Course Outline: UNIT TOPIC CHAPTERS APPROX. NO. OF WEEKS 1 Quantum Theory & Atomic Structure Electron Configurations & Chemical Periodicity 8 2

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1 CHEMISTRY 1120 GENERAL CHEMISTRY I Instructor: Dr. Shirley Wacowich-Sgarbi Office: A264f Tel: Office Hours: Posted on my office door, or by appointment. swsgarbi@langara.bc.ca Required Textbooks: Chemistry A Molecular Approach, 2 nd Ed., Tro, bookstore Organic Chemistry for Chem 1120 (Supplement) - online Laboratory Manual for Chemistry bookstore Other Essentials: Learning Outcomes: Scientific calculator bring to EVERY class and lab Upon successful completion of this course, the student should be able to: Describe laboratory procedures and give the names and uses of laboratory equipment to allow for the safe and efficient performance of chemistry experiments. Make use of careful measurement techniques and correctly interpret data to solve typical problems in general chemistry. Demonstrate an understanding of quantum theory as it relates to the wave-particle duality of matter. Assign a valid set of quantum numbers to each electron in a given atom. Write electron configurations of elements in the three different forms. Correlate atomic structure with chemical reactivity and interpret key atomic property trends found in the periodic table. Explain how a particular type of chemical bond, whether ionic, covalent, metallic, or some blend of these, is governed by the properties of the bonding atoms. Describe different bonding models (e.g. localized electron model and Molecular Orbital Theory) and point out their usefulness as well as their limitations. Predict the geometry and dipole moments of simple molecules based on VSEPR theory. Explain how bonding orbitals are utilized by atoms within molecules, based on the different models of hybridization and molecular orbital theory. Correlate molecular structure with physical properties. Demonstrate a foundational understanding of organic chemistry, with a focus on structure. Describe how carbon, hydrogen, and a few other elements, can combine in innumerable ways, resulting in complex structures that can be studied in a systematic way. o apply IUPAC nomenclature to relatively simple organic compounds and identify the most common functional groups o draw organic compounds using full structural formulas, condensed formulas and line (skeletal) formulas o describe different isomers; constitutional, geometric (cis trans and E Z) and stereoisomers (enantiomers) o conduct a conformational analysis on simple alkanes (using Newman Projections) as well as on cycloalkanes

2 Course Outline: UNIT TOPIC CHAPTERS APPROX. NO. OF WEEKS 1 Quantum Theory & Atomic Structure Electron Configurations & Chemical Periodicity Models of Chemical Bonding Molecular Geometry & Bonding Theories 9 & Organic Chemistry Marking Scheme: Midterm #1 15% Midterm #2 20% Quizzes 15% Labs 15% Final Exam 35% 20 & Supplement & classnotes Numerical to Letter Grade Conversion: A+ = % B+ = 76 79% C+ = 64 67% D = 50 54% A = 85 89% B = 72 75% C = 60 63% F = 0 49% A- = 80 84% B- = 68 71% C- = 55 59% Operational Details: The lab: MINIMUM GRADE TO BE ACCEPTED IN THE NEXT CHEM LEVEL COURSE IS C- 3 It is department policy that students must satisfactorily complete the laboratory section to pass the course. This means that attending all labs is mandatory. The lab marks are handled exclusively by the lab instructor. The course: This is a problem-solving course. The lectures are intended to be a GUIDE to your studies, and are not meant to be a substitute to individual effort. Several problems will be solved in class, but YOU should attempt to solve ALL problems from the unit problem sets posted on the course s website and the problems from the textbook.

3 o o Solutions to the text book are found in the solution guide that can be borrowed from the library. Solutions to the problem sets are posted on the course s website. To access the course s website, students must go through mylangara : my.langara.bc.ca Students will receive announcements, updates and memos through , using the student s address they have provided e; students are encouraged to contact the instructor via as well. Students are responsible for all information given in the lecture, in the laboratories, and otherwise found in the website or received by , including important dates (tests, withdrawal deadline, etc.), updates, cancellations, etc. No cell phone, pagers, PDAs, texting, and music devices are allowed in class; these devices MUST be turned off during the lecture. If there is an urgent need to be in touch with family members due to illness or other difficulties, set the device to vibrate or some other silent mode and take your call outside. The dates for the quizzes and term tests will be announced in class and posted in the course s calendar (website). The dates are fixed. There are no make-up quizzes or tests; the grade of record to a missed test is ZERO. Answer keys to tests and midterms will be made available online once the tests have been marked and returned to the class. No answer key will be provided for the final examination. You will be allowed to review your final examination BY APPOINTMENT ONLY. The procedure on how to do so will be provided by the end of the term. Policies, rules and Important Dates The withdrawal date this term: March 4, No late withdrawal will be permitted. Final examinations: April 12-20, 2011 Repeating the course: A student who has taken or is taking a chemistry course in a given semester will not be allowed to attempt to register to repeat that course in the immediately following semester until the registration date and time assigned to those who have 8 (eight) registration points. A student who has taken or is taking a course means a student who has received or will receive any grade, including a W, for the course. Cheating ( Langara College is dedicated to the pursuit of academic excellence, and committed to creating an environment that promotes scholarly activity and integrity. Students of e have the responsibility to pursue all educational activities in an honest and forthright manner. ( ) Cheating and fraud are serious offences. The College will investigate all allegations of cheating and fraud, and will issue penalties where necessary and appropriate.

