CHEM100 Preparatory Chemistry
Department of Science, Technology, Engineering & Mathematics: Chemistry
 I. Course Number and Title
 CHEM100 Preparatory Chemistry
 II. Number of Credits
 4 credits
 III. Number of Instructional Minutes
 3750
 IV. Prerequisites
 MATH103 (C or better)
 Corequisites
 MATH120
 V. Other Pertinent Information

Fourhour lecture and twohour laboratory/recitation per week. Safety glasses or goggles required. Nonprogrammable, nongraphing scientific calculator required.
Students are expected to use the Science Learning Center and/or the Tutoring Center outside of class time to complete assignments.
 VI. Catalog Course Description
 This lecture and laboratory course introduces some basics of chemistry for students with inadequate preparation for Chemistry I. The development of skills for solving quantitative (numerical) problems is emphasized. Topics include measurement, basic chemical concepts and theories, and nomenclature of simple ionic and covalent compounds.
 VII. Required Course Content and Direction

This course is designed to meet the needs of science and engineering students who are academically unprepared for Chemistry I, a required course in their programs of study. These students generally have deficiencies in their chemistry and/or mathematics backgrounds. The course content has been carefully chosen to correct these deficiencies and to enable the student to complete Chemistry I successfully. Students must have completed Intermediate Algebra, MATH103, before enrolling in CHEM100. They must take College Algebra, MATH120, concurrently with this course if they have not already done so because they must develop their mathematical sophistication simultaneously with their study of chemistry in order to understand the chemical concepts presented.
In order to prepare students for Chemistry I, the major focus of the course is in solving quantitative problems based on chemical laws and principles. Students are given a review of basic arithmetic and algebraic methods used in Chemistry I, as well as instruction in the use of the scientific calculator. Students are introduced to the metric system, to laboratory instruments used in the determination of the chemical and physical properties of matter, to scientific notation of chemistry including chemical symbols, chemical formulas, nomenclature, and chemical equations. Relative atomic and molecular weights and the mole concept are used in dealing with quantitative problems in stoichiometry. The use of the Periodic Law enables students to make valid predictions of the chemical behavior of the typical elements. Throughout the course, students are expected to translate the laws and principles learned into mathematical relationships needed in the solution of quantitative problems dealing with chemical phenomena.
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 will integrate important technological advances and their impact in the formulation of chemical principles and their applications. Furthermore, the laboratory component of the course will help to illustrate and apply some of these technological advances.
In general, the lectures deal with the laws and principles of chemistry while the weekly recitation sessions provide opportunities for students to develop the skills needed for dealing with the quantitative solutions of chemical problems. The laboratory sessions provide handson experience with the tools of science and allow students to reinforce the theoretical considerations presented in lecture with observations in the real world.

Course Learning Goals
Students will:
 apply mathematical concepts and methods to chemical phenomena and to chemical problems;
 recognize the basic vocabulary and notation of chemistry, develop an awareness of the origin of scientific knowledge and realize the importance of experimental verification of such knowledge;
 demonstrate an understanding of some of the basic theories and concepts of chemistry and be able to use these in verbal, mathematical, and graphical representations. These include:
 the atomic theory;
 relative atomic weights and the mole;
 the chemical bond: ionic and covalent bonds; and
 the concepts of density, percentage, molarity, and dilution;
 demonstrate an understanding of the following laws governing chemical phenomena, and be able to apply these laws to the solution of qualitative and quantitative problems:
 conservation of mass;
 law of definite composition;
 law of multiple proportions; and
 the periodic law; and
 demonstrate basic laboratory skills as they pertain to: safety, management of both qualitative and quantitative work, ability to draw conclusions from experiments, and understanding the importance of technological advances and scientific knowledge.

