Week of September 01, 2013
Monday
Labor Day
Tuesday
N.RN.3 A.SSE.2
A.SSE.3 A.APR.6
A.APR.7 A.REI.3
F.BF.1.a
Wednesday
11-12.RST.4 11-12.RST.8 N.RN.3 A.SSE.2
9-12.P.1.5 9-12.N.1.2 9- A.SSE.3 A.APR.6
12.N.2.2 9-12.N.2.3A
A.APR.7 A.REI.3
Advanced Chemistry F.BF.1.a
Algebra III
Chapter P Preliminary
Concepts
Thursday
Algebra III
Chapter 1 - Matter and
Measurement
Section 1.1 - Chemistry:
Principles and
Section P.1 - The Applications
Real Number
Section 1.2 - Getting
System
Started: Some Key
Terms
Objectives
Section 1.3 - Scientific
Measurements
1. Sets
Section 1.4 - Precision
2. Union and
and Accuracy
Intersection of Sets Section 1.5 - A Problem
3. Absolute Value Solving Method
and Distance
Section 1.6 - Further
4. Interval Notation Remarks on Problem
5. Order of
Solving
Operations
6. Simplifying
Objectives
Variable
Expressions
1. Describe the usual
method used to study
Assessment
science.
Chapter P Preliminary
Concepts
Section P.2 Integer and
Rational Number
Exponents
Friday
11-12.RST.4 1112.RST.8 9-12.P.1.1
9-12.P.1.2 9-12.P.1.5
9-12.P.1.1A 912.P.1.2A 912.P.1.8A 9-12.N.2.2
Advanced
Chemistry
Chapter 1 - Matter
and Measurement
Section 2.1 - Laws
of Chemical
Combination
Section 2.2 - John
Dalton and the
Objectives
Atomic Theory of
Matter
1. Properties of
Section 2.3 - The
Exponents
Divisible Atom
2. Scientific
Section 2.4 Notation
Atomic Masses
3. Rational
Section 2.5 - The
Exponents and
Periodic Table:
Radicals
4. Simplify Radical Elements
Organized
Expressions
Section 2.6 Molecules and
Assessment
Molecular
Pgs. 15-17 (1-113 2. Classify a sample of Pgs. 31-34 (1-123 Compounds
every other odd) matter as being
every other odd) Section 2.7 - Ions
and Ionic
substance or mixture,
Compounds
element or compound,
Section 2.8 - Acids,
homogeneous or
Bases, and Salts
heterogeneous.
Section 2.9 Organic
3. Classify properties
Compounds
and changes as chemical
or physical,
Objectives
and
understand
the differences between
1. State and apply
them.
the laws of
constant
4. Recognize and use the
composition
common SI units and
prefixes.
5. Express and convert
measurements using the
common SI
prefixes
and
exponential notation.
6. Convert, when
relevant data are given,
measurements between
the
SI and other
systems of measurement.
7. Use the appropriate
number of significant
figures in writing
numbers and
expressing calculation
results.
8. Explain the difference
between accuracy and
precision.
9. Solve problems,
including those
involving density, using
the unitconversion
method.
Assessment
Chapter 1 Test
(definite
proportions),
multiple
proportions, and
conservation of
mass.
2. Relate Dalton's
atomic theory to
these fundamental
laws of chemical
combination.
3. Describe the
important
properties of
protons, neutrons,
and electrons.
4. Define isotope,
and determine the
number of
neutrons, protons,
and electrons from
atomic and mass
numbers.
5. Define atomic
mass unit and
atomic mass.
6. Calculate the
weighted average
atomic mass of an
element from
isotopic masses
and natural
abundances.
7. Distinguish
metals from
nonmetals, using
the periodic table.
8. Write empirical
and molecular
formulas.
9. Relate the names
and formulas of
binary molecular
compounds.
10. Define the ion
and ionic
substance, and be
able to write the
names and
formulas of
monatomic ions
and their
compounds.
11. Relate the
names and
formulas for
polyatomic ions
and name
compounds
containing them.
12. Describe the
characteristics of
acids, bases, and
salts according to
the Arrhenius
concept.
13. Relate the
names and
formulas of simple
acids and bases.
14. Recognize
alkane
hydrocarbons,
relate the names
and formulas of
simple alkanes, and
represent them
with molecular,
structural,
condensed
structural, and lineangle formulas.
15. Recognize the
alcohol and
carboxylic acid
functional groups,
and relate the
names and
formulas of simple
molecules
containing them.
16. Identify organic
molecules that are
isomers.
