East Side Union High School District
Marking Period 3. Chemistry Daily Objectives
2010-2011
Important Notes:
A. Review Isotopes and concept of atomic mass review atomic mass and isotopes
1. Review atomic mass and isotopes
B. Three facets of the mole: mass, number of particles, volume
C. Review mass versus volume
D. Concept of particle in chemistry (atoms, molecules, formula units, ions etc)
E. Point out that molar volume only applies to gases and under very specific conditions (STP)
2. Remind students that molar volume only applies to gases and only under specific conditions.
F. Only mass is substance specific - the other two are constants
G. The mole is a unit of counting equal to 6.02 x 1023 particles
H. The mole is defined as the number of carbon 12 atoms having a mass of exactly 12 grams
I. Masses on the periodic table represent the gram equivalent of one mole of each element
J. Parts of an equation: Plus signs, arrows etc.
K. Write a chemical equation using proper formatting
L. Demonstrate appropriate use of subscripts and coefficients
M. Calculate the moles produced or consumed in a chemical reaction
N. One mole of a gas has a volume of 22.4 L at STP
O. Successfully use a unit conversion method (Dimensional Analysis, Factor Label, T Chart)
P.
Chemical Reactions (Std. 3a-3e)
 Writing Equations (word eqns./formulas)
 Balancing Equations
 Types of Reactions
“Formula” Stoichiometry (Std. 3a-3e)
 The Mole (formula mass/molar mass, Avogadro’s number)
 Mole Conversions (massmole, molemass, molparticles, molvolume)
Reaction Stoichiometry (Std. 3a-3e)
 “massmolmolmass” (particles, molar volume)
School days this MP are __22____. By the end of the period today, my students will be able to:
(Should start with this?)
1.
Recognize that matter is conserved in chemical reactions.
2.
Recognize products and reactants in a chemical equation
3.
Convert between a passage and a word equation
4.
Translate between word and formula equations
5.
Balance a chemical equation using coefficients (atom inventory)
6.
Identify reaction types
7.
Identify the missing reactants or products of a known reaction type
8.
Unit Test I
9.
Recall that the quantity one mole is set by defining one mole of carbon 12 atoms to have a mass of
exactly 12 grams.
10.
Recognize that one mole equals 6.02 x 1023 particles, 22.4 L of a gas at STP and that the masses
on the periodic table are gram equivalents of one mole.
11.
Calculate the Molar (Molecular/Formula) mass of a substance
12.
Successfully use a unit conversion method (Dimensional Analysis, Factor Label, T Chart)
13.
Convert between grams and moles
14.
Use Avogadro’s # (6.02 x 1023 particles) to convert between # of particles and # moles
15.
Convert between moles and Liters of a gas at STP
16.
The coefficients in balanced chemical equation represent the mole ratios of products and reactants
17.
Convert between moles of various species (reactants/products) in a chemical equation
18.
Convert between masses of various species (reactants/products) in a chemical equation
19.
Convert between different amounts of various species (reactants/products) in a chemical equation
20.
Review for Benchmark Test #3 Unit Test II
21.
Benchmark Test #3
Possible activities
1. Copper cycle
2. Silver cycle
3. Chemical changes and equations
4. Hydrates lab
5. Chalk assessment
6. Stoichiometry and the decomposition of sodium bicarbonate
7. Stoichiometry in the reaction between sodium bicarbonate and acetic acid
Possible assignments
Important Notes:
School days this MP are 22. By the end of the period today, my students will be able to:

Conservation of matter

Intro to Chemical equations

Writing Word equations

Translating to Formula

Balancing Chemical Equations

Classifiying Reaction Types

Reinforce balancing

Prediction of reactants and Products
“Formula” Stoichiometry (Std. 3a-3e)
 The Mole (formula mass/molar mass, Avogadro’s number)
 Mole Conversions (massmole, molemass, molparticles, molvolume)
Chemical Reactions (Std. 3a-3e)
 Writing Equations (word eqns./formulas)
 Balancing Equations
 Types of Reactions
Conservation of Matter and Stoichiometry
3. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and
the ability to calculate the mass of products and reactants. As a basis for understanding this concept:
a. Students know how to describe chemical reactions by writing balanced equations.
b. Students know the quantity one mole is set by defining one mole of carbon 12 atoms to have a mass of
exactly 12 grams.
23
c. Students know one mole equals 6.02� particles (atoms or molecules).
�10 d. Students know how to determine the molar mass of a molecule from
its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance
to moles, number of particles, or volume of gas at standard temperature and pressure.
3 7California Department of Education Reposted June 11, 20 09 GRADES NINE THROUGH
TWELVE—CHEMISTRY
e. Students know how to calculate the masses of reactants and products in a chemical reaction from
the mass of one of the reactants or products and the relevant atomic masses.
f.* Students know how to calculate percent yield in a chemical reaction. g.* Students know how to
identify reactions that involve oxidation and reduction and how to balance oxidation-reduction
reactions.