SC 230 Chemistry Course Outline

College of Micronesia-FSM

Course Description

The course is an investigation of the fundamentals of general chemistry and an introduction to organic chemistry. The course will emphasize the role of chemistry in modern human life. The laboratory supports the lecture topics, through both qualitative and quantitative experiments. The topics include: Basic concepts, chemical substances, chemical reactions, atomic structure, states of matter, and an introduction to organic chemistry

Outline prepared by: Dr. Anca Dema.
Date prepared: April 2003

Prerequisite course: MS 098 Transition to Algebra

1. Science Program Outcomes
   Students will be able to:
   • define fundamental concepts, principles, and theories of science.
   • gather scientific information through experiments, field work, and research.
   • perform experiments that support the development of scientific theory.
   • utilize appropriate laboratory and field work procedures.
   • interpret and express the results of experiments.
   • explain observations of new phenomenon, systems, and entities, using the theories of science.
2. General Objectives (Course outcomes)
   Students will be able to:
   1. Define basic concepts.
   2. Make basic measurements.
   3. List, identify, and characterize states of matter and energy.
   4. Define and describe atoms, molecules, ions, and their formulas.
   5. Write chemical names and formulas.
   6. Balance chemical reactions and equations.
   7. Define and describe the electron structure and configuration of atoms.
   8. Define and describe chemical bondings.
   9. Identify and describe simple organic compounds including biochemical compounds.
3. Specific Objectives (Specific outcomes)
   Students will be able to:
   1. Define basic concepts.
      1. Define matter and identify different forms of matter. 
                                                                                                           
      2. Define chemical reactions and their characteristics.
      3. Define chemistry and state the major objectives of this science. 
                                                            
