CHEM 1041 - Principles of Chemistry I Credits: 5
Hours/Week: Lecture 5 Lab 3
Course Description: This is the first course in a two-course introduction to chemistry. Students will investigate the basic concepts of chemistry, including atomic theory and structure, chemical nomenclature, chemical equations and stoichiometry, electron configuration and periodicity, chemical bonding, molecular structure, enthalpy changes associated with chemical reactions, the behavior of gases, and an introduction to organic chemistry. Quantitative laboratory experiments emphasize observation, organization of data, and analysis of data. This course is intended for students who need a course in general chemistry to fulfill a requirement for a variety of majors such as: chemistry, medicine, biology, nursing, dentistry, physical therapy and liberal arts.
3 Natural Science
Prerequisite(s): Course placement into MATH 1061 or above, or completion of MATH 0070 with a grade of C or higher. Course placement into college-level English and Reading OR completion of ENGL 0950 with a grade of C or higher OR completion of RDNG 0940 with a grade of C or higher and qualifying English Placement Exam OR completion of RDNG 0950 with a grade of C or higher and ENGL 0090 with a grade of C or higher OR completion of ESOL 0051 with a grade of C or higher and ESOL 0052 with a grade of C or higher.
- Matter and Measurement
- Atomic Structure
- Chemical Bonding and Molecular Structure
- Chemical Equations and Stoichiometry
- Electron Configuration and Periodicity
- Inorganic Nomenclature
- Introduction to Organic Chemistry
- Reactions in Aqueous Solution
At the end of this course students will be able to:
- determine the number of significant digits in a number, and round measured and calculated results to the appropriate number of significant digits.
- apply dimensional analysis with proper attention to units and significant figures.
- describe and apply the scientific method.
- name or provide formulas for molecular and ionic compounds, including those with polyatomic ions.
- 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, given a periodic table.
- calculate the average atomic mass of an element from isotopic abundances and masses.
- correlate wavelength, frequency, and energy of light with electron energy level transitions in an atom using the Bohr model.
- apply the wave-particle duality and the uncertainty principle to describe properties of electrons.
- 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.
- identify valence and core electrons, and predict trends in atomic size, ionization energy, electron affinity, and charges on main-group ions.
- use Avogadro’s number to calculate the number of particles.
- balance chemical equations and perform stoichiometry calculations, including limiting reagent and percent yield calculations.
- determine the empirical formula of an unknown compound from percent mass data.
- use molarity in calculations involving solutions, including dilution and titration calculations.
- identify insoluble ionic compounds, strong and weak acids and bases, and oxidizing and reducing agents in precipitation, acid-base neutralization, and oxidation-reduction reactions.
- write molecular, total, and net ionic equations for precipitation and acid-base reactions.
- explain and write a formula for the First Law of Thermodynamics.
- determine the amount of heat associated with reacting a specified mass of reactant for a reaction with a given enthalpy change.
- use heat capacity or specific heat to relate the amount of heat associated with a temperature change for a substance.
- use Hess’s Law or enthalpies of formation to determine the enthalpy change for a reaction.
- describe bonding in pure covalent, polar covalent, and ionic compounds.
- draw Lewis structures for compounds including resonance, formal charge, and exceptions to the octet rule.
- use VSEPR theory and Valence Bond Theory to predict molecular shape, polarity, and bonding.
- explain the postulates of the kinetic molecular theory of gases.
- use the ideal gas law and the combined gas law in calculations.
- apply Dalton’s Law to determine the mole fraction, partial pressures, and total pressure of a gas mixture.
- use chemicals and basic laboratory equipment safely and with proper technique.
- record observations and analyze the results of experiments.
Competency 1 (1-6)
03. 01. Demonstrate understanding of scientific theories.
03. 02. Formulate and test hypotheses by performing laboratory, simulation, or field experiments in at least two of the natural science disciplines. One of these experimental components should develop, in greater depth, students’ laboratory experience in the collection of data, its statistical and graphical analysis, and an appreciation of its sources of error and uncertainty. 03. 03. Communicate their experimental findings, analyses, and interpretations both orally and in writing.
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