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Regular & Honors Chemistry

Chem is Chool! 

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32 Week
Course
 
2 Semesters

Regular
$300
/Semester

$500/Year

Honors

$350/Semester
$600/Year

Don't You Know It's Time for Class Now
00:00 / 00:43

One LIVE Class / Week
Tuesday 9:15 - 10:45 am
OR
Create a Class (click here)
Eastern Time

Pearson Chemistry.jpg

Pearson Chemistry Text

 

Copyright @ 2017

Wilbraham, Staley, Matta, Waterman 

ISBN-13: 

978-1-32-320591

Course Requirements

  1. Student Pre-Assessment as part of Registration / Enrollment (click here).

  2. Enrollment Agreement (Parent Survey) as part of Registration / Enrollment (click here).

  3. Textbook (hardcopy or etext).

  4. Free Zoom account with audio / video capability for classes.

  5. Tablet with stylus for writing is highly recommended (e.g. Wacom).

  6. MAC users get compatible software (Word, Powerpoint, Excel), if possible.

 

Regular Chemistry

  1. Students will spend 8-10 hours per week for this course.

  2. Four (4) Formal Lab Reports based on Hands-on experiments.

  3. Fifty (50) labs and/or hands-on activities.

 

Honors Chemistry

  1. Students will spend 9-11 hours per week for this course.

  2. Students will do percent error for formal lab reports.

  3. Five (5) Formal Lab Reports based on Hands-on experiments.

  4. Fifty (50) labs and/or hands-on activities, taking pictures of major procedures/results.

  5. Students will do an EXTRA lab most units (taking a picture of reactants and/or products, and explaining its relevance).

  6. Students will incorporate Organic Chemistry into 2nd semester.

  7. Students will complete some extra assignments beyond the General Chemistry course.

Requirements

32 Week Course  ...  2 Semesters

Regular
$300 / Semester
$500 / Year

Honors

$350 / Semester

$600 / Year

Pearson Chemistry Text

 

Copyright @ 2017

Wilbraham, Staley, Matta, Waterman 

ISBN-13: 

978-1-32-3205907

Edition 2012 is acceptable but there are some differences (question numbers may vary).

Pearson Chemistry.jpg

Lab Supplies Needed

[Click here for Link]

  • Mass Scale  

  • 100 ml Plastic Grad Cylinder 

  • 250 ml GLASS Beaker / Cup    

  • -10 C to 110 C Thermometer (non-immersion) 

  • Safety Goggles 

  • 10 Copper Coins

  • Household Items 

Description

Course Description

 

For many students, Chemistry is one of the most challenging courses in high school – this highly interactive college prep course overcomes that hurdle for motivated students even if they are not strong in science. Curriculum includes a qualitative and quantitative study of scientific measurement and processes, matter, atomic theory, the periodic table, bonding, stoichiometry, gas laws, and chemical reactions (including solutions, thermochemistry, reaction rates, equilibrium, acid-base chemistry, and oxidation-reduction reactions). Particular emphasis is placed on solving scientific problems and using scientific evidence to support conclusions.

Course resources include detailed directions for all assignments, comprehensive / scaffolded class notes, and tutorial / enrichment materials including over 150 videos that model and enhance learning.

Chemistry caters to the non-science major AND to the science major desiring more study skills and math support, while laying a firm foundation for AP Chemistry and/or other sciences. Pedagogy emphasizes inquiry-based learning, critical thinking skills, study skills, and strategies for problem solving. Rote memory and basic comprehension are downplayed while processing information through synthesis (putting together), analysis (breaking down), and evaluation (prioritizing) is stressed.

The weekly laboratory component includes video-based lab experiments, and physical, hands-on labs performed at home using common household chemicals. Students will learn to write FOUR (4) technical (formal) lab reports throughout the year (detailed guidelines and models are provided) as well as opportunity to revise the lab report.

For reflection, reteaching, and mastery, students will be encouraged to correct some of their tests and to revise their lab reports. This helps them learn to think critically and will offer bonus points.

 

Note:

Chemistry can be challenging (even for solid students), particularly the math-related aspects of it. If your Chemistry student would benefit from more instruction, more time to ask questions, and more opportunity to go over trouble-areas with a teacher, please consider adding Chemistry Recitation to your Chemistry course. Chemistry Recitation is an additional low-cost seminar course for Q&A, review, reflection and re-teaching of difficult concepts. Content objectives, homework, labs, and tests are also primary topics of discussion. The Chemistry Recitation class enhances study skills, nurtures critical thinking, and provides extra practice in problem solving.

