Chemistry Pacing Chart
2012 – 2013
Important Points During Instruction
Comprehensive curriculum may not follow the order of the text book. Embedding inquiry investigations and process skills into content instruction means
shifting the emphasis from teachers presenting information and covering textbook topics to students doing science. In other words, the Science as Inquiry GLEs
should be embedded within the content and hands-on activities throughout the year. Also, integrate technology, science in society and engineering, whenever
possible.
Mandatory Testing Components and Lab Reports
To help prepare all students for the ACT, “Science Skills” shall be assessed on every major test. Also, two (2) lab reports per nine weeks are required. One lab is
governed from the district level; the other is the choice of the teacher. The following lab activities are mandated by the district and the directions can be found
in Moodle in the Core Curriculum course in a folder labeled District Mandated Labs unless otherwise indicated. You will also find lab report formats that you
may use.
1st Nine Weeks: Separating Mixture Lab
2nd Nine Weeks: ½ Life Lab Using Pennies (see p. 708 in Holt)
3rd Nine Weeks: Dissolving Penny Lab (Flinn Kit AP-5609)
4th Nine Weeks: Titrations (see p. 626 in Glencoe)
Important Testing Dates
Midterm Examinations: December 12 – 19, 2012 (school-based decision)
Explore (9th), PLAN (10th), and ACT (11th): March 19, 2013
End-of-Course Testing: April 23-May 23, 2013 (school-based decision)
Final Examinations: April 23 – May 21, 2013
Winter Break
Time
Aug. 15 –
Sept. 7
4 weeks
Sept. 10 Sept. 28
3 Weeks
Textbook Chapters
Modern Chemistry
Holt McDougal © 2012
Chapter 2.2, 2.3
Scientific Method
Chapter 2.1
Chapter 1.2
Topics
CC Units
Old Textbook Chapters
Measurement & Problem
Solving
(CC: Unit 1)
Chapter 1
Chapter 2
Matter
(CC: Unit 2)
Chapter 3
Key Concepts
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Oct. 1 –
Nov. 2
5 Weeks
Atoms
Chapter 3
Radioactive Decay
Chapter 21
Atoms and The Periodic Table
(CC: Unit 3)
Chapter 4
Chapter 25-Sec. 1-3
Chapter 5
Chapter 6
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Electron Configuration
Chapter 4
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Periodic Law
Chapter 5
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Metrics
Accuracy & Precision
Significant Figures (stress all year)
Scientific Notation (stress all year)
Factor-label method/dimensional analysis (stress all
year)
Graphing
Scientific Method
Lab Safety
Physical vs. chemical properties
Physical vs. chemical changes using diagrams &
descriptions of energy changes
Classification of matter based on physical properties
(elements, mixtures, compounds; solids, liquids, gases)
Design and conduct a laboratory investigation in which
physical properties are used to separate the substances
in a mixture
Analyze the development of the modern atomic theory
from a historical perspective
How atoms differ (atomic number, atomic mass,
isotopes, etc.)
Differentiate among alpha, beta, and gamma emissions
Calculate amount of radioactive substance remaining
given number of half-lives passed.
