CHEM 1061 - Principles of Chemistry I

• Placement into MATH 0120 /MATH 1200 , or appropriate score on math placement test or equivalent

AND

• CHEM 1020  or CHEM 1050  or high school chemistry or equivalent

1. At the conclusion of the lecture portion of this course, learners will demonstrate competency in the following areas:
   • Quantitative Skills/Problem Solving/Scientific Method
     • Determine the number of significant digits in a number, and round numbers and calculated results to an appropriate number of significant digits.
     • Apply dimensional analysis with proper attention to units and significant figures.
     • Describe and apply the scientific method used by scientists in solving problems.
   • Nomenclature
     • Given the name of a polyatomic ion, give the correct formula and charge, and vice-versa.
     • For ionic and simple inorganic molecular compounds, given a chemical formula, give the correct name, and vice-versa.
   • Atomic Structure
     • Describe electrons, protons, and neutrons, and the general structure of the atom.
     • Define isotope and determine the atomic number, mass number, and number of neutrons for a specified isotope.
     • Identify the atomic number and atomic mass for any element.
     • Calculate the average atomic mass of an element from isotopic abundances and isotopic masses.
     • Correlate wavelength, frequency, and energy of light with electron energy levels in the atom via the photoelectric effect and the Bohr model.
     • Apply wave-particle duality and the uncertainty principle to describe properties of electrons.
     • Apply the results of the Schrödinger quantum mechanical model of the atom to assign quantum numbers to electrons and write electron configurations of multi-electron atoms and ions.
     • Identify valence vs. core electrons and predict trends in atomic size, ionization energy, electron affinity, and charges on main-group ions.
   • Stoichiometry
     • Given a chemical formula, calculate molar mass; given the amount of a substance, use Avogadro’s number to calculate number of particles.
     • Balance chemical equations and use stoichiometric relationships to calculate product and reactant amounts, determine limiting reagents, and calculate percent yields.
     • Determine the empirical formula of an unknown compound using composition by mass or combustion analysis data.
     • Calculate molarity; give amount or mass of solute and volume of solution; determine how to prepare a solution of a given molarity from the solute and water or by dilution of a more concentrated solution.
     • Apply titration principles to determine the concentration of an unknown aqueous solution.
   • Reaction Types
     • Identify insoluble ionic compounds, strong and weak acids and bases, and oxidizing and reducing agents in precipitation, acid-base neutralization, and oxidation-reduction (redox) reactions.
     • Predict products, identify spectator ions, and write net ionic equations.
   • Thermochemistry
     • Explain the First Law of Thermodynamics and express relationships among heat, work, energy, and enthalpy.
     • Apply thermochemical equations to relate amount of heat energy to the quantity of substance reacted.
     • Calculate heat transferred using temperature measurements, heat capacity or specific heats.
     • Apply Hess’s Law and enthalpies of formation to determine enthalpies of reaction.
     • Calculate reaction enthalpies using calorimetry data.
   • Molecular Structure: Bonding, Geometry, and Polarity
     • Describe bonding in pure covalent, polar covalent, and ionic structures.
     • Draw Lewis structures for compounds including resonance, formal charge, and exceptions to the octet rule.
     • Interpret VSEPR theory, Valence Bond Theory, and possibly Molecular Orbital Theory to predict molecular shape, polarity, and bonding.
   • States of Matter: Gas Phase
     • Explain the major points of the kinetic molecular theory of gases.
     • Describe the relationship between pressure, volume, moles, and temperature using gas laws.
     • Write the equation for the ideal gas law and use it in calculations.
     • Apply Dalton’s Law to determine the mole fraction, partial pressures, and total pressure of a gas mixture.
2. At the conclusion of the laboratory portion of this course, learners will demonstrate competency in the following areas:
   • Conduct laboratory work in compliance with guidelines for personal lab safety and responsible management of chemical waste; this includes appropriate use of personal protective equipment and interpretation of Globally Harmonized System for Hazard Communication (GHS) labels.
   • Measure quantities such as mass, volume, temperature, and absorbance with proper technique, and record the results of measurements with the appropriate number of significant figures and units.
   • Record observations of chemical processes (such as precipitate formation, gas evolution, etc.) and write chemical reactions consistent with their observations.
   • Use proper techniques for laboratory procedures such as titration, filtration, solution preparation, spectrophotometric measurements, etc.
   • Properly use glassware and equipment including beakers, Erlenmeyer flasks, volumetric pipets, burets, volumetric flasks, watch glasses, graduated cylinders, filtration apparatus, single-beam spectrophotometer, pH meter, and balances.
   • Effectively communicate lab procedures, observations, and results in the form of a laboratory notebook, written reports, and a verbal presentation.
   • Interpret and analyze qualitative observations and quantitative results, incorporating graphs and tables as appropriate.

1. Major Areas of Lecture Content
   • Measurement and dimensional analysis
   • Atomic theory including the historical development of atomic structure and isotopes
   • Inorganic nomenclature including polyatomic ions, ionic and binary molecular compounds and acids
   • Identification of reaction types including redox, precipitation, acid-base, and combustion; prediction of double replacement reactions products
   • Determining percent composition and empirical and molecular formulas
   • Stoichiometry including balancing chemical equations, mole calculations, limiting reactant, and percent yield
   • Solutions including molarity calculations, titrations, and dilution
   • Gas laws including ideal and combined, kinetic molecular theory, and effusion/diffusion
   • Thermochemistry including enthalpy, Hess’s Law, and calorimetry
   • Quantum theory including the historical development of quantum mechanics, atomic orbitals, quantum numbers, electron configurations, and periodicity
   • Bonding theory including ionic and covalent, Lewis electron dot structures, formal charges and resonance, polarity, and dipole moments
2. Major Areas of Laboratory Content
   • Collection of data using a variety of equipment, especially computer-interfaced probeware
   • Spreadsheet software for calculation, data analysis, and graphing
   • Measurement of physical properties, e.g. density
   • Microscale reaction technique
   • Volumetric gas collection
   • Reaction stoichiometry and limiting reactant
   • Observation/interpretation of precipitation and redox reactions
   • Empirical gas laws
   • Titrimetric and colorimetric determination of analyte concentration
   • Reaction enthalpy measurement
   • Laboratory project and presentation