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Hawaii Pacific University
CHEM 2050 General Chemistry I Section ____
Semester and year, meeting times
Instructor: Name, contact information and other relevant information about the instructor.
Course description: This course is the first half of a 2-semester sequence in which students gain a solid
foundation in chemical principles and science in general. This foundation is needed for advanced
courses in the physical and natural sciences. Other key objectives of this course include learning how to
use correct mathematical expressions to solve chemistry problems, gaining experience in solving
complex problems, improving critical thinking skills, and increasing the understanding of how chemistry
complements other disciplines and is irreversibly woven into the fabric of society.
Course prerequisite: WRI 1100 or 1150 (or verbal SAT of 510 or English ACT of 21 or above) and MATH
1130 (or Math SAT of 550, or Math ACT of 24 or greater).
General Education Requirement: This course is classified under the Global Systems Theme and meets
the requirement for a course in Global Systems C: Other Global Systems Courses.
General Education Student Learning Outcomes and the Five Themes: HPU’s general education
curriculum is focused around five themes. This course emphasizes the Global Systems Theme and
provides students with opportunities to achieve the following related general education student
learning outcomes.
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Students will utilize various systems approaches or theories to comprehend global
processes. Many aspects of communicating chemistry are system approaches (elements,
symbols, chemical equations, SI units, etc…). Topics covering the structure of an atom,
especially electrons, rely on modern atomic theory.
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Students will comprehend the global impact of . . . physical science . . . systems.
Recognizing how matter is classified is a key way of comprehending the impact of
chemistry on the world. Also, certain topics in kinetics, gases, equilibrium, pH, and
radioactivity also address global impact.
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Students will understand the importance of global environmental systems and the
interactions between humans and the environment. Topics in chemical reactions, solution
processes, equilibrium, and radioactivity all address how humans and the environment are
impacted by these topics in chemistry and stress their importance. Humans, and all life
on earth, are made up of chemicals, and life consists of chemical reactions. The
environment at each level in a global system influences these reactions and equilibria.
Humans consume complex carbohydrates, oxidize them to release energy and exhale
carbon dioxide. Using chemistry, modern humans synthesize and release environmental
toxins as well as many useful products.
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The course also addresses the Research and Epistemology Theme by providing students with
opportunities to achieve the following related general education student learning outcome:
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Students will utilize methods and technologies appropriate to the discipline to
investigate research questions, generate predictions, test hypotheses and/or solve
problems. Key objectives of this course include learning how to use correct
mathematical expressions to solve chemistry problems, gaining experience in solving
complex problems, and improving critical thinking skills. In chemistry, individuals often
use the scientific method to test predictions of hypotheses and theories. Students will
work with a number of important theories used to predict chemical behavior.
Note: Purple text shows places where specific course information must be filled in. Red text contains
explanatory notes to the instructor which should be deleted before using the syllabus. Blue explanations
above should be rephrased by the individual instructor to reflect the specific approach in that section of
the course. Course-specific outcomes below are provided as an example and may also be rephrase,d
modified or condensed by the instructor.
Course-Specific Student Learning Outcomes for CHEM 2050
By the end of this CHEM 2050 course, each student should be able to:
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Recognize the interdisciplinary nature of chemistry.
Use the factor-label method (dimensional analysis) to solve problems.
Define and use metric units of measurement.
Do conversions between the metric and British systems of measurement.
Express numbers in scientific notation.
Define and use significant figures in calculations.
Name the symbols for common elements given in the periodic table.
Differentiate between protons, neutrons, electrons, atoms, molecules.
Recognize and name chemical formulas for simple compounds (ionic and molecular) and ions.
Determine the atomic weight or molecular weight (molar mass) of a compound using its chemical formula
and the periodic table.
Differentiate between elements, compounds, and mixtures.
Define matter.
Identify the three states of matter.
Differentiate between the physical properties and chemical properties of matter.
Differentiate between a physical change and a chemical change.
Define density and perform calculations involving density.
Define isotope.
Describe the simple structure of an atom, including the nucleus and electron orbitals or clouds.
Recognize how positive and negative ions are formed.
