Chemistry for Engineering

Upon completion of this course, the successful student should be able to:

• Carry out measurements using the correct number of significant figures, and demonstrate an understanding of precision and accuracy.
• Carry out calculations involving the ideal gas equation.
• Solve stoichiometry problems of the following types: gram-gram or gram-volume (of a gas), solution stoichiometry, limiting reactant, problems involving two simultaneous or two sequential reactions.
• Explain the Bohr Theory of atomic structure.
• Provide the electronic configuration of any of the common elements in the periodic table.
• Determine relative sizes, ionization energies, and electron affinities of elements using the periodic table.
• Explain and apply the concepts of dipole moment and electronegativity to covalent bonds.
• Draw Lewis structures for a given molecule, including those exhibiting resonance or expanded valence shells.
• Use the VSEPR theory to predict the geometry of any polyatomic molecule.
• Use the Molecular Orbital Theory of bonding to describe the bonding in any diatomic molecule involving hydrogen atoms.
• Predict the most likely intermolecular forces present in a bulk sample of a compound.
• Predict trends in boiling point and heat of vaporization among a group of two or more compounds.
• Determine whether chemical reactions will occur spontaneously under standard conditions by using a table of standard electrode potentials.
• Determine the relative strengths of oxidizing agents or reducing agents by using a table of standard electrode potentials.
• Distinguish between various types of heats of reaction and write the corresponding chemical equation.
• Interpret the signs of enthalpy changes.
• Describe both qualitatively and quantitatively the contributions of delta H and delta S to reaction spontaneity.
• Predict the sign of delta S for various chemical and physical processes.
• Interpret equilibrium in terms of thermodynamic driving forces.
• Write the chemical equation for equilibrium involving weak acids and bases in aqueous solution.
• Define any of the chemical terms or describe any of the chemical processes used in the course (e.g. anode, state function)
• Solve problems of the following types:
• Determination of the amount of material produced in an electrolytic cell;
• Calculation of the E.M.F of a galvanic cell;
• Calculation of delta G from electrochemical data;
• Calculations involving the First Law of Thermodynamics;
• Calculation of enthalpy change in a chemical or physical process;
• Calculation of any quantity in a Hess’s Law equation;
• Calculation of delta S from absolute entropies;
• Calculation of delta G for a chemical reaction;
• Calculation of K from delta G°;
• Calculation of quantities relating to aqueous acid-base equilibria (e.g. pH, weak acid ionization constant) and;
• Determination of the order and rate law of a chemical reaction.

Laboratory Objectives:

• State the name and describe the use of common laboratory equipment.
• Accurately perform standard laboratory procedures, such as titration, weighing, pipetting, using accepted methods and techniques.
• Identify the random and systematic errors inherent in common quantitative techniques used in the laboratory.
• Write a report based on observations and data obtained in the laboratory using a standard report format.
• Apply appropriate mathematical techniques (e.g. graphical analysis, solution of equations, etc.) to obtain a numerical result when given a set of experimental data (obtained in the laboratory or otherwise).
• Determine the relationship between experimental variables using the data, observations or results of an experiment.
• Identify the theory upon which an experiment is based.