Describe the uses of radioactive isotopes and radiation
in such areas as plant and animal research, health care,
and food preservation
Draw accurate valence electron configurations and
Lewis dot structures for selected atoms
Identify the number of bonds an atom can form given
the number of valence electrons
Predict the physical and chemical properties of an
element based only on its location in the periodic table
Predict the stable ion(s) an element is likely to form
when it reacts with other specified elements
Use the periodic table to compare electronegativities
and ionization energies of elements to explain periodic
properties, such as atomic size
GLEs
 PS:
 PS:
 PS:
 PS:
 PS:
1
2
3
4
1
 SI: 2, 4, 5, 7
 SI: 1-4, 7, 9, 15
 SI: 10
 PS: 14, 15
 PS: 31
 PS: 14, 21
 PS: 21
 PS: 8
 PS: 8
 PS: 10
 PS: 11
 PS: 12
 PS: 9
 PS: 13
 PS: 15
 PS: 16
 PS: 17
Nov. 5 –
Dec. 11
4 Weeks
Chemical Bonding
Chapter 6
Formulas & Names
Chapter 7
Chemical Bonding & the
Formation of Compounds
(CC: Unit 4)
Chapter 8
Chapter 9
 Represent ionic bonds using Lewis dot structures,
electron configurations, orbital notation, etc. & predict
bond type using the periodic table
 Ionic Compounds (properties; naming & formulas)
 Ionic bonds vs. metallic bonds
 Represent covalent bonds using Lewis dot structures,
electron configurations, orbital notations, molecular
formulas, molecular shape, etc. & predict bond type
using the periodic table
 Covalent Compounds (properties; naming & formulas)
 Distinguish between ionic compounds, polar molecules
& nonpolar molecules using electronegativity
difference
 PS: 16, 22, 23
 PS: 5, 6, 16, 22 – 24, 38, 46
 PS: 15, 22
 PS: 15, 22
 PS: 5, 6, 22 – 24, 38, 46
 PS: 22, 23
Midterm Examinations: December 12-19, 2012 (school-based decision)
After Winter Break
Time
Jan. 7 –
Feb. 20
6 Weeks
Textbook Chapters
Modern Chemistry
Holt McDougal © 2012
Stoichiometry
Chapter 9
Chemical Reactions &
Equations
Chapter 8
Feb. 21 Apr. 12
6 Weeks
Gases
Chapter 11
KMT
Chapter 10.1
Equilibrium
Topics
CC Units
Old Textbook Chapters
Moles, Reactions, &
Stoichiometry
(CC: Unit 5)
Chapter 11-Sec. 1 & 2
Chapter 11- Sec. 3-5
Chapter 10
Chapter 20-Sec. 1
Chapter 12
States of Matter, Energy
Changes, and LeChatelier’s
Principle
(CC: Unit 6)
Chapter 13-Sec. 1 & 2
Chapter 14
Chapter 13-Sec. 4
Key Concepts
 Describe the mole as a counting word/quantity and
demonstrate the ability to solve mole conversion problems
 Chemical formulas & the mole (molar mass, percent
composition, calculate empirical & molecular formulas)
 Evidence of chemical reactions
 Writing & balancing chemical equations
 Types of chemical reactions (synthesis, combustion,
decomposition, single replacement, double replacement,
redox)
 Stoichiometry (conversion problems, limiting reactants,
percent yield)
 Kinetic Molecular Theory
 The gas laws (Boyle’s, Charles’, Gay-Lussac’s, Combined, Ideal)
 Gas stoichiometry
 Energy in physical & chemical changes (specific heat,
thermochemical reactions, calorimetry)
 Equilibrium
 LeChatelier’s Principle
GLEs
 PS: 1, 4, 8
 PS: 5, 40, 41
 PS: 6, 7, 31, 34
 PS: 6, 7, 31, 34, 38, 39
 PS: 7, 31, 34 – 36, 38,
39, 45
 PS: 40, 41
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PS:
PS:
PS:
PS:
29
29
41
30, 42 – 44
 PS: 37
 PS: 37
Chapter 18
Apr. 15 –
May 16
5 Weeks
Solutions
Chapter 12
Colligative Properties
Chapter 13.2
Chapter 16-Sec. 1-3
Chapter 18
Solutions & Acids vs. Bases
(CC: Unit 7)
Chapter 15
Chapter 19
Acids & Bases
Chapter 14
May 21 –
end
Titration & pH
Chapter 15
Organic Chemistry
Chapter 22
Carbon & Its Compounds
(CC: Unit 8)
Chapter 22-Sec. 1-3
Chapter 24-Sec. 1-4
 Equilibrium constants
 PS: 37
 Solutions (ionic vs. molecular) & factors affecting solubility
 Solutions vs. suspensions & colloids
 Solution concentration (percent concentration; molarity;
molality)
 Colligative properties (esp. freezing point depression & boiling
point elevation)
 Acids & bases (properties, names, formulas, etc.)
 pH
 Titrations
 PS: 14, 19
 PS: 14, 19
 PS: 20
 selected structural formulas of organic compounds
 common biological molecules, such as carbohydrates, lipids,
proteins, and nucleic acids by using structural formulas
 investigate and model hybridization in carbon compounds
 name, classify, and diagram alkanes, alkenes, and alkynes
 PS: 25 – 28
 PS: 25 – 28
Final Examinations: May 17 – 24, 2013 (school-based decision)
 PS: 18
 PS: 35
 PS: 32, 33, 35
 PS: 32, 33, 35
 PS: 25 – 28
 PS: 25 – 28