Chem 10301, General Chemistry 1



Chem 10301, General Chemistry 1

Fall 2009

Sections T, T2, T3

Lecture:

Tu, Th 6:30-7:45 pm, Room MR-2

Lab (MR-1001):

T: Th 8:00-9:50 pm

T2: Tu 8:00-9:50 pm

T3: Th 4:30-6:20 pm

Workshop (MR-1029):

T: Tu 8:00-9:50 pm

T2: Th 8:00-9:50 pm

T3: Tu 4:00-5:50 pm

Instructor: Dr. Themis Lazaridis

email: tlazaridis@ccny.cuny.edu, tel: 650-8364

Office: MR-1338

Office hours:

Before class (5:45-6:30 pm) for sections T, T2

After class (7:45-8:30) for section T3

Course web site:

Course Description

This course is the first of a two-semester sequence and provides an in-depth introduction to the fundamental laws and techniques of chemistry for majors in science and engineering. Topics include: measurement; stoichiometry; the gaseous state; thermochemistry; atomic structure; chemical bonding; redox reactions; solids, liquids and intermolecular forces. It consists of three components (lecture, laboratory, and workshop), which are integrated to provide a comprehensive but thorough introduction to the principles of chemistry. The laboratory component introduces students to common laboratory methods including visible spectroscopy and titration. The workshop is a peer-led, small group discussion of concepts and problem solving in general chemistry.

Prerequsites: Math 19000

Pre- or Corequisites: Math 19500, 20100, 20500

Textbook

Hill, Petrucci, McCreary,Perry, “General Chemistry”, 4th Edition, Pearson, 2005. Chem 10301 covers the first 10 chapters. Chem 10401 covers the rest.

Bookstore has Part 1 bundled with Solutions Manual (Hassell) and Workshop Manual (Gosser et al., 2nd ed.)

Textbook companion website:

Learning outcomes

After completing this course, students should be able to:

1. Perform unit conversions and express values with the correct number of significant figures.

2. Express and interpret atomic symbols, atomic number, mass number, and molar mass.

3. Understand and apply concepts of balancing chemical reactions,

and be able to perform stoichiometric calculations.

4. Define enthalpy and solve thermochemical equations.

5. Express quantum energy levels of atoms and relate these to atomic properties.

6. Draw and interpret Lewis-dot structures, predict three dimensional structure of simple molecules, and draw simple molecular orbital diagrams.

7. Apply the ideal gas law to problems involving changes in moles, pressure, volume and temperature.

8. Solve problems involving solution chemistry such as titrations, precipitation, and colligative properties.

9. Write a laboratory report including data and analysis.

10. Be able to conduct a variety of experiments (titrations, spectroscopic) including accurate recording of results and preparation of calibration curves.

11. Be aware and follow the safety requirements in a chemical laboratory.

12. Analyze molecular modeling and graphic plots using computers.

13. Communicate concepts and problem solving of chemistry that have been presented in lecture.

14. Work as part of a problem solving team to solve chemistry problems.

15. Apply chemical principles to selected applications in life science or technology.

Exams and grading

There will be three midterm exams during the semester and a comprehensive final examination. The lowest grade of the three midterms will be dropped.

40% Midterms: I (Chapters 1-3), II (Chapters 4-6), III (Chapters 7-9)

35% Final Exam (Chapters 1-10 cumulative)

15% Laboratory

10% Workshop

The conversion from points to letter grades is done as follows:

96-100 : A+ 77-79: C+

90-95 : A 72-76: C

88-89 : A- 70-71: C-

86-87: B+ 60-69: D

82-85: B 0-59: F

80-81: B-

No makeups are offered for the midterm exams. A makeup for the final exam is offered only under compelling circumstances.

Tips

Learning Chemistry is cumulative – if you miss a class you will miss a significant building block, which will affect your exam performance, scores, and final grade as well as your ability to understand material in future courses. So, attendance for all lectures, labs, and workshops while required is critical to your success. Further, your own practice by doing homework and becoming engaged with the material as well as engaged with your classmates in workshop and lab discussions of chemical concepts will help you build your knowledge to succeed. Learning these skills will prepare you for your chosen major and professional career. You will need a simple scientific calculator for this course.