Topics and Objectives:

  • Chemistry Introduction

    • Have a great start to Chemistry!

    • Go over practical and technical issues to navigating GP6, Study Place, and other non-course related issues.

    • Show that many great scientists were believers in Jesus. Science and the Bible are compatible.

    • Give examples of inquiry based learning throughout the lesson.

    • Define Chemistry and understand its place in science.

    • Present steps of the scientific method and be able to distinguish each.

    • Understand basic graphing protocols (independent and dependent variables) as part of experimentation and data collection.

    • Learn a problem solving strategies: "AGES" for use throughout the course.

  • Matter and Change

    • Describe & Distinguish between Extensive, Intensive & General Properties

    • Explain why all samples of a substance have the same intensive properties.

    • Classify Matter as Pure versus Mixture

    • Explain how mixtures can be separated.

    • Identify the states of Matter (s, l, g)

    • Be able to use the Periodic Table to find information about elements

    • Distinguish Physical Changes from Chemical Changes

    • Describe how the mass of the reactants and products of a chemical reaction is conserved.

    • Describe the law of definite (fixed) proportions and using calculation determine if compounds are alike or not.

  • States of Matter

    • Describe the three assumptions of the kinetic theory as it applies to gases.

    • Define, measure, and calculate pressure in terms of atmospheric, gas & normal (standard) pressure.

    • Compare the physical properties of solids, liquids and gases in terms of shape, volume, motion (fluidity), density, expansivity and compressibility.

    • Distinguish the properties of liquids: average kinetic energy (temperature), dynamic equilibrium, vapor pressure versus temperature, boiling versus evaporation.

    • Distinguish the properties of solids and the phase changes involved.

    • Decipher phase diagrams, identifying pressure, temperature, phase changes and triple point.

    • Understand the relationship between intermolecular forces and kinetic energy for each state of matter and phase change.

  • Scientific Measurement

    • Use the Metric System versus the English System

    • Write numbers & do calculations in scientific notation.

    • Evaluate Accuracy & Precision in Measurements (significant figures)

    • Calculate Percent Error as a Measure of Precision

    • Understand & Use Units of Mass, Volume, Distance (emphasize Metric)

    • Identify the temperature units scientists commonly use

    • Understand & Calculate Density

    • Learn to solve problems using dimensional analysis (factor Labeling)

  • Atomic Structure

    • Explain Atomic History from specific scientists perspectives (Democritus, Dalton, Thomson, Millikan, Goldstein, Chadwick, Rutherford).

    • Understand subatomic particles in a typical atom (charge, mass, location).

    • Explain what makes elements (atomic number, mass), use nuclear symbols, and understand isotopes.

    • Determine the weighted average of an element on the Periodic Table using relative abundance.

  • Modern Atomic Theory: Electrons in Atoms

    • Describe contributions to the revised atomic theory (Bohr, DeBroglie, Shroedinger, Heisenberg, wave-particle duality, Photoelectric effect, Absorption & Emission Spectra)

    • Explain and calculate the relationship of wavelength, frequency and energy of emitted light related to changes in electron energies.

    • Understand Quantum Mechanics model of the atom and write electron configurations of elements. Give the 4 quantum numbers of elements 1 -11.

  • The Periodic Table

    • Explain the history of the Periodic Table (Dobereiner, Newlands, Mendeleev, Moseley).

    • Describe the arrangement of the periodic table (periods, groups, periodic law, classes of elements).

    • Classify elements based on electron configuration for Valence (outer electrons that bond).

    • Explain periodic trends (electronegativity, atomic & ionic size, ionization energy)

  • Ionic and Metallic Bonding

    • Understand the conditions of stability for atoms related to bonding.

    • Explain and show how elements become ions (cations and anions).

    • Explain the ionic compounds in terms of formation, electrical charge, structure and Electronegativity Difference.

    • Learn the properties of ionic compounds.

    • Understand Metallic Bonds and properties, including alloys.

  • Covalent Bonding

    • Explain covalent bonding in terms of bonds (nonpolar, polar, and coordinate covalent) and molecules (nonpolar & polar).

    • Define and recognize polyatomic ions.

    • Understanding how to represent molecules, compounds and types of covalent bonds (single, double, triple) in various ways (molecular & structural formulas, Lewis structures).

    • Define bond dissociation in relation to bond strength.

    • Recognize molecular orbitals (sigma and pi bonds) that relate to single, double and triple bonds.

    • Understand and draw molecules that have exceptions to the octet rule and demonstrate resonance (when bonds are intermediate in length).

