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CHEM141

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Principles Gen & Inorganic Chemistry I

ChemistryScience, Tech, Engr & Math
OverviewGoals, Topics, and ObjectivesAssessment, Requirements, and OutcomesRegister for this Course

Course Goals

This course is designed to prepare students for further courses in chemistry or to satisfy the requirement for a first semester course in chemistry for other fields of science. In addition to acquainting the student with the basic principles of chemistry, the course objective for course is to assist the student in developing critical thinking and problem solving skills.

Core Course Topics

  1. The classification of matter: phases, mixtures, compounds, and elements

  2. Measurements: metric system, significant figures

  3. Dimensional analysis: unit conversions, problem solving, percentages

  4. Basic atomic theory: atoms, protons, neutrons, electrons, and ions

  5. Periodic table: symbols, names, periods, groups, atomic weights

  6. Nomenclature: naming compounds and writing formulas

  7. Chemical equations: balancing; molecular, ionic, and oxidation-reduction

  8. Mole conversions: Avogadro’s number, molecular weights

  9. Stoichiometry: including limiting reactant

  10. Empirical formulas: from per cent composition and experimental data

  11. Solutions: molarity, dilutions, solution stoichiometry, titrations

  12. Gases: gas laws, gas stoichiometry, kinetic molecular theory, real gases

  13. Thermochemistry: calorimetry, Hess’ Law, enthalpies of formation, First Law of thermodynamics, heat and work, (optional: warming/cooling curves)

  14. Electromagnetic radiation: wavelength, frequency, photon energies, photoelectric effect

  15. Atomic Hydrogen: Bohr theory, wavefunctions, quantum numbers

  16. Electron configurations: ground state atoms and ions

  17. Periodic properties: atomic size, ionization energies, electron affinities, electronegativity

  18. Chemical bonding: ionic, covalent, orbital overlap, bond lengths, bond energies

  19. Lewis Dot Diagrams: resonance, molecular shapes and polarities

  20. Valence Bond Theory: hybridization, double and triple bonds

  21. Safety and related environmental concerns in the chemistry laboratory

  22. (Molecular Orbital Theory: optional)

Upon successful completion of this course, students will be able to:

Write and balance chemical equations, including molecular, ionic, and redox.

Name chemicals from formulas.

Write formulas from names of chemicals.

Distinguish among elements, compounds, and mixtures.

Describe the structure of atoms and ions in terms of subatomic particles.

Predict chemical and physical properties using the periodic table.

Solve problems using dimensional analysis (unit conversion).

Solve chemical problems using mole conversions.

Solve chemical problems using concentrations.

Differentiate the various electromagnetic radiations and their interaction with matter.

Use quantum theory to describe the hydrogen atom.

Write ground state electron configurations for atoms and ions.

Relate electron configurations to various periodic properties.

Relate thermochemical properties to heat changes in chemical processes.

Draw Lewis Dot structures.

Use Lewis Dot structures to predict molecular geometry and properties.

Solve gas law problems.

Relate kinetic molecular theory to the states of matter.

Display professional behavior, courtesy, and attitude.

Observe, analyze, and interpret laboratory data, collected from experiments built on core course topics, both qualitatively and quantitatively.

Demonstrate proficiency in laboratory techniques used in various experiments.

Demonstrate critical thinking skills in identification of laboratory unknowns.

Practice appropriate safety procedures in the laboratory.

Use environmentally sound chemical laboratory practices.

Prepare neatly and accurately written lab reports using calculations, graphs,explanations, and chemical equations.