Home » Academics » Schools & Programs » School of Science » Transfer Programs » Chemistry » CHEM 111 General Chemistry I

SYLLABUS

Catalog Description

Part I of the general study of atomic systems including: scientific and dimensional analysis, states of matter, thermochemistry, atomic structure, chemical bonding, molecular geometry, and modern materials (liquid crystals, thin films, etc). For engineering and pre-professional majors. Prerequisite: MATH 115 or equivalent; high school chemistry with grade of B or better within last four years, or CHEM 110 with grade C or better. Semester Offered-Fall and spring.

General Objectives: Upon completion of the course, the student should have a working knowledge of the following:

1. Physical measurement
2. Dimensional analysis (factor-label, unit analysis)
3. Chemical nomenclature
4. Stoichiometry
5. Aqueous reactions
6. Thermochemistry
7. Atomic structure
8. Quantum mechanics
9. Atomic properties
10. Chemical bonding
11. Molecular Geometry
12. Gases
13. Liquids
14. Solids
15. Modern Materials

Specific Objectives: Upon completion of the course, the student should be able to:

• 1.1 Safely and effectively manipulate solid, liquid, and gaseous chemical samples.
• 1.2 Obtain valid data from analog and digital instrumentation.
• 1.3 Explain precision and accuracy and how these are determined.
• 1.4 Express experimental data in valid precision using the correct number of significant digits in scientific and engineering notations with appropriate units.
• 1.5 Express experimental results to the correct number of significant digits in scientific and engineering notations with appropriate units.
• 1.6 Calculate average, average deviation, and standard deviation from experimental data and use to express precision.
• 2.1 Convert between units using dimensional analysis.
• 2.2 Determine meaningful quantities from given parameters without the use of a specific formula using dimensional analysis.
• 3.1 Give the names and charges of common cations, anions, and polyatomic ions.
• 3.2 Name common ionic compounds from a given chemical formula and vice versa.
• 3.3 Name common binary compounds of nonmetals from a given chemical formula and vice versa.
• 3.4 Name common acids from a given chemical formula and vice versa.
• 4.1 Calculate formula weights and molecular weights.
• 4.2 Perform mass to mole and mole to mass calculations.
• 4.3 Perform moles to particle calculations.
• 4.5 Write and balance molecular, ionic, and net ionic chemical equations.
• 4.6 Calculate theoretical yields (from limiting reagent) and percentage yields for reactions.
• 5.1 Calculate molarity from given masses, moles, volumes, and dilutions.
• 5.2 Identify strong and weak electrolytes.
• 5.3 Predict the reactivity of metathesis reactions.
• 5.4 Predict the reactivity of oxidation-reduction couples.
• 5.5 Calculate solution stoichiometry using titration data.
• 6.1 Distinguish and describe kinetic and potential energy.
• 6.2 Distinguish a system from surrounding.
• 6.3 Define internal energy.
• 6.4 Relate heat and work through the first law of thermodynamics.
• 6.5 Calculate energy or temperature changes in calorimitry.
• 6.6 Use Hess's law, enthalpies of formation, and stoichiometry to calculate enthalpies of reaction.
• 6.7 Calculate energy changes involved in heating curves using heat capacities and phase change enthalpies.
• 6.8 Draw and label phase diagrams given critical point, triple point, and melting point data.
• 7.1 Describe the operation of a cathode ray tube.
• 7.2 Describe the behavior of radioactive rays in an electric field.
• 7.3 Describe Rutherford's gold foil experiments and how this supports the current model of the atom.
• 7.4 Know the charges and approximate masses of protons, neutrons, electrons, and photons.
• 7.5 Describe what alpha, beta, and gamma radiation is.
• 7.6 Describe the planetary (Bohr) model of the atom consisting of protons, neutrons, and electrons.
• 7.7 Determine the number of protons, neutrons, and electrons from the AZX isotopic notation.
• 8.1 Calculate energy, wavelength, and frequency of electromagnetic radiation.
• 8.2 Describe how transitions between quantized energy levels in an atom give rize to absorbtion/emmission line spectra.
• 8.3 Calculate the wavelength of absorbed/emmitted photons in the Bohr atom.
• 8.4 Calculate the wavelength of particles.
• 8.5 Use the Pauli exclusion principle, and Hund's rule to determine valid quantum numbers, electron configurations, and orbital diagrams of elements and ions.
• 8.6 Relate quantum numbers to orbital shapes
• 8.7 Draw s,p, and d orbitals.
• 9.1 Use effective nuclear charge and shell theory to predict relative sizes, ionizatin energies, and electron affinities of elements and ions.
• 9.2 Locate metals, metalloids, and nonmetals on the periodic table.
• 10.1 Describe the role of lattice energy for ionic compounds.
• 10.2 Determine bond polarity from electronegativities
• 10.3 Draw lewis resonance structures.
• 10.4 Use VSEPR to predict electron pair and molecular geometry.
• 10.5 Describe orbital overlap in covalent bonding.
• 10.6 Determine orbital hybridization from VSEPR theory.
• 10.7 Describe a sigma bond.
• 10.8 Describe a pie bond.
• 10.9 Relate lewis resonance structures to delocalized pie bonding.
• 10.10 Describe bonding and antibonding molecular orbitals.
• 10.11 Give the molecular orbital diagram, bond order, and magnetic behavior of second row diatomic molecules.
• 11.1 Define pressure.
• 11.2 Relate kinetic molecular theory to the ideal gas law.
• 11.3 Account for deviations from ideal gas behavior as in the van der Waals equation.
• 11.4 Use Dalton's law of partial pressure to find the pressure of a gas collected over water.
• 12.1 Describe ionic, dipole, and dispersion intermolecular forces.
• 12.2 Predict relative vapor pressures using intermolecular force considerations.
• 12.3 Define and give examples of hydrogen bonding.
• 13.1 Distinguish between amorphous and crystalline solids.
• 13.2 Define primitive cubic, body-centered cubic, and face-centered cubic unit cells.
• 13.3 Determine the number of atoms contained in a unit cell.
• 13.4 Distinguish between molecular, covalent-network, ionic, and metallic solids.
• 14.1 Discuss how a liquid crystal works, and predict whether a given molecule would exhibit liquid crystalline behavior.
• 14.2 Distinguish between condensation and addition polymers.
• 14.3 Discuss the processing and application of ceramics.
• 14.4 Discuss the formation and uses of thin films.