Lab Text: "Laboratory Manual for General Chemistry Principles 1" by Mark, et al

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Course Profile and Outline

1. Course overview and goals: The course requires students to formulate intuitive and numerical answers in problems related to nomenclature, gases, balancing equations, stoichiometry and thermochemistry. In addition, the student should be able to perform inductive and deductive reasoning as it relates to atomic structure, bonding and molecular structure. It is our intention that the inductive and deductive reasoning gained by our students in this course will serve them well in all their future endeavors.
2. Methodology: The course is structured to include 45 hours of lecture and 45 hours of laboratory experience. Utilization is made of in-house prepared manuals, models and demonstrations. Lectures are designed to generate critical thinking to solve chemical concept problems and where possible to relate the answers to real world problems.

II. TERMINAL BEHAVIOR OBJECTIVES

The objectives given below are keyed to the lecture sections:

Section I: At the end of this section, the student should be able to:

1. Know the System Internationale S.I. (Metric System) units and observations and perform conversions of length, mass and volume.
2. Calculate density from appropriate data and or interconvert to mass or volume from density data.
3. Recognize states of matter, both homogeneous and heterogeneous; know the difference between chemical and physical properties and relate it to elements and compounds.
4. Dalton's Atomic Theory should be understood as it relates to the Laws of Conservation of Mass, Definite Proportions and Multiple Proportions.
5. From subatomic particle data calculate the Atomic Number, Neutron Number and Mass Number; from % isotopic abundance data calculate Atomic Weights/Mass. From Atomic Weights/Mass data calculate Molecular Weight.
6. Calculate % Composition from both a Molecular Formula and Experimental Data.
7. Understand the mole concept; calculate moles of elements and compounds and numbers of atoms and molecules.

Section II: At the end of this section, the student should be able to:

1. Predict the correct formula of an ionic compound formed between one element and another element or a polyatomic ion. Given a formula write the name of the compound.
2. Balance an equation using the simplest whole number.
3. Calculate moles and number of molecules for more complex substances.
4. Solve stoichiometry problems of the following types, mole-mole, mass-mole, mass-mass, %-mass. Solve limiting reagent problems.
5. Calculate the molarity of a solution given the mass of solute and volume of solution. Given the molarity and volume predict amount of solute needed.
6. Perform dilution calculations.

Section III At the end of this section, the student should be able to:

1. Understand the Kinetic Molecular Theory as it relates to the physical properties and behavior of gases.
2. Solve Boyle's, Charle's and Amonton's Gas Law problems.
3. Solve Combined Gas Law and Ideal Gas Law problems.
4. Solve Volume-Volume Problems.
5. Solve Avogadro's and Gay Lussac Combining Gas Law problems.
6. Understand the concept of vapor pressure, boiling point and solve for the partial pressure of a gases in a mixture of gases.
7. Recognize that gases can become non ideal, know when and why.
8. Recognize the names of scientists and their contributions in developing an understanding of atomic structure including, Nicholson, Carlisle, Crooke, J.J. Thompson, Goldstein and Rutherford.

Section IV At the end of this section the student should be able to:

1. Understand the relationship between wavelength frequency and speed of electromagnetic radiation.
2. Know the contributions of Bohr in determining the structure of the Hydrogen atom.
3. Calculate the energy of Hydrogen atom from the orbit number, n.
4. Interconvert between energy, frequency and wavelength via the Plank equation.
5. Recognize and know the significance of the deBroglie equation and quantum theory.
6. Describe electron distribution via the Bohn Model and the Modern Concept of an atom. Understand and use quantum numbers to describe electrons.
7. Interconvert between nlx notation and quantum numbers.
8. Recognize and know which elements in the Periodic Table are 
   classified as representative, transition and inner transition elements.
9. Recognize trends in the Periodic Table as they relate to Atomic Size, Ionization Energy and Electron Affinity.
10. Know that differences in Electronegativity lead to the formation of polarized bonds resulting in covalent, hydrogen and ionic bonding as well as it being responsible for differences in solubility.
11. Draw the structure of covalent molecules.
12. Understand the difference between temperature in heat. Calculate the heat lost or gained using water as a calorimeter . Be able to extend the results of heat lost and gained to determine the specific heat of a metal. 
13. Using Hess' Law calculate the Heat of a Reaction.
14. Using the First Law of Thermodynamics calculate g, w or E.
    

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Laboratory Schedule

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