The first semester of a two-semester sequence in College Chemistry for students in science and engineering.  The topics include principles of atomic structure, bonding, stoichiometry, chemical equations, ideal gas laws, solutions and colloids, and oxidation-reduction.  Class meets for 3 hours of lecture and 3 hours of lab per week.

Place into MATH111; CHEM100 or its equivalent is recommended.

A lab is required for this course. Some sections will require a separate lab, while other sections will include the lab.

Students completing this course will exhibit knowledge and competency in describing properties and reactivity of matter through words, calculations and experimental procedures.  The student must be able to:

• Describe and categorize types of matter using proper vocabulary and nomenclature by:
• Listing the characteristics of solids, liquids and gases.
• Distinguishing between and listing examples of physical properties, chemical properties, physical changes and chemical changes.
• Identifying an element as a metal, nonmetal or metalloid given a Periodic Table.
• Identifying a compound as either ionic or molecular given the compound’s name or chemical formula.
• Naming a compound appropriately using either the prefix or stock system of naming given the chemical formula.
• Apply basic concepts and principles of atomic structure and bonding through:
• Descriptions of the various models of the atom.
• Calculating the energies of electronic transitions using the Rydberg equation.
• Identification of the orbitals in each energy level and the electrons that occupy those orbitals.
• Drawing correct Lewis dot diagrams to aid in the drawing of Lewis structures of chemical compounds.
• Predicting properties and chemical reactivity of elements or compounds based on trends of the Periodic Table.
• Predicting molecular shapes using VSEPR Theory.
• Evaluate chemical reactivity of chemical species by:
• Writing balanced, chemical equations.
• Distinguishing between different types of chemical reactions based on the reagents and conditions given.
• Calculating molecular weights, percent composition, mole ratios, limiting reagents and yields of chemical reactions through stoichiometry and the use of chemical formulas and balanced chemical reactions.
• Apply knowledge of chemical properties and reactivity in a laboratory setting by:
• Creating appropriate experimental setups with glassware and equipment.
• Completing experiments in a time-efficient manner.
• Describing experiment success through calculations of percent error and percent yield.
• Summarizing the results and analyzing experimental methods through writing.

• Fundamental Concepts (15%)
  • Definitions of matter, energy, mass, weight, physical and chemical properties and changes.
  • Metric system and dimensional analysis including exponential notation and significant figures.
  • Density and specific heat.
• Atoms, Molecules, Ions and Chemical Reactions (15%)
  • Symbols and formulas.
  • Composition of atoms; isotopes.
  • Ionic verses molecular compounds.
  • Oxidation numbers and formulas of compounds.
  • Naming of compounds.
  • Classification of chemical reactions and balancing.
  • Balancing chemical equations.
• Chemical Stoichiometry (15%)
  • Atomic and molecular mass.
  • Moles of atoms and Avogadro’s Number.
  • Percent composition and derivation of formulas.
  • Stoichiometric calculations.
  • Limiting reagents and percent yield.
  • Molarity and titrations.
• Kinetic Molecular Theory and the Ideal Gas Laws (10%)
  • Kinetic molecular theory and Boyle’s, Charles’, and Graham’s laws.
  • The ideal gas law equation.
  • Dalton’s law of partial pressures.
  • Avogadro’s hypothesis and applied stoichiometry.
• Atomic Structure and Bonding (15%)
  • Fundamental properties of electrons, protons, and neutrons and how they arrange to make up the nuclear atom.
  • The outdated, but understandable Bohr model of planetary electronic structure.
  • How the hydrogen spectrum can be explained using the Bohr model.
  • The electromagnetic spectrum in general.
  • Calculations using the Rydberg equation.
  • Basic concepts of the Quantum-Mechanical model of the atom which has replaced the Bohr model. (Quantum numbers will not be tested.)
  • Heisenberg uncertainty principle.
  • The theory of main shells made up of subshells, subshells made up of orbitals and orbitals holding only two electrons maximum.
  • The relationship between s,p,d,f subshells and the periodic table.
  • Be able to write out electronic structure, EX: 1s2, 2s2, 2p6..
  • Identify the valence electrons of an atom and predict multiple oxidation states or valence for atoms.
  • Account for the variation in chemical and physical properties from one group or family on the periodic table to the other.
  • The variation of atomic and ionic radii and ionization potential from one element to another on the periodic table.
  • The variation of metallic and nonmetallic properties of the elements.
  • Understand the general concept of ionic and covalent bonding.
  • Draw Lewis dot diagrams for the elements.
  • Show bonding by drawing Lewis dot diagrams for molecules.
  • Electronegativity difference between atoms in a molecule and its effect on the polarity of the molecule.
  • Determine the formal charge of elements in compounds.
  • Use oxidation numbers to write formulas for compounds.
  • Predict reaction products.
  • Use the Valence Shell Electron-Pair Repulsion Theory, (VSEPR) to predict the shapes of molecules.
• States of Matter: Liquids and Solids  Solutions (15%)
  • Intermolecular forces and molecular arrangements for the liquid and solid state.
  • The heating curve, and energy associated with phase changes.
  • Predict relative intermolecular attractive forces, vapor pressure, boiling point, heat of vaporization, and solubility for selected compounds.
  • Definitions of various solutions and factors which effect solubility.
  • Dissolution of ionic compounds and electrolytes.
  • Percent composition (concentration), molarity, molality, mole fraction
  • Colligative properties, freezing point depression and boiling point elevation.
• Electrochemistry and Oxidation-Reduction (15%)
  • Electrochemical cells.
  • Balancing oxidation -reduction reactions.
  • Titration involving oxidation-reduction.
  • Electrolysis.

