This course: Explores the fundamental laws, theories, and mathematical concepts of chemistry. Designed primarily for science and engineering majors. Requires a strong background in mathematics. Part II of II. Lecture 3 hours. Laboratory 3 hours. Total 6 hours per week
In this course, the student will be responsible for learning the course materials that are generally taught in the first half of a general or college chemistry class. This is a transfer course and will cover the same material presented in any college or university course. Chemistry 111-112 is an introductory general inorganic chemistry course primarily for students majoring in the sciences or engineering. The principles and processes of chemistry developed in this course provide students with the ability to critically evaluate chemical information, both as scientists and as citizens. The course also provides the background material required for other courses in chemistry, biology, physics and engineering.
This course will cover the materials discussed in the text book with homework, quizzes, tests and writing assignments. The topics covered correspond to the objectives of the course as provided in the Course Outline or presented in the Chapter Objectives from the text.
Help students develop an understanding of basic chemical vocabulary, concepts and problem solving techniques.
Expose students to the role of chemistry in their world.
The general purpose of this course is to prepare the student for advanced study in science so that the student will be able to
(CLO1). Explain basic chemical concepts related to chemical changes, energy, and properties of matter.
(CLO2). Apply principles of chemical change and energy to understanding equilibrium and spontaneity in chemical reactions
(CLO3). Analyze evidence to decide if generalizations or conclusions based on the obtained data are warranted
(CLO4). Interpret and utilize mathematical formulas while solving problems
The student should be familiar with the learning objectives for CHM 111. Module learning objectives from CHM 111 will be listed where appropriate.
Measurement, Significant figures, Accuracy and Precision
CHM 111 MLO1-1 Demonstrate significant figure rules in calculations, using algebraic methods, scientific notation, and rounding numbers.
CHM 111 MLO1-2 Apply units of mass, temperature, time, length, and derived units, such as volume and density using dimensional analysis to solve problems with single or multiple steps or conversions. Recall the common base SI units of measurement, prefixes, and their associated symbols
CHM 111 MLO1-3 Evaluate the uncertainty, accuracy, and precision of measurements.
Chapter 11: Gases
Chapter 11 Topic 1: Property of Gases and the Kinetic Molecular Theory Sections 11.1, 11.2 and 11.3
CHM 111 MLO1-5 Differentiate between states (phases) of matter, pure substance or mixture, atoms, elements, compounds and molecules. Differentiate between a mixture that is heterogeneous or homogeneous.
CHM 111 MLO8-1 Apply the kinetic molecular theory to describe the characteristics of gases and what distinguish them from solids and liquids.
CHM 111 MLO8-2 Demonstrate the ability to convert between units of pressure, volume, temperature and amount (grams to moles) and describe the tools used to make these measurements.
Chapter 11 Topic 2: Gas Laws - Sections 11.4
MLO8-3 Use the Gas laws, combined gas law and ideal gas equation to perform calculations to determine pressure, volume or temperature for a given gas using values at standard temperature and standard pressure of gases.
Chapter 11 Topic 3: Ideal and Real Gases
Apply the ideal gas equation to determine characteristics of a gas including density and molar mass.
Explain the difference between real and ideal gasses and identify factors that may cause gases to deviate from ideal gas behavior.
Chapter 11 Topics 4 & 5: Dalton's Law and Stoichiometry
Use Dalton’s law of partial pressures to determine the mole fraction or partial pressure of gasses in a mixture of gasses.
Use the ideal gas equation in stoichiometric calculations.
Lewis Structure, Geometry and Polarity Review: Chapter 6 and 7
CHM 111 MLO4-1 Determine the polarity of a bond using differences in electronegativity to differentiate between ionic, polar covalent and nonpolar covalent bonds.
CHM 111 MLO4-3 Apply rules for drawing Lewis structures of compounds.
CHM 111 MLO4-5 Predict the electronic and molecular geometry, bond angles, and polarity using the Valence shell electron pair repulsion model.
CHM 111 MLO4-6 Identify the intramolecular (bonding) and intermolecular (attractive) forces between molecules: dipole-dipole, hydrogen bonding, and dispersion forces present in a given substance.
