| Originator: | Mittelstaedt, Denice Status: Approved Department: CHM Chemistry |
| Date Created: | 11/12/2015 Submitted: 11/13/2015 Completed: 12/18/2015 |
| Effective Semester: | Fall |
| Catalog Year: | 2016-17 |
| Course Prefix: | CHM |
| Course Number: | 151 |
| Course Full Title: | General Chemistry I with Lab |
| Reason for Evaluation: | Competencies Change Description Change |
| Current Credit: | 4 |
| Lecture Hours: | 3 |
| Lab Hours: | 3 |
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| If the credit hour change box has been marked, please provide the new credit hour: | |
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| SUN Course?: | Yes |
| AGEC Course?: | Yes |
| Articulated?: | Yes |
| Transfer: | ASU NAU UA |
| Prerequisite(s): | TRE 089, MAT 121 |
| Corequisite(s): | CHM 151L |
| Catalog Course Description: | Chemistry is the study of the properties, composition, and transformation of matter. This course examines the principles of chemistry, chemical reactions, thermochemistry, quantum theory, the periodic table, and chemical bonding. The proper use of lab equipment and the application of the scientific method are also covered. This course is appropriate for students majoring in science and other programs requiring one year of chemistry. |
| Course Learning Outcomes: | 1. Describe the properties of, and relationships between, various types of matter (gases, solids, liquids, and solutions) and energy.(2,3 and 6)
2. Evaluate the intermolecular forces acting within substances (gases, liquids, solids) and identify the properties resulting from these forces.(2,3,5 and 6) 3. Differentiate between the effects of kinetic and potential energy on states of matter and phase changes, and apply these energy changes to chemical reactions.(2,3,5 and 6) 4. Evaluate multiple atomic theories and apply quantum theory to explain the electronic structure of, chemical bonding between atoms and determine the molecular geometry of molecules using VSEPR theory.(2,3,5 and 6) 5. Analyze how periodic behavior of the elements results from the properties of the atom.(2,3,5 and 6) 6. Demonstrate mathematical skills to analyze chemical problems in mass relationships and stoichiometry.(2,3,5 and 6) 7. Explain the principles of chemical reactivity both quantitatively and qualitatively.(2,3 and 6) 8. Determine solubility concentrations and ionic properties of compounds dissolved in aqueous solutions.(2,3,5 and 6) 9. Conduct experiments and prepare laboratory reports which are supported by data represented graphically or through a spreadsheet.(2,3,5 and 6) 10. Express gravimetric, volumetric, and spectroscopic chemical data to formulate conclusions according to scientific inquiry.(2,3,5 and 6) |
| Course Competencies: | Competency 1 Describe the properties of, and relationships between, various types of matter (gases, solids, liquids, and solutions) and energy.
Objective 1.1 Examine fundamental ways to classify materials, distinguishing between pure substances and mixtures Objective 1.2 Assess properties that are used to characterize, identify, and separate substances Objective 1.3 Calculate exact numbers and inexact numbers related to scientific work Objective 1.4 Execute calculations by obtaining correct units for the analysis. Competency 2 Demonstrate the basic structure of an atom and briefly discuss the formation of molecules and ions. Objective 2.1 Describe experiments that led to the discovery of electrons and to the nuclear model of the atom Objective 2.2 Explain the modern theory of atomic structure, including atomic numbers, mass numbers and isotopes Objective 2.3 Describe the concept of atomic weights related to the proton/neutron relationship for atoms Objective 2.4 Demonstrate the organization of elements into the periodic table Objective 2.5 Explain how molecule compositions are represented by empirical and molecular formulas Objective 2.6 Demonstrate how to use the periodic table to predict the charges on ions and the empirical formulas of the ionic compounds Objective 2.7 Describe how nomenclature is developed and applied Competency 3 Develop balanced chemical reactions by using chemical formulas to represent actions and quantitative information obtained about the amounts of substances involved in the reactions. Objective 3.1 Develop chemical formulas by writing equations that represent chemical reactions. Objective 3.2 Compare and contrast combination reactions, decomposition reactions, and combustion reactions Objective 3.3 Develop chemical formulas to relate the masses of substances to the number of atoms, molecules, or ions contained in the substances. Objective 3.4 Relate how the mole concept is applied to determine chemical formulas from the masses of each element in a given quantity of a compound Objective 3.5 Predict the amounts of substances consumed or produced in chemical reactions using knowledge of the combined processes Competency 4 Analyze chemical reactions by focusing on aqueous solutions using the correct vocabulary and aqueous chemical concepts. Objective 4.1 Identify reactions in which soluble reactants yield an insoluble product Objective 4.2 Describe oxidation/reduction reactions in which protons and H+ ions are transferred between reactants Objective 4.3 Describe the number of ways in which "Concentration" can be expressed Objective 4.4 Analyze stoichiometry and concentration to calculate the concentrations of substances in a solution chemical reactions and energy changes involving heat. Competency 5 Explain aspects of thermodynamics that involves the relationships between chemical reactions and energy changes involving heat. Objective 5.1 Compare and contrast kinetic energy and potential energy and the roles they play in accomplishing work or in transferring heat Objective 5.2 Describe 'internal energy" and how it relates on a state using the "First Law of thermodynamics" Objective 