AP Chemistry Summer Assignment

AP Chemistry Summer Assignment Required Text Chemistry by Zumdahl AP Edition (This book will be provided in the beginning of the school year) Kaplan AP Chemistry Book 2015-2016 (You will need this book for the summer homework assignments as well as throughout the year. We recommend you preorder this book on Amazon.com, for example). Recommended Text Cracking the AP Chemistry Exam by Princeton Review 2016 edition Handouts Handouts are posted the Lane Tech website. A hardcopy of the handout packet will be provided for summer homework. Instructions will be emailed to you. Homework Policy Homework will be collected on the first day of school after summer break. On the first day of school, you should also be prepared for a quiz on 1 & 2 from the Kaplan book. Teacher contact information Please feel free to email us with questions or concerns Mr. Bartlet [email protected] Mr. Kopack, NBCT [email protected] Mr. Reid, NBCT [email protected]

Homework Assignments The assignments below are intended to be a review over the summer. You may wish to look over the sample problems to help you. For each problem you must use units, show your work, include significant figures, and provide complete sentences (when asked to explain). Please DO NOT Write Out The Questions! Week #

Homework Assignment

1

 Read “Why Do I have to Study Chemistry” Article Posted Online  Review Naming Compounds Flow Chart & Predicting Products Handout

2 3

4

 Make Flash Cards and Memorize the Solubility Rules Handout  Make Flash Cards and Memorize the VSEPR Chart Handout  Answer the Free Response Question Posted Online.  Answer Multiple Choice Questions Posted Online.  Read Green Chemistry Lab :Analysis of a Mixture (Investigation 7)  Answer Pre-Lab Questions and be prepared to complete the Introductory Activity (Decomposition of Group 1 Bicarbonates) for the first week of class.  Read Chapter 1 and 2 from the Kaplan AP Chemistry Book  Make Flash Cards and Memorize Ions Handout

1

In the 'Cla st-oon-1

Why Do I Have to Study Chemistry? 0. Kenneth Barker Jr.

Chemistry Department, lenape Area Vocational Technical School, 2215 Chaplin Avenue, Ford City, PA 16226-1692; [email protected] 2.pa

Students frequently believe that the study of biology is more relevant to their daily lives than the study of chemistry or physics, As instructors, we face the task of focusing students' attention on the numerous, often subtle, ways that chemistry and physics impact nearly every facet of their daily routines. As a student who majored in both biology and chemistry, and as an instructor of both, I clearly see that chemistry provides more practical explanations of the science and technology that surround us than does biology. In a conversation with an instructor of physics, an article entitled, "Why Do I Have to Study Physics?" was mentioned (1). Offered here is a similar article for instructors of chemistry. Instructors of introductory, general, or consumer chemistry courses for nonmajors, who are most likely very familiar with the question posed in the title of this article, should take interest in the questions posed by the student in the scenario. The text written from the student's point of view could be used as a culminating activity for such classes. One possible activity could be a writing-in-chemistry assignment in which students answer the questions posed in the scenario below It is unlikely that any single reference text or textbook contains the answers to all the questions posed in the scenario. If students were assigned the writing-in-chemistry activity, it is likely that they would need access to a library with fairly extensive references in chemistry.

Oh boy, there's my alarm. Six-thirry, the morning I've dreaded all week—the day of my first big chemistry exam. I should get ready. Where's that toothpaste? Fluoride sounds familiar; I wonder why that's in there. There's baking soda and peroxide too. Why would they put those in toothpaste? It's time for a shower. I wonder why soap and water clean so much better than just plain water. How is shampoo different from soap? I wonder why I feel so cool before I dry off. There's isobutane in this mousse. I wonder if that's anything like the butane in lighters. Why would something like that be in this hair styling stuff? It's time for some tunes. The news is on. They say this beautiful late summer morning will become an ozone action day. I wonder what ozone is. How does it get into the air? Why is it a problem? They keep telling us not to stay out in the sun too long because the ozone layer is disappearing. How can it just disappear, and how is the ozone layer different from the ozone they tell us we shouldn't breathe? I wonder how a sunblock works. I had better turn on the light. I wonder what's in a light bulb that lets it get so hot and still not melt or catch on fire. It's time to check the laundry and get dressed. How does a detergent work? Maybe I'll wear that tie-dyed T-shirt. I wonder how they tie-dye clothing. How do dyes stay on the clothes without coming off onto my skin? Boy, these jeans are really 1300

