CHM1033 Syllabus (Podona) PDF

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MIAMI-DADE COLLEGE Kendall Campus Spring 2005 COURSE DETAILS INSTRUCTOR: Tchao Podona, Ph.D. e-mail address: [email protected] Phone: 305-237-2590 Office Hours: R 3391-12 (Wed, 4:30 - 5:30 PM) LECTURE: Course: Reference No.: Day: Time: Location: Textbook:

CHM 1033 271754 Wednesday 5:40 PM. – 8:10 PM Kendall Campus, Room# 4308 CHEMISTRY: An Introduction to General, Organic and Biological Chemistry by Karen C. Timberlake, Eighth Edition

Suggested Material: Study Guide: Exploring Chemistry General, Organic, Biochemistry, by E. Delgado Johann, A. Ciereszko, D. Gottlieb, Sixth Edition A calculator is strongly suggested. Attendance: Attendance is required for optimal learning to take place. You are expected to attend all classes. If you do miss class, it is your responsibility to obtain class notes, assignments and work missed. “Attending” means being in class on time and staying until the class is dismissed. Four incomplete attendance events will be considered as one absence. Conduct:

Food and drink are not allowed in the classroom. It is expected that you will not be disruptive of the class by late arrivals, early departures, or class behaviors. Cellular phones must be turned off and pagers should be on vibration mode.Your conduct should adhere to the standards of academic honesty. Violations will result in a formal charge of academic dishonesty as outlined in the Students’ Rights and Responsibilities Handbook. You should familiarize yourself with this information.

COURSE DESCRIPTION This course emphasizes chemistry topics related to the allied health sciences through study of the essentials of inorganic and organic chemistry and some biochemistry.

LEARNING OUTCOMES Study Goals

Ch.

1. Learn the units and abbreviations for the metric (SI) system and use these units and U.S. units to write conversion factors. 2. Distinguish between measured and exact numbers. 3. Determine the number of significant figures in a measurement. 4. Calculate the density of a substance and use it to convert between mass and volume. 5. Calculate temperature values in degrees Celsius and Kelvin.

1 1

1. Write the name of an element from its symbol or its period and group number. 2 2. Classify an element as a metal or nonmetal. 3. Describe the three important particles in the atom, their location, charges, and masses. 4. Use atomic number and mass number of an atom to determine number of protons, neutrons, and electrons in the atom. 5. Understand the relationship of isotopes to the atomic mass of an element. 6. Write electron shell arrangements for elements 1-18 in the periodic table.

1. Identify the types of radiation as alpha particles, beta particles or gamma radiation. 3 2. Describe the methods required for proper shielding for each type of radiation. 3. Identify some radioisotopes used in nuclear medicine. 4. Calculate the amount of radioisotope that remains after a given number of half-lives. 5. Describe nuclear fission and fusion.

4

1. Write an electron dot formula for an atom of a representative element.

2. Use the octet rule to determine the ionic charge of ions for representative elements. 3. Use charge balance to write an ionic formula. 4. Write ionic formulas and names of compounds with polyatomic ions. 5. Write the correct names for ionic and covalent compounds. 6. Predict the polarity of a molecule.

1. Classify a change in matter as a chemical change or a physical change. 5 2. Write a balanced equation for a chemical reaction when given the formulas of the reactants and products. 3. Classify an equation as a combination, decomposition, replacement and/or combustion reaction. 4. Describe the features of an oxidation-reduction reaction. 5. Use the molar mass to convert between the grams of a substance and the number of moles. 6. Use a mole-mole conversion factor to determine the corresponding number of moles for a reactant or a product. 7. For a given mass of a substance in a reaction, use the appropriate mole factors and molar masses to calculate the mass of a reactant or a product.

6

1. Describe potential and kinetic energy. 2. Calculate the calories lost or gained by a specific amount of a substance for a specific temperature change. 3. Determine the kilocalories for food samples. 4. Determine the energy lost or gained during a change of state at the melting or boiling point. 5. Identify the states of matter and changes of state on heating and cooling curves. 6. Describe the factors that affect the rate of a reaction.

