistry (2/20)
Objectives:
• Clarify misconceptions with writing and balancing chemical equations.
• Validate the Law of Conservation of Mass
(Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

States of Matter Abbreviations
Fe
(s)
+ O
2 (g)
------> FeO
(s)
Abbreviations for state of matter in an equation.
• (s)= substance in solid state
• (g)= substance in gaseous state
• (l)= substance in liquid state
• (aq)= substance dissovled in water.
(aqueous solution)

Chemical Equations
1. magnesium chloride + fluorine yields magnesium fluoride + chlorine
2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

Reminder:
• Quiz tomorrow over writing and balancing chemical equations. (complete extra practice problems from paper or webpage)
Objective:
• Validate the Law of Conservation of Mass
(Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

Reminder:
• Quiz today over writing and balancing chemical equations. (complete extra practice problems from paper or webpage)
Objective:
• Validate the Law of Conservation of Mass
(Design, perform, and analyze chemical reaction between Alka Seltzer and tap water).

Chemical Equations
1. magnesium chloride + fluorine yields magnesium fluoride + chlorine
2. iron + sulfuric acid yield iron(II)sulfate + sulfur dioxide + dihydrogen monoxide

Law of Conservation of Mass Inquiry Lab
• Purpose ,Background, Hypothesis: completed
Objectives:
• List materials needed for each experiment.
• List procedures specific enough for someone else to repeat. (sign-off by Ms. Leeper)
• Perform experiments and record data.
(record all qualitative and quantiative data)

http://www.chem.umass.edu/people/botch/Chem122S08/Chapters/Ch6/InternalE.html

1. N
2
(g) + H
2
(g) --------> NH
3
(g) a. What is the chemical name of one of the reactants?
b. What is the chemical name of the product?
c. What state of matter is all the substances in this reaction?
d. Balance the chemical equation if needed.

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 (C x
H x
+ O
2
----> CO
2
+ H
2
O)
6. Neutralization (Acid + Base--> H
2
O + Salt)
*Each letter represents a substance*

Chemical Reactions Objectives
1. Identify and classify types of chemical reactions.
2. Identify energy changes involved with chemical reactions.
3. Predict products and energy changes in a chemical reaction.

Synthesis (Combination) Reaction
• 2 or more substances chemically combine to form a single substance.
• A + B ---> AB + energy
• Energy released into surroundings is more than energy absorbed by the system.
( Energy of surroundings > Energy of system)

Decomposition Reaction
• A compound breaks down into simpler substances.
• AB + energy ----> A + B
• Energy of system > Energy of surroundings
Why?

Single Replacement Reaction
• An element replaces another element in a compound.
• A + BC --------> B + A C + energy
• Energy of surroundings > Energy of system

Double Replacement Reaction
• Exchange of cations between two compounds.
• A B + C D + energy ----> C B + A D + more energy
• Energy of Surrounding > Energy of System

Combustion Reaction
• Fuel (hydrocarbons) reacts with oxygen to produce predictable substances and energy.
• C x
H x
+ O
2
----> CO
2
+ H
2
O + ENERGY
• Energy of Surroundings > Energy of System

• Acid and Base react to produce predictable products.
• Changes the pH to 7 (neutral).
Acid + Base -------> H
2
O + Salt
Salt: An ionic compound.
The cation comes from the base and the anion from the acid.

Class Reminders:
• Acid Rain Article (15pts.)
• Balance Chemical Equations Worksheet (10pts.)
(balance and classify equations)
• Word Equation Worksheet (10pts.)
*3 rd Quarter Ends: March 8 th*

Purpose:
• Perform and observe types of chemical reactions.
• Determine reactants and predict products.
• Classify chemical reactions.
• Balance chemical reactions.
• Write a formal lab report

3
4
1
2
5
6
7
8
Reaction Chemical Equation

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 (C x
H x
+ O
2
----> CO
2
+ H
2
O)
6. Neutralization (Acid + Base--> H
2
O + Salt)

Chemical Equations to Lab
Just need to check and see if they are balanced.
1. Mg + O
2
------>
2. Mg + HCl ---->
3. (NH
4
)
2
(CO
3
) -----> NH
3
4. Ca(CO
3
) + HCl ----> CaCl
2
+ CO
2
+ H
2
+ H
2
O
O + CO
2
5. Zn + CuCl
2
6. CuCl
2
+ Na
3
---->
(PO
4
) --->
7. HCl + Na(OH) ----> H
2
O + NaCl
8. C
2
H
6
O + O
2
----->