Identify compounds as ionic, molecular (inorganic or organic), metallic, or acids.
Chapter 12: Liquids and Solids
Chapter 12 Topic 1. Liquids
Explain how intermolecular forces and polarizability affect chemical and physical properties of liquids: vapor pressure, boiling point, surface tension, capillary action, density, volatility and viscosity
Explain vapor pressure, boiling point and evaporation of a liquid.
Chapter 12 Topic 2. Solids
Explain how intermolecular forces affect the physical properties of solids: vapor pressure, melting point
Identify the number and location of atom or molecules in the unit cell (lattice point, side, edge or face) for simple cubic, body centered cubic, face centered cubic/cubic close packed and hexagonal close packed unit cells
Determine the atomic radius or density of an atom given its unit cell packing.
Identify key characteristics and examples of the major types of crystals: ionic, covalent, molecular, or metallic.
Chapter 12 Topic 3. Phase Changes and Phase Diagrams
Understand changes in energy when a substance undergoes a phase, pressure and/or temperature change.
Explain phase boundary, triple point, critical point. and the phase of a substance at a given temperature and pressure based on a phase diagram.
Chapter Thirteen: Physical Properties of Solutions
Chapter 13 Unit 1. Definitions and properties
(CHM 111 MLO1) Differentiate between states (phases) of matter, pure substance or mixture (homogeneous or heterogeneous), atoms and molecules
(CHM 111 MLO6) Describe and predict properties of electrolytes to categorize compounds as nonelectrolytes, weak electrolytes or strong electrolytes.
(CHM 111 MLO6) Apply solubility rules of ionic compounds toward determining whether a reaction will produce a precipitate.
(CHM 111 MLO6) Calculate the molarity of a solution using molar mass and the mole concept: convert between mass, moles, and molarity.
(CHM 111 MLO6) Determine the concentration of a solution that has been diluted in addition to applying dilution principles toward serial dilutions.
Explain how solubility is affected by intermolecular forces, temperature and pressure (Henry's Law) and enthalpy between solute and solvent particles is related to saturated, unsaturated and supersaturated solutions.
Calculate solution concentration or interchange concentration units of molarity, molality, Percent and mole fractions.
Chapter 13 Unit 2. Colligative Properties
Describe and perform calculations involving colligative properties: vapor pressure lowering, boiling point elevation, freezing point depression and osmotic pressure.
Use van’t Hoff factors to determine the colligative properties of electrolyte solutions.
Chapter 14 Unit 1. Definitions and Collision Theory
Describe the main factors that can increase the rate of a reaction.
Utilize collision theory to describe effective collisions and activation energy using the Arrhenius equation.
Determine the average rate of a reaction or instantaneous rate given appropriate data.
Chapter 14 Unit 2. Determination of Rate Law
Determine the rate law and reaction order from experimental data.
Predict the units of the rate constant k for a reaction.
Calculate concentration, time, the rate constant or 1/2 life using the integrated rate law for the reaction.
Chapter 14 Unit 3. Mechanisms
Determine the overall balanced reaction, intermediates, catalyst and elementary steps in a reaction mechanism.
Determine the rate law of a reaction given its rate determining step.
Understand the criteria that must be met for a proposed mechanism to be plausible.
Chapter 15 Unit 1. Definitions, Enthalpy and Entropy
(CHM 111 MLO7) Describe and employ basic Thermochemistry principles to identify an open, closed or isolated system and the surroundings.
(CHM 111 MLO7) Explain enthalpy as a state function and identify a process as endothermic or exothermic
(CHM 111 MLO7) Use Hess's law, enthalpies of formation and bond energies to calculate heats of reactions or perform energy calculations that accompany reactions.
Predict the sign of ΔS of a process and use the sign to indicate whether the system has undergone an increase or decrease in entropy.
Explain the first, second and third law of thermodynamics.
Chapter 15 Unit 2. Gibbs free energy
Use Hess's Law to determine ΔH, ΔS and ΔG to determine whether a process is spontaneous under standard and non standard conditions. .
Explain, using thermodynamic terms, why energetically unfavored metabolic reactions can occur.
