College Prep. Chemistry Course Syllabus

Unit #1 MATTER AND ENERGY

Objectives:

Introduce chemistry as a scienceDiscuss nature of science, both pure and appliedEmphasize the reliance of science on measurementDevelop skills in expressing measurements and calculated resultsExplain the use of dimensional analysis, scientific notation, and significant figuresClassify matter into elements, compounds and mixturesDiscuss physical and chemical changes Characterize phases of matterDefine and describe energy and its forms and conversionsExplain heat and temperature in terms of the kinetic molecular theory

State Standards:

3.1.10 D3.1.12 D3.2.10 B3.2.12 B3.4.10 A

3.4.12 A3.4.10 B3.4.12 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 proportionsSummarize the five essential points of Dalton’s atomic theoryExplain the relationship between Dalton’s atomic theory and the law of conservation of mass, the law of

definite proportions, and the law of multiple proportionsSummarize the observed properties of cathode rays that led to the discovery of the electronSummarize the experiment carried out by Rutherford and his co-workers that led to the discovery of the nucleusList the properties of protons, neutrons, and electronsDescribe how atomic number and mass number apply to isotopesGiven the identity of an isotope, determine its number of protons, neutrons, and electronsExplain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic radiationDiscuss the dual wave-particle nature of lightDiscuss 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 atomCompare and contrast the Bohr model and the quantum model of the atomExplain how the Heisenberg uncertainty principle and the Schrodinger wave equation led to the idea of atomic orbitals

State Standards:

3.1.10 E3.1.12 E3.4.10 A

3.4.12 A3.4.10 B3.4.12 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 formulaDetermine the formula of an ionic compound formed between two given ionsName an ionic compound given its formulaUsing prefixes, name a binary molecular compound from its formulaWrite the formula of a binary molecular compound given its nameGive the oxidation number for each element in the formula of a chemical compound

Name binary molecular compounds using oxidation numbers and the stock systemCalculate the formula mass or molar mass of any given compoundUse molar mass to convert between mass in grams and amount in moles of a chemical compoundCalculate the number of molecules, formula units, or ions in a given molar amount of a chemical compoundCalculate the percentage composition of a given chemical compoundDefine empirical formula, and explain how the term applies to ionic an molecular compoundsDetermine an empirical formula from either a percentage of a mass compositionExplain the relationship between the empirical formula and the molecular formula of a given compoundDetermine a molecular formula from an empirical formula

State Standards:

3.1.10 D3.1.12 D3.4.10 A3.4.12 A3.4.10 B3.4.12 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 C3.1.12 C

3.1.10 D3.1.12 D3.4.10 A3.4.12 A3.4.10 B3.4.12 B

Shared Activities and Assessments:

Reaction Practice #1 Reaction Practice #2 Reaction and Stoichiometry Practice

Available Equipment and Materials, Storage LocationMisc. 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 C3.1.12 C3.1.10 D3.1.12 D3.4.10 A3.4.12 A3.4.10 B3.4.12 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 C3.1.12 C3.4.10 A3.4.12 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 theoryIdentify the common shapes of small moleculesExplain what determines the polarity of a molecule

Explain why water is a polar moleculeComplete Lewis dot structures of simple molecules

State Standards:

3.1.10 B3.1.12 B3.1.10 C3.1.12 C3.4.10 A3.4.12 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 D3.1.12 D3.4.10 A3.4.12 A

3.4.10 B3.4.12 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 formationDetermine the free energy change of the reaction when given standard free energies of formationDetermine the change in free energy when given entropy, temperature, and enthalpy

State Standards:

3.1.10 D3.1.12 D3.2.10 B3.2.12 B3.4.10 A3.4.12 A3.4.10 B3.4.12 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 principleDetermine the mass action expression of chemical equationsDetermine the equilibrium constant of a reaction when given the concentrationsDetermine the equilibrium concentrations of substances in a reaction when given the equilibrium constant and original concentrationsDetermine the solubility of a substance when given the solubility product constantDetermine the solubility product constant of a substance when given the solubility of a substance

State Standards:

3.2.10 B

3.2.12 B3.4.10 A3.4.12 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 C3.1.12 C3.4.10 A3.4.12 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 A3.2.12 A3.4.10 A3.4.12 A3.4.10 B3.4.12 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 alkanesIdentify 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 D3.2.12 D3.4.10 A3.4.12 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 C3.2.12 C3.4.10 A3.4.12 A3.4.10 B3.4.12 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