Course Outline and Evaluation

Transcription

1 NORTHERN SECONDARY SCHOOL Grade 12 Chemistry (SCH 4U) Course Outline and Evaluation Textboook: Chemistry 12 Nelson Prerequisite: Grade 11 Chemistry Academic The grade 12 Chemistry course is based on the Ministry of Education and Training document entitled The Ontario Curriculum Grades 11 and 12 (2008 Revised). The secondary science program is designed to promote three goals: to relate science to technology, society and the environment, to develop the skills, strategies, and habits of mind required for scientific inquiry to understand the basic concepts of science. The evaluation policy reflects these three goals by evaluating you according to the achievement categories shown in the box below. Your final grade in chemistry will be calculated on the following basis: Knowledge & Understanding % Thinking & Investigation... 30% Communication... 10% Application % Summative Evaluation % Achievement Categories Students are evaluated according to the four categories described below. ACHIEVEMENT CATEGORIES Knowledge & Understanding This evaluation includes quizzes, tests, assignments, in-class exercises. It will test your understanding of concepts, laws and knowledge of facts and terms. Thinking and Investigation This evaluation is based on lab experiments and problem-solving skills. Communication For this category your ability to communicate information and ideas in a clear manner is evaluated. You will show this in the form of lab reports, proper solutions to solving problems and presentations. Applications Your understanding of the connections among science, technology and society is evaluated here. This will involve research assignments to show the impact of science on society and the environment using library and internet sources.

2 Learning Skills These are the day-to-day skills which students need to have in order to be successful in a science course as well as most courses at the high school level. These skills will be tracked by the teacher and noted by a letter on the report card: E=excellent; G=good; S=satisfactory; N=needs improvement LEARNING SKILLS Responsibility Fulfils responsibilities and commitments within the learning environment. Completes and submits class work, homework and assignments according to agree-upon timelines Takes responsibility for and manages own behaviour Organization Devises and follows a plan and process for completing work and tasks. Establishes priorities and manages time to complete tasks and achieve goals. Identifies, gathers, evaluates and uses information, technology and resources to complete tasks. Independent Work Independently monitors, assesses and revises plans to complete tasks and meet goals. Uses class time appropriately to complete tasks. Follows instructions with minimal supervision. Collaboration Works with others to resolve conflicts and build consensus to achieve group goals. Shares information, resources and expertise and promotes critical thinking to solve problems and make decisions. Initiative Looks for and acts on new ideas and opportunities for learning. Seeks assistance when needed. Demonstrates curiosity and interest in learning. Self-Regulation Seeks clarification or assistance when needed. Sets own individual goals and monitors progress towards achieving them. Perseveres and makes an effort when responding to challenges.

3 Course Policies For convenience, some of our course policies are outlined here. Refer to the first several pages in the Agenda for further details. Assignments You are expected to hand in assignments on time. If assignments are persistently late, appropriate measures will be taken, including referral to the Vice Principal. Assignments will be accepted until your teacher returns them to the class. If the assignment has not been submitted by this time you will receive a mark of zero. It is the policy of the Science department not to provide extra assignments for the purpose of boosting marks. Absences from Class If you foresee missing a science class (a trip, game or appointment) it is your responsibility, in order to avoid missing important evaluations, to see your science teacher beforehand: to hand in assignments due or write quizzes to find out what you will be missing to complete those assignments and have them ready to be checked, or handed in for extended illness, arrangements will be made to help you keep up with work missed. Missed Tests Tests will be announced well in advance. You will always know if an absence will cause you to miss a test. Please observe the following if this happens: Foreseen Absence If you know you are going to miss a test only by prior discussion with your teacher will you be advised of your options to avoid the zero mark that is otherwise recorded for a missed test. It is your responsibility to make these alternate arrangements with your teacher. Illness If you are ill and miss a test it is expected that you see your teacher the day you return, even if you do not have that class that day. It is your responsibility to find your teacher immediately. Failure to do this may generate a mark of zero. If you are in good health and able to attend school, be prepared to write the test immediately on your return. A note explaining your absence from the test will be required. Please sign below, indicating that you have read this sheet and understand the expectations of the course. If you have any questions please ask your teacher immediately. Student s Signature: Parent/Guardian s Signature:

