College Prep. Chemistry Course Syllabus
Unit #1 MATTER AND ENERGY
Objectives:
Introduce chemistry as a science
Discuss nature of science, both pure and applied
Emphasize the reliance of science on measurement
Develop skills in expressing measurements and calculated results
Explain the use of dimensional analysis, scientific notation, and significant figures
Classify matter into elements, compounds and mixtures
Discuss physical and chemical changes
Characterize phases of matter
Define and describe energy and its forms and conversions
Explain heat and temperature in terms of the kinetic molecular theory
State Standards:
3.1.10 D
3.1.12 D
3.2.10 B
3.2.12 B
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· Density Lab
· Recycling Factory Inquiry Problem
Available Equipment and Materials, Storage Location:
Misc. chemicals and glassware in room 420 and the chemical storage closet
Unit #2 ATOMIC STRUCTURE
Objectives:
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
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
Describe how atomic number and mass number apply to isotopes
Given the identity of an isotope, determine its number of protons, neutrons, and electrons
Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic radiation
Discuss the dual wave-particle nature of light
Discuss the significance of the photoelectric effect and the line-emission spectrum of hydrogen to the development of the atomic model.
Describe the Bohr model of the hydrogen atom
Compare and contrast the Bohr model and the quantum model of the atom
Explain how the Heisenberg uncertainty principle and the Schrodinger wave equation led to the idea of atomic orbitals
State Standards:
3.1.10 E
3.1.12 E
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· Isotopes Worksheet
· Conservation of Matter Lab
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
Unit #3 CHEMICAL FORMULAS
Objectives:
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
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
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
Define empirical formula, and explain how the term applies to ionic an molecular compounds
Determine an empirical formula from either a percentage of a mass composition
Explain the relationship between the empirical formula and the molecular formula of a given compound
Determine a molecular formula from an empirical formula
State Standards:
3.1.10 D
3.1.12 D
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· Empirical Formula Lab
· Naming Compounds Flow Chart
· Writing Formulas Practice Sheet
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
Unit #4 CHEMICAL REACTIONS
Objectives:
Given a word equation for a reaction, write a balanced chemical equation.
Given the reactants of one of the 4 basic types of reactions, determine the products and write a balanced chemical equation.
Given the reactants of a possible ionic reaction, determine if the reactions would proceed and write a net ionic equation for the reaction.
Given the mass or volume at STP of one substance in a chemical reaction, determine the mass or volume at STP of another substance taking part in the same reaction.
State Standards:
3.1.10 C
3.1.12 C
3.1.10 D
3.1.12 D
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· Reaction Practice #1
· Reaction Practice #2
· Reaction and Stoichiometry Practice
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
Unit #5 PHASES OF MATTER
Objectives:
Given 3 of 4 out of P1, P2, V1, and V2, find the fourth.
Given 3 of 4 out of T1, T2, V1, and V2, find the fourth.
Given 5 of 6 out of P1, P2, T1, T2, V1, and V2, find the sixth.
Given 3 of 4 out of P, V, T, and number of moles (or mass and formula), find the fourth.
Given the molecular weight of a gas and its rate of diffusion, determine the molecular weight of a second gas when its rate of diffusion at the same conditions is given.
State Standards:
3.1.10 C
3.1.12 C
3.1.10 D
3.1.12 D
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· Review Problems
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT#6 ELECTRON CONFIGURATION AND PERIODICITY
Objectives:
Describe a given atom in terms of its atomic orbitals.
Determine the electron configuration for a given element.
Explain why elements in a group have similar properties.
Identify the four blocks of the periodic table.
Identify four periodic trends and explain how each reflects the electron
configurations of the elements.
State Standards:
3.1.10 C
3.1.12 C
3.4.10 A
3.4.12 A
Shared Activities and Assessments:
· Electron Configuration Practice
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #7 BONDING
Objectives:
Describe the VSEPR theory
Identify the common shapes of small molecules
Explain what determines the polarity of a molecule
Explain why water is a polar molecule
Complete Lewis dot structures of simple molecules
State Standards:
3.1.10 B
3.1.12 B
3.1.10 C
3.1.12 C
3.4.10 A
3.4.12 A
Shared Activities and Assessments:
· Electron Dot Diagram Practice
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #8 SOLUTIONS
Objectives:
Describe the properties of solutions.
Identify the different types of solutions.
Measure the concentration of solutions in terms of molarity and molality.