Chapter 16 Unit 1. Definitions of Equilibrium and the Equilibrium Expression
(CHM 111 MLO5) Write the reactants and products of a reaction with state of matter and balance the reaction using stoichiometric coefficients.
Write the equilibrium constant expression for a given reaction containing gases, liquids, solids and aqueous solutions
Determine the value of the equilibrium constant given equilibrium concentrations of reactants and products or the equilibrium concentrations given the value of the equilibrium constant.
Determine the relationship of Kc and Kp and between reactions that are reversed, multiplied by a factor of added to another reaction .
Chapter 16 Unit 2. Q, K and spontaneity
Write the equilibrium constant and reaction quotient for a given reaction
Calculate ΔG and ΔGº and of a reaction at a temperature given Q or K.
Chapter 16 Unit 3. Equilibrium concentration
Construct an ICE equilibrium table for a reaction and use it to determine equilibrium, initial or final concentrations of a reactant or product.
Chapter 16 Unit 4. Le Chatelier's principle
Apply Le Châtelier’s principle toward determining the shift of a reaction at equilibrium given a change in one of the following: removal or addition of reactant or product, change in volume or pressure, and temperature change.
Chapter 17 Unit 1. Definition of Acids and Bases
Identify an acid or base as being strong or weak and determine the conjugate acid or conjugate base pairs for monoprotic and polyprotic acids .and identify the amphoteric conjugates of polyprotic acids.
Determine the value of Ka, Kb and Kw and the relationship between these values for acid base conjugate pairs and the relative strength of the conjugate pair, hydrohalic, oxoacids, and carboxylic acids.
Chapter 17 Unit 2. pH and pH scale
Calculate pH, pOH, concentration of hydroxide ion, or hydronium ion utilizing the definitions and relationships between these terms and use the pH scale to classify a solution as being acidic, basic or neutral.
Chapter 17 Unit 3. Weak Acids and Bases
Calculate the pH of solution using the acid-dissociation constant (Ka) or the base disociation constant, Kb in equilibrium calculations.
Use the pH of a weak acid or pOH of a base solution to calculate the Ka or Kb, respectively.
Chapter 17 Unit 4. Salts
(CHM111 MLO3) Predict from the elements present in a compound whether it contains ionic or covalent bonds.
(CHM111 MLO6) Describe and predict properties of electrolytes to categorize compounds as nonelectrolytes, weak electrolytes or strong electrolytes.
Classify a salt as being basic, acidic or neutral based upon the acid and base used to form the salt amd determine the pH of a salt solution.
Chapter 18 Unit 1. Buffers
Calculate equilibrium concentrations or pH of a buffer solution using equilibrium calculations or the Henderson-Hasselbach equation. involving a common ion.
Describe how to prepare a buffer with a given pH.
Chapter 18 Unit 1. Titration
Calculate, Graph and explain the pH of a titration given the type of acid and base (strong or weak). the endpoint and equivalence point and select an appropriate indicator for the given titration.
Chapter 18 Unit 3. Solubility Product
Write a solubility reaction, the solubility product constant (Ksp), determine the molar solubility. and explain how pH or a common ion can affect the solubility product.
Use Ksp to predict whether a precipitation will occur and perform fractional precipitation/qualitative analysis.
Chapter 19 Unit 1: Definitions and Redox Reactions
(CHM111 MLO6) Apply oxidation number rules toward determining the oxidation number of each element in a compound or polyatomic ion.
(CHM111 MLO6) Identify the various components of an oxidation-reduction reaction including reducing/oxidizing agents and half-reactions to be able to balance the redox reaction.
Explain a galvanic cell, electrolytic cell, anode, cathode and salt bridge and the standard hydrogen electrode.
Calculate Eºcell of a reaction and interconvert between ΔG and K to determine spontaneity of the reaction
Chapter 19 Unit 2: Nernst equation
Use the Nernst equation to calculate the Ecell of a cell under non-state conditions and describe the relationship between concentration and cell voltage.
Chapter 19 Unit 3: Application of Electrochemistry
Distinguish between different types of batteries including: dry cell, alkaline, lead storage, lithium and fuel cells.