4 Course Outline Northern Secondary School Chemistry SCH4U Order of Topics 1. Organic - hydrocarbons 2. Organic - functional groups 3. Thermochemistry 4. Rates of Reaction 5. Equilibrium (general) 6. Equilibrium (solutions) 7. Equilibrium (acids & bases) 8. Structure and Properties of Matter 9. Electrochemistry Evaluation Items A) Tests: Tests are based on the major sections shown above. They are usually a full period in length. B) Labs: Laboratory experiments are done in small groups but written up individually. Instructions for the write up will accompany each lab. A Duotang is required to keep all labs and will be handed in each time with the most recent lab on top. C) Assignments: A series of assignments and short quizzes will be given for each major section. These will serve as preparation for the test on that section. A second, separate Duotang will be needed for this. D) Summative Evaluation: Thirty percent of your grade will be based on an evaluation given near the end of the year. The evaluation will be either a written exam in June or a combination of written exam and lab practical exam. Text: Chemistry 12 Nelson Organic Chemistry - Hydrocarbons Hydrocarbon Nomenclature p.22:2,3 Reactions of Hydrocarbons 1.3 p.27:3 p.30:4,5 Aromatic Nomenclature Benzene structure and resonance hybrids Substitution reaction vs addition reaction Naming: singly substituted e.g. Cl, Br, NO 2, CH3-, CH-, 2 5 CH- 3 7 Trivial names -toluene, aniline, phenol, benzoic acid Ortho, meta, para-numbering on ring for > 2 groups Constitutional and Geometric Isomers pp.19-20, teacher notes teacher notes 1

5 Organic Chemistry - Functional Groups Alcohols Naming alcohols; IUPAC and common names primary, secondary, tertiary alcohol, diols,triols polyhydroxy alcohols, ethylene glycol, glycerol, nitroglycerine 1.5 p.41:1 p.42:5 Ethers Naming: IUPAC and common names p.46:11 p.48:3-7 Aldehydes & Ketones Naming by IUPAC and certain common names; e.g. formaldehyde, acetone 1.6 p.52:4,5 p.57:1-4 Carboxylic Acids Naming by IUPAC and common name, benzoic acid. others: oxalic, malonic, citric, lactic 1.7 p.68:1-4 Esters Naming esters Aromas: Table 15.5 banana, rum, pineapple Amines & Amides Naming amines and amides 1.8 p.76:4-6 p82:1,2 p.96:odd nos. Laboratory experiments Tests for saturation (Br 2 and KMnO 4) Synthesis of esters 2

6 Text: Chemistry 12 Nelson Thermochemistry Energy potential and kinetic translation, vibration, rotation, electronic, nuclear p.302:8,10,12 Heat heat vs temperature specific heat capacity p.310:4,5 Enthalpy of Reaction exo- and endothermic reaction definition of ÄH 0 enthalpy of combustion, ÄH comb. Application of Hess Law Enthalpy changes for combustion and solution reactions Standard Enthalpy of Formation, ÄH f Definition Use of ÄH f values from Table for calculation of enthalpies of reaction p.320:1-4 p.327:3 p.329:4,5 p.335:2,3 p.338:7 p.339:3,4 Laboratory Experiments Heat of combustion of a candle. Heat of solution (dissolving NH4Cl) Heat of reaction (combustion of Mg - Hess Law) 3

7 Text: Chemistry 12 Nelson Rates of Reaction Rate of Reaction Definition of average rate and instantaneous rate Measurement of rates by graphical means How rates are measured Factors affecting rates Collision Theory of Rates Collision frequency; orientation Maxwell-Boltzmann distribution of kinetic energies Activation energy Transition State Theory of Rates Potential energy diagram Activated complex teacher notes Catalysis Effect on rate in collision theory and transition state theory Homogeneous & heterogeneous catalysis Application - catalytic converter Reaction Mechanism Relation to stoichiometry Concepts of molecularity and elementary reactions Concept of rate-determining step pp p.396:3-5 p.391:1-3 Rate Law Rate constant Finding rate law & rate constant from exptl. data 6.3 p.377:2-4 p.381:2-4 p.408:7 p.415:15 Laboratory Experiments Iodine clock 4