4 Code of conduct ( Members of the College Community must conduct themselves responsibly and with propriety. The College does not tolerate misconduct and will take steps to deal with allegations that a member of the College Community has engaged in misconduct. Concerns about Instruction ( Concerns about instruction, that is, concerns about course content and/or the instructional process, should be brought to the attention of the teacher who is the subject of the concern, as soon as possible after they arise. ( )If the individual who has concerns is unable to approach the teacher directly, or if s/he is not satisfied with the response by the teacher following discussion, s/he should report the concerns to the individual who is responsible for the program (normally the coordinator, department chair or program manager). Exam Rules: o Student may not make use of any books, papers, memoranda, audio or visual memory devices. o All bags, books, notes, pencil cases and other items are to be left at the front of the room. o No cellular phones, pagers, or other electronic devices (other than approved calculators) are allowed on the desk or table or may be used during an exam. o Purposely exposing written papers to the view of other students is forbidden. The plea of accident or forgetfulness is not acceptable. Blackboard Orientation: This course uses Blackboard (formerly WebCT) as a means to make class notes, answer sets, and other goodies available to the students. Therefore, using the class Blackboard site is essential! If you are not familiar with Blackboard, please check out the following link titled Blackboard CE self-directed Online Orientation and Help Guide for an introduction to Blackboard. This link can be found in the Blackboard channel just above your course listing in mylangara (

5 UNIT #1 Quantum Theory & Atomic Structure Tro - Chapter 7 A/ Review - Characteristics of atoms B/ Electromagnetic Radiation - Characteristics of light - light as a wave: frequency, amplitude, wavelength, speed of light, - Mathematical relationship between ν and λ - Electromagnetic spectrum C/ Intro to Quantum Theory and the Bohr Model - The Photoelectric effect - Einstein s photon theory particle nature of light - Absorption and emission spectra - Quantization of energy - The Bohr atom and energy level diagrams - Ground states, excited states - Balmer series, Lyman series, Paschen series - Energy states, energy changes & ionization energy calculations using the Bohr equation D/ Progression Towards a New Quantum Mechanics - Properties of electrons - Wave-Particle duality and de Broglie s relationship - The Heisenberg Uncertainty Principle - From classical to quantum-mechanical theory - Wave mechanics & wave functions (briefly) - Intro to the Schrödinger Wave Equation (2.6) ( ) ( ) (7.4 & notes) E/ The Quantum-Mechanical Model of the Atom - Use of the Schrödinger equation - Probability (ψ 2 ) - Quantum numbers: principle quantum number (n), angular momentum quantum number (l), magnetic quantum number (m l ), spin orientation quantum number (m s ) - Shells, subshells and orbitals - Orbital shapes (for s, p and d) and contour plots - Diagrams: electron density, probability (ψ 2 ) vs. distance from the nucleus, radial probability distribution plots ( )

6 UNIT #2 Electron Configuration & Chemical Periodicity Tro - Chapter 8 A/ Orbital Energies - Effect of nuclear charge - Effect of other electrons - Screening B/ Writing Electron Configurations - Aufbau Principle, Pauli Exclusion Principle, Hund s Rule of Maximum Multiplicity - Orbital (box) diagrams, electron configurations & condensed electron configurations (noble gas configurations) - Exceptions to the rules - Classification of electrons: outer electrons, valence electrons, inner electrons - Excited States C/ The Periodic Table and Periodic Trends - History of the periodic table - Periodic trends - Atomic radii (covalent, metallic and ionic radii) trends and anomalies - Atomic size vs. ionic size - Ionization energy trends and anomalies - Electron affinity D/ Chemical Properties - Ion formation - Writing electron configurations of ions - Pseudo-noble gas configurations - Magnetism: diamagnetism, paramagnetism, gouy balance (8.3) ( ) (8.2 & ) (8.7)

