Revised 07.08.15

St Charles Parish Public Schools

Chemistry Curriculum Map 2015-16

First and Second Quarters
Topic / Chapter / Outcomes / GLEs / Time Frame
Classroom Policies and Procedures / n/a / 1 Day
Lab Safety & Equipment /
  • Explain expectations and procedures in the laboratory. (F & PK)
  • Identify laboratory safety procedures and choose appropriate laboratory safety procedures given a lab scenario. (T & R)
/ 2 Days
Lab Teacher-made Assessment -- 1 day
Chemistry is a Physical Science (Section 1) / 1 /
  • Define chemistry
  • List examples of the branches of chemistry
  • Compare and contrast basic research, applied research, and technological development
/ SI.12
PS.14
PS.17
PS.31 / 1 Days
Matter and Its Properties (Section 2) /
  • Distinguish between the physical properties and chemical properties of matter.
  • Classify changes of matter as physical or chemical.
  • Explain the gas, liquid, and solid states in terms of particles.
  • Explain how the law of conservation of energy applies to changes of matter.
  • Distinguish between a mixture and a pure substance.
/ 2 Days
Elements (Section 3) /
  • Use a periodic table to name elements, given their symbols.
  • Use a periodic table to write the symbols of elements, given their names.
  • Describe the arrangement of the periodic table.
  • List the characteristics that distinguish metals, nonmetals, and metalloids.
/ 2 Days
Chapter 1 Teacher-made Assessment -- 1 day
Scientific Method (Section 1) / 2 /
  • Describe the purpose of the scientific method.
  • Distinguish between qualitative and quantitative observations.
  • Describe the differences between hypotheses, theories, and models.
/ PS.1
PS.2
PS.3
PS.4
SI.2 / 2 Days
Units of Measurement (Section 2) /
  • Distinguish between a quantity, a unit, and a measurement standard.
  • Name and use SI units for length, mass, time, volume, and density.
  • Distinguish between mass and weight.
  • Perform density calculations.
  • Transform a statement of equality into a conversion factor.
/ 2 Days
Using Scientific Measurements (Section 3) /
  • Distinguish between accuracy and precision.
  • Determine the number of significant figures in measurements.
  • Perform mathematical operations involving significant figures.
  • Convert measurements into scientific notation.
  • Distinguish between inversely and directly proportional relationships.
/ 1 Days
Measurements Lab / 1 Day
Chapter 2 Teacher-made Assessment -- 1 day
The Atom: From Philosophical Idea to Scientific Theory (Section 1) / 3 /
  • Explain the law of conservation of mass, the law of definite proportions, and the law of multiple proportions.
  • Summarize the five essential points of Dalton’s atomic theory.
  • Explain the relationship between Dalton’s atomic theory and the law of conservation of mass, the law of definite proportions, and the law of multiple proportions.
/ PS.4
PS.7
PS.8
PS.17 / 1 Day
The Structure of the Atom (Section 2) /
  • Summarize the observed properties of cathode rays that led to the discovery of the electron.
  • Summarize the experiment carried out by Rutherford and his co-workers that led to the discovery of the nucleus.
  • List the properties of protons, neutrons, and electrons.
  • Define atom.
/ 1 Day
Counting Atoms (Section 3) /
  • Explain what isotopes are.
  • Define atomic number and mass number, and describe how they apply to isotopes.
  • Given the identity of a nuclide, determine its number of protons, neutrons, and electrons.
  • Define mole, Avogadro’s number, and molar mass, and state how all three are related.
  • Solve problems involving mass in grams, amount in moles, and number of atoms of an element.
/ 4 Days
Chapter 3 Teacher-made Assessment -- 1 day
Electron Configurations (Section 3) / 4 /
  • List the total number of electrons needed to fully occupy each main energy level.
  • State the Aufbau principle, the Pauli exclusion principle, and Hund’s rule.
  • Describe the electron configurations for the atoms of any element using orbital notation, electron configuration notation, and, when appropriate, noble-gas notation.
/ PS.8
PS.15 / 2 Days
Flame Test Lab / 1 Day
Chapter 4 Teacher-made Assessment -- 1 day
History of the Periodic Table (Section 1) / 5 /
  • Explain the roles of Mendeleev and Moseley in the development of the periodic table.