    • Understand the theory behind molecular geometric shapes (linear, bent, trigonal planar, pyramidal, and tetrahedral).

    • Explain hybrid orbital theory in terms of molecular geometry.

    • Identify and define intermolecular attractions (Van Der Waals, Hydrogen Bonding, Network Solids) and how these affect chemical properties of the molecules.

  • Chemical Names and Formulas

    • Explain how to determine the charges (oxidation numbers) of monatomic ions.

    • Apply the rules for naming and writing formulas for compounds with polyatomic ions.

    • Determine the names and formulas of ionic and covalent compounds, of acids and bases.

    • Understand Law of Definite Proportions

  • Molar Quantities

    • Understand and utilize the mole in mathematical computations according to the mole concept (Avogadro's Number).

    • Calculate Molar Mass of Elements and Compounds. Interconvert moles and mass.

    • Calculate Molar Volume at STP. Interconvert moles and liters, molar mass and density.

    • Calculate Percent Composition (Percent by Mass of elements in a compound) using mass, formulas, and percentages.

    • Determine mole ratios of elements within a formula.

    • Understand and calculate Empirical Formulas using mass, percentages, and moles.

    • Determine Molecular Formula from Empirical Formulas.

​​

1st

Semester

Objectives
  • Chemical Reactions

    • Write and balance chemical equations based on chemical reactions.

    • Identify and characterize the types of reactions, including synthesis, decomposition, single replacement, double
      replacement, and combustion.

    • Recognize and write balanced chemical equations for synthesis, decomposition, single replacement, double replacement, or combustion reactions.

    • Use the activity series to determine whether a single replacement reaction will occur.

    • Write ionic equations, net ionic equations, and recognize spectator ions based on reactions with aqueous solutions.

  • Stoichiometry

    • Understand and use stoichiometry in balanced chemical equations (particularly regarding molar quantities of mass, volume, and number).

    • Explain and calculate the interconversion of reactants and products using mole ratios.

    • Identify the limiting and excess reactants for a given reaction.

    • Use the limiting reactant to predict the theoretical yield of a reaction.

    • Calculate the percent yield of a reaction.

  • The Behavior of Gases

    • State Boyle’s law, Charles’s law, Gay-Lussac’s law, and Avogadro's law and apply these laws to calculate the relationships between volume, temperature, and pressure.

    • Derive the combined gas law from Boyle’s law, Charles’s law, and Gay-Lussac’s law and calculate for pressure, volume, or temperature.

    • Define partial pressure and apply Dalton’s law of partial pressures to describe the composition of gases.

    • State the Ideal Gas Law (PV = nRT) and calculate moles of a gas, understanding the difference between ideal and real gases.

    • Understand Graham's Law which states that gases of lower molar mass diffuse and effuse faster than gases of higher molar mass.

  • Water & Solutions

    • Describe how the structure of water accounts for its polarity

    • Explain why water has unique properties including high surface tension and high boiling point

    • Describe the unique role of water as the “universal solvent”

    • Identify factors affecting solubility and the rate at which a substance dissolves

    • Define solubility and differentiate between saturated, supersaturated, and unsaturated solutions

    • Define & calculate concentration in terms of mass, volume, & molarity, and molality

    • Describe the relationship of the molality of a solute in solution and the solution’s depressed freezing point or elevated boiling point. Calculate freezing point depression & boiling point elevation.

  • Thermochemistry

    • Distinguish aspects of heat flow (endothermic, exothermic, potential energy, kinetic energy, heat and temperature).

    • Identify heat flow, potential and kinetic energy, phase changes, and heating or cooling for phase diagrams of a substance.

    • Calculate heat flow for heating and cooling of substances using mass, specific heat, and the change in temperature or heat of fusion or heat of vaporization.

    • Define and calculate the specific heat of a substance and the heat flow related to calorimetry.

    • Identify reactants, products, heat of reaction, and heat flow in potential energy diagrams.

    • Calculate heat flow in thermochemical equations using heat of reaction, standard heats of formation, and Hess's Law

  • Reaction Rates and Equilibrium

    • Explain the concept of reaction rate.

    • Describe collision theory and explain how various factors, including concentration, temperature, and pressure affect the rate of a chemical reaction.

    • Interpret reaction pathways (PE diagrams) to identify exothermic versus endothermic reactions and to define and explain the role of the activation energy in a chemical reaction.

    • Explain what a reaction mechanism is and understand the concept of rate determining step for a reaction.

