Course title
SCCAR and SCCBRPre-requisite
NACourse description
Chemistry
Chemistry A and B
Course Description: Chemistry A and B consist of the fundamental principles of chemistry and their applications. The scientific method; atomic structure; bonding theories; ionic equations; chemical compositions; ; stoichiometry; periodic properties; gas laws; the properties of solids and liquids solution properties; chemical reactions; equilibrium; thermodynamics and nuclear chemistry are taught in the course content. Through the course labs; students will have an opportunity to test and verify ideas and concepts; familiarize themselves with laboratory equipment and the scientific method; and communicate scientific information in a logical manner.
After completing this course; students are able to:
1. State the general purpose for the study of chemistry.
2. List several fields of study where knowledge of chemistry is important.
3. Use scientific units of measurement.
4. Describe the structure and components of basic atoms.
5. Use the periodic table to locate important chemical information.
6. Describe several types of chemical bonds.
7. Manipulate common chemical formulas and equations.
8. List and describe types of chemical reactions.
9. List some physical characteristics of common gases; liquids; and solids.
10. Describe the behavior of solutions and ions.
11. Describe reaction energy and reaction kinetics.
12. Discuss important aspects of nuclear chemistry.
Laboratory descriptions
Observing Changes Lab
Objectives:
? Make observations of each substance used in the lab.
? Make observations of the changes that occur while following each procedure.
? Based on your observations; identify each change as a chemical or physical change. Design a data table that organizes the goals listed above.
? Answer the questions after completing all procedures using complete sentences.
Liquid Density Lab
Objectives:
Lean how to conduct basic measurements using simple lab instruments. We will compute the densities of three different cubes; first by using the less precise methods and instruments and then by using more advanced instruments and techniques.
Students learn to use and read: Mechanical Balance; Graduated Cylinder; Vernier Calipers; and digital balances
Polymer Lab
Objectives:
? To make a polymer using some common household chemicals.
? To manipulate the ratios of the substances used to produce a desired physical property.
? To research polymers and uses of polymers.
? To make a Non-Newtonian fluid and observe its unusual physical properties.
Empirical Lab
Objectives:
Students perform an experiment to
1. Find the percent composition of a hydrate salt.
2. Understand t he meaning of the empirical formula of a chemical compound and calculate the empirical formula of a hydrate slat.
3. Document findings
Stoichiometry Lab ?
Objectives: Calculate theoretical yields of chemical reactions and verify theoretical yields by determining actual values using chemicals in the virtual lab
Acid and Base Lab
Objectives:
? Predict the pH of several different household items before testing them.
? Make an acid-base indicator solution from Red Cabbage.
? Use the indicator solution to test the pH of several household items.
? Compare your predictions with your test results.
? Observe and analyze the color changes associated with a neutralization reaction.
Temp and the Solubility of Salts Lab
Objectives:
? To determine how the solubility of a salt is dependent upon temperature.
? To identify the dissolution of several salts as an endothermic or exothermic process.
? To determine how solubility temperature dependency relates to the endothermic and
exothermic nature of salts.
Chemistry A
Measurement and Density Lab:
In this lab students will use various scientific instruments to identify three mystery elements. To find the identify of these elements students will compute the densities of three cubes; first by using less precise methods and instruments and then by using more advanced instruments and techniques.
Tools that students will use during this scientific investigation are:
? mechanical balance
? graduated cylinder
? vernier caliper
? digital balance
Once students calculate the densities of the cubes using different techniques they will then determine which method is most accurate by calculating the percent error. Student will turn in their completed lab in a lap report along with a set of post lab questions.
Lab Report: Measurement and Density
Your Name: ______________________________________________________________
Purpose of this Lab
What is the goal of this lab? What question are you trying to answer; or what problem are you trying to explain?
Hypothesis
After reading the lab instructions - but before starting the lab - record your best ?educated guess? about what will happen in the experiment. Explain what lead you to this hypothesis.
Experimental Design
List the materials used in this lab; and a brief explanation of the procedures you followed. (You do not need to retype the procedure; simply summarize your procedures). Add #?s where necessary.
Materials:
1.
2.
3.
4.
5.
Procedure (summarize methods used):
1.
2.
3.
4.
5.
Data
Record the data you collect in the lab below. Show all calculations performed in the data analysis section below.
Experiment-1
Measuring densities of the cubes using water overflow method: Low precision method of measuring the density of a substance.