Plan at least three hours of study (reading the chapter and completing the problem sets -“homework”) time for every hour you spend in class. Do the problem sets individually (without help from friends or classmates) initially. Please look at a related problem in the solution manual to help you solve the assigned problem. If you are still unable to solve the problem, then ask a friend, classmate, workshop leader, TA, or Professor for help.

Attend workshop: finish the Self-Test, finish the workshop problems, and ask questions.

Seek help when you have difficulty (office hours, tutoring, study groups with workshop).

Free tutorial service

Available in the Chemistry Learning Center (MR-1029). Schedule is posted near door.

Key learning objectives and homework for each chapter

The homework is due at workshop following the last lecture of each chapter. Students must hand in homework to workshop leader, who will grade it as (10) complete, (5) incomplete, or (0) no assignment.

* Chapter 1. What you should know from this chapter: Be able to get derived units from basic units, be able to convert between units, be able to tell the number of significant figures, be able to give the result of your calculations in the correct number of significant figures. Homework: 24, 26, 28, 36, 38b, 50, 52, 54, 60, 64, 81.

* Chapter 2. What you should know: The symbols of the elements in the first four periods of the periodic table (and a few important others), be able to read the atomic number from the periodic table, understand the meaning of "molecule","ion","compound", be able to name common compounds from the molecular formula, be able to write down the molecular formula given the name, memorize Fig. 2.10 and Table 2.4, be able to calculate the chemical atomic weight of an element from the natural abundance of isotopes, be able to calculate the molar mass of a compound. Homework: 22, 26, 32, 40, 50, 52, 58, 64, 68

* Chapter 3: you should be able to: distinguish physical from chemical changes and properties, balance equations, calculate percentage composition from combustion analysis and from a molecular formula, obtain empirical formulas from percent composition, be able to distinguish types of chemical reactions, be able to determine limiting and excess reactants and do stoichiometric calculations, be able to calculate theoretical and percent yield. Don't read 3.11 (solution stoichiometry) now. We'll do together with chapter 4. Homework: 18a,f, 22a, 24c, 34, 36, 54a-e, 58a, 64, 74

* Chapter 4 (and Section 3.11). You should be able to: distinguish solutions from heterogeneous mixtures, calculate solution concentrations in different units, do stoichiometric calculations (e.g. acid-base titrations etc), recognize electrolytes, acids and bases, name the common acids and bases, understand the concept of solubility and saturated solution, write net ionic equations from molecular equations and vice versa, predict whether a precipitate will form given the solubility rules, predict the outcome of a metal displacement reaction given the activity series, use dilution to produce solutions of a certain concentration, calculate oxidation numbers, recognize oxidation-reductionreactions and the species that gets oxidized or reduced. Homework: 86 and 94 from chapter 3; 26, 30, 37, 46, 54, 58, 68, 73, 78 from chapter 4.

* Chapter 5. What you should know from this chapter: Be able to calculate hydrostatic pressure, convert between different pressure units, use the ideal gas law to obtain changes in T,P,V and compute the density of gases, do stoichiometric calculations involving gases, use Dalton's law to compute properties of gas mixtures, and use Graham's law to compute relative effusion/diffusion rates. Homework: 22a,b, 32, 38, 48, 54, 68, 74, 82, 94.

* Chapter 6. What you should know: Be able to apply the 1st law of thermodynamics to obtain the change in internal energy given heat and work or vice versa, compute heat amounts given the standard enthalpy of a reaction, compute heats of reaction given the enthalpies of formation of all species in the reaction, apply Hess's law to compute enthalpies of reaction from enthalpies of other related reactions, use heat capacities to relate amounts of heat to changes in temperature, and determine enthalpies of reactions given calorimetric data. Homework: 20, 26, 28, 34, 38, 56, 66, 68, 72.