    • Write equilibrium expressions, distinguishing molar concentrations of reactants and products for reactions.

  • Ksp and Free Energy

    • Use Le Chatelier’s principle to predict shifts in equilibrium caused by changes in pressure, concentration, and temperature.

    • Write expressions for the solubility product constant (Ksp) and solve problems involving Ksp and ion concentrations.

    • Use Ksp to predict the solubility of compounds.

    • Compare spontaneous and nonspontaneous reactions.

    • Describe and give examples of entropy and describe how enthalpy and entropy affect a reaction's spontaneity.

    • Define free energy and use Gibbs free energy equation to determine whether a reaction is spontaneous.

  • Acids, Bases and Salts

    • Explain Arrhenius acids and bases based on the dissociation of water.

    • Define pH and pOH. Use the pH scale to characterize the acidity and basicity of solutions and properties of acids and bases.

    • Convert between pH, pOH, hydrogen ion concentration and hydroxide ion concentration.

    • Describe Bronsted-Lowry acids and bases.

    • Identify conjugate acids and conjugate bases as well as conjugate pairs in a Bronsted-Lowry acid–base reaction.

    • Describe Lewis acids and bases. [Enrichment]

    • Differentiate between strong and weak acids and bases based on dissociation and ionization.

    • Explain how the acid-dissociation constant, Ka, and the base dissociation constant, Kb, relate to the acid & base strength.

    • Differentiate between the concentration & strength of solutions.

    • Predict the products of acid-base neutralization reactions, and calculate the molar concentrations of acid or base needed.

    • Explain the use of titration in chemistry, and describe the steps of the titration process. Recognize & describe titration graphs for strong and weak acids & bases.

    • Explain hydrolysis (reverse reaction of neutralization). Show how salt solutions can be acidic, neutral, or basic.

    • Explain buffers and write the resulting chemical equations when an acid or base is added to the system.

  • Oxidation-Reduction (REDOX) Reactions

    • Follow rules to assign oxidation numbers to atoms in compounds.

    • Recognize oxidation-reduction (REDOX) reactions and define oxidation and reduction, distinguishing oxidized & reduced species and oxidizing & reducing agents in a REDOX reaction.

    • Write half reactions for oxidation-reduction reactions.

    • Use the half-reaction method to balance oxidation-reduction equations.

    • Use the Electron transfer method/Oxidation number method to balance oxidation-reduction equations.

  • Electrochemistry

    • Define electrochemistry and describe the components of an electrochemical cell.

    • Identify the types of electrochemical cells based on spontaneity.

    • Use the relative strengths of oxidizing and reducing agents to make predictions of an oxidation/reduction reaction.

    • Describe voltaic cells and explain how voltaic cells work.

    • Give examples and a brief description of common voltaic cells.

    • Describe electrolytic cells and compare electrolytic cells with voltaic cells.

    • Describe the electrolytic processes that happens during electroplating and recharging batteries.

2nd

Semester

Organic Chemistry for HONORS only

Objectives:

  • Understand the bonding tendencies of the carbon atom.

  • Define hydrocarbon and identify / distinguish unsaturated hydrocarbons from saturated hydrocarbons.

  • Draw and identify alkanes, alkenes, and alkynes.

  • Describe features and structural characteristics of alkanes, alkenes, and alkynes.

  • Explain organic isomers and illustrate with various compounds.

  • Distinguish the two types of stereoisomers.

  • Identify and describe the general structure of cyclic hydrocarbons with examples.

  • Identify hydrocarbons found in nature and explain their origin and refinement.

  • Classify organic compounds by their functional group.

  • Describe how substitution reactions are used.

  • Identify, draw, and explain the general formula of alcohols, ethers, amines, carboxylic acids, aldehydes, ketones and esters.

  • Describe how polymers are formed.

  • Distinguish addition reactions, dehydrogenation, and condensation reactions and which molecules are involved.

Grade Weighting

10%    Homework

 5%    Participation 

30%   Labs

50%   Unit Tests

  5%   Semester Exam

Unit Assessments

Textbook Reading

Class Notes (Powerpoint)

Notes / Study Guide

Homework (Text or Worksheets)

Lab (Quiz; Worksheet or Report)

Test (Multiple Choice; Problems)

Grading & Unit Assessments

Craig T. Riesen

CTR pic 9 2011.jpg

Certifications

  • Biology

  • Chemistry

  • Physics

  • General Science 7-12

  • Basic Administation K-12

  • Online Instructor

30+ years Teaching Experience

  • Public Schools (26+yr)

  • Online (7+yr)

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