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Course Description:
Course Description:
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 I 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 first year college level 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.
General Course Goals:
General Course Goals:
Help students develop an understanding of basic chemical vocabulary, principles and problem-solving techniques.
Expose students to the role of chemistry in their world.
Course Learning Objectives:
Course Learning Objectives:
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 changes, energy, and properties of matter.
(CLO2). Explain the properties of the atomic theory and the periodic table and how it relates to an understanding of chemistry
(CLO3). Analyze evidence to decide if generalizations or conclusions based on the obtained data are warranted
(CLO4). Interpret and utilize mathematical formulas and relationships while solving problems
Module Learning Objectives (MLO)
Module Learning Objectives (MLO)
The following objectives are linked to the textbook Chemistry, Atoms First, 4th edition by Julia Burdge and Jason Overby. However, these are general objectives that are present in a General chemistry course using any textbook.
Chapter 1 Topic 1: Measurement presentation (This link opens the Google Slide file containing the presentation of the materials for topic 1 of Chapter 1) - Sections 1.3 and 1.4
Chapter 1 Topic 1: Measurement presentation (This link opens the Google Slide file containing the presentation of the materials for topic 1 of Chapter 1) - Sections 1.3 and 1.4
MLO1-1 Demonstrate significant figure rules in calculations, using algebraic methods, scientific notation, and rounding numbers.
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
MLO1-3 Evaluate the uncertainty, accuracy, and precision of measurements.
MLO1-4 Explain the key components of the scientific method and differentiate between observations, inferences, and conclusions.
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.
MLO1-6 Categorize properties of matter as being quantitative or qualitative, physical or chemical, extensive or intensive.
MLO1-7 Evaluate an isotope to determine the atomic number, mass number, the number of electrons, protons or neutrons and charge.
MLO1-8 Identify the forms of radiation and balance nuclear reactions in which these particles are emitted or absorbed
MLO1-9 Describe isotopes and calculate the average atomic mass of an element given the atomic mass and relative abundance each of its naturally occurring isotopes.
MLO1-10 Convert between mass, moles and number of atoms using the relationships between Avogadro’s number, moles, molar mass and grams.
MLO1-11 Identify the symbols and names of common elements on the periodic table.
MLO1-12 Explain the organization of the Periodic Table of Elements in terms of families, groups, periods, metals, semimetals and nonmetals
Module 2: Electronic Structure of Atoms and the Periodic Table
Module 2: Electronic Structure of Atoms and the Periodic Table
MLO2-1 Utilize the electromagnetic spectrum to distinguish and convert between wavelength, frequency and energy of different types of radiation.
MLO2-2 Distinguish how light and spectroscopy lead to the understanding of the electronic structure of an atom (Bohr and Quantum model).
MLO2-3 Apply quantum number (principal, angular momentum, magnetic and electron spin) rules to determine allowable values for each type of quantum number and how the quantum numbers relate to atomic orbitals.
MLO2-4 Explain how the Pauli exclusion principle and Hund's rule are used to determine electron configurations and orbital diagrams.
MLO2-5 Utilize the periodic table to determine the electron configuration of a neutral atom or an ion.
MLO2-6 Predict the charge of an ion formed utilizing the number of valence electrons and its location on the periodic table.
MLO2-7 Predict properties of effective nuclear charge, ionic or covalent radius, ionization energy, electron affinity and electronegativity using the periodic table.
OP-MLO2-8 Use the periodic table to predict general trends in reactivity of main group metals.
Module 3: Compounds
Module 3: Compounds
MLO3-1 Predict from the elements present in a compound whether it contains ionic or covalent bonds.
MLO3-2 Apply the rules of nomenclature to write formulas or to name ionic compounds, molecular compounds and acids
MLO3-3 Identify polyatomic ions, their formula and charge
MLO3-4 Calculate molar mass of a compound and convert between mass and moles
MLO3-5 Calculate the percent composition of a compound or determine the empirical and molecular formula of a compound from percent composition.
