Prerequisite(s): (1) MAT 9010 or MAT 9B0 or MAT 900 and CHM 200, or (2) MAT 9010 or MAT 9B0 or MAT 900 and Chemistry Ready Placement Score placing into CHM 1100 or (3) Department Permission OR
Corequisite(s): (4) CHM 100 based on Chemistry Ready Placement Score. Contact Department for Chemistry Ready Placement information.
Required Core: Life and Physical Sciences
Flexible Core: Scientific World (Group E)
Section: CHM 1100-05
Time: Monday & Wednesday 10:20AM – 12:30PM (Lecture); Wednesday 12:40PM – 2:50PM (Lab)
Room: T7204 (Lecture); S324 (Lab)
Instructor: Hun Bok Jung (Office: S-323)
Email: [email protected]
Office Hours: Monday 3:00PM-5:00PM & Wednesday 3:00PM-4:00PM or by appointment
Source materials: The textbook is Chemistry, 6th edition, By Julia Burdge. ISBN10: 126408577X | ISBN13: 9781264085774.
Open textbook: General Chemistry: Principles, Patterns, and Applications by Bruce Averill
- Use the relationships between Avogadro’s number, moles, molar mass and grams to conduct calculations.
- Understand the nature of chemical equations and what information can be obtained from them (reactants/products, physical states, stoichiometric ratios between reactants and products).
- Produce the molecular, ionic and net ionic equations for a reaction.
- Predict the neutralization reaction between an acid and base.
- Identify the various components of an oxidation-reduction reaction including reducing/oxidizing agents and half-reactions.
- Calculate the molarity of a solution.
- Apply concepts of stoichiometry toward reactions in solution and their associated problems including gravimetric analysis and titrations.
- Understand the law of conservation of energy and the first law of thermodynamics.
- Identify a process as endothermic or exothermic
- Calculate the enthalpy of a reaction and understand how it is dependent upon stoichiometric amounts of products and reactants.
- Perform calorimetric calculations involving specific heat or heat capacity.
- Apply Hess’ Law in the determination of the heat of reaction of a multi-step process.
- Describe the major characteristics of the various gas laws: Boyle’s, Charles, Avogadro and combined and use these laws to interconvert measurements of pressure, volume or temperature for a given gas.
- Use the ideal gas equation to determine the pressure, volume, moles or temperature of a gas given all of the other values.
- Apply the ideal gas equation to determine characteristics of a gas including density and molecular weight.
- Use the ideal gas equation in stoichiometric calculations.
- Use Dalton’s law of partial pressures to determine the mole fraction or partial pressure of gases in a mixture of gases.
- List the basic assumptions of the kinetic molecular theory of gases.
- Describe properties of waves including wavelength, frequency and amplitude.
- Understand the basis of quantum theory and its relationship to the frequency of radiation.
- Provide the meaning of each type of quantum number (principal, angular momentum, magnetic and electron spin).
- Use the periodic table to determine the electron configuration of an atom.
- Describe the importance of valence electrons to chemical characteristics.
- Predict differences in effective nuclear charge, atomic radius, ionization energy, and electron affinity between elements using periodic trends.
- Explain why the similarity in chemical properties of groups of elements is due to their electron configurations.
- Define ionic bonding and provide examples of compounds that form ionic bonds.
- Use Coulomb’s law and distance between ions to rank lattice energies of ionic compounds.
- Determine the polarity of a bond using differences in electronegativity.
- Apply rules for writing Lewis structures toward determining the Lewis structure of compounds. Use formal charges to identify the most likely structure of a compound when more than one Lewis structure can be drawn.
- Define resonance and determine the resonance structures of a compound.
- Use the VSEPR model to determine the molecular shape of a molecule.
- Explain why a molecule is polar or nonpolar based upon molecular geometry.
- Use the Lewis structure and number of electron domains of a compound to determine the hybridization of its bonds and provide the number of sigma and pi bonds in a molecule or around a central atom.
