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Syllabus

Chemistry II
CH106

YEAR:

2023-2024

CREDIT HOURS:

5.00

PREREQUISITES:

CH105 Chemistry I with a C or Higher.

COREQUISITES:

None

COURSE NOTES:

Students must also enroll in CH106L Lab.

CATALOG COURSE DESCRIPTION:

Continuation of CH105 Chemistry I focusing on solutions and colloids, thermodynamics, kinetics, ionic equilibria and electrochemistry with laboratory experiences including quantitative experiments from the above areas plus visible spectroscopy and brief qualitative analyses. 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. Describe the effects of intermolecular forces in chemical systems and perform calculations involving solution concentrations and colligative properties.
    1. Explain how London forces arise and how they vary with the number of electrons in an atom or molecule.
    2. Describe dipole-dipole interactions and hydrogen bonds and explain why hydrogen bonds are the strongest type of intermolecular forces.
    3. Explain why viscosity and surface tension vary with temperature and depend on the strengths of the intermolecular forces.
    4. Interpret the major features of a phase diagram.
    5. Identify molecules that can take part in hydrogen bonding.
    6. Explain the basis for the like-dissolves-like rule.
    7. Predict the relative solubility of solutes in a given solvent.
    8. Explain how solutions result from the tendency of energy and matter to disperse.
    9. Calculate the solubility of a gas at a given pressure, given its Henry's law constant.
    10. Explain how a nonvolatile solute lowers the vapor pressure, raises the boiling point, and lowers the freezing point of a solvent.
    11. Interpret a measured value of the van't Hoff i factor.
    12. Calculate the molarity, molality, mole fraction, and mass percent of a given compound and convert between them.
    13. Calculate the vapor pressure of a solvent in a solution by using Raoult's law.
    14. Find the molar mass of a substance using colligative properties.
    15. Describe the formation of a solution at the molecular level.
    16. Describe the process of osmosis and reverse osmosis.
    17. Predict the relative vapor pressures of two substances.
    18. Predict the boiling temperature of a substance.
    19. Use a phase diagram to identify the stable phase of a substance at given temperature and pressure and predict phase transitions.
    20. List properties of water that is anomalous as a result of hydrogen bonding.
    21. Distinguish metals, ionic solids, network solids, and molecular solids by their structures and by their properties.
  2. Apply the concepts of chemical kinetics to evaluate rates and to describe the energetics and mechanisms of chemical reactions.
    1. Show how the instantaneous rate is obtained by drawing a tangent to the graph of concentration against time.
    2. Explain how collision theory and activated complex theory account for the temperature dependence of reactions.
    3. Interpret a reaction profile.
    4. Show how the rate of change of one species in a reaction is related to that of another species.
    5. Determine the order of a reaction, its rate law, and its rate constant from experimental data.
    6. Calculate a concentration or rate constant by using an integrated rate law.
    7. For a first-order process, calculate the half-life, given the rate constant, and vice versa.
    8. Use the Arrhenius equation and the activation energy to find the rate constant at given temperature.
    9. Determine the molecularity of an elementary reaction and write its rate law.
    10. Deduce a rate law from a mechanism.
    11. Explain the action of enzymes and catalysts.
    12. Describe the various steps in a mechanism and explain how each affects the progress of the reaction.
  3. Apply and demonstrate an understanding of equilibrium concepts to predict qualitative and quantitative properties of a chemical system.
    1. Interpret chemical equilibrium as a dynamic process involving change at the molecular level.
    2. Show how the equilibrium constant is related to the forward and reverse rate constants of the elementary reactions contributing to an overall reaction.
    3. Explain how the value of the reaction quotient, Q, allows the direction of the reaction to be predicted.
    4. Explain the basis of Le Chatelier's principle.
    5. Write the equilibrium constant for a chemical reaction, given its balanced equation.
    6. Calculate the effect on K of reversing a reaction or multiplying the chemical equation by a factor.
    7. Determine the equilibrium constant given equilibrium concentrations.
    8. Determine an equilibrium concentration or partial pressure, given K and all other equilibrium concentrations.
    9. Determine the direction of a reaction, given K and the concentrations of all reactants and products.
    10. Use an equilibrium table to calculate K and equilibrium composition.
    11. Use Le Chatelier's principle to predict how the equilibrium composition of a reaction mixture is affected by adding or removing reagents.
  4. Define acids and bases and evaluate strengths using chemical equilibrium concepts.
    1. Distinguish Arrhenius, Bronsted, and Lewis acids and bases.
    2. Explain how the pH of a solution is related to its hydronium ion and hydroxide ion concentrations.
    3. Explain why solutions of weak acids have higher pH values than solutions of strong acids at the same concentrations.
    4. Show how the acidity constant of an acid is related to the basicity constant of its conjugate base.
    5. Use Ka values to predict the relative strengths of two acids or two bases.
    6. Write the formulas for conjugate acids and bases.
    7. Identify the common strong acids and bases.