Determine the percent composition of each element in a compound.
Determine the empirical formula and molecular formula of a compound using appropriate data.
Differentiate between metals and non-metals.
Write and balance chemical equations for chemical reactions.
Differentiate between molecular equations and net ionic equations and identify spectator ions.
Identify some common types of chemical reactions.
Determine the oxidation number of each element in a compound.
Define mole and Avogadro's number.
Convert between atoms or molecules, moles, and grams of a substance.
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Determine the amount of reactants needed and the amount of products
formed (yield) in a chemical reaction using appropriate data.
Determine the limiting reagent and the excess reagents in a chemical reaction.
Define the stoichiometry of a chemical reaction.
Define and determine the percent yield for a reaction.
Define solution and molarity.
Perform calculations involving the molarity of a solution.
Understand and apply gas laws involving pressure, volume, temperature, and amount of a gas.
State the ideal gas law and perform calculations involving the ideal gas law.
Discuss the Kinetic Molecular Theory of Gases.
Understand energy changes in a chemical reaction.
Define the terms exothermic and endothermic.
Define and discuss electromagnetic radiation (waves) and its properties.
Discuss Bohr's Theory of the Hydrogen Atom in simple and general terms.
Differentiate between covalent bonds and ionic bonds.
Draw Lewis electron dot structures for atoms, ions, and simple covalent compounds.
Determine the formal charge for each atom in a compound based on the Lewis electron dot structure.
Define polarity and predict the polarity of chemical bonds.
Use the Valence Shell Electron Pair Repulsion Theory to predict shapes of molecules and ions.
Predict the polarity of a molecule.
Identify and discuss intermolecular forces.
Determine the percent composition of each element in a compound.
Determine the empirical formula and molecular formula of a compound using appropriate data.
Determine the limiting reagent and the excess reagents in a chemical reaction,
and calculate the amount of excess reagent that remains in a chemical reaction.
Calculate the mole fraction of an element or compound in a mixture or solution.
Understand energy changes in a chemical reaction.
Define the terms exothermic, endothermic, enthalpy, and heat of reaction.
Calculate the heat of reaction based on stoichiometry and appropriate data.
Use Hess's Law to determine the heat of reaction.
Define and calculate the specific heat and heat capacity of a substance.
Define and discuss electromagnetic radiation (waves) and its properties.
Discuss Planck's quantum theory in simple and general terms.
Discuss Bohr's Theory of the Hydrogen Atom in simple and general terms.
Discuss the dual nature of an electron in simple and general terms.
Define and identify the four quantum numbers for an electron in an atom in simple and general terms.
Discuss the concept of atomic orbitals in simple and general terms.
Determine the electron configuration of atoms and ions.
Understand the Pauli Exclusion Principle, Hund' Rule, Aufbau Principle, diamagnetism, and
paramagnetism as they relate to electron configurations.
Discuss the development of the Periodic Table of Elements in simple and general terms.
Define ionization energy, electron affinity, electronegativity, atomic radius, and ionic radius.
Use trends in the periodic table and electron configurations to qualitatively and relatively predict
ionization energy, electron affinity, electronegativity, atomic radius, and ionic radius.
Differentiate between covalent bonds and ionic bonds.
Discuss the concept of hybridization and identify hybridization of atomic orbitals in chemical compounds.
For the rest of these required syllabus items see the details in the faculty handbook. Delete this note
once the syllabus is complete. For online courses there are some additional requirements given at this
link.
Texts List textbooks with ISBN’s and include this language as well
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All textbook information (pricing, ISBN #, and e-books) for this course can be found on the HPU
Bookstore website: hpu.edu/bookstore.
If you have any questions regarding textbooks, please contact the HPU Bookstore at:
Phone:
808-544-9347
Or e-mail:
jyokota@hpu.edu
mmiyahira@hpu.edu
Assignments and mode of evaluation
Summary of important dates and deadlines (if the schedule is a separate document and due dates are
not given with the description of the assignments).
Class rules and policies (including regarding attendance, late work and academic dishonesty)
Schedule of events (may be attached separately)