5.3 Describe how the function called enthalpy is useful in relation to energy involving heat Objective 5.4 Describe how calorimetry is used to measure heat changes in chemical processes Objective 5.5 Explain how to establish standard values for enthalpy changes in chemical reactions and how to use them to calculate enthalpy changes for reactions Competency 6 Describe the quantum theory and its importance in chemistry, including quantum mechanics and the arrangements of electrons in atoms (electronic structure of atoms). Objective 6.1 Compare and contrast radiant energy and electromagnetic radiation Objective 6.2 Demonstrate how electrons are arranged in atoms using orbitals Objective 6.3 Describe "Heisenberg's Uncertainty Principle" and "The Pauli Exclusion Principle" Objective 6.4 Compare and contrast classical and quantum mechanics in their relationship to matter Objective 6.5 Interpret graphs of electron density based on VSEPR and orbitals Competency 7 Explain how properties of atoms/elements change as they move across a row or down a column of the periodic table in ways that enable predictions about the physical and chemical properties of elements. Objective 7.1 Explain the history of the periodic table Objective 7.2 Explore the many properties of atoms that depend both on the net attraction of the outer electrons to the nucleus and on the average distance of those electrons from the nucleus Objective 7.3 Demonstrate how the size of atoms and ions follow trends that are related to their placement on the periodic table Objective 7.4 Analyze requirements using VSEPR and ionization energy to remove one or more electrons from an atom Objective 7.5 Examine ways the physical and chemical properties of metals and nonmetals are distinctly different and how they can be understood from the fundamental characteristics of atoms Competency 8 Express the relationship between the electronic structures of atoms and the chemical bonds formed. Objective 8.1 Predict chemical bonds by using the Lewis symbols technique for keeping track of the valence electrons in atoms and ions Objective 8.2 Explain the energetic of formation of ionic substances in terms of the lattice energy of these substances Objective 8.3 Describe electronegativity and the way it relates to covalent bonds Objective 8.4 Compare and contrast Lewis and resonance structures Objective 8.5 Describe the Octet Rule and the exceptions to the rule Competency 9 Demonstrate the nature of covalent bonds by demonstrating the relationship between two-dimensional Lewis structures and three-dimensional molecular shapes using VSEPR Objective 9.1 Predict molecular geometries by examining some common geometries exhibited by molecules Objective 9.2 Relate molecular geometries using a simple model based on Lewis structures and the repulsions between regions on high electron density Objective 9.3 Determine whether a molecule is polar or nonpolar Objective 9.4 Explain covalent bonding and orbital overlap Objective 9.5 Describe single bonds and multiple bonds Objective 9.6 Evaluate a treatment of bonding that uses molecular orbital theory, which introduces the concepts of bonding and antibonding molecular orbitals arising from atomic orbitals. Objective 9.7 Describe how molecular orbital theory is used to construct energy level diagrams for second-row diatomic molecules Competency 10 Distinguish the physical properties of gases in terms of the behavior of gas molecules. Objective 10.1 Compare the distinguishing characteristics of gases with those of liquids and solids Objective 10.2 Express the ways gas pressure is measured and the units used to express it in relation to the Earth's atmosphere and the pressure it exerts Objective 10.3 Describe the relationships between volume, pressure, temperature, and quantity of gas Objective 10.4 Calculate density and molar mass of a gas using the "ideal-gas equation" Objective 10.5 Describe the ways the "Kinetic-Molecular Theory" helps account for such gas properties as effusion and diffusion Competency 11 Explain the physical properties of liquids and solids and the phase changes that occur between states of matter. Objective 11.1 Compare and contrast solids, liquids, and gases from a molecular perspective Objective 11.2 Examine the intermolecular forces that occur within and between substances Objective 11.3 Define viscosity and surface tension Objective 11.4 Explain phase changes and their associated energies Objective 11.5 Examine the dynamic equilibrium that exists between a liquid and its gaseous state Objective 11.6 Explain how the structure of a crystalline solid can be conveyed in terms of its unit cell and how simple molecules and ions are most efficiently arranged in three-dimensions Competency 12 Demonstrate that the observable, macroscopic properties of materials are the result of atomic- and molecular-level structures and processes. Objective 12.1 Characterize materials according to the predominant bonding interactions and their ability to conduct electricity Objective 12.2 Compare and contrast semiconductors and superconductors Objective 12.3 Describe how the shapes, interactions, and bonding between polymer chains affect the physical properties Objective 12.4 Express how physical and chemical properties of bulk materials change when their crystals become very small Competency 13 Compare the physical properties of solutions, with the properties of their components using solubility, intermolecular forces and colligative properties. Objective 13.1 Explain what happens at a molecular level when a substance dissolves in relationship to the role of intermolecular forces in the process Objective 13.2 Explain saturated solutions and solubility and the factors affecting solubility Objective 13.3 Define "colligative properties" and "colloids" Objective 13.4 Define boiling point elevation and Freezing point depression |