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Syllabus

Honors Chemistry I
CH105H

YEAR:

2023-2024

CREDIT HOURS:

5.00

PREREQUISITES:

ACT Math Score of 21 or higher, or MA105 or higher math, or Accuplacer NextGen QuantReason, Alg,Stats Score 263 or Above, or Accuplacer Math Score of 81+.

COREQUISITES:

None

COURSE NOTES:

Prior completion of or concurrent enrollment in MA106(or higher math course) or department consent. Previous background in chemistry or physical science recommended. Must also enroll in CH105L Lab.

CATALOG COURSE DESCRIPTION:

Atomic theory, chemical bonding, chemical reactions, energy, gasses, solids, liquids, and solutions. Laboratory experiments include analysis, synthesis and acquisition of quantitative data. Lecture and lab.

HutchCC INSTITUTION-WIDE OUTCOMES:

  1. Demonstrate the ability to think critically and make reasonable judgments by acquiring, analyzing, combining, and evaluating information.
  2. Demonstrate the skills necessary to access and manipulate information through various technological and traditional methods.
  3. Demonstrate effective communication through reading, writing, listening, and speaking.
  4. Demonstrate effective interpersonal and collaborative skills.
  5. Demonstrate effective quantitative-reasoning and computational skills.

COURSE OUTCOMES AND COMPETENCIES:

  1. Apply dimensional analysis and mathematical techniques to solve chemical problems, including significant figures throughout calculations in all content learning outcomes.
    1. Explain the significance of units for reporting measurements.
    2. Interpret prefixes as they relate to the metric system.
    3. Distinguish between accuracy and precision.
    4. Calculate the density of a substance from the mass and volume of a sample.
    5. Convert a measurement from one unit to another using dimensional analysis.
    6. Use the correct number of significant figures when reporting measurements and the results of calculations.
    7. Convert between Kelvin, Celsius, and Fahrenheit temperatures.
  2. Identify and differentiate between atoms, pure elements, compounds, and ions, and correlate chemical formulas with chemical names.
    1. Identify and define each of the major steps in the scientific method.
    2. Classify the three states of matter.
    3. Distinguish heterogeneous mixtures, solutions, compounds, and elements.
    4. Identify physical and chemical changes.
    5. Describe how mixtures are separated by filtration, distillation, and chromatography.
    6. Describe the nature of the fundamental chemical laws and their historical development.
    7. Describe the historical and modern views of the nuclear atom.
    8. Distinguish between molecules and ions.
    9. Distinguish by their properties metals, metalloids, and nonmetals and locate them in the periodic table.
    10. Write the symbols for the elements, given their names, and vice versa.
    11. State the numbers of neutrons, protons, and electrons in an isotope, given its atomic number and mass number, and write the symbol for an isotope.
    12. Predict the anion or cation that a main-group element is likely to form.
    13. Interpret chemical formulas in terms of the number of each type of atoms present.
    14. Name ions.
    15. Name and write the formula for binary ionic and molecular compounds, compounds with common polyatomic ions, and hydrates.
    16. Describe the function and operation of a mass spectrometer.
  3. Construct balanced chemical equations given a set of reactants and/or products, use a balanced chemical equation to solve stoichiometry problems, and analyze chemical reactions with regards to stoichiometry and thermochemistry.
    1. Explain the significance of the stoichiometric coefficients in a chemical equation.
    2. Use the Avogadro constant to convert between number of moles and the number of atoms, molecules, or ions in a sample.
    3. Calculate the average molar mass of an element, given its isotopic composition.
    4. Determine the molar mass of a compound.
    5. Convert between mass and number of moles by using the molar mass.
    6. Calculate the mass percentage of an element in a compound from the formula.
    7. Determine the mass percentage composition of a compound from mass measurement.
    8. Calculate the empirical formula of a compound from its mass percentage composition.
    9. Determine the molecular formula of a compound from its empirical formula and its molar mass.
    10. Identify the state of matter from chemical formula.
    11. Carry out mole-to-mole calculations for any two species involved in a chemical reaction.
    12. Carry out mass-to-mole and mass-to-mass calculations for any two species involved in a chemical reaction.
    13. Calculate the theoretical and percentage yields of the products of a reaction, given the mass of starting material.
    14. Identify the limiting reactant of a reaction and calculate the amount of excess reactant present.
    15. Give the definition of a mole in your own words.
    16. Explain the significance of a balanced chemical equation.
    17. Write, balance, and label a chemical equation when given the information in a sentence.
    18. Explain how diluting a solution affects the concentration of the solute.
    19. Calculate the molarity of a solute in a solution, volume of solution, and mass of solute, given the other two.
    20. Prepare a solution of given molarity.
    21. Determine the volume of solution needed to prepare a dilute solution of a given molarity.
    22. Calculate the molar concentration (molarity) of a solute from titration data.
    23. Calculate the mass of a substance that reacts with a known volume of titrant solution.
  4. Identify predominant species present in an aqueous solution and identify the reactants and/or products of common aqueous reactions: acid/base, redox, precipitation, etc.
    1. Identify substances as electrolytes or nonelectrolytes.
    2. Explain the difference between solutions of strong and weak acids and bases.
    3. Define oxidation and reduction in terms of oxidation number and electron transfer.
    4. Identify the oxidizing and reducing agents in a reaction.
    5. Identify a reaction as precipitation, neutralization, or redox.
    6. Construct the balanced complete ionic and net ionic equations for reactions involving ions.
    7. Use the solubility rules to select appropriate solutions that, when mixed, will produce a desired precipitate.
    8. Predict the outcome of a neutralization reaction and write the net ionic equation.
    9. Recognize common Arrhenius acids and bases from their formulas.
    10. Identify an oxide as acidic or basic from the position of the element in the periodic table.
    11. Determine the oxidation number of an element in an ion or compound.
    12. Predict the products of a reaction based on general reaction types.
    13. Describe a procedure that can be used to perform a gravimetric analysis.
    14. Describe the purpose and procedure of a titration.
    15. Explain the significance of the stoichiometric point of a titration.
  5. Apply the Kinetic Molecular Theory to describe an ideal gas and use the Ideal Gas Law to calculate a state variable for a given set of conditions.
    1. Explain the origin of pressure in molecular terms.
    2. List and explain the assumptions of the kinetic theory of gases and show how they can be used to interpret the ideal gas law.
    3. Describe the effect of molar mass and temperature on the distribution of molecular speeds.
    4. Explain how real gases differ from ideal gases.
    5. Convert between pressure units.
    6. Use Boyle's law to calculate the change in pressure due to compression.
    7. Use Charles's and Gay-Lussac's laws to calculate the change in volume or pressure due to a temperature change.
    8. Use Avogadro's principle to predict the change in volume due to a change in the number of moles of gas.
    9. Use the ideal gas law to calculate P, V, T, and n for given conditions or after a change in conditions.
    10. Calculate the volume of a gas from its mass.
    11. Calculate the volume of a gas produced or consumed in a reaction.
