K1: INTENSIFIED CHEMISTRY UNIT OUTLINE
UNIT K: CHEMICAL REACTIONS, BALANCING EQUATIONS, & STOICHIOMETRY
TOPICS:
OBJECTIVES:
This unit is designed to teach you how to:
 predict the products of a chemical reaction for 5 general types of chemical reactions,
 balance chemical equations by applying the law of conservation of mass,
 classify chemical reactions as synthesis (combination), decomposition (analysis), single displacement, double displacement, or combustion.
 use the coefficients from balanced chemical equations to derive information regarding moles, particles, relative volumes, and molar masses;
 use the above information to solve and products.
quantitative problems regarding reactants
Upon completion of this unit, you will be expected to:
1.
differentiate between the reactants and products of a chemical reaction;
2.
classify a reaction as one of the four following categories, given the methods used to identify: synthesis (combination), decomposition, single displacement, double displacement (ionic/metathesis), and combustion;
3.
write symbols for the reactants and products of a chemical reaction given the “rules” associated with the five categories of chemical reactions,
4.
write the correct formulas for the reactants and products of a chemical reaction by supplying subscripts for compounds and diatomic molecules,
5.
balance the overall equation to conform to the Law of Conservation of Mass by supplying coefficients where necessary
6.
predict reaction products of reactions given the reactants and the type of reaction.
7.
Determine if a theoretical reaction will actually occur.
8.
list what information can derived from the coefficients of a balanced equation
(moles, molecules/particles, liters, etc.),
9.
determine the relative number of moles, molecules/particles, and liters represented by the coefficients of a balanced equation,
10.
convert the number of moles of a substance into sample mass ,
11.
convert the number of moles of a substance into molecules/particles ,
12.
convert the number of moles of a substance into liters ,
13.
use stoichiometric analysis and dimensional analysis (factor label method) to solve problems involving the calculation of the mass, moles, particles and/or liters of a product given quantitative information about a reactant ,
14.
use stoichiometric analysis and dimensional analysis (factor label method) to solve problems involving the calculation of the mass, moles, particles and/or volume (in mL or L) of a product given quantitative information about a product.
CHEMISTRY FRAMEWORK
STRANDS:
LEARNING
STANDARDS:
CLASSROOM
HANDOUT
MATERIALS
CHEMISTRY: CH.1 g; CH..3 a, b, c, d, e ; CH.4 a, b
K1: UNIT OUTLINE
B2: PERIODIC TABLE
H3: Naming Compounds Flowchart
K2: Chemical Word Equations Worksheet
K3: Activity Series/Solubility Chart
K4: DOUBLE REPLACEMENT ACTIVITY
K5: Activity of Metals Activity
K6: Ellen Conant’s Sinful Brownies-Intro to Stoichiometry Using a Recipe
VOCABULARY/
CONCEPTS/
SCIENTISTS
K1-1
K1-2
K7: Stoichiometry Practice Problems/Unit K Study Guide
K8: Unit K Reading Notes
You are expected to be thoroughly familiar with the following. You will find definitions, explanations, and information about these in your reading (reference sections are noted).
They will also be explained, discussed, and illustrated through classroom and lab activities. chemical reaction (11.1) reactants, products (11.1)


K1-3
K1-4
K1-5
K1-6
K1-7
K1-8
K1-9
K1-10
K1-11
K1-12
K1-13
K2-1
K2-2
K3-1
K3-2
K3-3
K3-4
K3-5
K3-6
K3-7
K3-8
K3-9
K3-10
K4-1
K4-2
K4-3
K4-4
K2-3
K2-4
K2-5
K2-5
K2-6 chemical equation (11.1) indications of a chemical reaction vs physical change (11.1) word equation (11.1) formula equation (11.1) exothermic, endothermic (revisited, 11.1) phase designations and other symbols used in chemical equations (11.1) significance of a balanced chemical equation (11.1) coefficients (11.1) balanced equation (11.1) conservation of mass (11.1) procedures for balancing chemical equations (11.1) combustion reactions (11.2) synthesis/combination reactions—reactions of elements or simpler compounds to form more complex species (11.2) decomposition reactions through electrolysis or heating (11.2) single displacement reactions—replacing a metal with another metal in a compound, replacement of hydrogen in water with a metal, replacement of hydrogen in an acid with a metal, replacement of halogens (8 activity of an element—the activity series—determining if a hypothetical single displacement or synthesis reaction occurs (11.2, Table 11.2) double displacement reactions in aqueous solutions and requirements for them to occur (11.2) solubility of cations in the presence of other ions—how to determine if a precipitate forms in a double replacemnt/displacement reaction(class notes, solubility rules on p.344) composition stoichiometry and reaction stoichiometry (12.1) types of reaction stoichiometry problems (12.1)
Avogadro’s Hypothesis (Law) (10.2, page 300)
STP (10.2, page 300) molar volume of gases (10.2, page 300) what coefficients can represent (mole ratios, volume ratios, molecule ratios) (12.1, unit notes) volume—volume problems (unit notes) stoichiometry using a recipe (unit notes) procedure for solving mass—mass problems (12.2, unit notes) procedure for solving mixed mass—volume—particle problems (12.2, unit notes) limiting and excess reactants (12.3) reasons for using excess reactants in real life (12.3) determining the limiting reactant, and calculating product yields(12.3) percent yield (12.3)
EVALUATION: You will be evaluated via the following:

Daily homework quizzes based on reading and written assignments

Unit Test—covers all objectives stated above.
ASSIGNMENTS:
#K-1 Reading:
Written:
#K-2 Reading
Written
#K-3 Reading
Written
#K-4 Reading
Written
11.1
Chemical Word Equations W/S (DO ON A SEPARATE SHEET OF PAPER)
11.2, 11.3 (don’t worry about net ionic equations—just predicting formation of a precipitate) pp. 339: #25, 27; p. 344 : #35 ; p. 34 8 #60
12.1, 12.2
Supplemental Stoichiometry Practice Problems W/S: # 1—7
12.3
Supplemental Stoichiometry Practice Problems W/S: # 8, 9 pp. 379—380 : # 47, 48