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    • Trimester 1 >
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    • Course Overview
  • APA Reporting
  • Integrated Math
    • Module 1 - Arithmetic Review
    • Module 2 - Know Your Calculator
    • Module 3 - Scientific Notation
    • Module 4 - Significant Figures
    • Module 5 - Units of Measurement
    • Module 6 - Basic Algebra
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General Chemistry

Congratulations on Completing Trimester 1 of Chemistry!

Week 11 Resources/ Assets


Updated November 8, 2018
Please make sure you READ everything on this page or you will miss important details. I will archive past weeks Announcements pages for a limited time only under the Trimester 1 and 2 tabs, if you need to go back to a particular weeks information for any reason.

Week 10 in Review

This last  week we started Chapter 7 - Chemical Quantities. Recollect it is broken down into the following sections:
  • Section 7.1 - The Mole: A Measurement of Matter
  • Section 7.2 - Mole-Mass and Mole-Volume Relationship
  • Section 7.3 - Percent Composition and Chemical Formulas
Hopefully you all remember what a mole is: it is a specific quantity (6.02 x 10^23) that describes how many particles (atoms, ions, formula units, molecules) are in a gram mass of a substance. As an example, one mole of carbon atoms (which has an atomic mass of 12.01 amu) contains 6.02 x 10^23 atoms, and weighs 12.01 grams. In class, we determined the gram mass of sucrose (C12H22O11) by calculating as follows:
  • ​12 carbons x 12.01 amu = 144.12 amu
  • 22 hydrogens x 1.01 amu = 22.22 amu
  • 11 oxygens x 16.0 amu = 176. amu
Making the total gram mass for one mole of sucrose equal to 342 g.
The concept of a mole enables scientists to "count" elements or compounds, by weighing them.

Looking Ahead to Week 11

On Tuesday, we will complete Chapter 7 by looking at mole-mass, and mole-volume relationships. Please feel free to read ahead and solve as many homework problems as you possibly can. Homework for Chapter 7 is not due until you return from Thanksgiving Break, November 27.

Finally, Chapter 7 will be completed learning how to calculate percent composition and empirical formulas. T
he percent composition of a compound, describes the relative amount (by mass) of each element within a compound. As an example, water, with a molar mass of 18.02 g/ mol, has a percent composition by mass of 11.2% hydrogen, and 88.8% oxygen. To calculate the percent composition of hydrogen in water, you divide the number of grams of the element H (2.02 g) by the gram molecular mass of water (18.02 g) =11.2%. Similarly, to calculate the percent composition of oxygen in water, you divide the number of grams of the element O (16.0) by the gram molecular mass of water (18.02 g) = 88.8%. We will go into more detail on this on Tuesday - please note that I have linked a Tyler Dewitt video covering this, at right - I encourage you to watch this. There is another helpful video  right below, explaining h ow to calculate empirical formulas.

On Tuesday, as a class we will carry out the lab,
Small-Scale Lab - Measuring Mass as a Means of Counting. Please print out the lab (linked right) and bring with you to class on Tuesday.

If time permits, we will start Chapter 8 - Chemical Reactions. Chapter 8 is divided accordingly:
  • Section 8.1 - Describing Chemical Change
  • Section 8.2 - Types of Chemical Reactions
  • Section 8.3 - Reactions in Aqueous Solution

The five major classes of chemical reactions are:
  1. Combination (synthesis) reactions
  2. Decomposition Reactions
  3. Single-Replacement Reactions
  4. Double-Replacement Reactions
  5. Combustion Reactions

Chapter 8 is not quite as math-intense as Chapter 7, and I believe you will find it much more interesting, as we learn about these different types of chemical reactions.

Trimester 2 Schedule

I will have the Trimester 2 Schedule prepared before next Tuesday's classes. Please be reminded that what appears on the class webpage always takes priority over the published schedule.

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Chapter 6 Worksheets
Chapter 6 WS Answer Key

So that you are adequately prepared for classes next week, please complete the following:
Tuesday, November 13th:
  1. ​Due in class: Test #2 - covering Chapters 5 and 6
  2. Due in class: Chapter 6 Homework.
  3. Feel free to watch the videos uploaded at right, covering Chapter 7 material.
  4. Print out Lab - Measuring Mass as a Means of Counting (linked below).
Lab - Meas Mass Means Count
Chapter 7 Worksheets
Chapter 7 WS Answer Key
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  • Chemistry
    • Trimester 3 >
      • Chemistry - Week 27
      • Chemistry - Week 26
      • Chemistry - Week 25
      • Chemistry - Week 24
      • Chemistry - Week 23
      • Chemistry - Week 22
      • Chemistry - Week 21
    • Trimester 2 >
      • Chemistry - Week 20
      • Chemistry - Week 18
      • Chemistry - Week 17
      • Chemistry - Week 16
      • Chemistry - Week 15
      • Chemistry - Week 14
      • Chemistry - Week 13
      • Chemistry - Week 12
      • Chemistry - Week 11
    • Trimester 1 >
      • Chemistry - Week 10
      • Chemistry - Week 9
      • Chemistry - Week 8
      • Chemistry - Week 7
      • Chemistry - Week 6
      • Chemistry - Week 5
      • Chemistry - Week 4
      • Chemistry - Week 3
      • Chemistry - Week 2
      • Chemistry - Week 1
    • Course Overview
  • APA Reporting
  • Integrated Math
    • Module 1 - Arithmetic Review
    • Module 2 - Know Your Calculator
    • Module 3 - Scientific Notation
    • Module 4 - Significant Figures
    • Module 5 - Units of Measurement
    • Module 6 - Basic Algebra