  • Describe the modern periodic table.
  • Explain how the periodic law can be used to predict the physical and chemical properties of elements.
  • Describe how the elements belonging to a group of the periodic table are interrelated in terms of atomic number.
/ PS.13
PS.15
PS.16
PS.17
PS.22 / 1 Day
Electron Configuration and the Periodic Table (Section 2) /
  • Describe the relationship between electrons in sublevels and the length of each period of the periodic table.
  • Locate and name the four blocks of the periodic table.
  • Explain the reasons for these names.
  • Discuss the relationship between group configurations and group numbers.
  • Describe the locations in the periodic table and the general properties of the alkali metals, the alkaline-earth metals, the halogens, and the noble gases.
/ 1 Day
Electron Configuration and Periodic Properties (Section 3) /
  • Define atomic and ionic radii, ionization energy, electron affinity, and electronegativity.
  • Compare the periodic trends of atomic radii, ionization energy, and electronegativity, and state the reasons for these variations.
  • Define valence electrons, andstate how many are presentin atoms of each main-groupelement.
  • Compare the atomic radii,ionization energies, and electronegativities of the d-block elements with thoseof the main-group elements.
/ 2 Days
Chapter 5 Teacher-made Assessment -- 1 day
Introduction toChemical Bonding (Section 1) / 6 /
  • Define chemical bond.
  • Explain why most atoms form chemical bonds.
  • Describe ionic and covalent bonding.
  • Explain why most chemical bonding is neither purely ionic nor purely covalent.
  • Classify bonding type according to electronegativity differences.
/ PS.5
PS.9
PS.13
PS.16
PS.23
PS.24
PS.46 / 1 Day
Covalent Bonding and Molecular Compounds (Section 2) /
  • Define molecule and molecular formula.
  • Explain the relationships among potential energy, distance between approaching atoms, bond length, and bond energy.
  • State the octet rule.
  • List the six basic steps used in writing Lewis structures.
  • Explain how to determine
  • Lewis structures for molecules containing single bonds, multiple bonds, or both.
  • Explain why scientists use resonance structures to represent some molecules.
/ 1 Day
Ionic Bonding and Ionic Compounds (Section 3) /
  • Compare and contrast a chemical formula for a molecular compound with one for an ionic compound.
  • Discuss the arrangements of ions in crystals.
  • Define lattice energy and explain its significance.
  • List and compare the distinctive properties of ionic and molecular compounds.
  • Write the Lewis structure for a polyatomic ion given the identity of the atoms combined and other appropriate information.
/ 1 Day
Chapter 6 Teacher-made Assessment -- 1 day
Chemical Names and Formulas (Section 1) / 7 /
  • Explain the significance of a chemical formula.
  • Determine the formula of an ionic compound formed between two given ions.
  • Name an ionic compound given its formula.
  • Using prefixes, name a binary molecular compound from its formula.
  • Write the formula of a binary molecular compound given its name.
/ PS.5
PS.40 / 1 Day
Oxidation Numbers (Section 2) /
  • List the rules for assigning oxidation numbers.
  • Give the oxidation number for each element in the formula of a chemical compound.
  • Name binary molecular compounds using oxidation numbers and the Stock system.
/ 1 Day
Using Chemical Formulas (Section 3) /
  • Calculate the formula mass or molar mass of any given compound.
  • Use molar mass to convert between mass in grams and amount in moles of a chemical compound.
  • Calculate the number of molecules, formula units, or ions in a given molar amount of a chemical compound.
  • Calculate the percentage composition of a given chemical compound.
/ 2 Days
Chapter 7 Teacher-made Assessment -- 1 day
CUMULATIVE MIDTERM EXAM (CHAPTERS 1-7) -- 1 day
Third and Fourth Quarters
Topic / Chapter / Outcomes / GLEs / Time Frame
Describing Chemical Reactions (Section 1) / 8 /
  • List three observations that suggest that a chemical reaction has taken place.
  • List three requirements for a correctly written chemical equation.
  • Write a word equation and a formula equation for a given chemical reaction.
  • Balance a formula equation by inspection.
