Course title
720 ChemistryPre-requisite
N/ACourse description
Paradise Valley Unified School District Online Course
pvONLINE
INTRODUCTION TO CHEMISTRY - 720
COURSE EXPECTATIONS AND GOALS
This course will cover concepts and theories relating to the scientific field of Chemistry. Experiments and activities are used to introduce concepts including the structure of atoms and chemical compounds; the relationships among the elements on the periodic table; chemical and physical transformations; and the measurement and calculations of chemical quantities. Students who complete this course will develop an understanding of interconnections among the sciences; technology; society; and the environment. Mostly; we will try to understand; a little better; this wonderful; amazing world of ours.
This course explores the fundamentals of chemistry without heavy emphasis on mathematics. It is recommended for those students who plan to enter junior colleges and/or who plan to pursue non-science careers at the college level.
Coursework
Assignments (computer-graded and teacher-graded)
Quizzes/Tests (computer-graded and teacher-graded): One attempt is given with a 60 minute time limit.
Final Exam
When you complete all of the coursework and your instructor has reviewed it; you will be given permission to take the final exam.
Role of Homework
Chemistry is very much a participatory sport. Complete the assignments in the order listed. There will be laboratories based on the chapters in the book and lab write-ups will be submitted for grading. I strongly urge you to keep your problems in an orderly fashion in a notebook. This notebook facilitates study for tests and final exams.
The online textbook we use is called Prentice Hall Chemistry.
Grading
Tests will be given at the end of each chapter; or at the end of two chapters. Tests will count for 56 percent of your grade; laboratory and homework 24 percent; and your final will be 20 percent of your grade.
Intro Chemistry I –
Unit I – Matter and Change
a. Matter
b. Elements; mixtures and compounds/
c. Physical and Chemical change
*Lab - Classifying Matter - Hand on lab
*Lab - Separating Mixtures - Hands on lab
Unit 2 - Atomic Structure
a. Dalton’s Theory
b. The History of the Development of the Atom
c. The Structure of the Atom
Lab – PhET Simulations......Build an Atom
Unit 3 - Electrons in Atoms & the Periodic Table
a. The Bohr Model of the Atom
b. History of the Periodic Table
c. Periodic Trends - atomic radii; ionization energy; ionic radii; electron affinity
*Lab - Atomic Emission Spectra - Hands on Lab
Unit 4 - Chemical Bonding
a. Describe ionic and covalent bonding.
b. Use the octet rule to write Lewis structures.
c. Explain how to determine Lewis structures for molecules containing single bonds; multiple bonds; or both.
d. List and compare the distinctive properties of ionic and molecular compounds.
*Lab - Solutions Containing Ions - Hands on Lab
Unit 5 - Chemical Formulas and Chemical Compounds
a. Name an ionic compound given its formula.
b. Using prefixes; name a binary molecular compound from its formula.
c. Calculate the formula mass or molar mass of any given compound.
d. Use molar mass to convert between mass in grams and amount in moles of a chemical compound.
e. Calculate the number of molecules; formula units or ions in a given molar amount of a chemical compound.
Unit 6 - Chemical Equations & Reactions
a. Balance a formula equation.
b. Classify a reaction as synthesis; decomposition; single-displacement; double-displacement; or combustion reaction.
c. Predicts the products of simple reactions given the reactants.
d. Use an activity series to predict whether a given reaction will occur and what products will be.
Lab – PhET Simulations......Balancing Equations
VLab - SAS Pathways Precipitation Reactions
Intro Chemistry II –
Unit 1 - Stoichiometry
a. Determine the number of moles or atoms in a sample when given the mass.
b. Write a mole ratio relating two substances in a chemical equation.
c. Calculate the amount in moles or mass of a reactant or product from the amount in moles or mass of a different reactant or product.
d. Calculate the amount in moles or mass in grams of a product; given the amounts in moles or masses in grams of two reactants; one of which is in excess.
Lab – PhET Simulations......Basic Stoichiometry
Unit 2 - States of Matter
a. State the kinetic molecular theory of matter and describe how it explains certain properties of matter.
b. Explain the relationship between equilibrium and changes of state.
c. Interpret phase diagrams.
d. Describe the processes of boiling; freezing; melting and sublimation.
*Lab - The Behavior of Liquids and Solids - Hands on Lab
Unit 3 - Gases
a. Use the kinetic molecular theory to explain relationships between gas volume; temperature and pressure.
b. Use Boyle’s law; Charles’s law; and Gay Lussac’s law to calculate pressure; volume and temperature changes.
c. Use the combined gas law to calculate volume-temperature-pressure changes.
d. Define standard molar volume of a gas and use it to calculate gas masses and volumes.
e. Using the ideal gas law; calculate pressure; volume; temperature; or amount of gas when the other three quantities are known.