    12. Determine molar mass from gas density and vice versa.
    13. Describe the construction and use of a barometer.
    14. Describe the structure of the atmosphere.
  6. Describe the relationships between heat, work, internal energy, and energy changes for chemical reactions and perform calculations involving these concepts.
    1. Distinguish the three types of thermodynamic systems.
    2. Distinguish between heat and work.
    3. State, and explain the implications of the first law of thermodynamics.
    4. Distinguish between ∆E and ΔH and show how they are related.
    5. Distinguish between exothermic and endothermic reactions by the direction of heat flow and by the sign of ΔH.
    6. Outline the various parts of a heating curve and explain its features.
    7. Explain how Hess's law depends on the fact that enthalpy is a state property.
    8. Calculate the change in internal energy due to heat and work.
    9. Calculate the work of expansion.
    10. Use specific heat capacity to determine the energy transferred as heat.
    11. Calculate enthalpy changes from calorimetry data.
    12. Determine the heat output of a reaction, given the temperature change of a calibrated calorimeter.
    13. Calculate an overall reaction enthalpy from the enthalpies of the reaction in a sequence.
    14. Calculate the heat output of a fuel from its standard enthalpy of combustion.
    15. Use standard enthalpies of formation to calculate the standard enthalpy of reaction.
    16. Describe the function of calorimeters and how they are calibrated.
    17. Define the standard state of a substance and recognize when a substance is in its standard state.
    18. Define and use the specific enthalpy and the enthalpy density of fuels.
  7. Relate the periodic properties of the elements to their electronic structure using the quantum mechanical model.
    1. Describe the nature of light as electromagnetic radiation and as a stream of photons.
    2. Explain the significance of the photoelectric effect.
    3. Use the Bohr frequency condition to explain the origin of the lines in the spectrum of an element.
    4. Describe the interpretation of atomic orbitals in terms of probabilities.
    5. Distinguish and sketch the boundary surfaces of s-, p-, and d- orbitals.
    6. Name and explain the relation of each of the four quantum numbers to the properties of electrons in orbitals.
    7. List the allowed energy levels of a bound electron in terms of the quantum number, n, l, and m.
    8. Describe the factors affecting the energy of an electron in a many-electron atom.
    9. Calculate the wavelength, frequency, and energy of light.
    10. Use the expression for the energy levels of a hydrogen atom to correlate the lines in a spectrum with specific energy transitions.
    11. State how many orbitals of each type are contained in the shell corresponding to a given principal quantum number and how many electrons can be accommodated in those orbitals.
    12. Write the ground-state electron configuration for an atom.
    13. Write the group-state electron configuration for an ion.
    14. Use the periodic table to predict and explain trends in physical and chemical properties.
    15. Describe the general characteristics of elements in the s, p, and d blocks.
    16. Describe and explain the significance of diagonal relationships in the periodic table.
  8. Apply VSEPR and Valence Bond Theory to predict the three-dimensional structure of molecules and relate macroscopic physical and chemical properties of matter to its atomic scale chemical bonding, intermolecular forces, and three-dimensional structure.
    1. Distinguish between ionic and covalent bonds.
    2. Define resonance hybrid and explain its relation to the individual Lewis structures that contribute.
    3. Explain the characteristics of Lewis acids and bases and how they form bonds.
    4. Explain the significance of electronegativity and what is meant by the ionic or covalent character of a bond.
    5. Predict and explain periodic trends in the polarizability of anions and the polarizing power of cations.
    6. Explain why pairs of electrons are more likely to be found in certain locations around a central atom and how and why they affect the bond angles in a molecule.
    7. Define the electric dipole moment of a bond and explain how it depends on the electronegativities of the two atoms in a bond.
    8. Explain how bond enthalpy is related to bond multiplicity, atomic radius, and the presence of unpaired electrons.
    9. List the factors affecting bond length and explain the effect of each.
    10. Use a table of electronegativities to predict which of two bonds has greater ionic or covalent character.
    11. Use average bond enthalpies to estimate a reaction enthalpy.
    12. Predict the chemical formula of a binary ionic compound and write its formula and Lewis structure.
    13. Write the Lewis structure of a molecule of ion.
    14. Write the resonance structure for a molecule.
    15. Write the Lewis structure of a molecule or ion with an expanded valance shell.
    16. Use formal charges to evaluate alternative Lewis structures.
    17. Predict the shape of a molecule or polyatomic ion from its formula, giving each bond angle approximately.
    18. Predict the polarity of a molecule.
    19. Describe some of the properties of ionic compounds.
    20. Predict which atoms are likely to form molecules in which they have an expanded valence shell.
    21. Distinguish sigma and pi bonds by their shapes, properties, and component orbitals.
    22. Explain why hybridization arises from atomic orbitals and how it is used to describe molecular shape.
    23. Explain how molecular orbitals are constructed for diatomic molecules.
    24. Describe hybridization, including sp3, sp2 and sp hybridization.
    25. Predict hybridization from VSEPR structures.
    26. Determine bond orders and relate them to relative bond strength.
    27. Describe the MO theory description of bonding and antibonding orbitals.
    28. Relate MO theory to concepts such as the structural, energetic, spectroscopic, and magnetic properties of molecules.
    29. Account for the structure of a molecule in terms of hybrid orbitals and sigma and pi bonds.
  9. Execute laboratory skills in accordance with proper laboratory and chemical safety practices.
    1. Demonstrate ability to weigh and measure volumes with various types of glassware.
    2. Demonstrate understanding of safe chemical disposal and use of laboratory safety equipment.
  10. Collect, evaluate, and interpret qualitative and quantitative data from laboratory procedures in a productive and meaningful manner.
    1. Demonstrate knowledge of lecture material by completing labs and evaluating accuracy and precision of data collected through error analysis.