Chemical Reaction Review
1. What are the coefficients that will balance the chemical equation below?
AlCl
3 a. 1,3,1,3
+ Na(OH) ----> Al(OH)
3
+ NaCl b. 3,1,3,1 c. 1,1,1,3 d. 1,3,3,1
2. What type of chemical reaction is in question 1?
3. Predict the product and balance if needed:
Ba (s) + O
2
(g) ---------->

Balancing and Classifying Chemical Reactions

Chemical Equations to Lab
Just need to check and see if they are balanced.
1. Mg + O
2
------> MgO
2. Mg + HCl ----> MgCl + H
2
3. (NH
4
)
4. Ca(CO
2
3
(CO
3
) -----> NH
3
) + HCl ----> CaCl
2
+ CO
2
+ H
2
O
+ H
2
O + CO
2
5. Zn + CuCl
2
6. CuCl
2
+ Na
3
----> ZnCl
2
+ Cu
(PO
4
) ---> Cu
3
(PO
4
)
2
+ NaCl
7. HCl + Na(OH) ----> H
2
O + NaCl
8. C
2
H
6
O + O
2
-----> CO
2
+ H
2
O

Conclusion
Needs to include the following:
• Identify and explain the types of reactions obsvd. ?
• Which reaction(s) did you like the best and why?
• Based on data section explain which reactions were exothermic and endothermic.
• What did you learn from this lab?

• Chemical Reaction Lab (20pts.)
• Balancing Chemical Equation Wksht.(10pts.)

1. Classify the type or reaction and balance if needed: a. C
6
H
12
+ O
2
---------> CO
2
+ H
2
O b. LiCl ------> Li + Cl
2 c. H
2
(SO
3
) + Al(OH)
3
-------> H
2
O + Al
2
(SO
3
)
3

Predicting Products in a Chemical Reaction a. Ca + N
2
--------> ?
b. Cu
2
S -------> ?
c. NaBr + F
2
------> ?
d.CH
4
+ O
2
----->

Balancing and Classifying Equations Quiz
Types of Chemical Reactions
1. Synthesis
2. Decomposition
3. Single Replacement
4. Double Replacement
5. Combustion
6. Neutralization

• Check my webpage for correct chemical formulas prior to balancing.

Predicting Single Replacement Reactions
• An Activity Series can help us predict if a single replacement reaction will take place.

Copper (s)
Magnesium (s)
Activity Series Lab Hypothesis
CuCl
2
(aq) Ag(NO
3
) HCl (aq) dH(OH) (l)
Zinc (s)
Calcium (s)

• Complete conclusion
• Complete Post Lab Questions

1. Using the Activity Series Table, predict whether the following single replacement reactions would occur: a. Li + MgCl b. Hg + Na
3
P c. Pb + HF

• Chpt. 9.4 Acids and Bases
• Chpt. 11: Balancing, Classifying, and Predicting
Chemical Reactions
• Chpt. 18.1: Reaction Rates

Predicting Single Replacement Reactions
• An Activity Series can help us predict if a single replacement reaction will take place.

Predicting Single Replacement Reactions
1. Determine which single replacement reactions below can occur using your Activity Series diagram: a. K + MgCl
2 b. Al + Li
3
(PO
4
) c.
Sn 2+ + HCl d.
Ag + HCl e. Pb 4+ + H
2
(SO
3
)

Chemical Reaction Study Guide Changes
1. Vocabulary words: Thermochemistry
10. HgO + energy ------> Hg + O2
11. Fe + F
2
12. CH
4
+ O
2
----------> FeF
3
---------> CO
2
+ energy
+ H
2
O + energy
15. K(OH) + H
3
(PO4) ------->
18.
Omit last word equation. 

Chemical Reaction Review
1. What are the coefficients that will balance the chemical equation below?
AlCl
3 a. 1,3,1,3
+ Na(OH) ----> Al(OH)
3
+ NaCl b. 3,1,3,1 c. 1,1,1,3 d. 1,3,3,1
2. What type of chemical reaction is in question 1?
3. Predict the product and balance if needed:
BaS + Mg ---------->

Energy changes that occur within reactions.
Endothermic Reactions Exothermic Reactions

Exothermic Reaction
• Energy absorbed < Energy released.
• The chemical reaction becomes cooler and its surroundings gets warmer.
• Energy is on the product side.
• C
8
H
18
+ O
2
-------> CO
2
+ H
2
O + energy

• Energy absorbed > Energy released
• Chemical reaction gets warmer and its surroundings gets cooler.
• Energy is on the reactant side.
Ex. Photosynthesis

1. Using the Activity Series diagram would the following reactions take place?
a. Al + Cu(OH) b. Ag + HCl
2. Classify the type or reaction and balance if needed: a. C
6
H
12
+ O
2
---------> CO
2 b. LiCl ------> Li + Cl
2 c. H
2
(SO
3
) + Al(OH)
3
+ H
2
O
-------> H
2
O + Al
2
(SO
3
)
3

Endo
Exo

• Chemical Reaction Lab(20pts.)
• Activity Series Lab (10pts.) (1,2,4,6)
• Balancing Chemical Equation Wksht.(10pts.)
• Word Equation Worksheet (10pts.)