Table for Mechanical Balance:
No. Red Cube Green Cube Blue Cube
1
Table for Graduated cylinder:
No. Red Cube Green Cube Blue Cube
1
2
3
4
5
Average Volume
Cube Mass (in grams) Volume
(cm3) Density( g/ cm3)
=Mass/Volume Element
Present
Red
Green
Blue
Element Standard Density
(g/cm3) Calculated Density
(g/cm3)
Iron 7.8
Copper 8.9
Zinc 7.1
Experiment-2
Measure densities of the cubes using Vernier Calipers and Digital Weighing balance : High precision way of computing the densities.
Table for Digital Balance:
No. Red Cube Green Cube Blue Cube
1
2
3
4
5
Average mass
Table for Vernier Caliper:
No. Red Cube
Length (L) Width (W) Height (H) L x W x H
1
2
3
4
5
Average Volume
No. Green Cube
Length (L) Width (W) Height (H) L x W x H
1
2
3
4
5
Average Volume
No. Blue Cube
Length (L) Width (W) Height (H) L x W x H
1
2
3
4
5
Average Volume
Cube Mass (in grams) Volume
(cm3) Density( g/ cm3)
=Mass/Volume Element
Present
Red
Green
Blue
Element Standard Density
(g/cm3) Calculated Density
(g/cm3)
Iron 7.86
Copper 8.96
Zinc 7.13
Data Analysis
Analyze the data you collected in the lab. Support your calculated densities by showing the calculations that lead you to your results. Calculate your percent error (see explanation below). Compare your percent error from experiment 1 to your percent error in experiment 2
Calculating Percent Error
In most cases; the values you obtain through experimentation will be slightly different from the documented accepted values. Using very precise measuring devices and utilizing the measuring devices correctly reduces the amount of error. The calculation for % error is similar to the calculation you would use to determine your average on an exam. The formula for % error is listed below. Calculate the % error for each substance in experiment 1 and 2.
The accepted values are given in the table above. The experimental values are the values you found in the lab.
Percent Error = Experimental Value ? Accepted Value x 100
Accepted Value
Conclusion
After conducting the experiment; how would you now explain the problem(s) or answer the question(s) raised when you described the purpose of the lab? Be sure to base your answer on the data you collected. Consider whether your conclusion is the only explanation for the data you collected; or if there could be alternate explanations.
Post Lab Questions
Answer the following questions before submitting your report to your teacher. Show all work in all questions requiring calculations. Use the following density table when needed.
Density Table
Substance Density (g/cm3)
Aluminum 2.70
Oak 0.75
Pine 0.42
Polypropylene 0.92
PVC 1.40
Steel 7.9
Water 1.0
Lead 11.4
Bismuth 9.78
1. Suppose you were asked to find the density of a metal object that appears to be a cube. You notice that the metal looks old and has a few chips in it. Without any other information; would it be correct to measure 1 side of the object and cube (^3) the value to determine the volume? Explain.
2. Suppose you determined the density of a cube to be 1.40 g/cm3. Would the density of the cube be different if you had a cube made of the same material with twice as much mass? Explain.
3. A cube with a mass of 0.0084 kilograms has a volume of 20.0 cm3. Using the density table above; identify the object. Don?t forget to convert if needed.
4. A cube of lead is 7.00 centimeters per side. What is the mass of the cube? (See table for density of lead).
5. You fill a graduated cylinder with 50.00 milliliters of water. You drop a piece of aluminum with a mass of 15.00 grams into the graduated cylinder causing the water to rise. What would the new volume of the graduated cylinder be after dropping the aluminum?
6. How many of the substances listed in the density table above would float in water?
Empirical Lab:
Objectives: In this lab; students will perform an experiment to:
1. Find the percent composition of a hydrate salt
2. Understand the meaning of the empirical formula of a chemical compound and calculate the empirical formula of a hydrate salt
Scientific tools and materials used:
? hydrate salts
? desiccator
? crucible
Students will complete lab and calculate the empirical formula for various compounds. Students must submit lab report and pre and post lab questions.
Lab Report: Percent Composition and Empirical Formula of Hydrate
Your Name: __________________________________________________________________
Prelab Questions
Answer each of the following before starting the lab. Some of your answers will be used throughout the lab. You may enter the data for these questions directly into data table 1 in the report below.