Planned Sequence of Topics and/or Learning Activities
Course Outline:
 Introduction to Chemistry and the Scientific Method
 Graphs
 How to Plot and Interpret Graphs
 Straight Lines on Graphs and Their Equations
 Scientific Notation
 How to Use a Scientific Calculator
 Measurement, the SI Units, and Significant Figures
 Problem Solving and Dimensional Analysis
 How to Read and Translate Problems from English to Math
 Density
 Matter, Elements, Compounds, and Mixtures
 Introduction to Atomic Theory, Atomic Structure, and the Periodic Table
 Formulas and Names of Ions, Ionic Compounds, Binary Covalent Compounds, and Acids
 Chemical Reactions and Chemical Equations
 Atomic Masses and the Concept of the Mole
 Molar Mass
 Percent Composition of Compounds
 Empirical Formulas and Their Calculation
 Stoichiometry in Chemical Reactions: Mole and Mass Relationships
 Solutions: Solubility, Concentration (Percentage, Molarity), and Dilution
 Introduction to Good Laboratory Practice
 How to Take and Record Data in the Laboratory
 How to Report Laboratory Results
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: Safety and Transfer and Measurement of Chemicals
 SI Units, Measurement, and Significant Figures
 Relationship of Mass and Volume, Part 1, Liquids
 Relationship of Mass and Volume, Part 2, Solids
 The Application of Density to the Composition of Solutions
 Separation of Sand and Salt
 Precipitation Reactions in Aqueous Solutions
 An Introduction to Some Chemical Reactions
 Counting by Weighing, Relative Mass, and The Mole Concept
 Stoichiometry: Relationship Between Amount of Reactant and Amount of Product
 Simple Qualitative Analysis Experiment
 Acid Base Titration
Learning Activities:
Instruction aims to enable the student to: use a scientific calculator correctly; add, subtract, multiply, and divide with signed numbers, whole numbers, decimal numbers, and fractions; and solve simple algebraic equations;
 draw graphs from experimental data and explain the meaning of such graphs in both physical and mathematical terms;
 use common laboratory equipment and the SI system to make measurements, and use exponential notation and the concept of significant figures to express those measurements and the results of calculations;
 describe and explain ratios and proportions and the concept of percent, identify their occurrence in chemical problems, and use them in conjunction with dimensional analysis to solve problems including those involving composition of matter, solutions, and stoichiometry;
 describe science and the scientific method and distinguish between facts, laws, hypotheses, and scientific and unscientific theories;
 state the postulates of Dalton's Atomic Theory, and the laws of Conservation of Mass, Definite Proportions, and Multiple Proportions, and explain how Dalton's Atomic theory accounts for these laws. Describe and distinguish among the following terms: pure substance, mixture, element, compound, atom and molecule;
 write the names and symbols of the elements, the names and symbols of the stable ions of the representative elements and common polyatomic ions, and the formulas and names of the compounds formed from those ions;
 state the periodic law; identify elements by period or group, or one of the common classes;
 describe a chemical bond, describe and distinguish between ionic and covalent bonds, and identify which elements are most likely to form which bonds. Identify the diatomic elements and name binary covalent compounds and the common acids;
 given a word description of a chemical reaction, write and balance the "molecular" chemical equation and explain its meaning;
 explain the meaning of mole, molar mass, atomic weight, formula weight, and molecular weight;
 solve chemistry problems involving density, percentage, molarity, dilution and stoichiometry, whether stated in words or encountered in an experimental setting; and
 use appropriate current technology in the laboratory to obtain data and understand the impact that this recent technology has on the field.

Assessment Methods for Course Learning Goals
Course learning goals are continuously assessed by: periodic written examinations, class exercises, laboratory preparation, laboratory results, laboratory reports, and assigned work. 
Reference, Resource, or Learning Materials to be used by Student:
Students use approved text, laboratory modules and handouts, laboratory and demonstration equipment, library, science learning center, tutoring center, and computer programs. Please refer to the course syllabus for specific information.

Review/Approval Date  3/99; Revised 2/08; Revised 6/08; Revised 8/14; New Core 8/2015