Southeastern Louisiana University Dual Enrollment Program--Chemistry

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1 Southeastern Louisiana University Dual Enrollment Program--Chemistry The Southeastern Dual Enrollment Chemistry Program is a program whereby high school students are given the opportunity to take college chemistry courses at their high schools and receive credit on their high school and university transcripts. Southeastern is offering a progressive pair of courses in chemistry during the academic year. Each course consists of about 130 hours of instruction and practice; schools in which students only meet with the teacher an hour or less per day will not be successful completing a dual enrollment course in just two quarters. The courses are: CHEM 101 General Chemistry I (for non-science majors). Credit 3 hours. The first of a two semester sequence covering the following general topics: metric and temperature conversions, density, calorimetry, mixtures/compounds/elements, chemical and physical properties, structure of the atom and electron configuration, periodic table, bonding, chemical formulas and nomenclature, moles, stoichiometry, chemical reactions, gas laws, and properties of gases, liquids and solids CHEM 102 General Chemistry II (for non-science majors). Credit 3 hours. Prerequisite: Chemistry 101. A continuation of Chemistry 101 covering topics such as: solutions, concentrations (% composition and molarity), acids/bases, ph, buffers, kinetics, equilibrium, solubility, oxidation/reduction, nuclear chemistry, and an introduction into organic chemistry and biochemistry. Program Requirements From the High School: A computer lab must be available to all Dual Enrollment chemistry classes two times per week (or once per week if another day per week is devoted to solving homework problems on paper) for the practice portion of the course. This can be a hard-wired classroom or a wireless cart. From the Teacher: Any teacher new to the program must complete the corresponding workshop during the summer at Southeastern s main campus in Hammond. Any teacher already in our program who would like to teach new classes must complete the workshop for those new classes during the summer at Southeastern s main campus. All teachers (new and returning) must attend one half-day workshop at the end of the summer to copy all online course materials and receive any revisions to the Program Guidelines. The teacher(s) must agree to follow the rules of the program as given by Southeastern and outlined in the Dual Enrollment Eligibility Framework and Memorandum of Understanding. It is highly recommended that the teacher be certified in the area for the course they wish to teach. From the Students: Students must be in the 10 th, 11 th or 12 th grade. Students must be on track to complete the Core 4 curriculum with no developmental coursework required. Students must have a PLAN, ASPIRE or ACT equivalent composite score of 18 or greater Students must have a PLAN, ASPIRE or ACT equivalent Mathematics sub-score of 19 or greater Students must be enrolled in a high school chemistry course while dual enrolled To enroll in CHEM 102, the student must have successfully completed CHEM 101 with a D or better. Program Costs To the School or Student: One access code must be purchased by the high school on behalf of each student per course. Each code costs $25 (if billed in bulk to the school) and gives the student access to the software used in the courses. Schools may handle this fee in different ways. Some schools fund it and some pass the fee on to the parents as a course fee. Southeastern rental textbooks are provided to the dual enrolled students at no cost. If there are other students in the high school course who are not dual enrolled, they will not be able to borrow a textbook (they will only have the high school textbook). Any lost text shall be reimbursed to Southeastern by the high school. The school, in turn, can request the fee from the student who lost the book. Reduced tuition will be charged for each dual enrollment course enrolled in with year-long courses being billed in the spring. Please see the Eligibility Framework document for complete details. To the Teacher: There is no cost to the teachers.

