CHEMISTRY SYLLABUS GRADE 11
Grade 11-Chemistry
The Chemistry curriculum is designed to continue student investigations of the
physical sciences that began in grades K-8 and provide students the necessary skills
to be proficient in chemistry. This curriculum includes more abstract concepts such
as the structure of atoms, structure and properties of matter, and the conservation
and interaction of energy and matter. Students investigate chemistry concepts
through experience in laboratories and field work using the processes of inquiry.
Grade 11 - Curricular Content
The course has been developed taking into consideration the standards used by the
National Academies of Science, science as inquiry, physical science, life science,
earth and space science, science and technology, personal and social perspectives,
history, and nature of science.
QUARTER ONE
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INTRODUCTION TO CHEMISTRY
UNIT CONVERSION TO BASE UNITS
ANALYZING DATA
MATTER
STATES OF MATTER
THE STRUCTURE OF THE ATOM
QUARTER TWO
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ELECTRONS IN ATOMS
PERIODIC TABLE AND PERIODIC LAW
IONIC COMPOUNDS AND METALS
COVALENT BONDS
CHEMICAL REACTIONS
SEMESTER REVIEW FOR EXAM
QUARTER THREE
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THE MOLE
STOICHIOMETRY
QUARTER FOUR
 MIXTURES AND SOLUTIONS
 ACIDS AND BASES
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GASES
ENERGY AND CHEMICAL CHANGE
REACTION RATES
CHEMICAL EQUILIBRIUM
REVIEW FOR END OF SEMESTER EXAMS
THE FOLLOWING TOPICS AND OBJECTIVES RELATE TO THE NATIONAL
STANDARDS FOR CHEMISTRY AND ARE ALIGNED TO THE GLENCOE SCIENCE
CHEMISTRY MATTER AND CHANGE TEXTBOOK (with chapters noted in
brackets next to each topic).
Quarter 1
Introduction to Chemistry (Chpt 1)
 Define terminology
 Define areas of study
 Compare and contrast scientific method and enquiry
Analyzing Data (Chpt2)
 Define SI base units for time, length, mass, temperature, volume and density
 Express numbers in scientific notation
 Convert units using dimensional analysis
 Describe the accuracy of experimental data using error and percent error
Matter (Chpt 3)
 Distinguish between physical and chemical properties
 Define physical change and list several common physical changes
 Define chemical change and list several indications that a chemical change
has taken place
 Apply the law of conservation of mass to chemical reactions
 Compare and contrast mixtures and substances
 Distinguish between elements and compounds and mixtures
The Structure of the Atom (Chpt 4)
 Relate element to atomic number and atomic mass
 Determine atomic mass
 Describe modern atomic model
 Define an isotope
 Historical discoveries and models of atoms
 Average Atomic Mass Calculation
Quarter 2
Electrons in Atom (Chpt 5)
 Quantum electron configuration and orbitals
 Relationship between orbitals and energy levels
 Brief discussion of Planck’s equation and spectral lines
 Explain the quantum mechanical model
The Periodic Table and Periodic Law (Chpt 6)
 Associate elements with groups and periods
 Identify trends in periodic table
 Valence number and reactivity
 Trace the development of the periodic table
Ionic Compounds and Metals (Chpt 7)
 Define a chemical bond
 Describe the formation of ionic bonds and the structure of ionic compounds
 Describe the properties of ionic bonds and ionic compounds
 Name and write formulas for ionic compounds
 Describe metallic bonds
Covalent Bonds (Chpt 8)
 Describe the formation of single, double and triple covalent bonds
 Describe the properties of covalent compounds
 Name and write formulas for covalent compounds
 Compare and contrast Hydrogen Bond and Van der Waals Forces - polar and
nonpolar covalent bonds and polar and nonpolar molecules
Chemical Reactions (Chpt 9)
 Balance chemical equations
 Recognize evidence of chemical change
 Classify chemical reactions
 Describe aqueous solutions
 Write complete ionic and net ionic equations for chemical reactions in
aqueous solutions
 Predict products in chemical reactions
Semester Review for End of Semester Exam
Quarter 3
The Mole (Chpt 10)
 Explain how a mole is used to indirectly count the number of particles of
matter
 Relate the mole to a common everyday counting unit
 Convert between moles and number of representative particles