Assessment
Pgs. 66-73 (1-113
odd)
Assigned over the
course of multiple
class periods.
Prep
A.REI.11 F.BF.1 F.BF.1.a Prep
F.BF.1.b
Algebra II
A.REI.11 F.IF.9
F.BF.1 F.BF.1.a
F.BF.1.b F.BF.3
Algebra II
Chapter 1 - Models,
Functions, and
Permutations
Chapter 1 Models, Functions,
and Permutations
Section 1.3 - Relations
and Functions
Quiz 1.1-1.4
Objectives
Section 1.5 Vertical and
Horizontal
Translations
1. Design and use
relations and functions.
2. Determine whether a
relation is a function.
Assessment
Pgs. 23-25 (1-11 odd,
12, 17-29 odd, 35-41
odd)
Objectives
1. Analyze vertical
and horizontal
translations of a
function.
Assessment
Section 1.4 - Working
with Functions
Pgs. 35-37 (1-41
every other odd)
Pg. 37 -
Objectives
Checkpoint (2-14
even)
1. Combine functions.
2. Add functions.
Assessment
Lunch
Pgs. 29-31 (1-67 every
other odd)
Lunch
Lunch
11-12.RST.3 1112.RST.4 1112.RST.5 1112.RST.6 9-12.N.2.1
9-12.N.2.2 912.N.2.3A
11-12.RST.1 11-12.RST.2 11-12.RST.3 1111-12.RST.3 9-12.N.2.2 9- 12.RST.4 1112.N.2.3A
12.RST.5 1112.RST.6 9-12.N.2.1
Applied Chemistry
9-12.N.2.2 912.N.2.3A
Unit 1 - Chapter 2 -
Chemistry
Chapter 1 - An
Introduction to
Chemistry
Chapter Objectives
Measurements
Chemistry
Section 2.1 - Units of
Measurement
Chapter 1 - An
Introduction to
Chemistry
Objective
Write the names and
1. Define all of the abbreviations for the
terms in the
metric SI units used in
Chapter Glossary. measurements of length,
volume, mass,
Section 1.3 - The temperature, and time.
Scientific Method
Section 2.2 - Scientific
2. Describe how Notation
science in general
is done.
Objective
Section 1.4 Write a number in
Measurement and scientific notation
Units
Section 2.3 - Measured
3. Use the
Numbers and
International
Significant Figures
System of
Measurements (SI) Objective
base units and their
abbreviations to
Identify a number as
describe length,
measured or exact;
mass, time,
determine the nuber of
temperature, and significant figures in a
Lunch
11-12.RST.1 1112.RST.2 1112.RST.3 9-12.N.2.2
9-12.N.2.3A
Applied
Chemistry
Unit 1 - Chapter 2 Measurements
Section 2.1 - Units
of Measurement
Chapter Objectives
Objective
1. Define all of the
terms in the
Write the names
Chapter Glossary. and abbreviations
for the metric SI
Section 1.3 - The units used in
Scientific Method measurements of
length, volume,
2. Describe how mass, temperature,
science in general and time.
is done.
Section 2.2 Section 1.4 Scientific Notation
Measurement and
Units
Objective
3. Use the
Write a number in
International
scientific notation
System of
Measurements (SI) Section 2.3 base units and their Measured
abbreviations to
Numbers and
describe length,
Significant
mass, time,
Figures
temperature, and
volume.
measured number.
volume.
4. Describe the
Section 2.4 - Significant 4. Describe the
relationship
Figures in Calculations relationship
between liters and
between liters and
cubic meters.
Objective
cubic meters.
Objective
Identify a number
as measured or
exact; determine
the nuber of
significant figures
in a measured
number.
5. State the
Adjust calculated
5. State the
numbers or
answers to give the
numbers or
fractions
correct number of
fractions
represented by the significant figures.
represented by the Section 2.4 following metric
following metric Significant
prefixes, and write Section 2.5 - Prefixes prefixes, and write Figures in
their abbreviations: and Equalities
their abbreviations: Calculations
giga, mega, kilo,
giga, mega, kilo,
centi, milli, micro, Objective
centi, milli, micro, Objective
nano, and pico.
nano, and pico.