7 UNIT #3 Models of Chemical Bonding Tro - Chapter 9 A/ Types of Chemical Bonding - Lewis Theory - Ionic bonding - Covalent bonding - Metallic bonding, electron sea model - Bond energy & Coulomb s Law - Lewis electron-dot symbols B/ Ionic Bonding Model - Octet rule - Ionic compound formulae and electron transfers - Lattice energy, ΔH lattice and its calculation - Hess s Law and the Born-Fajans-Haber cycle (and steps) - Lattice energy trends C/ The Covalent Bonding Model - Formation of a covalent bond and bond energy diagrams - Bonding pairs and lone pairs of electrons - Types of bonds and bond order - Properties of covalent bonds (bond length and bond energy) - Bond order and trends with length and energy - Predicting ΔH rxn s from bond energies ( , 9.11) (9.4) (9.5, 9.10) D/ Electronegativity & Polar Bonding - Electronegativity, Pauling s electronegativity values - Electronegativity trends - Differences in electronegativity and applications to bonding - Polar bonding, partial charges ( + and - ), dipoles and net dipoles - Determining polarity of compounds - Predicting relative polarity of bonds (9.6) E/ Bonding & Chemical Properties - Properties of ionic solids, covalent compounds & metallic aggregates - How properties relate to bonding and intermolecular forces (Notes)

8 UNIT #4 Molecular Geometry & Bonding Theories Tro - Chapter 9-10 A/ Lewis Structures - Review of Lewis symbols and structures (ionic compounds and covalent compounds - Lewis structure of coordinate covalent compounds - Steps for writing a Lewis structures of covalent compounds - Formal charge - Resonance, resonance forms, resonance hybrids - Exceptions: radicals, expanded octets, incomplete octets B/ VSEPR Theory - Basic principles of valence shell electron pair repulsion theory - Bond angles and pictoral representations of bonding geometries - VSEPR notation, electron groups, electron group arrangement, molecular geometry - Electron group arrangements: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral - Molecular geometries: including above electron group arrangements, bent, trigonal pyramidal, seesaw, t- shaped, square pyramidal, square planar - Using VSEPR to predict and describe molecules - Molecular shapes and polarity C/ Valence Bond Theory & Hybridization - Overlapping orbitals and a localized electron model of bonding - Overlap and bond strength - Orbital orientation and projection of orbitals - Applying VB Theory to simply molecules - Need for orbital hybridization, orbital addition (adding wave functions) - Hybrid orbitals: sp, sp 2, sp 3, sp 3 d, sp 3 d 2 - Predicting hybrids based on Lewis structures and VSEPR theory - Sigma bonds vs pi bonds - Double and triple bonds - Free rotation ( ) ( ) (10.6, 10.7) D/ Molecular Orbital (MO) Theory - Molecular orbitals (MO s) - Formation of MO s: bonding and antibonding orbitals (10.8)

9 UNIT #5 Organic Chemistry (notes & supplement) Tro - Chapter 20 A/ Introduction to Organic Chemistry & I.U.P.A.C. Nomenclature - Classification of organic compounds: saturated, unsaturated - Carbon hybridization - Structures: Lewis dot, structural diagram, condensed structure, skeletal/bond line diagram, 3-D wedge dash - Hydrocarbon classification: alkane, alkene, alkyne - Nomenclature of aliphatic alkanes, (including with branches/substituents) - Cyclic alkanes and nomenclature - Haloalkanes - Alkene & alkyne nomenclature B/ Functional Groups - Recognizing: alcohols, amines, aldehydes, ketones, carboxylic acids, esters, amides. - General nomenclature rules - Recognizing 1 o, 2 o, 3 o, 4 o carbon atoms, 1 o, 2 o, 3 o hydrogen atoms and 1 o, 2 o, 3 o amines C/ Isomerism - Structural isomers (also called skeletal isomerism or constitutional isomerism) - Conformational isomers of alkanes, including conformers (anti, gauche, eclipsed, staggered), Newman projections, conformational analysis - Conformational isomers of cycloalkanes, including conformers (boat, chair), identifying stability (torsional strain, conformational analysis & energy diagrams), axial/equatorial hydrogens or substituents. - Stereoisomerism - Diastereomers, cis/trans isomers, E/Z designation and configurational isomers. - Stereoisomerism - Enantiomers, optical activity, chiral/achiral, stereogenic centers, R/S designations, Fisher projections , notes and supplement ***Chapter 20.6, 20.7 and will not be covered.