Ap syllabus 96 - Alvin Independent School District



Alvin High School (2015-2016)

Advanced Placement Chemistry

Instructor: Tonya Patterson

Room: A207

Voice mail: (281) 245-3000 ext. 4287

Email: tpatterson@

Website: (go to staff directory at Alvin High School)

Remind for AP Chemistry – Text @a530a to 81010 to receive reminds for AP chemistry.

I. Course Description The AP Chemistry course is designed to be the equivalent of the general chemistry course usually taken during the first year of college. For most students, the course enables them to undertake, as a freshman, second year work in the chemistry sequence at their institution or to register in courses in other fields where general chemistry is a prerequisite. AP Chemistry should meet the objectives of a good general chemistry course. Students in such a course should attain a depth of understanding of fundamentals and a reasonable competence in dealing with chemical problems. The course should contribute to the development of the students’ abilities to think clearly and to express their ideas orally and in writing with clarity and logic.

II. Tutoring Hours - I am available on Monday afternoon from 3:00 – 3:30 pm, Thursday afternoon from 3:00 – 3:30pm and Tuesday 7:00 – 7:20 am. If a parent needs to contact me, please call or preferably e-mail me for a meeting.

III. Materials - 3 ring binder, 4 dividers, duplicate carbonless lab notebook and calculator (preferred Graphing Calculator TI84)

IV. Textbook – Chemistry: The Central Science (12th edition) (Check out from the bookstore)

V. Required Reading: The Disappearing Spoon: and Other True Tales of Madness, Love, and the History of the World from The Periodic Table of the Elements. Sam Kean. ISBN# 978-0-316-05164-4.

VI. Study Habits - The material in this course must be studied and learned daily as it is presented because the units build upon one another. The AP course description booklet states that students should spend at least 5 hours a week studying outside of class. The actual amount of time spent will depend upon each student's background. If a student does not understand a concept, he or she should see me as soon as possible.

VII. Grading Policy

• Major tests - 50% - will be announced at least 2 days in advance

• Laboratory reports - 30%

• Daily – 20% - includes homework, quizzes and class participation

Homework You should have a homework tab where you will keep all homework assigned. If you don’t work on the homework regularly, you will not do well on the quizzes and exams.

Quizzes will mimic the homework and can cover any homework that was to be done by the day we have the quiz. Some of the quiz problems will be copied directly from the homework and others will be the same with different numbers used.

Labs are taken very seriously so you need to follow a specific format. If you don’t follow the format in the write up instructions provided, you will get a 50 and the lab will be returned to you ungraded. After the 1st 9 weeks (for the 1st 9 weeks see district late policy) NO Late labs will be accepted.

VIII. Make-up Work: According to the school handbook, students have one day for everyday absent to make up missing work. I will only make exceptions in the event of extenuating circumstances. Students will also be responsible to take any quiz or test scheduled on the day they return from an absence if no new material was covered in regards to that quiz/test. Students who actually miss quizzes and tests need to expect to make them up on the day they return during lunch, before school, or after school unless otherwise arranged with me.

XI. Tardiness: You will be counted tardy if you are not in class when the bell rings. After 5 minutes, you will be counted absent. I take tardiness seriously and make no exceptions without a pass from a teacher or an admit from the attendance office.

Cell Phones & Other Electronic Devices: We will occasionally be using your electronic devices in class for various activities. Electronic devices may only be used when permission is granted. If electronic devices are used for non-class related activities they will be taken up and turned into the office, in which the district policy for retrieval will apply.

AP Chemistry Content

Big Idea 1: The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangements of atoms. These atoms retain their identity in chemical reactions.

Big Idea 2: Chemical and physical properties of materials can be explained by the structure and the arrangement of atoms, ions, or molecules and the forces between them.

Big Idea 3: Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons.

Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions.

Big Idea 5: The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in mater.

Big Idea 6: Any bond of intermolecular attraction that can be formed can be broken. These two processes are in a dynamic competition, sensitive to initial conditions and external perturbations.

AP CHEMISTRY Flow

Unit 1 - Science Fundamentals

• Scientific Method

• Classification of Matter

• Separation Science, example distillation and chromatography

• Physical and Chemical Properties

• Temperature and Density - Demos

• Meet the Elements

• Math Review, Significant Figures, and Statistical techniques

• Dimensional Analysis and Proportions

• Units of Measurement

• Conversion of units

• Dimensional Analysis

• Uncertainty in Measurements and Significant Figures

• Length and Volume

• Mass and Weight

• Density and Specific Gravity

• Temperature and its Measurement

Unit 2 - Nuclear and Atomic Structures

• Types of Subatomic Particles

• The Nucleus

• Mass Spectroscopy and Isotopes

• Stability of the Nucleus

• Atomic Structure

• Rutherford Experiment

• Cathode Ray Experiments

• Atomic Structure Terms

• Electromagnetic Radiation

• Quantization of Energy

• Photoelectric Effect

• PES data

• Bohr Atom

• Spectroscopy

• Orbital Model of Atom

• Aufbau Diagram

• Paramagnetism

• Quantum Model

Unit 3 - Periodicity and Introduction to Bonding

• Atomic Properties

• Periodic Law

• Elemental Properties

• Types of Bonds

• Metallic Bonding

• Properties of Group 1

• Properties of Group 2

• Metals vs. Non Metals

• Multiple Oxidation States of Transition Metals

• Ionic Bonding

• Ionic Bonding and Potential Energy Diagrams

• Energy of Formation of Ionic Compounds

• Lattice energy

Unit 4 – Covalent Bonding and Molecules

• Types of Covalent Bonds

• Nonpolar Covalent Bonds

• Polar Covalent Bonds

• Coordinate Covalent Bonds – Lewis Acids and Lewis Bases

• Lewis Structures

• Resonance

• Hybridization

• Molecular Geometry

• Energy Effects on Molecules

• Isomerism

• Functional Groups

• Interactions of Functional Groups

• Classification of Molecules

• Intermolecular Interactions

• Dipole moments

• Dielectric Constants

• Types of Compounds

• Properties of Metallic, Molecular, Macromolecular and Ionic Compounds

Unit 5 - Organic Chemistry

• Properties and Bonding in Carbon Compounds

• Compounds

o Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties.) Physical and chemical properties of simple organic compounds