Use the numerical values
Adjust calculated
6. Describe the
of prefixes to write a
6. Describe the
answers to give the
relationships
metric equality
relationships
correct number of
between the metric
between the metric significant figures.
units that do not
Section 2.6 - Writing units that do not
have prefixes (such Conversion Factors
have prefixes (such Section 2.5 as meter, gram, and
as meter, gram, and Prefixes and
liter) and units
Objective
liter) and units
Equalities
derived from them
derived from them
by the addition
Write a conversion
by the addition
Objective
of prefixes.
factor for two units that of prefixes.
describe the same
Use the numerical
7. Given a metric quantity.
7. Given a metric values of prefixes
unit, write its
unit, write its
to write a metric
abbreviation; given Section 2.7 - Problem abbreviation; given equality
an abbreviation,
an abbreviation,
Solving
write the full name
write the full name Section 2.6 of the unit.
Objective
of the unit.
Writing
Conversion
8. Use everyday
Use conversion factors 8. Use everyday
Factors
examples to
to change from one unit examples to
describe the
to another.
describe the
Objective
approximate size of
approximate size of
a millimeter, a
Write a conversion
Section 2.8 - Density a millimeter, a
centimeter, a
centimeter, a
factor for two units
meter, and a
Objective
meter, and a
that describe the
kilometer.
kilometer.
same quantity.
Calculate the density of
9. Use everyday
a substance; use the
9. Use everyday
Section 2.7 examples to
density to calculate the examples to
Problem Solving
describe the
mass or volume of a
describe the
approximate size of substance.
approximate size of Objective
a milliliter, a liter,
and a cubic meter.
Assessment
10. Describe the
relationship
between cubic
centimeters and
milliliters.
11. Describe the
relationship
between mass and
weight.
Worksheet Packet
a milliliter, a liter,
and a cubic meter. Use conversion
factors to change
10. Describe the from one unit to
relationship
another.
between cubic
centimeters and
Section 2.8 milliliters.
Density
12. Name the two
factors that cause
the weight of an
object to change.
11. Describe the Objective
relationship
between mass and Calculate the
weight.
density of a
substance; use the
12. Name the two density to calculate
factors that cause the mass or volume
the weight of an
of a substance.
object to change.
13. Use everyday
examples to
describe the
approximate size of
a gram, a kilogram,
and a megagram.
13. Use everyday Assessment
examples to
describe the
Worksheet Packet
approximate size of
a gram, a kilogram,
and a megagram.
14. Describe the
relationships
between metric
tons, kilograms,
and megagrams.
14. Describe the
relationships
between metric
tons, kilograms,
and megagrams.
15. Describe the
Celsius,
Fahrenheit, and
Kelvin temperature
scales.
15. Describe the
Celsius,
Fahrenheit, and
Kelvin temperature
scales.
16. Describe the
relationship
between a degree
Celsius, a degree
Fahrenheit, and a
kelvin.
16. Describe the
relationship
between a degree
Celsius, a degree
Fahrenheit, and a
kelvin.
Section 1.5 Reporting Values
from
Measurements
Section 1.5 Reporting Values
from
Measurements
17. Given values
for a series of
measurements,
state the precision
of the
measurements.
17. Given values
for a series of
measurements,
state the precision
of the
measurements.
18. Report
measured values so
as to show their
degree of
uncertainty.
18. Report
measured values so
as to show their
degree of
uncertainty.
19. Given a value
derived from a
measurement,
identify the range
of possible values
it represents based
on the assumption
that its uncertainty
is ±1 in the last
position reported.
19. Given a value
derived from a
measurement,
identify the range
of possible values
it represents based
on the assumption
that its uncertainty
is ±1 in the last
position reported.
Assessment
Assessment
Pgs. 27-31 (15-47
Pgs. 27-31 (15-47
odd)
odd)
A.REI.11
F.BF.1
F.BF.1.a
A.REI.11 F.BF.1
SRB
SRB
F.BF.1.b
F.BF.1.a F.BF.1.b
Algebra II
Algebra II
Chapter 1 - Models,
Functions, and
Permutations
Chapter 1 Models, Functions,
and Permutations
Section 1.3 - Relations
and Functions
Section 1.3 Relations and
Functions
Objectives
Objectives
1. Design and use
relations and functions.
2. Determine whether a
relation is a function.
Assessment
1. Design and use
relations and
functions.
2. Determine
whether a relation
is a function.
Pgs. 23-25 (1-11 odd,
12, 17-29 odd, 35-41
odd)
Section 1.4 - Working
with Functions
Objectives
1. Combine functions.
2. Add functions.
Assessment
Pgs. 23-25 (1-11
odd, 12, 17-29 odd,
35-41 odd)
Section 1.4 Working with
Functions
Objectives
Assessment
Pgs. 29-31 (1-67 every
other odd)
1. Combine
functions.
2. Add functions.
Assessment
Pgs. 29-31 (1-67
every other odd)