      4. List ways in which chemistry has contributed to the science and technology.
      5. Differentiate among the terms experiment, law hypothesis, and theory.
      6. Describe the scientific method.
   2. Make basic measurements.
      1. Define the metric units.
      2. Identify the two units, or parts of a measurement.
      3. Describe the procedure you would use to make a measurement using a standard unit measure.
      4. Write measurements in scientific notations.
      5. Convert decimal numbers to scientific notations and vice-versa.
      6. Describe the role of base units and prefixes in modern metric system (SI).
      7. Identify the SI base units used to measure lengths and mass and the derived SI unit used to measure volume.
      8. List and define the eight common SI prefixes used in chemistry.
      9. Contrast the mass and the weight of an object.
      10. Distinguish significant figures and uncertainty in measurement.
      11. Define an absolute temperature scale.
      12. Convert between Kelvin, Celsius, and Fahrenheit.
      13. Define density.
      14. Rearrange the equation that defines density, using algebraic manipulations, to obtain equations for volume and mass.
      15. Calculate two of the quantities, calculate the third from:density, mass, or volume.
   3. List, identify, and characterize states of matter and energy.
      1. List and characterize the three states of matter.
      2. Explain changes of states of matter.
      3. Identify the physical state of a substance under given conditions.
      4. Differentiate between a physical change and chemical change.
      5. Differentiate between a physical property and a chemical property.
      6. Identify the properties as physical or chemical, given a description of a material
      7. Define substance and mixtures.
      8. Describe the filtration and distillation methods of separating mixtures.
      9. Define homogeneous mixture(solutions) and heterogeneous mixture, and give examples of each.
      10. Differentiate between an element and a compound,and give an example of each.
      11. State the law of definite proportions and give an example of illustrating the law.
      12. Define energy, kinetic energy and potential energy.
      13. Define the energy units.
      14. Converting between Joules and Calories
   4. Define and describe atoms, molecules, ions, and their formulas.
      1. Define and describe atoms.
      2. State the four main postulates of Dalton's atomic theory.
      3. Describe the Particle Structure of the Atom, and the experiments in which the scientists discovered such particles.
      4. Define the terms atomic numbers, mass number and isotope.
      5. Write the isotope symbol for an atom of a given number of protons and the neutrons.
      6. Define the percentage abundance of an isotope.
      7. Define atomic mass unit.
      8. Define atomic weight.
      9. Calculate the atomic weight of an element given the isotope masses and percentage abundances.
      10. Describe how the elements are arranged in a modern periodic table.
      11. Define periods and groups(family)for a periodic table.
      12. Locate any element in the periodic table given only its period and group.
      13. Define main group and transition metal group.
      14. Define metal, nonmetal and metalloid.
      15. Define molecules and ions.
      16. Discuss the meaning of the molecular basis of substances.
      17. Predict whether a compound is molecular or ionic given the elements in the compound.
      18. Compare the melting points of molecular and ionic compounds.
      19. Define molecular formulas and structural formulas, give examples of some molecular and structural  formulas.
      20. Give formulas of the elements.
      21. Define anion and cation.
      22. Define monoatomic ion and polyatomic ion.
      23. Describe the structure  of the sodium chloride crystal,as a simple example of an ionic solid.
      24. Describe how the relative number of cations and anions in an ionic solid is fixed.
      25. Explain why a water solution of sodium chloride is an electrical conductor,whereas pure water is nonconducting.
      26. Describe what happens as an ionic solid dissolves in water.
   5. Write chemical names and formulas.
      1. Write the formulas for ionic compounds.
      2. Predict the charge of a main group monoatomic ion.
      3. Write the formula for binary ionic compound, given the ions.
      4. Assign the systematic name, given the formula of a binary ionic compound,when metal can form a single kind of cation.
      5. Determine the charge on a metal ion ,given the formula of a compound.
      6. Assign the Stock name to a binary ionic compound,given its formula when the metal can form several kinds of cations
      7. Assign the classical name to a binary ionic compound ,given its formula when the metal can form several cations
      8. State the names and formulas of polyatomic ions.
      9. Write the formulas for the compounds containing polyatomic ions.
      10. Name the compounds containing polyatomic ions.
      11. Name a binary molecular compound using Greek prefixes.
      12. Name the acidic solution corresponding to a binary compound of hydrogen with nonmetal.
      13. Write the name and formula of the oxyacid corresponding to a given oxyanion.
   6. Balance chemical reactions and equations.
      1. Recognize five telltale signs that a chemical reaction has occurred.
      2. Given a chemical equation, identify the reactants and products, as well as the number of molecules or formula units of each substance.
      3. Given  a chemical equation, note the physical states of the reactants and products and any reaction conditions, if this information is available in equation.
      4. Balance a chemical equation using the smallest whole-number coefficients.
      5. Identify a chemical equation as a combination reaction or a decomposition if you are given one of these types
      6. Identify a chemical equation as a double replacement reaction or a combustion reaction, if you are given one of these types.
   7. Define and describe the electron structure and configuration of atoms.