    8. Explain why salts of weak bases produce acidic solutions and salts of weak acids produce basic solutions.
  5. Perform calculations involving pH, titrations, and buffers to describe acid/base and solubility equilibria.
    1. Calculate the molar concentrations of hydronium and hydroxide ions in a solution of strong acid or base.
    2. Calculate the pH and pOH of a solution of a strong acid or base.
    3. Calculate the molar concentrations of hydronium and hydroxide ions from the pH or pOH of a solution of a strong acid or base.
    4. Calculate the pH of a weak acid or base.
    5. Calculate the pH of a solution of a polyprotic acid.
    6. Interpret the features of the pH curve for the titration of a strong or weak acid with a strong base, or a strong or weak base with a strong acid.
    7. Explain how buffer solutions resist changes in pH.
    8. Select an appropriate buffer for a given pH.
    9. Explain what is meant by the buffer capacity of a solution.
    10. Calculate the pH of a salt solution.
    11. Calculate the pH at any point in a strong base-strong acid, strong base-weak acid, or weak base-strong acid titration.
    12. Calculate the pH of a buffer solution.
    13. Calculate the pH change when acid or base is added to a buffer solution.
    14. Determine the relative concentrations of conjugate acid and base needed to prepare a buffer solution with a given pH.
    15. Determine solubility constant from molar solubility and vice versa.
    16. Estimate the effect of a common ion on solubility.
    17. Calculate molar solubility in the presence of complex ion formation.
  6. Evaluate data and perform calculations involving thermodynamic quantities for a process, demonstrate the relationship between these quantities, and use the relationship to predict the spontaneity of chemical reactions.
    1. State and explain the implications of the second law of thermodynamics.
    2. Explain how temperature, volume, and state of matter affect the entropy of a substance.
    3. Show how entropy of surroundings is related to enthalpy for a change at constant temperature and pressure and justify the relationship.
    4. Show how the free energy change accompanying a process is related to the direction of spontaneous reaction and the position of equilibrium.
    5. Predict which of two systems has the greater entropy, given their compositions and conditions.
    6. Calculate the change in entropy of a system due to heat transfer and phase changes.
    7. Estimate the relative molar entropies of two substances.
    8. Calculate the standard reaction entropy from standard molar entropies.
    9. Judge the spontaneity of a reaction from its standard reaction enthalpy and standard reaction entropy.
    10. Predict the boiling point and melting point of a substance from the changes in entropy and enthalpy of the substance.
    11. Calculate a standard free energy of formation from the standard enthalpy of formation and standard molar entropies.
    12. Calculate the standard reaction free energy from free energies of formation.
    13. Calculate the reaction free energy from change in free energy for the reaction at standard state and the reaction quotient.
    14. Calculate an equilibrium constant from change in free energy for the reaction at standard state at a given temperature.
    15. Predict the temperature at which a process with known enthalpy and entropy becomes spontaneous.
    16. Describe the criteria for spontaneity of a reaction.
    17. Identify thermodynamically unstable compounds from their standard free energies of formation.
  7. Describe an electrochemical cell and utilize reduction potentials to predict the outcome of a given redox reaction.
    1. Distinguish galvanic and electrolytic cells and describe their operation; identify anode, cathode, and the direction of current flow for each.
    2. Explain the relationship between the standard free energy, standard cell potential and equilibrium constant of a reaction.
    3. Predict the effect of changes in concentration of reactants and products on the cell potential.
    4. Balance chemical equations for redox reactions by the half-reaction method.
    5. Write the chemical equation, cell diagram, and description of the galvanic cell in which two given half-reactions take place.
    6. Deduce the standard potential of an electrode.
    7. Predict relative oxidizing strength by using the electrochemical series.
    8. Calculate a standard cell potential, given the standard electrode potentials, and predict the spontaneous direction of the cell reaction.
    9. Assess the reaction free energy from a cell potential.
    10. Calculate the equilibrium constant for a reaction from electrochemical data.
    11. Use the Nernst equation to calculate a cell potential under nonstandard conditions.
    12. Predict the standard potential of a fuel cell.
    13. Predict the products of electrolysis of an aqueous solution from the electrochemical series.
  8. Execute laboratory skills in accordance with proper laboratory and chemical safety practices.
    1. Demonstrate ability to appropriately measure chemical amounts.
    2. Demonstrate understanding of safe chemical disposal and use of laboratory safety equipment.
  9. 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.
    2. Assess the order of precipitation of a series of salts
    3. Show how ions can be separated and detected by a qualitative analysis scheme.

HutchCC course outcomes are equivalent to the Kansas core outcomes.

KRSN:

CHM1020

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:

1. Homework assignments 2. Quizzes 3. Examinations 4.Special assignments 5. Laboratory reports 6. Final examination

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: 01/10/2019