7. Use the concept of reversible reactions to explain chemical equilibrium.

1. Describe the kinetic molecular theory of gases. 7 2. Describe the units of measurement used for pressure and change from one unit to another. 3. Use the gas laws to determine the new pressure, volume or temperature of a specific amount of gas. 4. Use the combined gas law to find the new pressure, volume, or temperature of a gas when changes in two of these properties are given. 5. Describe the relationship between the amount of a gas and its volume. 6. Use partial pressures to calculate the total pressure of a gas mixture.

8

1. Identify the solute and solvent in a solution. 2. Describe hydrogen bonding in water. 3. Describe electrolytes in a solution. 4. Define solubility. 5. Calculate the percent concentrations and molarity of a solution. 6. Describe how to prepare a dilute solution of an acid or a base. 7. Distinguish between a solution, a colloid, and a suspension. 8. Describe the behavior of a red blood cell in hypotonic, isotonic, and hypertonic solutions.

1. Describe the characteristics of acids and bases. 9 2. Identify conjugate acid-base pairs for Bronsted-Lowry acids and bases. 3. Use the ion product of water to calculate concentrations of hydroxide and hydronium ions, and pH.

4. Write a balanced equation for reactions of acids with metals, carbonates, and bases. 5. Describe the function of a buffer.

1

1. Describe properties that are characteristic of organic compounds.

0 2. Describe the tetrahedral shape of carbon with single bonds in organic compounds. 3. Write expanded and condensed structural formulas for the first ten continuous Alkanes. 4. Write IUPAC names for branched Alkanes, Alkenes, Alkynes and Aromatic Hydrocarbons. -13 5. Identify the functional groups in organic compounds and name compounds containing these groups: Alcohols, Phenols, Ethers, Aldehydes and Ketones; Carboxylic acids, Esters, Amines and Amides.

1

4-

1

6

1. Understand properties and types of carbohydrates, lipids, and proteins.

GRADING POLICY 1. Three regular exams will be given. Each exam will constitute 20% of the final grade. In addition, a final exam will be administered which will be comprehensive and represent 40% of the final grade. 2. NO MAKE-UP EXAMS WILL BE GIVEN. 3. Attendance is mandatory and will be taken every class. 4. Cheating will not be tolerated. A grade “zero” will be automatically given to the cheater for the assignment. GRADING SYSTEM 90-100 80-89 70-79 60-69 < 60

A B C D F

COURSE OUTLINE

wk

1

Date

Topics Chap. 1 - Measurements

Activity Last day to withdraw with 100% refund; register, add, drop or change sections (M, 1/10/2005)

Chap. 1 – Measurements 2 Chap. 2 – Atoms and Elements

Chap. 2 - Atoms and Elements 3 Chap. 3 – Nuclear Radiation

4

Chap. 4 – Compounds and their Bonds

5

Chap. 4 - Compounds and their Bonds

6

Chap. 5 – Chemical Reactions and Quantities

Exam # 1 (Chaps. 1-3)

Chap. 6 – Energy and Matter 7

Chap. 7 - Gases 8

Exam # 2 (Chaps. 4-6)

Chap. 7 - Gases 9

Chap. 8 - Solutions 10

11

Chap. 9 – Acids and Bases

Chaps. 10-13 – Selected topics on Introduction to Organic Chemistry

12

3

1

Chaps. 10-13 – Selected topics on Introduction to Organic Chemistry

14

Chaps. 14-16 – Selected topics on Introduction to Biochemistry 1

5

Last day to withdraw with a grade of “W” ( Wed. March 16, 2005)

Exam # 3 (Chaps. 7-10)

Chaps. 14-16 – Selected topics on Introduction to Biochemistry

Review 16

Final Exam 17

Comprehensive – emphasis on Chaps. 10-16...