1. Differentiate between a hydrated salt and an anhydrous salt.
2. Calculate the formula weight of H2O. (Data Table 1)
3. Calculate the formula weight of each of the following anhydrous salts. (Data Table 1).
CuSO4 NiCl2 CoCl2 CuCl2 MgSO4
Purpose of this Lab
What is the goal of this lab? What question is it trying to answer; or what problem is it trying to explain?
Hypothesis
After reading the lab instructions - but before starting the lab - record your best ?educated guess? about what will happen in the experiment. Give your reasons and outline any assumptions that lead you to this hypothesis.
Experimental Design
List the materials used in this lab; and the procedure you followed.
Materials:
1.
2.
3.
Procedure (list steps in the order in which you performed them):
1.
2.
3.
Data
Record the data you collected in the lab.
Percent water Composition of a Hydrate / Empirical Formula
Experiment 1:
? Find the percent composition of a hydrate salt.
? Understand the meaning of empirical formula of a chemical compound and calculate the empirical formula of a hydrate salt.
Data Table 1:
S.No. Formula of anhydrous salt Formula wt. of anhydrous salt
Formula wt. of water Mass of crucible+ cover
(in g) ?a? Mass of crucible + cover
+ sample before heating
(in g) ?b? Mass of crucible + cover
+ sample after heating
(in g) ?c?
1.
2.
3.
4.
5.
Data Table 2:
Weight Of Anhydrous Salt in grams
(w1 = c-a ) Number of moles[nsalt] of the anhydrous salt [=w1/formula weight] Number of grams of water in grams (w2 = b ? c) Moles (nwater) of water in hydrate sample = w2/ formula wt. of water Moles of water associated with 1 mole of the anhydrous salt Empirical formula for the hydrate.
CALCULATIONS:
Empirical Formula Calculation
1. Calculate the number of grams [w1] of the anhydrous salt you prepared. This is a simple subtraction from your data. (w1 = c ? a)
2. From the number of grams of the anhydrous salt in step 1; calculate the number of moles[nsalt] of the anhydrous salt you prepared [=w1/formula weight]
3. Calculate number of grams of water [w2] in your hydrate sample. This is the difference in mass; between the hydrate and the anhydrous salt. (w2 = b ? c)
4. Calculate moles of water[nwater] in your hydrate sample = w2/ formula wt. of water.
5. Calculate number of moles of water associated with 1 mole of the anhydrous salt = Number of moles of water / Number of moles of anhydrous salt. (nwater / nsalt)
REMEMBER; we cannot use part of a water molecule; so round your answer to the nearest whole number.
Shoe work here:
Analysis
Using your data above; you can determine how much water evaporated from each of the hydrated salts. This allows you to determine the percent of water that was present before evaporation in each of the hydrates. This is the experimental percent composition of water. Using the true empirical formulas of each hydrated salt (listed below in order from left to right on lab bench); the expected percent of water in each of the hydrated salts can be determined. This is the actual percent composition of water. The experimental value and the actual value of each salt can be used to determine the percent error that resulted in the lab. Use the steps and the table below to determine the percent error for each of the hydrates.
1. Calculate the mass of the hydrated salt (x). This is a simple subtraction from your data (b-a).
2. Calculate the mass of water lost as a result of heating the substance. This is also a simple subtraction from your data (b-c).
3. Calculate the experimental percent composition of water using the formula below.
Experimental % Comp. of water = (Mass of water / Mass of Hydrate) x 100.
4. Use the true chemical formula of each hydrated salt to determine the actual percent
composition of water.
Actual % Comp. of water = (Mass of water in true formula / Mass of Hydrate) x 100.
5. Use the values from steps 3 and 4 to determine the percent error for each salt.
Percent Error = Experimental Value ? Accepted Value x 100
Accepted Value
Data Table 3:
True Formula of Hydrate Experimental % of water Accepted % of water % Error
CuSO4 ? 5H2O
NiCl2 ? 6H2O
CoCl2 ? 6H2O
CuCl2 ? 2H2O
MgSO4 ? 7H2O
Show work here:
Conclusion
After conducting the experiment; how would you now explain the problem(s) or answer the question(s) raised when you described the purpose of the lab? Be sure to base your answer on the data you collected. Consider whether your conclusion is the only explanation for the data you collected; or if there could be alternate explanations.