* Chapter 7. Do not emphasize historical information. What you should know: be able to convert between wavelength and frequency, compute energy from frequency, calculate energy changes upon transitions in the H atom, convert between wavelength and momentum (de Broglie), know the quantum numbers and their possible values, know the shapes of the various orbitals, and understand the meaning of radial electron densities. Homework: 28, 32, 38, 40, 46, 48, 60, 62, 64.

* Chapter 8. What you should know: be able to write down the electron configuration, orbital diagram, valence shell and valence electrons, of any atom or ion in the first 5 periods, tell whether an atom or ion is diamagnetic/paramagnetic, rank atoms in terms of radius, ionization energy, electron affinity, and metallic character. Homework: 24, 28, 36, 44, 46, 50, 58a,b.

* Chapter 9. What you should know from this chapter: Be able to write Lewis structures, compute formal charges, tell the most important resonance structures, compute lattice energies using Hess's law, rank atoms in terms of electronegativity, tell polar from nonpolar bonds, compute reaction enthalpies from bond energies and vice versa, be able to write the formula for a hydrocarbon given the name and vice versa. Homework: 26, 28, 34, 36, 40, 46, 48, 50, 54, 70.

* Chapter 10. What you should know from this chapter: predict molecular geometries using the VSEPR method, write down VSEPR notation from Lewis structure, predict whether a molecule is polar or nonpolar, determine hybridization scheme and bonding scheme using VB theory, determine whether a molecule exhibits geometric isomerism, determine bond order and bond stability in a diatomic molecule using MO theory. Homework: 22, 24, 30, 44, 46, 54, 62.

Statement on Academic Integrity

The CCNY policy on academic integrity will be followed in this course. The document can be found through the CCNY website by clicking on Current Students → Academic Services → Policy on Academic Integrity. All students must read the details regarding plagiarism and cheating in order to be familiar with the rules of the college. Cases where academic integrity is compromised will be prosecuted according to these rules. In addition, the Policy of Academic Integrity can be found in the Undergraduate Bulletin 2007-2009 in Appendix B.3 on page 312.

Tentative lecture schedule

|9/1: Introduction/Chapter 1 |10/27: Chapter 6 |

|9/3: Chapter 2 |10/29: Chapter 7 |

|9/8: " |11/3: " |

|9/10: Chapter 3 |11/5: 2nd Midterm (Ch. 4-6) |

|9/15: " |11/10: Chapter 8 |

|9/17: " |11/12: " |

|9/22: " |11/17: Chapter 9 |

|9/24: Review/Prep Exam |11/19: " |

|10/1: 1st Midterm (Ch. 1-3) |11/24: Review |

|10/6: Chapter 4 |12/1: Chapter 10 |

|10/8: " |12/3: 3rd Midterm (Ch. 7-9) |

|10/13: " |12/8: Chapter 10 |

|10/15: Chapter 5 |12/10: Review |

|10/20: " | |

|10/22: Chapter 6 |Final Exam: Chapters 1-10 |

Tentative workshop schedule

|T 9/1: Unit 1 |R 10/29: Unit 7 |

|R 9/3: Unit 1 |T 11/3: Unit 7 |

|T 9/8: Unit 2 |R 11/5: Over 2nd exam/Unit 8 |

|R 9/10: Unit 2 |T 11/10: Over 2nd exam/Unit 8 |

|T 9/15: Unit 3 |R 11/12: Unit 9 |

|R 9/17: Unit 3 |T 11/17: Unit 9 |

|T 9/22: Unit 4 |R 11/19: Unit 10 |

|R 9/24: Unit 4 |T 11/24: Unit 10 |

|R 10/1: Over 1st exam |T 12/1: Unit 11 |

|T 10/6: Over 1st exam |R 12/3: Over 3rd exam |

|R 10/8: Unit 5 |T 12/8: Over 3rd exam |

|T 10/13: Unit 5 |R 12/10: Unit 11 |

|R 10/15: Unit 12 | |

|T 10/20: Unit 12 | |

|R 10/22: Unit 6 | |

|T 10/27: Unit 6 | |

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