*Lab - Carbon Dioxide from Antacid Tablets - Hands on Lab
Unit 4 - Solutions
a. Distinguish between electrolytes and nonelectrolytes.
b. List and explain three factors that affect the rate at which a solid solute dissolves in a liquid solvent.
c. Explain solution equilibrium and distinguish among saturated; unsaturated; and supersaturated solutions.
d. Given the mass of solute and volume of solvent; calculate the concentration of a solution.
*Lab - Surfactants - Hands on Lab
Unit 5 - Acids and Bases
a. Name common binary acids and oxyacids; given their chemical formulas.
b. Explain the differences between strong and weak acids and bases.
c. Describe a conjugate acid and conjugate base.
d. Explain the process of neutralization.
e. Explain and use the pH scale.
f. Find [H3O+] or [OH-] or pH given the other two.
*Labs - Indicators from Natural Sources - Hands on Lab
Unit 6 - Thermochemistry
a. Define heat and state its units.
b. Perform specific-heat calculations.
c. Explain enthalpy change; enthalpy of reaction; and enthalpy of combustion.
Example Labs
HANDS ON EXAMPLE - 2
Carbon Dioxide from Antacid Tablets
Purpose -
To measure the amount of carbon dioxide gas given off when antacid tablets dissolve in water.
Materials -
6 effervescent antacid tablets
3 rubber balloons (spherical)
plastic medicine dropper
water
clock or watch
metric tape measure
graph paper
Procedure -
1. Break six antacid tablets into small pieces. Keep the pieces from each tablet in a separate pile. Put the pieces from one tablet into the first balloon. Put the pieces form two tablets into a second balloon. Put the pieces from three tablets into a third balloon.
Caution If you are allergic to latex; do not handle the balloons.
2. After you use the medicine dropper to squirt about 5 mL of cold water into each balloon; immediately tie of the balloon.
3. Shake the balloons to mix the contents. Allow the contents to warm to room temperature.
4. Measure and record the circumference of each balloon several times during the next 20 minutes.
5. Use the maximum circumference of each balloon to calculate its volume. (Hint: Volume of a sphere = 4/3r3)
Analyze and Conclude -
1. Make a graph of volume versus number of tablets. Use your graph to describe the relationship between the number of tablets used and the volume of the balloon.
2. Assume the balloon is filled with carbon dioxide at 200C and standard pressure. Calculate the mass and the number of moles of CO2 in each balloon at maximum inflation.
3. If a typical antacid tablet contains 2.0 g of sodium hydrogen carbonate; how many moles of CO2 should one tablet yield? Compare this theoretical value with your results.
Example - Virtual lab
VLab: Precipitation Reactions: Data & Observations
Navigate to:
http://www.sascurriculumpathways.com/portal/#/search?searchString=&searc...
Enter 867 GO
There are thirty-five combinations of aqueous solutions for you to investigate. (Note Table 1 on the Data Sheet.) Some of these combinations will produce precipitates; others will not.
Step-by-step instructions for experimenting with the first combination (AgNO3 and NaCl) are listed below.
For the first solution; select AgNO3.
For the second solution; select NaCl.
The Erlenmeyer flasks that appear are filled with the two aqueous solutions.
Note the color of each solution. This information has already been recorded for you in Table 1.
If a reaction were to occur between these two aqueous solutions; what would the products be?
(Given your knowledge of exchange reactions; you should expect the products to be NaNO3 and AgCl.)
Begin building the chemical equation by dragging a sodium ion to the first product box and a nitrate ion to the second product box. Place your cursor over each ion to display its charge. Since these ions have equal but opposite charges (+1 and -1); you do not need to drag any additional ions to this area. NaNO3 is a valid chemical formula.
Finish building the chemical equation by dragging a silver ion and a chloride ion to the third and fourth product boxes; respectively. These two ions also have equal but opposite charges (+1 and -1); so you have produced another valid chemical formula.
Balance the chemical equation by selecting any needed coefficients. For this example; the equation is already balanced. (The simulation recognizes blanks as coefficients of "1.")
Select the Check button to check your work. If your product(s) had been incorrect; the product box(es) would have turned red. Likewise; any incorrect coefficients would have turned red.
Now; select the React button to see what actually happens when aqueous solutions of AgNO3 and NaCl are combined. It turns out that combining aqueous solutions of AgNO3 and NaCl does produce a precipitate.
c. In the first block of Table 1; note the color of this precipitate.
Notice the chemical equation at the end of the video. Since a precipitate forms; the product ions for the insoluble compound are shown as a molecule (rather than separate ions). Thus; you can see that the precipitate for this reaction is AgCl.
In the first block of Table 1; record the formula for this precipitate.