Post Lab Questions:
1. In an actual laboratory setting; the best method for performing this lab would be to perform the evaporation and weighing of the salt 3 times. In doing so; the goal is to end up with a constant mass. Explain why this important.
2. Some experimental error exists in the performance of all labs. Describe 2 possible sources of error in this lab. (Calculation errors are not acceptable answers).
3. Popcorn kernels are made mostly of starch and water. The water is found between the kernels of starch. Explain a procedure that you could use to determine the percent composition of water in popcorn.
Chemistry B
Acid-Base Indicator Tests Lab:
Objectives:
? Predict the pH of several different household items before testing them.
? Make an acid-base indicator solution from Red Cabbage.
? Use the indicator solution to test the pH of several household items.
? Compare your predictions with your test results.
? Observe and analyze the color changes associated with a neutralization reaction.
Using several household substances and household supplies student will conduct an experiment to determine their pH balances.
Procedure:
1. Using a cutting board and a sharp knife; carefully chop up 2 cups (475 mL) of red cabbage.
2. Pour the chopped cabbage into a blender. If you don?t have access to a blender; you can chop the cabbage up into very small pieces and move to step 4.
3. Blend the ingredients for about 2 minutes.
4. Pour the chopped or blended cabbage into a large cup.
5. Pour approximately 1.5 cups (350 mL) of hot water into the cup so it covers the red cabbage and stir well.
6. Let the cup sit for about 10 minutes.
7. Using a sieve or a strainer; strain the red cabbage liquid extract into a second large cup.
1. Obtain 13 white; plastic cups. Small Dixie cups will work well.
2. Label the cups with a marker from A-L. Label an additional cup as ?Control?.
3. Pour 1 tbsp (about 15 mL) of the indicator solution into the cup labeled ?Control?.
4. Predict whether each substance in the list below is an acid or base.
5. Write A or B on the bottom of the cup based on your prediction.
6. Add 1 tablespoon of each of the substances listed below to the labeled cups.
7. Add 1 tablespoon of the indicator solution to cup A and record your observations.
8. Repeat step 6 until all substances are tested (see Notes below).
9. Determine whether each substance is acidic or basic based on the color change.
10. Compare your results to your predictions in step 4.
11. Save the cups and solutions for part C
12. Add 4 additional tablespoons (60 mL) of Vinegar to cup A.
13. Add 1 additional tablespoon (15 mL) of Ammonia solution to cup K.
14. Slowly pour a small amount of the vinegar in cup A into cup K and observe.
15. Very slowly; pour the rest of cup A into cup K and observe.
16. Explain the color changes observed in step 4.
17. Use cup H to neutralize an acid other than vinegar.
18. Explain in the analysis section of your report sheet how your observations are similar to using Tums to rid of heartburn (see analysis section of report sheet).
Lab Report: Acid-Base Indicator Test
Your Name: __________________________________________________________________
Purpose of this Lab
Hypothesis
After reading the lab instructions - but before starting the lab - record your best ?educated guess? about what will happen in the experiment. Give your reasons and outline any assumptions that lead you to this hypothesis.
Experimental Design
List the materials used in this lab; and the procedure you followed.
Materials:
1. Several Household Items (see list below).
2.
3.
Procedure (summarize each part):
1.
2.
3.
Data and Observations
Record the observations you made in the lab.
Part B: Acid-Base Tests of Household Solutions
Material Color-Indicator Added Approximate pH Acid or Base
Part C: Acid-Base Neutralization
Describe what you observed when you mixed the vinegar with the ammonia solution.
Describe what you observed when you mixed the Tums with one of the acids.
Analysis
Analyze the data you collected in the lab by answering the following questions.
1. Did all of the ?acid or base? predictions you made prior to the lab match the identifications you made during the lab?
2. In each of the substances; at least one ingredient contributes to the acid or base nature of the substance. Choose 5 of the 12 substances to research on the Internet. Identify the chemical name and chemical formula of the ingredient that makes the substance acidic or basic. List the 5 substances; the formulas; and the names below.
3. Many people believe that all acids are dangerous. Using your observations made in the lab; write one paragraph that explains why this is not completely true.