Differentiate among saturated, unsaturated, and supersaturated solutions.
Define solubility and describe the factors that affect solubility.
Describe the factors that affect the rate at which a solute dissolves in a solvent.
Define a colligative property of a solution.
Describe four colligative properties of solutions.
State Standards:
3.1.10 D
3.1.12 D
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· Solutions Practice
· BP Elevation and FP Depression Lab
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #9 KINETICS AND THERMODYNAMICS
Objectives:
Label the activation energy, heat of reaction, and activated complex on a potential energy diagram
Determine the heat of reaction when given standard heats of formation
Determine the free energy change of the reaction when given standard free energies of formation
Determine the change in free energy when given entropy, temperature, and enthalpy
State Standards:
3.1.10 D
3.1.12 D
3.2.10 B
3.2.12 B
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· Review
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #10 EQUILIBRIUM
Objectives:
Predict the result of stress on concentrations of substances in a reaction using LeChatlier’s principle
Determine the mass action expression of chemical equations
Determine the equilibrium constant of a reaction when given the concentrations
Determine the equilibrium concentrations of substances in a reaction when given the equilibrium constant and original concentrations
Determine the solubility of a substance when given the solubility product constant
Determine the solubility product constant of a substance when given the solubility of a substance
State Standards:
3.2.10 B
3.2.12 B
3.4.10 A
3.4.12 A
Shared Activities and Assessments:
· Equilibrium Review
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #11 ACIDS AND BASES
Objectives:
State the Bronsted-Lowry definition of acids and bases.
Identify the common physical and chemical properties of acids and bases.
Explain what dissociation constants indicate about an acid or base.
Calculate a dissociation constant using experimental data.
Explain what most acidic hydrogen atoms have in common.
Explain what most bases have in common.
Describe how acids are named.
Identify the ion concentrations in pure water.
Describe the pH scale.
Identify a buffer.
Explain how buffers work.
Describe and perform an acid-base titration.
Explain how indicators are used in titrations and how they are chosen.
State Standards:
3.1.10 C
3.1.12 C
3.4.10 A
3.4.12 A
Shared Activities and Assessments:
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #12 ELECTROCHEMISTRY
Objectives:
Define oxidation and reduction.
Explain what oxidation numbers are and how they are assigned.
Explain what is meant by the activity series of metals.
Describe some applications of redox reactions.
List the steps in balancing a redox equation.
Describe electrochemical cells.
Explain the operation of a voltaic cell.
Relate standard electrode potentials to standard cell potentials.
Describe the operation of rechargeable and non-rechargeable batteries.
Compare fuel cells and batteries.
Describe some applications of electrolytic cells.
State Standards:
3.2.10 A
3.2.12 A
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #13 ORGANIC CHEMISTRY AND BIOCHEMISTRY
Objectives:
Explain carbon’s unique bonding properties.
Define organic molecules and organic chemistry.
Explain how carbon and hydrogen atoms can form thousands of different
hydrocarbons.
Define alkanes
Identify conformations and structural isomers.
Identify the different classes of unsaturated hydrocarbons.
Define the term polymer.
Explain why recycling plastics is important.
Explain how several classes of organic compounds can be derived from
hydrocarbons.
Identify the differences among halocarbons, alcohols, and ethers.
Write formulas for halocarbons, alcohols, and ethers.
Identify the differences between and write formulas for aldehydes and ketones.
Identify the differences between and write formulas for carboxylic acids and
esters.
Identify the differences between and write formulas for amines and amides.
Describe the chemical composition and functions of carbohydrates, lipids,
proteins and nucleic acids.
State Standards:
3.2.10 D
3.2.12 D
3.4.10 A
3.4.12 A
Shared Activities and Assessments:
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet
UNIT #14 NUCLEAR CHEMISTRY
Objectives:
Explain what is meant by the half-life of a radioactive element.
Describe what happens in a nuclear fusion reaction.
Describe what happens in a nuclear fission reaction.
Describe how radiation affects living things.
Discuss several beneficial applications of radioisotopes.
Explain how nuclear reactors are used to produce energy.
State Standards:
3.2.10 C
3.2.12 C
3.4.10 A
3.4.12 A
3.4.10 B
3.4.12 B
Shared Activities and Assessments:
· TMI Movie Guide
Available Equipment and Materials, Storage Location
Misc. chemicals and glassware in room 420 and the chemical storage closet