      1. List various types of electromagnetic radiation and their properties.Relate the color of the light to its energy.
      2. Define energy level.describe how Bohr's theory explains the different colors in the line spectrum of an atom.
      3. Describe the two concepts of  Bohr's theory that are retained in modern atomic theory (quantum mechanics).
      4. Define orbital,electron shell and subshell.
      5. Describe the values that are possible for the shell quantum number n, which denotes the different electron shells.
      6. Describe the two features that the orbitals in a shell have in common.
      7. Calculate the number of orbitals in a given shall from the shell quantum number n.
      8. Describe the meaning of  any given subshell notation.
      9. List the different subshells in a given shell using subshell notation.
      10. List the number of orbitals in a given subshell.
      11. List the five energy subshells, in order from the lowest to the highest orbital energy.
      12. Define electron configuration.
      13. Interpret the notation for a particular electron configuration.
      14. Describe the Pauli exclusion principle.
      15. Write down the electron configurations of the elements from hydrogen to argon, knowing the order of filing of the first five subshells.
      16. Draw orbital diagrams that correspond to the electron configurations of the elements from hydrogen to argon.
      17. Demonstrate the similarity in outer-shall electron configurations of the elements in any given group of the periodic table.
      18. Use the general pattern of the periodic table to obtain the order of filling  of the subshells and hence the complete electron configuration for an atom.
      19. Define valence electron.
      20. Use the position of element in the periodic table to obtain the valence shell configuration for an atom.
      21. Use the trends shown by atomic radii of the main-group elements to predict the relative sizes of two atoms.
      22. Use the trends shown by atomic radii of the main-group elements to predict the relative sizes of two ions
      23. Define ionization energy.State two periodic trends  shown by ionization energies for atoms of main groups elements.
      24. Explain how periodic trends in the ionization energy of atoms relate to periodic trends in
      25. their metallic character.
      For reactive nonmetals, compare the relative values of the ionization energy and the electron affinity of an atom.
   8. Define and describe chemical bondings.
      1. Define ionic bond.
      2. Describe three steps in formation of an ionic compound from atoms.
      3. Determine from the identity of the component elements whether a compound is likely to contain ionic bonds
      4. Describing ionic bond formation with Electron Dot formula.
      5. State the octet rule.
      6. Write the electron dot symbols for some common atoms and ions.
      7. Describe ionic bond formation between atoms using electron dot symbols.
      8. Define covalent bond.
      9. Describe the formation of a covalent bond between two hydrogen atoms in term of orbitals.
      10. Represent covalent bond formation between two hydrogen atoms or two halogen atoms using electron dot formula for the molecule.
      11. Define single bond, double bond, and triple bond.
      12. Identify the lone pairs in the electron dot formula of a molecule.
      13. Define electronegativity.
      14. Describe the trends in electronegativity in periodic table.
      15. Define polar covalent bond.Use delta notation to denote bond polarity, given any two atoms and their electronegativities
      16. Describe three types of small molecules according to their basic arrangement of atoms.Sate the four steps used to draw electron dot formula.
      17. Draw a molecule's electron dot formula, given its molecular formula.
   9. Identify and describe simple organic compounds including biochemical compounds..
      1. Define Organic Chemistry.Identify the four bonds to carbon in a variety of compounds and the chains of  carbon atoms in organic compounds.
      2. Differentiate between electron dot formula and structural formula.
      3. Write the structural formulas and condensed structural formula of isomers.
      4. Define Hydrocarbons and classify it.
      5. Write the structural formulas of different types of hydrocarbons.
      6. Define and write the structural formulas of different types of functional groups.
      7. Describe Carbohydrates, Proteins, and Lipids ,the structure and functions.
4. Textbook: Introductory Chemistry,Second Edition, Ebbin and Wentworth, Houghton Mifflin, 1998
5. Required course materials:
   • CD-ROM Chemistry Interactive 3.0 introductory Chemistry. Accompanies text. Supports the goals of the second edition by helping students visualize molecular behaviour and manipulate molecules in three dimensions. Tutorial, animations, videos, molecular models and problem sets are included.
   • Instructor's resource manual-with bank tests
   • Textbook
   • Lab Textbook
   • Some Supplies and equipment required for the chemistry lab.
6. Reference  materials:
   • Fundamental of Introductory Chemistry, Darell, Ebbing,2^nd, Houghton Mifflin,1998.
   • Experimental General Chemistry, compiled by Dr Anca Dema
   • Chemistry, Bernice S, 1995, John Wiley & Sons, Inc
7. Instructional costs: None anticipated at this time
8. Method of  Instruction: The course will be taught by lecture, class discussions, lab activity, problem solving in the classroom. The lab experiments will closely relate to the lectures. The models of atoms, compounds, chemical bondings, and the CD-ROM are directly tied to chemistry textbook. The textbook is supported with a laboratory manual because chemistry is an experimental science. Each experiment is introduced with a discussion of  the purpose of the lab, post-lab discussions,and questions in order to help students evaluate their understanding of experimental work.
9. Evaluation and assessment: homework, tests, quizzes,laboratory reports, a mid-term and final exam will be given.
10. A standard  90%=A, 80%=B,70%=C,60%=D, below 60%=F
.
11. Credit by examination: None
12. Attendance policy: As per the current college catalog

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