4. A friend who knows you are taking Chemistry asks you to explain to them how Tums help neutralize heartburn. Write a detailed explanation of the Chemistry involved. In your explanation; make sure address the following:
A. The type of chemical name and formula of stomach acid.
B. The function of stomach acid.
C. How stomach acid relates to heartburn.
D. How Tums help relieve heartburn.
E. Write an equation that demonstrates the reaction of an acid and base that relates to part D.
Conclusion
After conducting the experiment; how would you now explain the problem(s) or answer the question(s) raised when you described the purpose of the lab? Be sure to base your answer on the data you collected. Consider whether your conclusion is the only explanation for the data you collected; or if there could be alternate explanations.
Stoichiometry Lab:
In this virtual lab students will calculate the molar masses of various substances and conduct various stoichiometric calculations in order to solve problems in this virtual laboratory.
Link to virtual Lab: Chemcollective.org
Lab Report: [Stoichiometry Lab]
Your Name: __________________________________________________________________
Pre-lab Questions:
1. Using a period table; calculate the molar masses of the following: (you will need the molar
masses of some of these substances throughout the lab).
Periodic table: http://www.public.asu.edu/~dmatyus/teaching/chm101/periodic_table.gif
AgNO3 __________ AgCl __________ NaCl __________ KI ___________ PbI2 __________
2. A solution of potassium iodide reacts with a solution of Lead(II) nitrate to form solid
Lead(II) iodide and aqueous potassium nitrate according to the reaction below.
KI (aq) + Pb(NO3)2 (aq) ? PbI2 (s) + KNO3(aq)
How many grams of solid PbI2 can be produced if 5.00 grams of KI reacts with excess Pb(NO3)2?
(Show all work below)
Purpose of this Lab
What is the goal of this lab? What question is it trying to answer; or what problem is it trying to explain?
Hypothesis
After reading the lab procedure - but before starting the lab - record your best ?educated guess? about what will happen in each part of the experiment. Give your reasons and outline any assumptions that lead you to this hypothesis. You do not need to show calculations here. Simply state how the concepts you learned in this unit will help you solve these problems.
1)
2)
3)
Experimental Design
List all materials and equipment used in this lab; and the procedures you followed for each experiment. Add numbers below if needed.
Materials:
1.
2.
3.
4.
5.
Procedure for 2b (list steps in the order in which you performed them); add numbers if needed.
1.
2.
3.
Procedure for 3b (list steps in the order in which you performed them): add numbers if needed.
1.
2.
3.
Procedure for 3b (list steps in the order in which you performed them): add numbers if needed.
1.
2.
3.
Data
Record the data you collected in the lab on the lines provided. Show any calculations needed.
1a. mass of Na+ ______________
mass of Cl- ______________
1b. mass of Ag+ ______________
mass of NO3- ______________
1c. mass of Na+ ______________
mass of Cl- ______________
mass of Ag+ ______________
mass of NO3- ______________
mass of AgCl ______________
2a. mass of silver nitrate required _________________ (show all work below and circle answer)
2b. mass of Ag+ ______________
mass of Cl- ______________
2c. Note: This is not listed in the procedure; but should be completed.
In the solution viewer; click solid to determine how many grams of AgCl were formed by the
addition of 2.00 grams of NaCl to the AgNO3.
Mass of AgCl ______________
2d. Using the balanced equation provided in the lab and stoichiometry; show the calculation that indicates the maximum amount of AgCl that can be produced from 2.00 grams of NaCl.
3a. mass of AgCl _____________ (Show stoichiometric calculations below).
3b. mass of AgCl produced in virtual lab ______________
(Don?t forget to explain steps above in the procedure section of the report).
3c. Choose your own values for the stoichiometry problem listed below. Use values other than the values already used in this lab. Calculate the theoretical yields of your product and investigate the reaction in the virtual lab. Use the following sentence to help you write your question. Show all calculations and write the procedure you used in the lab to determine your actual product.
Sentence: ___________ grams of NaCl react with excess AgNO3;
Question: How many grams of solid AgCl are produced in this reaction? _____________
(Show calculations below).
Conclusion
After conducting the experiment; how would you now explain the problem(s) or answer the question(s) raised when you described the purpose of the lab? Be sure to base your answer on the data you collected. Consider whether your conclusion is the only explanation for the data you collected; or if there could be alternate explanations.
School Country
United StatesSchool state
ArizonaSchool city
TempeHigh school
Pinnacle Online High SchoolSchool Address
N/ASchool zip code
85282Requested competency code
Lab ScienceDate submitted
Approved
YesApproved competency code
- LCHM
- Chemistry