2 Program Benefits To the School: Academic Endorsement is received for each eligible student who enrolls in the Dual Enrollment Program. Certificates of completion are provided for all students who enroll in and successfully complete Dual Enrollment Courses. Note that high schools may choose to place ineligible students in the same class with eligible students to fill the classroom. Our experience over the past few years shows that ineligible students often benefit from being in these classes. For example, such students have experienced an increase of 2 7 points in their ACT Math subscores. To the Teacher: Ongoing support is provided, via telephone, and site visits, throughout the duration of any Dual Enrollment course from the Southeastern Dual Enrollment Chemistry Coordinators. All necessary assessment materials are provided, including all assignments, quizzes, practice tests, tests, and final exams. A free account with the online is also provided. All grading and grade book calculations for the university course requirements are done by Southeastern Professional Development credit is given for any summer training sessions attended To the Student: Regular periodic feedback and evaluations of student work by Southeastern faculty throughout the semester/academic year Any student eligible for the Dual Enrollment Program who enrolls in the Program and completes the course with a passing grade will receive college credit for that course 2015 Summer Workshops for Dual Enrollment Chemistry Session Title Dates Audience General Chemistry I (Chem 101) General Chemistry II (Chem 102) ½ Day Workshop May 26 & 27, am 3pm May 28, am 3pm July 21, am 12pm Mandatory for all new CHEM101 Dual Enrollment Chemistry teachers Mandatory for all new CHEM102 Dual Enrollment Chemistry teachers Mandatory for all Dual Enrollment Chemistry teachers Note: Once a teacher has completed the workshop for a particular course, he or she does not have to repeat that workshop in subsequent summers. The only mandatory workshop for returning teachers who do not wish to teach any new courses is a ½ Day Workshop at the end of the summer. This ½ Day Workshop must be repeated every summer.

3 Textbook: Chapters Covered: Chapters 1-12 Calculators: Chem 101 General Chemistry I Southeastern Dual Enrollment Program Introductory Chemistry, 4 th edition, by Nivaldo Tro Scientific Calculator with square root and scientific notation (eg. TI-30X or Casio FX-260) Teachers may choose to require a specific model for ease in teaching how to enter calculations Homework 25% of course grade, collectively. 12 homework assignments (one homework assignment per chapter) and submitted online through the online learning The lowest individual homework score will be dropped at the end of the semester. If the homework average is lower than all test grades, it will be dropped 12 additional instructional assignments will be supplied and graded to give students feedback, but the scores will not be included in the Southeastern grade calculation. Tests Each test is worth 25% of course grade. Tests are multiple choice, 60 minute tests worked on paper and submitted online through the online learning 3 tests, 100 points each The lowest grade is dropped (unless the homework average is lower, in which case it is dropped instead). Additional practice quizzes and tests will be supplied and graded to give students feedback, but the scores will not be included in the Southeastern grade calculation. Final Exam 25% of course grade. Multiple choice, 120 minute tests worked on paper and submitted online through the online learning 100 points Covers all sections. Learning Goals Note: All material must be covered by the end of the course, but it can be covered in a different order of chapters in the book (and tested in a different order). Teachers may discuss a different ordering of chapters with the coordinators. Chemistry in Our Lives 1. Define the term chemistry and identify substances as chemicals. 2. Describe some chemical and physical properties of matter. 3. Describe the activities that are part of the scientific method. Measurements 1. Write the names and abbreviations for the metric or SI units used in measurements of length, volume, mass, temperature and time. 2. Write a number in scientific notation. 3. Identify a number as measured or exact; determine the no. of significant figures in a measured number. 4. Adjust calculated answers to give the correct number of significant figures. 5. Use conversion factors to change from one unit to another. 6. Calculate the density of a substance; use density to calculate mass or volume of a substance. 7. Given a temperature, calculate a corresponding temperature on another scale. Atoms and Elements 1. Classify matter as pure substances or mixtures. 2. Given the name of an element, write its correct symbol; from the symbol, write the correct name. 3. Use the periodic table to identify the group and the period of an element and decide whether it is a metal or a nonmetal. 4. Understand Dalton s atomic hypothesis and the relevance of early experiments (cathode rays, electrolysis, oil drop, x-rays, radioactivity, etc.) toward developing a model of the atom. 5. Describe the electrical charge and location in an atom for a proton, a neutron, and an electron. 6. Given the atomic number and mass number of an atom, state the number of protons, neutrons, and electrons.