HutchCC course outcomes are equivalent to the Kansas core outcomes.

KRSN:

CHM1010

The learning outcomes and competencies detailed in this course outline or syllabus meet or exceed the learning outcomes and competencies specified by the Kansas Core Outcomes Groups project for this course as approved by the Kansas Board of Regents.

COURSE ASSESSMENT AND EVALUATION:

Competencies will be assessed through homework assignments, quizzes, hour exams, special assignments, laboratory reports, and a comprehensive final exam which must be taken in order to pass the class. Students may not receive credit toward graduation for both CH101 General Chemistry and this course.

ACCOMMODATIONS STATEMENT:

Any student who has a documented disability and wishes to access academic accommodations (per the 1973 Rehabilitation Act and Americans with Disability Act) must contact the HCC Coordinator of Disability Services, at 620-665-3554, or the Student Success Center, Parker Student Union. The student must have appropriate documentation on file before accommodations can be provided.

ACADEMIC HONESTY:

Education requires integrity and respect for HutchCC's institutional values. HutchCC students are required to maintain honesty through a "responsible acquisition, discovery, and application of knowledge" in all academic pursuits. Preserving and upholding academic honesty is the responsibility of Hut chCC students, faculty, administrators and staff.

I. Student Responsibilities

All HutchCC students are required to:

  • Submit all work in all courses without cheating, fabrication, plagiarism, dissimulation, forgery, sabotage, or academic dishonesty as defined below.
  • Provide all academic records such as transcripts and test scores that are free of forgery.
  • Refrain from participating in the academic dishonesty of any person.
  • Use only authorized notes and student aids.
  • Use technology appropriately, including refraining from submitting AI (Artificial Intelligence)-generated work without express written consent from your instructor.
  • Protect the security of passwords/login/privacy/electronic files, and maintain sole individual access for any online course information.

II. Definition of Academic Dishonesty

  • Academic dishonesty is any intentional act, or attempted act, of cheating, fabrication, plagiarism, dissimulation, forgery, or sabotage in academic work.
  • Cheating includes using unauthorized materials of any kind, whether hard copies, online, or electronic, such as unapproved study aids in any academic work, copying another student's work, using an unauthorized "cheat sheet" or device, or purchasing or acquiring an essay online or from another student.
  • Fabrica tion is the invention or falsification of any information or citation in any academic work, such as making up a source, providing an incorrect citation, or misquoting a source.
  • Plagiarism is the representation of words, ideas and other works that are not the student's own as being original to the student. A no n-inclusive list of examples includes work completed by someone else, work generated by an external entity (such as AI), omitting a citation for work used from another source, or borrowing the sequence of ideas, arrangement of material, and/or pattern of thought of work not produced by the student, even though it may be expressed in the student's own words.
  • Dissimulation is the obscuring of a student's own actions with the intention of deceiving others in any academic work, such as fabricating excuses for absences or missed assignments, or feigning attendance.
  • Forgery of academic documents is the unauthorized altering, falsification, misrepresentation, or construction of any academic document, such as changing transcripts, changing grades on papers or on exams which have been returned, forging signatures, manipulating a digital file of academic work, or plagiarizing a translation.
  • Sabotage is any obstruction or attempted obstruction of the academic work of another student, such as impersonating another student, stealing or ruining another student's academic work.
  • Aiding and abetting academic dishonesty is considered as knowingly facilitating any act defined above.
  • Academic honesty violations can also include the omission or falsification of any information on an application for any HutchCC academic program.

III. Sanctions for Academic Dishonesty

Students who violate the Academic Honesty Policy may be subject to academic or administrative consequences.

