PCC/ CCOG / CH

Course Content and Outcome Guide for CH 105

Course Number:
CH 105
Course Title:
Allied Health Chemistry II
Credit Hours:
5
Lecture Hours:
40
Lecture/Lab Hours:
0
Lab Hours:
30
Special Fee:
$12.00

Course Description

Includes stoichiometry, gases, oxidation-reduction, acid-base concepts, equilibrium, physical and chemical properties of solutions, nuclear chemistry, and organic hydrocarbons. This is the second course in a three course sequence. Prerequisites: CH 104 and its prerequisite requirements. Audit available.

Intended Outcomes for the course

Upon successful completion students should be able to:

  • Assess the impact of physical and organic chemical theory on phenomena encountered in everyday life including the environment and human health.
  • Apply critical thinking skills and an understanding of scientific inquiry to make evidence-based decisions on issues that affect the environment and the community and encourage lifelong learning.
  • Formulate mathematical and chemical models based on quantitative and qualitative reasoning in order to solve problems.
  • Communicate complex scientific concepts and reasoning effectively, both orally and through formal and informal writings and reports.
  • Collaborate effectively with a diverse team to solve complex problems and accomplish tasks effectively.
  • Critically evaluate sources of scientific information to determine the validity of the data.

Course Activities and Design

  1. Active Learning: Problem-solving assignments
  2. Full-class Learning: Recitation exercises
  3. Collaborative Learning: Laboratory activities
  4. Independent Learning: Reading and lecture

Outcome Assessment Strategies

  1. Hand in assignments for grading.
  2. Participation
  3. Lab reports
  4. Testing

Course Content (Themes, Concepts, Issues and Skills)

  1. GASES
    1. Explain the application of
      1. Boyle's law
      2. Charles' law
      3. Dalton's law of partial pressures
      4. standard conditions
      5. kinetic molecular theory
      6. gas constant R
    2. Solve problems using
      1. Ideal gas equation
      2. Combined gas equation
  2. WATER AND THE LIQUID PHASE
    1. Define the following terms and demonstrate appropriate use:
      1. vapor pressure
      2. boiling point
      3. melting point
      4. heat of vaporization
      5. heat of fusion
      6. heating curve
      7. hydrogen bonds
    2. Solve problems involving heat and phase changes
    3. Write equations for selected reactions of water.
  3. SOLUTIONS
    1. Define and apply the following terms
      1. solute
      2. solvent
      3. concentrate vs. dilute solution
      4. supersaturation
    2. Solve problems to demonstrate application of the following
      1. molarity
      2. molality
      3. normality
      4. percent
      5. dilutions
    3. Restate the relationship between concentration and
      1. freezing point
      2. boiling point
      3. osmotic pressure
    4. Use a solubility table to predict the outcome of mixing solutions.
  4. ACIDS, BASES, AND IONIC SOLUTIONS
    1. Define and apply the following terms
      1. Arrhenius acid
      2. Bronsted/Lowry acid
      3. Lewis acid
      4. salt
      5. neutralization
      6. strong vs. weak electrolytes
      7. nonelectrolytes.
    2. Write and balance net ionic equations.
    3. Write the equation showing the ionization of water
    4. Calculate pH and apply the pH scale
    5. Calculate the results of acid-base titrations
  5. CHEMICAL EQUILIBRIUM
    1. Define and apply the following terms
      1. equilibrium constants
      2. percent ionization
      3. buffering
    2. predict the effect of LeChatelier's principle on
      1. temperature
      2. concentration
      3. catalyst
      4. pressure
    3. Use equilibrium theory to solve problems using
      1. Ka
      2. Ksp
      3. Kw
      4. Keq
  6. ELECTROCHEMISTRY
    1. Define and apply the following terms
      1. oxidation
      2. reduction
    2. Apply redox theory to balance equations in acid or basic solution
    3. Sketch and describe the operation of an electrochemical cell
  7. NUCLEAR CHEMISTRY
    1. Define and apply the following terms
      1. alpha radiation
      2. beta radiation
      3. gamma radiation
      4. half-life
      5. fission
      6. fusion
    2. Describe the relationship between:
      1. radioactivity and atomic structure
      2. penetrating power and the types of radiation.
  8. HYDROCARBONS: ALKANES
    1. Describe the bonding of carbon in alkanes
    2. Identify the functional groups of carbon
    3. Use the IUPAC system to name a structure and vice versa
    4. Compare the effect of homologous series to physical properties of alkanes.
    5. Predict the products of the following reactions of alkanes combustion monohalogenation
    6. Identify the functional groups of organic molecules
  9. UNSATURATED HYDROCARBONS
    1. Define and apply the following terms
      1. sigma bond
      2. pi bond
      3. aromatic
      4. ortho, meta, and para
    2. Identify the following for unsaturated hydrocarbons
      1. structures
      2. nomenclature
      3. physical properties
      4. chemical reactions


THE FOLLOWING IS A BRIDGE TOPIC BETWEEN CH 105 AND CH 106. IT MAY BE INTRODUCED IF THE INSTRUCTOR HAS THE TIME.
 

  1. ALCOHOLS, PHENOLS, ETHERS
    1. Define and apply the following terms: Primary, Secondary, and Tertiary Alcohols
    2. Examine the IUPAC name and draw the structure of the molecule
    3. Analyze the structure and write the IUPAC and common name.
    4. Contrast the physical bonding properties of hydrogen-bonding compounds with the non-polar hydrocarbons.
    5.  Predict the products of chemical reactions involving each class of alcohols.