/ PS.7
PS.34
PS.35
PS.38
PS.45 / 1 Day
Chemical Reactions Lab / 1 Day
Types of Chemical Reactions (Section 2) /
  • Define and give general equations for synthesis, decomposition, single-displacement, and double-displacement reactions.
  • Classify a reaction as a synthesis, decomposition, single-displacement, double-displacement, or combustion reaction.
  • List three kinds of synthesis reactions and six kinds of decomposition reactions.
  • List four kinds of single-displacement reactions and three kinds of double-displacement reactions.
  • Predict the products of simple reactions given the reactants.
/ 2 Days
Chapter 8 Teacher-made Assessment -- 1 day
Introduction to Stoichiometry (Section 1) / 9 /
  • Define stoichiometry.
  • Describe the importance of the mole ratio in stoichiometric calculations.
  • Write a mole ratio relating two substances in a chemical equation.
/ PS.7
PS.41
PS.45 / 2 Day
Ideal Stoichiometric Calculations (Section 2) /
  • Calculate the amount in moles of a reactant or product from the amount in moles of a different reactant or product.
  • Calculate the mass of a reactant or product from the amount in moles of a different reactant or product.
  • Calculate the amount in moles of a reactant or product from the mass of a different reactant or product.
  • Calculate the mass of a reactant or product from the mass
  • of a different reactant or product.
/ 2 Days
Limiting Reactants and Percentage Yield (Section 3) /
  • Describe a method for determining which of two reactants is a limiting reactant.
  • Calculate the amount in moles or mass in grams of a product, given the amounts in moles or masses in grams of two reactants, one of which is in excess.
  • Distinguish between theoretical yield, actual yield, and percentage yield.
  • Calculate percentage yield, given the actual yield and quantity of a reactant.
/ 2 Day
Limiting and Excess Reactant Lab / 1 Day
Chapter 9 Teacher-made Assessment -- 1 day
Changes of State (Section 4) / 10 /
  • Explain the relationship between equilibrium and changes of state.
  • Interpret phase diagrams.
  • Explain what is meant by equilibrium vapor pressure.
  • Describe the processes of boiling, freezing, melting, and sublimation.
/ PS.46 / 1 Day
Gases and Pressure (Section 1) / 11 /
  • Define pressure, give units of pressure, and describe how pressure is measured.
  • State the standard conditions of temperature and pressure and convert units of pressure.
  • Use Dalton’s law of partial pressures to calculate partial pressures and total pressures.
/ PS.29 / 1 Day
The Gas Laws (Section 2) /
  • Use the kinetic-molecular theory to explain the relationships between gas volume, temperature, and pressure.
  • Use Boyle’s law to calculate volume-pressure changes at constant temperature.
  • Use Charles’s law to calculate volume-temperature changes at constant pressure.
  • Use Gay-Lussac’s law to calculate pressure-temperature changes at constant volume.
  • Use the combined gas law to calculate volume-temperature-pressure changes.
/ 2 Days
Gas Volumes and the Ideal Gas Law (Section 3) /
  • State the law of combining volumes.
  • State Avogadro’s law and explain its significance.
  • Define standard molar volume of a gas and use it to calculate gas masses and volumes.
  • State the ideal gas law.
  • Using the ideal gas law, calculate pressure, volume, temperature, or amount of gas when the other three quantities are known. Reading Skill Builder
/ 2 Days
Chapter 10 & 11 Teacher-made Assessment -- 1 day
Types of Mixtures (Section 1) / 12 /
  • Distinguish between heterogeneous and homogeneous mixtures.
  • List three different solute solvent combinations.
  • Compare the properties of suspensions, colloids, and solutions.
  • Distinguish between electrolytes and nonelectrolytes.
/ PS.14
PS.19
PS.20 / 1 Day
The Solution Process (Section 2) /
  • List and explain three factors that affect the rate at which a solid solute dissolves in a liquid solvent.
  • Explain solution equilibrium, and distinguish among saturated, unsaturated, and supersaturated solutions.
  • Explain the meaning of “like dissolves like” in terms of polar and nonpolar substances.
  • List the three interactions that contribute to the enthalpy of solution, and explain how they combine to cause dissolution to be exothermic orendothermic.
  • Compare the effects of temperature and pressure on solubility.
