Main Navigation

Home » eCore » Courses » Course Descriptions

CHEMISTRY II AND LAB - CHEM 1212K (4 Credit Hours)

Description:  Second course in a two-semester sequence covering the fundamental principles and applications of chemistry designed for science majors. Laboratory exercises supplement the lecture material.

Prerequisites:

  • CHEM 1211K
  • College algebra.  Precalculus as a prerequisite or co-requisite is highly recommended.

Course Structure:

Units:

  1. Intermolecular Forces, Liquids and Solids
  2. Properties of Solutions
  3. Chemical Kinetics
  4. Chemical Equilibrium
  5. Acid-Base Equilibrium
  6. Additional Aspects of Aqueous Equilibria
  7. Chemical Thermodynamics
  8. Electrochemistry

Laboratories:

  1. Safety
  2. Vapor Pressure and the Clausius-Clapeyron Equation
  3. Freezing Point Depression
  4. Making Solutions
  5. Titration
  6. Back titration
  7. Fading of Phenolphthalein
  8. Chemical Equilibrium:  Finding a Constant, Kc
  9. Temperature Effects on Equilibrium Constant
  10. Oxidation State of Iron
  11. Qual Scheme Simulation

Course Objectives:

Unit 1:  Intermolecular Forces, Liquids and Solids

  1. Identify types of intermolecular forces, namely, ion-ion, ion-dipole, dipole-dipole, London forces and hydrogen bonds
  2. Predict the relative magnitudes of melting and boiling points based on intermolecular forces
  3. Describe properties of liquids such as viscosity and surface tension
  4. Identify phase changes that interconnect solids, liquids and vapor phases
  5. Predict relative vapor pressures of liquids based on intermolecular forces
  6. Construct and interpret phase diagrams
  7. Identify types of solids based on their structure
  8. Identify and describe synthetic and natural polymers

Unit 2:  Properties of Solutions

  1. Identify the components of a solution
  2. Explain why solutes dissolve in solvents
  3. Calculate the solubility of a solution
  4. Describe the effects of pressure and temperature on solutions
  5. Use units of concentrations to describe solutions
  6. Identify the colligative properties of a solution
  7. Calculate an unknown molecular weight of a solute using colligative properties;
  8. Describe a colloidal suspension

Unit 3:  Chemical Kinetics

  1. Define the terms “reaction rates” and “rate laws”
  2. Identify the parameters that affect reaction rates
  3. Calculate rates of reactions based on balanced equations
  4. Determine the order with respect to each reactant, based on experimental data
  5. Determine the order of a reaction graphically based on variations in concentration as a function of time
  6. Calculate concentrations as a function of time and determine half-lives
  7. Rationalize changes in reaction rates as a function of temperature
  8. Identify practical examples where rate phenomena can be applied, for example, catalytic converters in automobiles, souring of milk, etc.

Unit 4:  Chemical Equilibrium

  1. Write down an equilibrium constant expression
  2. Predict the abundances of products and reactants using the equilibrium constant
  3. Solve for an equilibrium constant when given equilibrium concentrations of reactants and products
  4. Solve for equilibrium concentrations when given the initial concentrations of reactants and equilibrium constant
  5. Determine the effect of changing reaction conditions such as pressure, volume, concentration, and temperature on a chemical equilibrium
  6. Explain and give examples of the role of a catalyst in a chemical reaction

Unit 5:  Acid-Base Equilibrium

  1. Identify acids and bases
  2. Calculate the pH of solutions of weak and strong acids and bases
  3. Solve for equilibrium concentrations of acids and bases given the initial concentrations of reactants and equilibrium constant
  4. Calculate Kb from Ka

Unit 6:  Additional Aspects of Aqueous Equilibria

  1. Understand the common ion effect.
  2. Prepare a buffer solution and calculate the pH.
  3. Perform calcutions of pH for acid-base titrations.
  4. Calculate solubility equilibria and predict precipitation.
  5. Appreciate chemistry behind qualitative analysis scheme.

Unit 7:  Chemical Thermodynamics

  1. Define the term entropy
  2. Compare qualitatively the entropy of two substances
  3. State and appropriately apply in problems the first, second and third laws of thermodynamics
  4. Define the term free energy
  5. Determine change in enthalpy, entropy and free energy for a chemical reaction using data in thermodynamic tables
  6. Determine, based on calculations of free energy, if a process is spontaneous
  7. Determine the equilibrium constant, given the free energy or vice versa

Unit 8:  Electrochemistry

  1. Identify reduction-oxidation (redox) reactions by calculating oxidation numbers
  2. Balance redox equations by the “half-reaction” method;
  3. Describe the processes in a galvanic cell
  4. Use reduction potentials to construct galvanic cells
  5. Predict spontaneity of reactions based on reduction potentials
  6. Determine cell potentials under non-standard conditions using the Nernst equation
  7. Carry out simple calculations on electrolysis
  8. Describe common batteries
  9. Describe the process of corrosion in terms of redox reactions

Other Required Materials:
Chemistry laboratory materials (Commonly found household items that may be purchased at local retailer for about $30.).

A kit comprised of laboratory equipment and glassware.  This kit, which may be leased, requires a usage fee and a refundable deposit.