• Hydrocarbons

o Petroleum

o Fractional Distillation

o Cracking

o Alkanes

o Alkenes

o Alkynes

o Benzene series

o General Formulas

o Structural Formulas

o Saturated/unsaturated compounds

• Nomenclature

o Alkyl groups

o IUPAC Nomenclature

o Isomers

• Other Organic Compounds

o Alcohols

▪ Primary, secondary, and tertiary alcohols

o Aldehydes

o Ketones

o Acids

o Esters

o Ethers

o Amines

o Polymers

▪ Addition polymerization

▪ Condensation polymerization

▪ Natural polymers

• Organic reactions

Unit 6- Predicting Reactions

• Naming compounds

• Balancing chemical reactions

• Types of chemical equations

• Types of chemical reactions

• Predicting based on stability

• Predicting based on type

• Chemical reactivity and products of chemical reactions

• Reaction types – organic functional group reactions, acid-base reactions; concepts of Arrhenius, Bronsted-Lowry, and Lewis; coordination complexes; amphoterism

Unit 7 – Measurement and Stoichiometry

• Law of Constant Composition and Calculations based on Law

• Using Moles to find a Quantity

• Stoichiometry

• Limiting Reagents

• Using Density

• Solution Terms

• Stoichiometry - Solutions

Unit 8 - Thermochemistry

• Introduction to thermodynamics

• Conservation of energy

• State functions

• Potential energy

• Kinetic energy

• Calorimetry

• Heat of Fusion

• Heat of Vaporization

• Specific Heat

• Heat of Dilution

• Heat of Solution

• Hess’s Law – direct and indirect

• Bond Dissociation energies

• Gibbs Free Energy Equation

Unit 9 – Gases, Liquids and Solids

• Real Gases versus Ideal Gases

• Ideal Gas Equation

• Derivations based on Ideal Gas Equation

• Gases collected over water

• Kinetic Molecular Theory

• Van Der Waals Equation

• Molecular Speeds

• Diffusion and Effusion

• Molecular Theory related to Phase

• Phase Changes

• Entropy

• Heating and Cooling Curves

• Interfaces

• Pressure

• Vapor Pressure

• Boiling Point and Freezing Points

• Vapor Pressure Curves

Unit 10 – Solutions

• Types of Solutions

• Electrolytes

• Miscibility and Immiscibility

• Process of Dissolution

• Dissolution versus Ionization

• Solubility Terms

• Solubility Curves

• Henry’s Law

• Concentration Terms – Molarity, Molality, %, mole fractions

• Dilution Problems

• Stoichiometry Problems with Solutions – Review

• Raoult’s Law

• Freezing and Boiling point of Solutions – Colligative Properties

• Van’t Hoff factor

• Osmosis

• Deviation from Raoult’s Law

• Colloids

Unit 11 - Kinetics

• Rates relationship to collisions

• Reaction Mechanisms

• Activation Energy

• Nature of Reactants and Interfacial Surface Area

• Temperature and Pressure effects on Rates

• Catalyst – Homogeneous and Heterogeneous

• Potential Energy Diagrams – Review

• Activated Complex and Intermediates

• Arrhenius Equation

• Maxwell – Boltzman Diagram

• Average Rate

• Rates relationship to Stoichiometry

• Graphical determination of Instantaneous Rate

• Rate Laws

• Determination of Rate Laws

• Determination of Mechanisms

• Order of Reactions

• Calculations based on Order

Unit 12 - Equilibrium

• Reversible processes and Reactions

• Types of systems

• Kinetics relationship to Equilibrium

• Equilibrium Expressions

• Equilibrium Constants

• LeChatelier’s Principle

• Equilibrium Stresses

• Equilibrium Calculations

• Molar Solubility

• Common Ion Effects

• Reaction Quotients

Unit 13 - Acids, Bases and Salts

• Dissociation versus Ionization

• Preparation of Acids, Bases and Salts

• Classification of Acids and Bases

• Bronsted-Lowry Theory of Acids and Bases

• Degree of Ionization

• Equilibrium Constants for Acids and Bases

• Weak Acids and Bases

• Binary acids versus Oxyacids

• Determination of Acid and Base properties based on structure

• Ionization of Water

• pH and pOH

• Acid-Base Stoichiometry Problems – Review

• Ionization calculations of Weak Acids and Bases

• Henderson-Hasselbalch Equation

• Titration Calculations

• Indicators

• Types of Salts

• Dissociation of salts and Buffers

Unit 14 - Electrochemistry and Thermodynamics

• Oxidation and Reduction

• Substances gaining potential

• Types of electrochemical cells

• Voltaic cells

• Cell Potential

• Concentration dependence of E

• Nernst Equation

• Cell potentials and Equilibrium

• Metal Electrodes

• Reference Electrodes

• Indicator Electrodes

• Applications of Voltaic Cells

• Electrolysis

• Faraday’s Law

• Electrolytic Cells

• Order of reduction

• Applications of Electrolytic cells

• Gibbs Free energy Equation (Free Work)

• Relationship of Equilibrium and Q

• Relationship to E

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