• Lab 1 - Safety & Procedures - Students will review safety information, as well as laboratory policies and procedures.
  
• Lab 2 -  Precision & Accuracy - Determine the precision of different graduated cylinders, Erlenmeyer flasks, and beakers.  Also, attempt to accurately determine the density of a simple solution.
  
• Lab 3 - A Salt from Metal - Synthesis of alum which teaches simple lab techniques, like filtration.
  
• Lab 4 - Precipitation Reactions - Perform a series of precipitation reactions to determine the contents of some unknown solutions.
• Lab 5 - Acid/Base Reactions - Accurately perform multiple titrations to explore the mathematical possibilities of acid/base reactions.
• Lab 6 - Juices - Determine the acidic content of common juices by titration with a standard base.
• Lab 7 - Calorimetry - Examine the process of an efficient heat transfer from a reaction mixture to water.
• Lab 8 - Polymers - Synthesis of multiple polymers displaying cross-linking effects.
  
• Lab 9 - VSEPR Theory - Examine geometric properties of molecules using model kits.
• Lab 10 - Spectrophotometry - Prepare multiple dilute solutions from a standard stock solution, then analyze their absorbance using a spectrophotometer.
• Lab 11 - Beer-Lambert Law - Using Beer’s Law, determine the molecular formula of an unknown solid.
• Lab 12 - Gases - Perform a reaction between an acid and a common metal and examine the relationship between gases and stoichiometry.
• Lab 13 - Carbonates & Bicarbonates - Examine limiting reagent concepts by reacting a simple acid with a known base.
• Lab 14 - Manganese Reactions - Examine the reaction of a metal with acid to produce reagent quality solids.
• Lab 15 - Le Chatlier’s Principle - Explores equilibrium effects of chemical reactions.
  
• Lab 16 - Luminol - Reactions of metal complexes and their luminescence.
  

1.  Text:  General Chemistry by Hill, Petrucci, McCreary, Perry, 4th edition.  It is not necessary to bring this text to class daily, although you should be practicing the problems from the book as it may be useful for asking questions.
2.  Solutions Manual (Optional):  Student Solutions Manual for General Chemistry by C. Alton Hassel, 4th edition.
3.  Study Guide (Optional):  Study Guide: General Chemistry by Dixie J. Gross, 4th edition. 
4.  Lab Manual:  CHEM 101 Lab Manual.
5.  Laboratory Notebook:  A bound laboratory notebook with duplicate sheets.  This is where you’ll record your data in lab.  I recommend the spiral bound 100 page carbon copy notebook from Hayden Mcneil Publishers.
6.  Safety Goggles:  Students must purchase their own laboratory safety goggles.  Goggles are available in the DACC Bookstore.  If you already have your own, they must offer complete protection of the side of your eyes.  (Look for the markings "Z87" stamped on the goggles.)  Lab safety glasses are not acceptable for students.
7.  Calculator:  Any simple scientific or graphing calculator is sufficient. 
8.  Enclosed Shoes & Pants:  For lab days.  If you are not dressed appropriately you will not be allowed to participate.

Grading is based on a weighted percentage of five different categories with overall grade divisions at 90, 80, 70 and 60 percent.  The five categories are:  four or more midterm tests accounting for forty percent of the course grade, fifteen lab reports accounting for twenty percent of the course grade, ten quizzes accounting for ten percent of the course grade, classroom work accounting for ten percent of the course grade, and a final exam accounting for twenty percent of the course grade.  Attendance is required and a student may be withdrawn from the class roster due to unexcused absences.  Laboratory work must be performed during the regularly scheduled laboratory period.  "Make-up" laboratory work at an alternate time will not be an option.  No credit will be given for laboratory reports submitted if the student was absent from that laboratory session.  If a student has a valid excuse for missing a lecture or laboratory class, credit for the missed period may be arranged with instructor.  It will not be "automatic".

Notes:
All students must pass the laboratory portion of the class in order to pass the course.

The final exam will include all the material that is covered in the semester.  Every student is required to take the final exam at the scheduled time.  Each student must take and pass the cumulative final exam in order to pass the course.

A curve may be applied at the instructor’s discretion.

Fall 2012

Feb 8 2013 11:42AM