 Relate the mass of an atom to the mass of a mole of atoms
 Convert between number of moles and the mass of an element
 Convert between numbers of moles and number of atoms of an element
 Recognize the mole relationships shown by a chemical formula
 Calculate the molar mass of a compound
 Convert between the number of moles and mass of a compound
 Discuss how to apply conversion factors to determine the number of atoms
or ions in a known mass of a compound
 Explain what is meant by the percent composition of a compound
 Determine the empirical and molecular formulas for a compound from mass
percent and actual mass data and perform calculation
Stoichiometry (Chpt 11)
 Law of Conservation of Matter
 Stoichiometric calculations
 Calculate percent yield
 Identify the limiting reactant in a chemical equation
 Identify the excess reactant and calculate the amount remaining after the
reaction is complete
 Calculate the mass of a product when the mounts of more than one reactant
are given – relate to ideal Gas Law – PV=nRT
States of Matter (Chpt 12)
 Use the kinetic molecular theory to explain the behavior of gases
 Explain how gas pressure is measured and calculate the partial pressure of a
gas
 Describe intramolecular forces
 Compare and contrast intermolecular forces
 Contrast the arrangement of particles in liquids and solids
 Describe the factors that affect viscosity
 Explain how the unit cell and crystal lattice are related
 Explain how the addition and removal of energy can cause a phase change
 Interpret a phase diagram
Gases (Chpt 13)
 State the relationships among pressure, temperature and volume of a
constant amount of gas
 Relate number of particles and volume using Avogadro’s principle
 Compare the properties of real and idea gases
 Determine volume ratios for gaseous reactants and products
 Apply gas laws
 STP calculations
 Kinetic-molecular theory
 Dalton’s law of partial pressures
 Graham’s law of effusion
 Boyle’s law
 Charles’s law
 Gay-Lussac’s law
 Combined gas law
 Ideal gas law
Quarter 4
STUDENTS MUST COMPLETE TOPICS MIXTURES AND SOLUTIONS, AND ACIDS
AND BASES BUT DEPENDING UPON THE PACE OF LEARNING TOPICS AFTER
THAT ARE OPTIONAL –ENERGY AND CHEMICAL CHANGE, REACTION RATES,
AND CHEMICAL EQUILIBRIUM.
Mixtures and Solutions (Chpt 14)
 Discuss Comparison of the properties of suspensions, colloids and solutions
 Describe concentration using different units
 Determine the concentration of solutions
 Calculate the molarity of a solution
 Define solubility  Understand what factors affect solubility
 Solutions and mixtures
 Factors that affect solvation
 Molarity
 Molality
Acids and Bases (Chpt 18)
 Properties of acids, bases, and salts
 Arrhenius definition of acid/base
 Bronsted-Lowry definition of acid/base
 Lewis definition of acid/base
 pH calculations
 Titrations
Energy and Chemical Change (Chpt 15)
 Define energy
 Distinguish between potential and kinetic energy
 Exothermic/endothermic reactions
 Specific heat and heat flow
 Molar enthalpies
 Hess’s law
 Gibbs free energy and spontaneity
Reaction Rates (Chpt 16)
 Calculate average rates of chemical reactions from experimental data
 Identify factors that affect the rates of chemical reactions
 Explain the role of a catalyst
 Interpret energy diagrams
 Factors that affect rates
 Reaction rates
 Rate laws
Chemical Equilibrium (Chpt 17)
 List the characteristics of chemical equilibrium
 Describe how various factors affect chemical equilibrium
 Le Chatelier’s principle
 Equilibrium constants
 Solubility
 Determine equilibrium concentrations of reactants and products
Semester review for End of Semester exam
GRADING POLICY
Student thinking, writing, reading, listening, and speaking are at the center of class
activity therefore student grades are viewed in this context. The teacher
continuously assesses student performance and progress, as evidenced by in-class
task commitment, finished written pieces, on-demand writing, homework, tests and
quizzes, threaded discussion responses, class notes, and daily preparation.
Evaluation System:
Student grades will be calculated as follows:
 Tests, projects and quizzes
60%
 Laboratory work
25%
 Homework
15%
Semester grades are developed based upon the following formula:
 Quarterly Grades
(average)
80%
 Exam Grade or Semester Project 20%