- Be able to describe the major relevance of the major bonding theories: Lewis-theory, VSEPR, valence bond theory, hybridization and molecular orbital theory.
- Describe the different types of intermolecular forces: dipole-dipole, hydrogen bonding, dispersion forces and ion-dipole.
- Rank molecules based upon relative strength of intermolecular forces as well as surface tension, viscosity and vapor pressure.
- Use the Clausius-Clapeyron equation to calculate the vapor pressure of a liquid at a given temperature.
- Identify key characteristics and examples of the major types of crystal: ionic, covalent, molecular, or metallic.
- Calculate the amount of heat lost or gained when a substance undergoes a series of phase and/or temperature changes.
- Use phase diagrams to determine the phase that a substance will exist under a given temperature or pressure.
- List and describe the factors that affect the solubility of a solute.
- Use concentration units to determine the concentration of a given solution or to interchange concentration units.
- List, describe and perform calculations involving colligative properties: vapor pressure lowering, boiling point elevation, freezing point depression and osmotic pressure.
Exam 1: 10%, Exam 2: 10%, Final Exam: 15%, Weekly Quizzes: 10% Weekly Exercises: 20%, Laboratory Performance: 25%, CURE Project: 10%
Grades will be awarded as follows: 97-100%=A+; 93-96%=A; 90-92%=A-; 87-89%=B+; 83-86%=B; 80-82%=B-; 77-79%=C+; 73-76%=C; 70-72%=C-; 67-69%=D+; 60-66%=D; <60%=F
If you miss an opportunity to demonstrate your knowledge of the subject matter by missing a duly scheduled exam, laboratory or other assignment, the grading scheme does not apply. Your grade will be determined at the discretion of the instructor. By missing a duly scheduled exam, laboratory or other assignment, you accept and recognize that the instructor must determine your grade within the context of determining the grade of students who did not miss a duly scheduled exam, laboratory or other assignment. Instructor Make-up Policy: SUGGESTED: NO MAKE-UP EXAMS, NO MAKE-UP LABORATORIES OR NO MAKE-UP OTHER ASSIGNMENTS. FINAL EXAM WEIGHTED WITH PENALTY (0-100%) FOR MISSED WORK.
Attending all classes is mandatory. The textbook is a guide for the course. Additional material will be covered during lecture meetings. If you miss class, you will miss out on taking notes and this will affect your ability to study for tests and quizzes. Except in extreme cases there can be no makeup exams and missing one is grounds for failure of the course. At all times, if you have any questions or need help, please ask your instructor. If you are having difficulties with the course, or if your life is affecting your performance in class, or your ability to attend, let the instructor know as soon as problems arise.
You may not enter the laboratory without Lab coat/Safety glasses or goggles/Lab gloves.
The laboratory component counts for 25% of your overall result in CHM1100. Failure to pass the laboratory component of the course will result in a grade of F in the course. It is important to note that the laboratory component of the course serves a dual purpose. It offers the opportunity for students to deepen their understanding of a specific experimental science. The laboratory also offers the instructor an opportunity to assess each student’s competence in the subject area.
The laboratory grade is based on the quality of your work in the laboratory and the quality of your laboratory assignments. Laboratory instructors may assess your competence in the subject through the use of pre-lab assignments, reports, quizzes or practical examinations. All laboratory meetings are mandatory. Performing an experiment at an alternate time will be considered only under exceptional cases. If you miss more than one laboratory meeting you may fail the laboratory portion of the course and, hence, the entire course. All laboratory assignments must be completed and handed in within the time limits set by your laboratory instructor.
Laboratory meetings are subject to the regulations of the New York City Fire Department and the laws of the State of New York. If your instructor is concerned that you are unprepared or unable to safely complete a given experiment you may be asked to leave the laboratory and will not receive credit for the meeting. Examples of reasons for an instructor’s duty of action include a student arriving late to the meeting, failure to bring approved safety glasses/goggles, improper attire, failure to study the laboratory experimental protocol, or a general lack of laboratory competence.
