CHEM 1041 - Principles of Chemistry I

1. Matter and Measurement
2. Atomic Structure
3. Chemical Bonding and Molecular Structure
4. Chemical Equations and Stoichiometry
5. Electron Configuration and Periodicity
6. Gases
7. Thermochemistry
8. Inorganic Nomenclature
9. Introduction to Organic Chemistry
10. Reactions in Aqueous Solution

1. determine the number of significant digits in a number, and round measured and calculated results to the appropriate number of significant digits.
2. apply dimensional analysis with proper attention to units and significant figures.
3. describe and apply the scientific method.
4. name or provide formulas for molecular and ionic compounds, including those with polyatomic ions.
5. describe electrons, protons, and neutrons, and the general structure of the atom.
6. define isotope and determine the atomic number, mass number, and number of neutrons for a specified isotope.
7. identify the atomic number and atomic mass for any element, given a periodic table.
8. calculate the average atomic mass of an element from isotopic abundances and masses.
9. correlate wavelength, frequency, and energy of light with electron energy level transitions in an atom using the Bohr model.
10. apply the wave-particle duality and the uncertainty principle to describe properties of electrons.
11. apply the results of the Schrödinger model of the atom to assign quantum numbers to electrons and write electron configurations of multi-electron atoms and ions.
12. identify valence and core electrons, and predict trends in atomic size, ionization energy, electron affinity, and charges on main-group ions.
13. use Avogadro’s number to calculate the number of particles.
14. balance chemical equations and perform stoichiometry calculations, including limiting reagent and percent yield calculations.
15. determine the empirical formula of an unknown compound from percent mass data.
16. use molarity in calculations involving solutions, including dilution and titration calculations.
17. identify insoluble ionic compounds, strong and weak acids and bases, and oxidizing and reducing agents in precipitation, acid-base neutralization, and oxidation-reduction reactions.
18. write molecular, total, and net ionic equations for precipitation and acid-base reactions.
19. explain and write a formula for the First Law of Thermodynamics.
20. determine the amount of heat associated with reacting a specified mass of reactant for a reaction with a given enthalpy change.
21. use heat capacity or specific heat to relate the amount of heat associated with a temperature change for a substance.
22. use Hess’s Law or enthalpies of formation to determine the enthalpy change for a reaction.
23. describe bonding in pure covalent, polar covalent, and ionic compounds.
24. draw Lewis structures for compounds including resonance, formal charge, and exceptions to the octet rule.
25. use VSEPR theory and Valence Bond Theory to predict molecular shape, polarity, and bonding.
26. explain the postulates of the kinetic molecular theory of gases.
27. use the ideal gas law and the combined gas law in calculations.
28. apply Dalton’s Law to determine the mole fraction, partial pressures, and total pressure of a gas mixture.
29. use chemicals and basic laboratory equipment safely and with proper technique.
30. record observations and analyze the results of experiments.

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