Module 4: Chemical Bonding
Module 4: Chemical Bonding
MLO4-1 Determine the polarity of a bond using differences in electronegativity to differentiate between ionic, polar covalent and nonpolar covalent bonds.
MLO4-2 Illustrate bonding or charge of an ion from its valence electrons and location on the periodic table.
MLO4-3 Apply rules for drawing Lewis structures of compounds.
MLO4-4 Determine the formal charge on the atoms in a Lewis structure to identify the most likely structure of a compound when more than one Lewis structure can be drawn.
MLO4-5 Predict the electronic and molecular geometry, bond angles, and polarity using the Valence shell electron pair repulsion model.
MLO4-6 Identify the intramolecular (bonding) and intermolecular (attractive) forces between molecules: dipole-dipole, hydrogen bonding, and dispersion forces present in a given substance.
MLO4-7 Apply hybrid orbital theory to predict the hybridization and explain sigma and pi bonding and resonance in molecules.
OP-MLO4-8 Explain how atomic orbitals combine to form bonding and antibonding molecular orbitals
Module 5: Chemical Reactions and Mass Stoichiometry
Module 5: Chemical Reactions and Mass Stoichiometry
MLO5-1 Identify the common reaction types and predict products of the reaction
MLO5-2 Write the reactants and products of a reaction with state of matter and balance the reaction using stoichiometric coefficients.
MLO5-3 Calculate theoretical yield, actual yield, percent yield and limiting reagent using stoichiometry.
MLO5-4 Calculate the empirical formula of a compound using combustion or elemental analysis.
Module 6: Aqueous Reactions and Volume Stoichiometry
Module 6: Aqueous Reactions and Volume Stoichiometry
MLO6-1 Describe and predict properties of electrolytes to categorize compounds as nonelectrolytes, weak electrolytes or strong electrolytes.
MLO6-2 Apply solubility rules of ionic compounds toward determining whether a reaction will produce a precipitate.
MLO6-3 Write net ionic equations and predict products for precipitation and acid/base reactions.
MLO6-4 Apply oxidation number rules toward determining the oxidation number of each element in a compound or polyatomic ion.
MLO6-5 Identify the various components of an oxidation-reduction reaction including reducing/oxidizing agents and half-reactions to be able to balance the redox reaction.
MLO6-6 Calculate the molarity of a solution using molar mass and the mole concept: convert between mass, moles, and molarity.
MLO6-7 Determine the concentration of a solution that has been diluted in addition to applying dilution principles toward serial dilutions.
MLO6-8 Apply concepts of stoichiometry toward reactions in solution and their associated problems including gravimetric analysis and titrations.
Module 7: Thermochemistry
Module 7: Thermochemistry
Chapter 10 Topic 1: Introduction to Thermochemistry and Calorimetry - Sections 10.1, 10.2, 10.3 and 10.4
Chapter 10 Topic 1: Introduction to Thermochemistry and Calorimetry - Sections 10.1, 10.2, 10.3 and 10.4
MLO7-1 Describe and employ basic Thermochemistry principles to identify an open, closed or isolated system and the surroundings and calculate energy from heat and work
MLO7-2 Explain enthalpy as a state function and identify a process as endothermic or exothermic
MLO7-3 Perform calorimetry calculations involving heat, specific heat or heat capacity.
MLO7-4 Use Hess's law, enthalpies of formation and bond energies to calculate heats of reactions, lattice energies or perform energy calculations that accompany reactions.
Module 8: States of Matter - Gases
Module 8: States of Matter - Gases
Chapter 11 Topic 1: Property of Gases and the Kinetic Molecular Theory - Sections 11.1, 11.2 and 11.3
Chapter 11 Topic 1: Property of Gases and the Kinetic Molecular Theory - Sections 11.1, 11.2 and 11.3
MLO8-1 Apply the kinetic molecular theory to describe the characteristics of gases and what distinguish them from solids and liquids.
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.
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.
MLO8-4 Apply the ideal gas equation to determine characteristics of a gas including density and molar mass.
MLO8-5 Use Dalton’s law of partial pressures to determine the mole fraction or partial pressure of gases in a mixture of gases.
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