/ 1 Day
Concentration of Solutions (Section 3) /
  • Given the mass of solute and volume of solvent, calculate the concentration of a solution.
  • Given the concentration of a solution, determine the amount of solute in a given amount of solution.
  • Given the concentration of a solution, determine the amount of solution that contains a given amount of solute.
/ 2 Days
Chapter 12 Teacher-made Assessment -- 1 day
Properties of Acids and Bases (Section 1) / 14 /
  • List five general properties of aqueous acids and bases.
  • Name common binary acids and oxyacids, given their chemical formulas.
  • List five acids commonly used in industry and the laboratory, and give two properties of each.
  • Define acid and base according to Arrhenius’s theory of ionization.
  • Explain the differences between strong and weak acids and bases.
/ PS.7
PS.35 / 1 Day
Acid-Base Theoriesm (Section 2) /
  • Define and recognize Brønsted-Lowry acids and bases.
  • Define a Lewis acid and a Lewis base.
  • Name compounds that are acids under the Lewis definition but are not acids under the Brønsted-Lowry definition.
/ 1 Day
Acid-Base Reactions (Section 3) /
  • Describe a conjugate acid, a conjugate base, and an amphoteric compound.
  • Explain the process of neutralization.
  • Define acid rain, give examples of compounds that can cause acid rain, and describe effects of acid rain.
/ 2 Days
Aqueous Solutions and the Concept of pH (Section 1) / 15 /
  • Describe the self-ionization of water.
  • Define pH, and give the pH of a neutral solution at 25°C.
  • Explain and use the pH scale.
  • Given [H3O+] or [OH−], find pH.
  • Given pH, find [H3O+] or [OH−].
/ PS.4
PS.20
PS.31
PS.32
PS.33 / 1 Day
Determining pH and Titrations (Section 2) /
  • Describe how an acid-base indicator functions.
  • Explain how to carry out an acid-base titration.
  • Calculate the molarity of a solution from titration data.
/ 2 Days
Titration Lab / 1 Day
Chapter 14 & 15 Teacher-made Assessment -- 1 day
Thermochemistry (Section 1) / 16 /
  • Define temperature and state the units in which it is measured.
  • Define heat and state its units.
  • Perform specific-heat calculations.
  • Explain enthalpy change, enthalpy of reaction, enthalpy of formation, and enthalpy of combustion.
  • Solve problems involving enthalpies of reaction, enthalpies of formation, and enthalpies of combustion.
/ PS.30
PS.31
PS.44 / 2 Days
Calorimeter Lab / 1 Day
Chapter 16 Teacher-made Assessment -- 1 day
Reaction Rates and Equilibrium / Topic 1
(Chapters 17 & 18) /
  • Explain the five factors that influence reaction rates on textbook pgs. 568-570 (Section 17.2)
  • Explain chemical equilibrium (Section 18.1)
  • Explain LeChatelier’s principle (Section 18.2)
/ PS.37 / .5 Day
Oxidation-Reduction Reactions / Topic 2 (Chapter 19) /
  • Define oxidation and reductions and give an example of each reaction. (Section 19.1)
/ PS.36 / .5 Day
Biochemistry / Topic 3 (Chapters 22 & 23) /
  • Determine the number of bond that carbon, hydrogen, and oxygen can make.
  • Distinguish among structures of alkanes, alkenes, and alkynes (Section 22.2)
  • Distinguish between structural characteristics of hydrocarbons, carbohydrates, nucleic acids, and proteins (Section 23.1)
/ PS.25
PS.26
PS.28
PS.45 / 1 Day
Nuclear Chemistry / Topic 4 (Chapter 21) /
  • Describe the different types of radioactive decay and their strength (Section 21.2)
  • Alpha Particle
  • Beta Particle
  • Gamma ray
  • Solve half-life problems on pg. 689 (Section 21.2)
  • Explain benefits of nuclear radiation on textbook pg. 695 (Section 21.3)
/ PS.10
PS.11
PS.12
PS.47 / 1 Day
Topics 1-4 Teacher-made Assessment -- 1 day
CUMULATIVE FINAL EXAM (CHAPTERS 8-16 & 4 Topics) -- 1 day

1