CHEM101 Chemistry A

Department of Science, Technology, Engineering & Mathematics: Chemistry

I. Course Number and Title
CHEM101 Chemistry A
II. Number of Credits
4 credits
III. Number of Instructional Minutes
IV. Prerequisites
Prerequisites: MATH095 (C or better) or Math Placement Test score of 5
V. Other Pertinent Information

Three-hour lecture and two-hour laboratory per week. Safety glasses or goggles required.

This course meets the General Education requirement for Scientific Literacy.
This course meets the General Education requirement for Quantitative Literacy.
This course meets the General Education requirement for Critical Thinking.

VI. Catalog Course Description
This lecture and laboratory course examines basic principles of general and organic chemistry. Topics include nature of matter, measurement, dimensional analysis, atomic structure, bonding, properties of gases, liquids, solids, and solutions, chemical reactions, acids and bases, hydrocarbons, functional groups, radiochemistry, and nomenclature. Knowledge of arithmetic and basic algebra is essential.
VII. Required Course Content and Direction
Science and chemistry are important in the education of non-science majors. Scientific and chemical literacy are needed for people to function effectively as responsible citizens and productive performers in many fields. Chemistry 101 is designed to serve as a basic course in general and organic chemistry for the non-science major. Completion of this course will help nursing, allied health, and liberal arts students to better understand science in general, and chemistry in particular. Science majors can benefit from it as an introductory course in which the laws of nature and chemical principles are discussed.

Chemistry, as one of the Natural Sciences, has evolved out of careful observation and experimentation; as technology evolves, so does the body of chemical knowledge. This course integrates relevant technological advances with chemical principles and their applications. Furthermore, the laboratory component of the course helps to illustrate and apply some of these technological advances. The impact of these chemical principles on medicine, the environment, and society is also discussed.

  1. Course Learning Goals

    Students will:

    1. demonstrate qualitative knowledge and understanding of the basic laws of nature upon which all chemical principles are based, such as the law of conservation of mass and energy, the periodic law, and the gas laws [Scientific Literacy];
    2. describe and distinguish among the following terms: pure substance, mixture, element, compound, atom, and molecule. Write the names and symbols for selected elements and ions, the formulas and names of ionic compounds and of selected covalent compounds (binary, hydrocarbons, acids), and identify functional groups;
    3. solve operations involving dimensional analysis for unit conversion, stoichiometry problems, and concentration of solutions [Quantitative Literacy];
    4. discuss matter and transformations of matter, including states of matter, chemical reactions, balancing chemical equations, chemical bonding, intermolecular forces, acids and bases, and nuclear chemistry; and
    5. demonstrate basic laboratory skills as they pertain to: safety, significant figures in measurement, the metric system of measurement, management of both qualitative and quantitative work, and ability to draw conclusions from experiments [Critical Thinking].
  2. Planned Sequence of Topics and/or Learning Activities

    Course Outline:

    2. MATTER
      1. Types of Matter
      2. States of Matter
      3. Physical/Chemical Properties
      1. Units of Measurement
      2. The Metric System
      3. Dimensional Analysis
      1. Atomic Theory
      2. Subatomic Particles
      3. Atoms, Isotopes, and Ions
      4. Atomic Number, Atomic Mass
      1. Electron Configuration and Periodicity
      2. Periodic Properties
      1. Ionic Compounds
        1. Formula Writing
        2. Nomenclature
        3. Polyatomic Ions
        4. Properties of Ionic Compounds
      2. Molecular Compounds
        1. Lewis Formulas
        2. Nomenclature
        3. VSEPR Theory
        4. Polarity
        5. Properties of Covalent Compounds
      1. General Properties of Organic Compounds
      2. Structural Formulas
      3. Functional Groups
      4. Nomenclature
      1. Writing Chemical Equations
      2. Balancing Chemical Equations
      3. Mass and Moles of Substances
      4. Simple Stoichiometry
      1. Characteristics of Gases
      2. Gas Laws (qualitative study)
      3. Intermolecular Forces
      4. Properties of Liquids
      5. Properties of Solids
      1. Definitions
      2. Concentration Expressions
      3. Water as a Solvent
      4. Colloids
      5. Colligative Properties
      1. Definitions
      2. pH
      3. Reactions of Acids and Bases
      4. Buffers
      1. Radioactivity
      2. Types of Radiation
      3. Half-Life
      4. Properties and Uses of Radiation

