2009 Summer Assignment

AP Chemistry

Please visit the GC-ISD website, locate CHHS, Science
Department, and select Ponzell Goff’s website. Click on AP Chemistry Lesson Plans for your summer assignment.

http://www.gcisd-k12.org/

Your summer assignment is designed to help you review your first year chemistry and to prepare you for the Unit 1 test which will be given on the 5th day of class (approximately the 2nd week of class). The first 3 chapters in the AP Chemistry textbook will be the test material for the Unit 1 test. Since you will not be able to pick up your textbook until the week before school starts, the website that accompanies the chemistry text that we use in class is located at the website given below.

Chapters 1, 2 and 3 are available at this website:

http://wps.prenhall.com/esm_brown_chemistry_9/

Open the website,

upper left-hand corner is the pull down menu for the chapters, select chapter

upper left will be select location menu

select the information you need to review.

Please complete the summer assignment prior to school starting in the fall.

Thank you,

Mrs. Ponzell Goff

WKS 1-1 CHEMISTRY SCAVENGER HUNT (1 pg.)

The following list of chemical compounds are found in common everyday products which are found in the kitchen, the garage, the bathroom or the laundry room. The compound listed may be the ONLY ingredient or it may be listed as the 1st, 2nd, or 3rd ingredient in the product. Write the brand name of the substance in which each of the following is found (more than one answer is correct on many of these).

1. acetaminophen ______

2. acetone ______

3. acetylsalicylic acid ______

4. boric acid ______

5. benzoyl peroxide ______

6. butyl acetate ______

7. dihydroxy aluminum sodium carbonate ______

8. ethanol or ethyl alcohol ______

9. ethylene glycol ______

10. glycerine ______

11. isopropyl alcohol or isopropanol ______

12. magnesium aluminum hydroxide ______

13. magnesium hydroxide ______

14. magnesium sulfate ______

15. monosodium glutamate ______

16. phenolphthalein ______

17. sodium bicarbonate ______

18. sodium bisulfate or sodium hydrogen sulfate ______

19. sodium hydroxide ______

20. sodium hypochlorite ______

21. sodium fluoride or stannous fluoride ______

22. sodium saccharin ______

23. ammonium nitrate ______

WKS 1.2 Measurement, Accuracy, Precision (2 pgs.)

1. Measure the following glassware to the correct number of significant figures (all certain plus one estimated). Include appropriate metric units.

A. Graduated Cylinders:

a. ______b. ______c. ______d.______

B. Burets C. Beaker

a. ______b. ______a. ______

D. Rulers

a. ______b. ______c. ______

E. Thermometers (Celsius)

WKS 1.2 cont.

a) ______b) ______c) ______

2. Write down the uncertain digit for the following mass measurements.

______a. 2.42 g ______c. 0.043 g

______b. 103 g ______d. 6.0 g

3. Four groups of students collected three sets of data to determine the melting point of naphthalene (moth balls). The accepted melting point is 79.0oC. Indicate whether the following sets of data are precise, accurate, both, or neither.

______Group One: 76.2oC, 79.5oC, 81.3oC

______Group Two: 76.2oC, 76.1oC, 76.3oC

______Group Three: 76.4oC, 82.8oC, 81.2oC

______Group Four: 79.1oC, 78.90C, 79.2oC

4. Label the following as either mistakes (M) or experimental errors (E)

______assumed the temperature of the water was equal to the temperature of the gas.

______accidentally added too much NaOH

______assumed the temperature was constant throughout the experiment.

______could not remove all air from the graduated cylinder

______dropped the crucible

______there was human error involved in determining the color of the solution

WKS 1-3 PERCENT ERROR (2 pgs.)

1. John uses his thermometer and finds the boiling point of ethyl alcohol to be 75.5ºC. He looks in a reference book and discovers that the actual boiling point of ethyl alcohol is 78.3ºC. What is the percent error?

2. Anna weighed an object on her balance and recorded a mass of 24.20 grams. Her teacher told her that there was probably something wrong with her balance because she was 33.2% too high in the mass she found. What was the actual mass of the object?

3. The density of water at 4ºC is known to be 1.00 g/cm3. Kim experimentally found the density of water to be 1.085 g/cm3. What is her percent error? ( 8.5% error)

4. Florence measured the volume of a cylinder and determined it to be 54.5 cm3. The teacher told her that she was 4.65% too high in her determination of the volume. What is the actual volume of the cylinder? (52.1 cm3)

5. Barry Um receives a laboratory report back with a “+2.77% error” written on it. He had found the mass of an object to be 100.30 grams. What is the actual mass of the object? (103 g)

WK 1-4 PHYSICAL VS CHEMICAL CHANGES (3 pgs)

In a physical change, the original substance still exists. It has only changed in form. IN a chemical change, a new substance is produced. Energy changes always accompany chemical changes.

Classify the following as being a physical or chemical change.

1. Sodium hydroxide dissolves in water. ______(endothermic or exothermic)

2. Hydrochloric acid reacts with potassium hydroxide to produce a salt, water and heat. ______.

3. A pellet of sodium is sliced in two. ______

4. Water is heated and changed to steam. ______

5. Potassium chlorate decomposes to potassium chloride and oxygen gas. ______

6. Iron rusts. ______

7. When placed in H2O, a sodium pellet catches on fire as hydrogen gas is liberated and sodium hydroxide forms. ______

8. Evaporation. ______(endothermic or exothermic)

9. Ice melting. ______(endothermic or exothermic)

10. Sugar dissolves in water. ______

11. Wood rotting. ______

12. A tire is inflated with air. ______

13. Food is digested in the stomach. ______

14. Water is absorbed by a paper towel. ______

15. Hydrogen is burned and produces water vapor.______

16. Cobalt solution turns blue when heated.______

17. When iron (III) chloride reacts with potassium thiocyanate a blood red substance is produced. ______

PHYSICAL VS CHEMICAL PROPERTIES

A physical property is observed with the senses and can be determined without destroying the object. For example, color, shape, mass, length and odor are all examples of physical properties.

A chemical property indicates how a substance reacts with something else. The original substance is fundamentally changed in observing a chemical property. For example, the ability of iron to rust is a chemical property. The iron has reacted with oxygen, and the original iron metal is changed. It now exists as iron oxide, a different substance.

Classify the following properties as either chemical or physical by putting a check in the appropriate column.

WKS 1.5 cont.

Physical Property / Chemical Property
Blue color
Density
Flammability
Solubility
Reacts with acid to form H2
Supports combustion
Sour taste
Melting point
Reacts with water to form a gas
Reacts with a base to form water
Boiling point
Can neutralize a base
Luster
Odor

MATTER-SUBSTANCES VS MIXTURES

All matter can be classified as either a substance (element or compound) or a mixture (heterogeneous or homogeneous)

Matter

______½______

½ ½

Substance Mixtures

Can write chemical formula variable ratios ______½______½______½ ½ ½ ½

Element Compound Homogeneous Heterogeneous

One type two or more different solutions colloids

atom atoms chemically bonded suspensions

Classify each of the following as to whether it is a substance or a mixture. If it is a substance, write Element or Compound in the substance column. If it is a mixture, write Heterogeneous or Homogeneous in the mixture column.

Type of Matter / Substance / Mixture
1. Chlorine
2. Water
3. Soil
4. Sugar water
5. Oxygen
6. Carbon dioxide
7. Rocky Road Ice cream
8. Alcohol
9. Pure air
10. Iron