8 Text: Chemistry 12 Nelson Equilibrium (General) Characteristics of Equilibrium Need for a closed system Reversible reactions, Dynamic nature, Constancy of properties Homogeneous & heterogenous equilibria Equilibrium Constant Equilibrium expression, K eq Equilibrium and reaction rate, concentration change Significance of large K eq and small K eq Value of K affected by amount, and eq reversing reaction Le Chatelier's Principle The effect on position of equilibrium by changes in -temperature, concentration, pressure, catalyst 7.1 p.438: p.449:6,9 7.3 p.457:1-5 p.459:3,6 Haber Process Industrial Synthesis of Ammonia Problem Solving Find Kc from equilibrium concentrations Find new equilibrium concentrations from K c Driving Forces st nd 1 & 2 Laws of Thermodynamics Entropy Gibbs Equation 7.4 & teacher notes 7.5 p.481: p.511:3,4 p.512:13,14 5

9 Equilibrium (Solutions) Solubility and solubility product constant, K sp meaning of soluble, slightly soluble, insoluble Finding K sp from ionic conc Finding ionic conc. from K sp Predicting formation of precipitate 7.6 p.493:7,11,12 Common ion effect Text: Chemistry 12 Nelson Equilibrium (Acids & Bases) Acids and Bases Arrhenius theory Bronsted-Lowry theory Amphoterism Conjugate acid-base pairs Self-ionization of water;definition of K w and pk Strong acids and bases ph Definition of ph and poh Weak acids and bases Definition ionization constants K, K, pk, pk Calculation of K a and K b from ph values and vice-versa Polyprotic acids Salt Solutions Hydrolysis of salts Calculate the ph of a salt solution a b a b Neutralization and Titration Neutralization reactions and ph of a neutralized solution Acid-base titrations w 8.1 p.532:1,2 8.2 p.556:3,5 p.570:9 8.3 p.588:1-5 p.589:8 8.4 Buffers 8.5 p.620:7,9 Laboratory Experiments K sp of potassium hydrogen tartrate (by gravimetry) K sp of potassium hydrogen tartrate (by titration) Behaviour of buffered solutions 6

10 Text: Chemistry 12 Nelson Structure & Properties of Matter Atomic theories Review atomic theories from Dalton to Bohr. 3.1 p.166:7,8,11,12 Quantum theory Schroedinger and wave mechanics 4 quantum numbers, n, l, m l, m s Pauli exclusion principle de Broglie and matter waves Heisenberg's Uncertainty Principle, Hund's rule shapes of s, p, d, orbitals, ground state electron configuration (Aufbau Principle) sigma and pi bonds (3.8 read for applications) pp p.180:10 p.194:7,8 p.220:1-19 Bonding Octet Rule & Exceptions Covalent, ionic & coordinate bonds Sigma and pi bonds Polar bonds and % ionic character VSEPR Theory polarity of molecules p.230:3,4 p.232:3,4 p.246:4 p.256:1,2 p.238:23 p.239:29 Aggregates of Matter Inter- and Intramolecular Forces Joule-Thomson & van der Waals Forces Dispersion forces, dipole-dipole forces Hydrogen bonding Ionic compounds and properties Molecular crystals and properties Network solids and properties Metallic solids and properties 4.5 pp p.260:1-5 p.266:11 p.273:1-7 p.281:self quiz p.282:1-22 7

11 Text: Chemistry 12 Nelson Electrochemistry Oxidation & Reduction (Redox) Oxidation numbers (and Rules) Oxidizing/reducing agents Activity series of metals Balancing redox equations Electrochemical cells Components & operation of cell Standard hydrogen half cell Half-cell reactions and E 0 0 Use of Table of E values Calculation of cell potentials Cells and Batteries Applications: primary & secondary batteries p.659:16 p.673:3,4 p.679: p.708:10, dry cells and mercury cell -lead acid storage cell and Ni-Cd cell -fuel cell Corrosion Corrosion of iron Electrolytic Cells Electrolysis of fused salts Electrolysis of aqueous solutions Electroplating Faraday s Law 9.6 Review p.714:5-7 p.726:10,13,19 p.735:1,4 p.748:1-4 p.752:9-13 Laboratory Experiments Cell voltages for Galvanic cells 8