4 7. Give the number of protons, electrons, and neutrons in the isotopes of an element. 8. Explain how atomic masses were defined and the standard by which atomic masses are presently defined. Electronic Structure and Periodic Trends 1. Define and discuss electromagnetic radiation (waves) and properties; discuss the electromagnetic radiation spectrum in terms of frequencies and wavelengths from radio waves to cosmic rays. 2. Explain how atomic spectra correlate with energy levels in atoms. 3. Describe the energy levels, sublevels, and orbitals in atoms. 4. Write the orbital diagrams and electron configurations. 5. Use the electron configurations of elements to explain periodic trends. 6. Predict the number of valence electrons for a representative element given its position on the periodic table. Ionic Compounds 1. Using the octet rule, predict the ion charge of simple ions for the representative elements. 2. Using charge balance, write the correct formula for an ionic compound. 3. Given the formula of an ionic compound, write the correct name; given the name of an ionic compound, write the correct formula 4. Write a formula of a compound containing a polyatomic ion. Molecules and Covalent Compounds 1. Given the formula of a covalent compound, write its correct name; given the name of a covalent compound, write its formula. 2. Diagram the Lewis structure for covalent molecules. 3. Write Lewis structures for covalent molecules or ions with multiple bonds and show resonance structures. 4. Predict the shape of a molecule using VSEPR. 5. Use electronegativity to determine the polarity of a bond. 6. Classify a molecule as polar or nonpolar. 7. Identify types of intermolecular forces and compare their relative strengths Chemical Quantities 1. Use Avogadro s number to convert between particles and moles. 2. Given the chemical formula of a substance, calculate its molar mass. 3. Use molar mass to convert between mass and moles. 4. Given the formula of a compound, calculate the percent composition. 5. Determine the empirical formula and molecular formula of a compound using appropriate data. Chemical Reactions 1. Identify a change in a substance as a chemical or physical change. 2. Write and balance chemical equations for chemical reactions. 3. Identify types of chemical reactions and predict their products. 4. Given a quantity in moles of reactant or product, use mole-mole factors from the balanced equation to calculate the moles of another substance in the reaction. 5. Use stoichiometry to determine the amount (moles, mass or volume) of reactants or products involved in a chemical reaction given appropriate data. 6. Given the actual quantity of product, determine the percent yield for a reaction. Energy and States of Matter 1. Describe different forms of energy and identify units of energy. 2. Use specific heat to calculate heat loss or gain, temperature change, or mass of a sample. 3. Describe solids, liquids, and gases at the level of the bulk material and at the level of the particle. 4. Describe the attractive forces between ions, polar molecules, and nonpolar molecules. 5. Describe various phase changes and calculate the energy involved. 6. Describe the energy changes in exothermic and endothermic reactions. Gases 1. Describe the kinetic theory of gases and the properties of gases. 2. Define pressure and the units involved. 3. Understand and apply the gas laws involving pressure, volume, temperature, and amount of a gas. 4. Use the ideal gas law to solve for P, V, T, or n of a gas when given 3 of 4 values in the ideal gas equation. 5. Determine the amount (moles, mass or volume) of a gas that reacts or forms in a chemical reaction. 6. Use partial pressures to calculate the total pressure of a mixture of gases. 7. Understand vapor pressure and its relationship to boiling point.