Instructor Sanctions for Violation:

Students suspected of violating the Academic Honesty Policy may be charged in writing by their instructor and any of the following may apply:

  • Assign Avoiding Plagiarism Bridge Module
  • Receiving written warning that could lead to more severe sanction if a second offense occurs
  • Revising the assignment/work in question for partial credit
  • Voiding work in question without opportunity for make-up
  • Reducing the grade for work in question
  • Lowering the final course grade
  • Failing the work in question

Institutional Sanctions for Violation:

Students charged with academic dishonesty, particularly in instances of repeated violations, may further be subjected to an investigation and any of the following may apply:

  • Instructor recommendation to the Vice President of Academic Affairs (VPAA) to dismiss the student from the course in which the dishonesty occurs
  • Instructor recommendation to the VPAA to dismiss student from the course in which the dishonesty occurs with a grade of 'F." Student will not be allowed to take a 'W' for the course
  • Instructor recommendation to the VPAA that the student be suspended and/or dismissed from the program
  • Student barred from course/program for a set period of time or permanently
  • May be recommended by the instructor (after documented repeated offenses) to the VP AA that the student be placed on probation, suspended and/or dismissed from the institution.

IV. Procedure

  • Instructor will communicate in writing via the student's HutchCC email account and/or LearningZone email account to the student suspected of violating the Academic Honesty Policy.  That communication may include sanction(s). Department Chair will notify the student's academic advisor upon receipt of the Academic Honesty Violation Form.
  • For each violation, the instructor will submit a completed Academic Honesty Violation Form to the Department Chair. Department Chair will notify the student's academic advisor upon receipt of the Academic Honesty Violation form.
  • Should the instructor choose to pursue institutional sanctions, the instruct or shall notify the student in writing via the student's HutchCC email account.  Instructor shall also submit a completed Academic Honesty Violation Form and all prior completed forms regarding said student to the Department Chair and the office of the VPAA with recommendation to proceed with specific Institutional Sanctions. Department Chair will notify the student's academic advisor upon receipt of the Academic Honesty Violation Form.
  • The decision of the VPAA on Institutional Sanction is final. The VPAA will notify the student's academic advisor of any institutional sanctions.

V. Due Process Rights

Students charged with violations of academic honesty have the right of appeal and are assured of due process through the Academic Honesty Appeal process.

Academic Honesty Appeal Process

I. Due Process Rights: Students charged with violations of academic honesty have the right of appeal and are assured of due process through the Academic Honesty Appeal process.

  • If an instructor has recommended course or program dismissal, the student may continue in coursework (provi ding there are no threatening or security behavioral issues) until appeal processes are concluded. However, if an issue has been documented at a partnership location (e.g., clinical sites, secondary institutions, correctional or military facilities), then the student is no longer eligible to continue participation in internships, apprenticeships, and/or clinical-based practice. For clinical sites, this sanction is immediate.

II. Process

If the student disagrees with the charge of a violation of academic honesty, the student has the right to due process as described in the Academic Honesty Appeal process below:

  • If the matter is not resolved upon communicating with the instructor about the violation, the student shall, within five business days of the issuance of the written notice of violation, submit a completed Academic Honesty Appeal Form and supporting documentation to the appropriate department chairperson to initiate an Academic Honesty Appeal.
  • Within two business days of receiving the student's completed Academic Honesty Appeal Form, the Department Chair and VPAA will review and the VPAA will render a decision.
  • Within two business days, a response will be sent to the student's HutchCC email address. The VPAA's decision is final.

INCOMPLETE GRADE:

Instructors may give a student a grade of Incomplete (I) under the following conditions:

  1. The student must initiate the request prior to the time final course grades are submitted to Records.
  2. The request must be made because of an emergency, illness or otherwise unavoidable life-event.
  3. The instructor must agree to the request before a grade of Incomplete can be submitted.
  4. A written contract between the instructor and student, signed by both, will document the work required and date needed to complete course work.
  5. If a student does not complete the course requirements within the time frame established by the instructor, a grade of "F" will be recorded on the student's transcript at the end of the next semester.

HLC ACCREDITATION:

Hutchinson Community College is accredited by the Higher Learning Commission (HLC). The Higher Learning Commission is one of six regional institutional accreditors recognized by the US Department of Education and the Council on Higher Education Accreditation (CHEA).

Last Revised: 06/06/2019