Write the complete balanced equation for this reaction. Indicate the state of each compound (aqueous or solid).
Continue experimenting with the remaining solution combinations. For each:
Note the color of each solution.
Record these colors in Table 1.
Build and balance the chemical equation for the predicted reaction.
Click the Check button to check your work. Make corrections as needed and click the Check button again.
Once you have built the correct chemical equation; select the React button.
Record your observations in Table 1. If a precipitate forms; indicate its color and formula. If no visible reaction occurs; write "NR."
When a combination yields a precipitate; write the complete balanced equation. Label each compound as aqueous or solid.
Table 1:
Solution 2
Solution 1
NaCl
colorless
NaF
NaOH
NaClO3
Na2CO3
Na2SO4
Na3PO4
AgNO3
colorless
Ca(NO3)2
Cu(NO3)2
Pb(NO3)2
KNO3
Developing Solubility Rules
Using the simulation; you have explored various precipitation reactions. And you have learned about solubility. Why are some products soluble and others not? You should now be able to develop a list of solubility rules.
Use the information you recorded in Table 1 to complete Table 2 as follows:
Column 2: Indicate whether solutes containing these ions are usually soluble or insoluble.
Column 3: List exceptions. That is; list any ions which; when combined with the Column 1 ions; produce compounds that do not follow the rules you wrote in Column 2. Note that some ions are already listed. (These are ions you did not investigate with the simulation.)
Table 2:
Compounds Containing
Are Usually
(soluble or insoluble)
Exceptions
K+ or Na+
(same rule applies to NH4+)
Cl-
(same rule applies to Br- and I-)
F-
(Sr+2; Ba+2; and Mg+2 are also exceptions.)
NO3- or ClO3-
(same rule applies to ClO4- and C2H3O2-)
SO42-
(Sr+2 and Ba+2 are also exceptions.)
CO3-2 or PO4-3
(same rule applies to C2O4-2; CrO4-2; and S-2)
(NH4+ is also an exception.)
OH-
(same rule applies to O-2)
(NH4+ is also an exception.)
Using Solubility Rules
Refer to Table 2 as you predict whether precipitation reactions will occur when the following aqueous solutions are combined. If you think a reaction will occur; write the balanced chemical equation. For each product; indicate whether it's solid or aqueous. If you think a reaction will not occur; write "NR."
FeCl3(aq) + NaOH(aq)
NH4NO3(aq) + K2CrO4(aq)
LiBr(aq) + AgNO3(aq) (Hint: You would expect lithium to react similarly to what other elements?)
BaCl2(aq) + Na2SO4(aq)
CuSO4(aq) + NH4Cl(aq)
KCl(aq) + Pb(NO3)2(aq)
CaCl2(aq) + Na2CO3(aq)
Na3PO4(aq) + Ni(NO3)2(aq)
(NH4)2C2O4(aq) + Na2O(aq)
Ca(C2H3O2)2(aq) + KF(aq)
Identifying Unknowns
With your list of solubility rules; you can predict what will happen when two aqueous solutions are combined. But can you identify unknown solutions? You can if you apply what you've learned about the physical characteristics of the precipitates that form from the reactions you've studied. These characteristics can help you identify solutes found in aqueous solutions. Consider the following problem:
Two days ago; Mr. Jones; a chemistry teacher at Somewhere High School; made six aqueous solutions in preparation for tomorrow's lab (Pb(NO3)2; KNO3; AgNO3; Na2CO3; NaOH; and Na3PO4). His students will be investigating precipitation reactions; just as you did using the simulation. This afternoon; Mr. Jones realized he made a mistake when he prepared the solutions. He was in such a hurry to get to the student council meeting (since he is the advisor) that he forgot to label the solutions. He attached the labels to each of the flasks; but he never wrote in the chemical formulas. For now; he has labeled them A-F.
Fortunately; Mr. Jones has come up with a solution to his "solution problem." Using a 36-well microplate; he reacted two drops of Solution A with two drops of each of the other solutions. He repeated this process for Solution B; Solution C; and so on; yielding the results shown below.
Unfortunately; Mr. Jones did not have time to analyze these results and needs your help. (He had to leave to meet with the principal to discuss the upcoming school dance.)
Given the results Mr. Jones obtained; and the information you recorded in Table 1; determine the identities of the unknown aqueous solutions. Record your answers in Table 3.
Explain the process by which you identified the solutions.
Table 3: Solutions and Identities
Solution A
Solution B
Solution C
Solution D
Solution E
Solution F
School country
United StatesSchool state
ArizonaSchool city
PhoenixSchool / district Address
15002 N 32nd Street Phoenix, AZSchool zip code
85032Requested competency code
Lab ScienceDate submitted
Approved
YesApproved competency code
- LCHM
- Chemistry