5 Textbook: Chapters Covered: Chapters Calculators: Chem 102 General Chemistry II Southeastern Dual Enrollment Program Introductory Chemistry, 4 th edition, by Nivaldo Tro Scientific Calculator with square root, log, 10 x and scientific notation (eg. TI-30X or Casio FX-260) Teachers may choose to require a specific model for ease in teaching how to enter calculations Homework 25% of course grade, collectively. 7 homework assignments (one homework assignment per chapter) submitted online through the online learning The lowest individual homework score will be dropped at the end of the semester. If the homework average is lower than all test grades, it will be dropped 7 additional instructional assignments will be supplied and graded to give students feedback, but the scores will not be included in the Southeastern grade calculation. Tests Each test worth 25% of course grade. Tests are multiple choice, 60 minute tests worked on paper and submitted online through the online learning 3 tests, 100 points each The lowest grade is dropped (unless the homework average is lower, in which case it is dropped instead). Additional quizzes will be supplied and graded to give students feedback, but the scores will not be included in the Southeastern grade calculation. Final Exam 25% of course grade. Multiple choice, 120 minute test worked on paper and submitted online through the online learning 100 points. Covers all sections. Learning Goals Solutions 1. Define solute and solvent; describe the formation of a solution. 2. Identify solutes as electrolytes or nonelectrolytes. 3. Define solubility; distinguish between an unsaturated and a saturated solution. Identify an insoluble salt. 4. Understand and perform calculations involving concentration, including mass percent and molarity. 5. Given the volume and molarity of a solution, calculate the amount of another reactant or product in the reaction. 6. Perform calculations involving dilutions of solutions. Chemical Equilibrium 1. Describe how temperature, concentration, and catalyst affect the rate of a reaction. 2. Use the concept of reversible reactions to explain chemical equilibrium. 3. Calculate the equilibrium constant for a reversible reaction given the concentrations of reactants and products at equilibrium. 4. Use an equilibrium constant to predict the extent of reaction 5. Use Le Chatlier s principle to describe the changes made in equilibrium concentrations when reaction conditions change. 6. Calculate the solubility product for a saturated solution; use the solubility product to calculate molar ion concentrations. Acids and Bases 1. Describe and name acids and bases using the Arrhenius and the Bronsted-Lowry concepts. 2. Identify conjugate acid-base pairs for Bronsted-Lowry acids and bases. 3. Write equations for the dissociation of strong and weak acids; identify the extent of reaction. 4. Write the equilibrium expression for a weak acid or weak base. 5. Use the ion product of water to calculate the [H 3 O + ] and [OH - ] in an aqueous solution. 6. Calculate ph, [H 3 O + ], and [OH - ] of a solution from appropriate data.

6 7. Write balanced equations for reactions of acids and bases. 8. Calculate the molarity or volume of an acid or base from titration information. 9. Predict whether a salt will form an acidic, basic, or neutral solution. 10. Describe the role of buffers in maintaining the ph of a solution. Oxidation-Reduction: Transfer of Electrons 1. Identify oxidation, reduction, oxidizing agents, and reducing agents in redox reactions. 2. Assign an oxidation number to all the atoms in a compound. 3. Balance oxidation-reduction equations (including ones in acidic or basic conditions). 4. Write the half-reactions that occur at the anode and cathode of a voltaic cell. 5. Describe the half-cell reactions and the overall reactions that occur in electrolytic cells. 6. Predict whether a reaction will occur spontaneously 7. Write a balanced chemical equation for a spontaneous reaction. Nuclear Radiation 1. Describe alpha, beta, and gamma radiation. 2. Write nuclear equations for radioactive decay. 3. Describe the detection and measurement of radiation. 4. Perform half-life calculations for radioisotopes. 5. Describe the practical applications of radioisotopes. 6. Describe the processes of nuclear fission and fusion. Organic Chemistry 1. Differentiate properties and characteristic of organic or inorganic compounds. 2. Classify organic molecules according to their functional groups, including alkanes, alkenes, alkynes, alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, amines and amides. 3. Write the IUPAC and/or common names for the functional groups listed above. 4. Draw structural, condensed and line formulas of the functional groups listed above. 5. Describe the bonding in benzene; name aromatic compounds and write their structural formulas. 6. Classify alcohols as primary, secondary, or tertiary 7. Identify and predict products for selected addition and condensation organic reactions. Biochemistry 1. Understand the classification schemes for carbohydrates. 2. Describe the monosaccharide units and linkages in disaccharides. 3. Describe structure and properties of lipids. 4. Describe protein functions, and draw the generic structure for amino acids monomers and the peptide linkage. 5. Identify the levels of structure of a protein. 6. Describe the role of an enzyme in an enzyme-catalyzed reaction. 7. Describe the structures of the nucleic acids in DNA and RNA. 8. Describe protein synthesis.

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