• Chemical Reaction Lab(20pts.)
• Balancing Chemical Equation Wksht.(10pts.)
• Word Equation Worksheet (10pts.)

Bell Ringer: Thermochemistry
1. Classify as exothermic (Ex) or endothermic. (Endo) a. C
8
H
18 b. BaBr
2
+ O
2
-------------> CO
2
+ H
2
O + energy
+ energy -----------> Ba + Br
2
2. During an experiment you observed the test tube getting cooler. Explain why this is happening including the terms system and surroundings.
3. Using the activity series determine which reactions will occur in nature:
Mg + FeCl
2
Cu + K(OH)
Al + H
2
(CO
3
)

Work on question 2 on Thermochemistry wksht.

Chemical Reaction Energy Diagram
• Activation Energy (Ea) : The amount of kinetic energy needed to be absorbed by the reactants in order for the chemical reaction to occur.
H : The amount of kinetic energy released into the surroundings.

Chemical Reaction Energy Diagram

Chemical Reaction Energy Diagram
Activation
Energy

Chemical Reactions Objectives
1.Classify and name compounds in chemical reactions
2.Describe chemical reactions in word and chemical equations.
3.Balance chemical equations based on the Law of
Conservation of Mass.
4.Identify and classify types of chemical reactions and energy changes involved.
5.Predict products and energy changes in a chemical reaction.
6.Identify and test factors that affect the rate of chemical reactions. (Chpt. 18.1)

Assignment:
Read Section: 18.1 in textbook (pg. 540)

Chemical Reactions Rates
• Reaction Rates = how fast the reactants chemically change into the products.
• Collision Theory: Reactant particles will form products when reactants collide:
- at the right position.
- and exchange the right amount of kinetic energy.

Rates of Chemical Reactions
• What are factors that can affect the speed of a reaction?

Rates of Chemical Reactions
• What are factors that can affect the rates of reactions?
• Temperature
• Concentration of Reactants
• Surface Area of Reactants
• Catalysts
• Inhibitors

Temperature of Reaction
What if we increase the temperature of a reaction?
What if we decrease the temperature of a reaction?

Concentration
• Increase concentration of reactants?
• Decrease concentration of reactants?

Surface Area
• Increase surface area of reactants?
• Decrease surface area of reactants?

Catalysts
• Catalysts speed up reactions, but they are not apart of the chemical reaction.
Ex. Enzymes keep your body temperature around 37 o C (98 o F) by speeding up important biological reactions.

Inhibitors
• Inhibitors slow down a chemical reaction.
• Inhibitors bind to a catalyst and prevent it from speeding up a reaction.
Ex. Preservation of food. Antioxidants prevent foods from becoming stale or moldy.

Time
Conc
Soln. A Concentration vs. Avg. Reaction Times
G1 G2 G3 G4 G5 G6 G7 Avg.
A1
(100%)
15 20 35 16 37 22 25
A2
(75%)
A3
(50%)
A4
(25%)
19
25
50
24
33
39
38
37
34
20
22
29
31
25
38
44
65
78
28
28
34

• Activation energy = minimum energy colliding reactants must have for a reaction to occur. (Energy hump.)

• Chpt. 9.4 Acids and Bases
• Chpt. 11: Balancing, Classifying, and Predicting
Chemical Reactions
• Chpt. 18.1: Reaction Rates

• Classifying Chemical Reaction lab (20pts.)
• Activity Series Lab (10pts.)
• Starch Iodine Lab (10pts.)-due Wed.
• ACT Test for Juniors: Tomorrow, March 6 th
• End of quarter: Thursday, March 8th

Chemical Reaction Study Guide

Infinite Campus Updated
• Activity Series Lab (10pts)
• Classifying Chemical Reaction Lab (15pts)
(Do NOT throw away-Formal Lab Report)
• Starch-Iodine Reaction Lab w/graph. (15pts)
• Quarter End: Tomorrow, March 8 th
(All assignments by Friday).

• Due: March 14 th (next Wed.)
• Written (legible) or Typed (save to flashdrive)