    Laboratory Experiments:
    While specific laboratory experiments vary depending on the instructor and the semester, the following list is representative of the experiments that are used:

    1. Safety Practices in the Chemistry Laboratory: safety equipment in the laboratory, safe handling of chemicals, responding to emergencies, as well as benefits and responsibilities when working in groups.
    2. Measurement and The Metric System
    3. Density
    4. Composition and Effect on Density
    5. Separation and Analysis
    6. Periodic Table (Videotape)
    7. Physical Properties
    8. Ionic/Covalent Compounds
    9. Paper Chromatography
    10. The Preparation and Properties of Soap
    11. An Introduction to Chemical Reactions
    12. The Synthesis of Aspirin
    13. Acids, Bases, and the pH Scale
    14. Titrating Vinegar
    15. Molecular Models

    Learning Activities:
    Instruction aims to enable the student to:

    1. describe the origin of scientific knowledge and the importance of experimental evidence in developing such knowledge;
    2. distinguish between facts, laws, hypotheses, and theories;
    3. explain major evidence for atomic structure, including the role of new technology to allow researchers to propose and test models;
    4. state the number of protons, neutrons, and electrons found in one atom, for any specified element. Draw electronic configurations in sub levels, and identify valence electrons;
    5. describe and distinguish between the following terms: pure substance, mixture, element, compound, atom, and molecule;
    6. write the names and symbols for selected elements and ions, and the formulas and names of compounds;
    7. state the periodic law and discuss trends (for example, size, ionic charge, metallic character) among elements of the periodic table. Describe the octet rule and the rule of two;
    8. explain how bonding occurs to form ionic and molecular compounds, and identify the elements most likely to form each type of compound;
    9. compare the structure of ionic compounds with that of molecular compounds, and explain how the physical properties of each are related to (or explained by) their structure;
    10. name the three intermolecular forces and state their relative strengths;
    11. write and balance a chemical equation, given either a written description or a laboratory observation of the reaction;
    12. explain the meaning of a chemical equation. Explain the role of a catalyst. Solve simple mole-to-mole stoichiometry problems;
    13. explain, for a solution of a given concentration (molarity or percent), what the concentration means in terms of mass of solute and volume of the solution. Calculate concentrations of solutions given mass and volume data. Explain how solutes interact with solvents;
    14. define pH, and relate it to the properties of solutions and the possible hazards to individuals and the environment;
    15. define acid and base, and relate these terms to hydrogen ion concentrations and the pH scale;
    16. name simple organic compounds;
    17. compare the structure and properties of the major types of functional groups (alcohols, esters, acids, amines, amides, aldehydes, and ketones);
    18. explain what happens to the nucleus of an atom during a nuclear reaction, such as α, β, or γ emission. Indicate the impact of such as such a reaction on a living organism. Describe the uses and environmental effects of nuclear reactions;
    19. explain specifically how the concepts taught in the course relate to medicine, industry, and to environmental problems to their solutions;
    20. carry out basic laboratory procedures, such as determining metric measurements, simple separation of mixtures, determining properties of ionic and covalent compounds, carrying out some simple chemical reactions, determining pH, and using molecular models; and
    21. work safely, accurately, and cooperatively in the laboratory.
  3. Assessment Methods for Course Learning Goals

    Course learning goals will be continuously assessed by: periodic written examinations, class exercises, laboratory preparation, laboratory results, laboratory reports, and assigned work.
  4. Reference, Resource, or Learning Materials to be used by Student:

    Students will use approved text, laboratory modules and handouts, laboratory and demonstration equipment, library, science learning center, and computer programs. Please refer to the course syllabus for specific information.

Review/Approval Date - 11/04; Core Goals/Objectives added 5/04; Revised 6/08; New Core 8/2015