CHEM 1614: General Chemistry I

Download as PDF
Subject
Chemistry
Credit Hours 4.0 Lecture Hours 4.0 Lab Hours 3.0
Type of Credit
Baccalaureate/Transfer
View Class Schedule
Course Description
The student will apply chemical concepts and principles to topics including atomic structure, chemical reactions and stoichiometry, thermochemistry, periodicity, chemical bonding, and states of matter. Quantitative applications are emphasized. IAI: CHM 911 Chemistry. IAI: P1 902L.
Prerequisite(s)
CHEM 1534 with a grade of C or better or appropriate high school chemistry course with a grade of C or better and MATH 1424 with a grade of C or better or appropriate assessment score, or STEM pathway of transitional math - Must be completed prior to taking this course.

At the end of this course, students will be able to:

  • Demonstrate appropriate safety precautions while in the chemistry laboratory and when handling chemicals and equipment.
  • Demonstrate skills in measurement and in clear communication of data and results.
  • Apply the concepts of significant figures and unit conversions to measurements and calculations.
  • Describe the modern model of the atom in terms of the subatomic structure of atoms, ions, and isotopes.
  • Relate the names and formulas of elements, ions, and compounds.
  • Describe various types of chemical reactions in terms of conservation of mass, bond rearrangement, balanced chemical reactions, and energy changes.
  • Perform calculations relating moles, mass, and molarity that involve compounds, solutions, gases, and chemical reactions.
  • Apply the concepts of heat and enthalpy to chemical and physical processes.
  • Relate atomic spectra to electron transitions in atoms.
  • Use the electronic structure of atoms and their positions in the Periodic Table to predict periodic trends in chemical and physical properties.
  • Draw Lewis structures and use them to predict the molecular geometry and polarity of simple covalent molecules.
  • Apply the gas laws to gases and mixtures of gases.
  • Use predicted intermolecular forces between molecules to make statements about their properties.
  • Describe types and properties of solids.
Topical Outline

1. Introduction to Matter, Energy, & Measurement

    a. States of matter

    b. Classifying matter

    c. Physical and chemical changes

    d. Forms of energy

    e. SI units

    f. Measurement of properties

    g. Precision vs. accuracy

    h. Significant digits

    i. Unit conversions

    j. Dimensional analysis
2. Atoms, Molecules & Ions

    a. Atomic theory

    b. Atomic structure and isotopes

    c. Atomic mass

    d. Periodic table

    e. Molecules

    f. Ions

    g. Ionic compounds

    h. Nomenclature of ionic, inorganic and simple organic compounds

3. Chemical Reactions & Stoichiometry

    a. Balancing chemical equations and reaction types

    b. Formula weight

    c. Percent composition

    d. Mole concept and conversions between chemical quantities

    e. Empirical/molecular formula

    f. Combustion analysis

    g. Stoichiometry

    h. Limiting reactants
4. Reactions in Aqueous Solution

    a. Electrolytes

    b. Solubility rules

    c. Precipitation reactions

    d. Ionic and net ionic equations

    e. Acid/base neutralization reactions

    f. Redox reactions

    g. Oxidation numbers

    h. Activity series

    i. Molarity calculations

    j. Dilution equation

    k. Solution stoichiometry

    l. Titrations
5. Thermochemistry

    a. 1st law

    b. Internal energy

    c. Heat and work

    d. Endo- and exothermic reactions

    e. Enthalpy of reaction

    f. Specific heat

    g. Calorimetry

    h. Hess's Law

    i. Enthalpy of formation

    j. Bond enthalpies
6. Electronic Structure of Atoms

    a. Wave properties of light

    b. Quantization

    c. Photons

    d. Line spectra

    e. Bohr model

    f. Wave properties of matter

    g. Atomic orbitals: shapes, quantum #'s, energies, spin

    h. Filling orbitals

    i. Electron configuration of atoms and ions

7. Periodic Properties of Elements

    a. Development of the periodic table

    b. Effective nuclear charge

    c. Sizes of atoms and ions

    d. Ionization energy

    e. Electron affinity

    f. Periodic trends

    g. Chemical properties by group
8. Chemical Bonding

    a. Octet rule

    b. Ionic and covalent bonds

    c. Electronegativity

    d. Bond polarity

    d. Lewis structures of atoms, ions and molecules

    e. Resonance structures

    f.  Exceptions to octet rule

    g. Bond strength and lengths

    h. Average bond enthalpies
9. Molecular Geometry & Bonding Theories

    a. Molecular shapes and polarity

    b. Applying the VSEPR model

    c. Orbital overlap

    d. Hybrid atomic orbitals

    e. Sigma and pi bonds

    f. Delocalization

    g. Molecular orbitals
10. Gases

    a. Pressure concept

    b. Gas law relationships (P, V, T, n)

    c. Ideal gas equation

    d. Gas density and molar mass

    e. Gas stoichiometry

    f. Gas mixtures

    g. Mole fraction and partial pressures

    h. Kinetic-molecular theory

    i. Effusion

    j. Diffusion

    k. Real gases
11. Intermolecular Forces and Liquids

    a. Interparticle forces (ion/dipole, hydrogen bonding, dipole/dipole, dispersion)

    b. Properties of liquids

    c. Phase changes

    d. Heating curves

    e. Vapor pressure

    f. Phase diagrams
12.Solids

    a. Properties and structures of different types of solids