faded. I wonder what made them fade so much. My socks came out nice and white. What is bleach, and how does it work? My new cross training shoes sure arc comfortable. I wonder how they made that foam rubber. I should fuel up with some breakfast. Maybe I'll fry an egg. I wonder why a fried egg tastes so much better than a raw egg. How does cooking change the egg? It's getting late; I'll just have some orange juice and cereal. Wait, every time I drink orange juice after I brush my teeth, it tastes really strange. I wonder why that is. I think I'll just try the cereal and skip the juice. I know it has vitamin C, but what does that do for me anyway? This cereal is "fortified with iron". I wonder what kind of iron they put in there; it couldn't be those iron filings we used in chemistry lab, could it? This milk has calcium in it; it surely isn't those little lumps we saw bubbling in water the other day in class. The milk says it has vitamin D added. I wonder what vitamin D is and why it's good for me. There's the calorie count. I wonder if that has anything to do with those energy measurements we read about in the chemistry book. Time to leave for school. I hope the car starts this morning. I wonder how a battery works. Oh great, the car needs gas. I'll pull in to the mini-mart and fill up the tank. The pump says something about an octane rating. I wonder what octane is and what that octane rating really means. This gas is unleaded; how could they put lead in gasoline? Why would it be used in gasoline anyway? It looks like that tire is a little low. This pressure gauge is reading lower than it did yesterday afternoon. I wonder if it's because it's so much cooler this morning. Before I leave, I think I'll get a can of soda. Oops, I dropped it; I better not open it until later. I wonder what those bubbles are and how they get them in there. I made it to school on time. It's supposed to be really hot today. I've heard of car windows popping when it gets really hot, so I'd better open them a little bit. I wonder why they sometimes break when the car gets really hot. I'm glad the windows arc coated to shade the inside. That should help, too. I wonder what that coating is, and how they get it in the glass, It sure is bright out this morning; I'm glad my glasses darken in the sun. I wonder how they do that. The air conditioning sure will feel good this afternoon. I'm glad I had my air conditioner fixed. What is the refrigerant that the service technician refilled? I wonder how air conditioning works. Well, here I am in chemistry class. Worrying about this exam is giving me heartburn. I wonder how this antacid works. Why do I have to study chemistry anyway? When will I ever use chemistry in my everyday life? What good is it to me? Why can't I study something that's practical—like biology? Literature Cited I. Gore, G. R. Phys. Mach. 1997, 35, 378.

Journal of Chemical Education • Vol. 77 No. 10 October 2000 • IChemEd.chem.wisc.edu

Chemical Names and Formulas

-

The following chart is designed to help you name simple compounds.

Does it begin with a metal or NH4? No

Yes

It is COVALENT

It is IONIC

Write the name of the first prefix. If the prefix is mono , do not write it down,

Does it begin with a metal from the first two columns of the periodic table, or Al, Cd, Zn, Ag, or NH 4?

Yes

-

No Write the name of the first element.

Write the name of the cation.

Write the name of the cation, followed by its Roman numeral in parentheses.

Write the name of the second prefix.

r Write the name of the anion.

Write the name of the second element.

Change the ending to ide. —

Solubility Rules Table The solubility classification of ionic substances according to their solubility in water is difficult. Nothing is completely "insoluble" in water. The degree of solubility varies from one "soluble" .substance to another. Nevertheless, a solubility classification scheme is useful even though it must be regarded as an approximate guideline. MAINLY WATER SOLUBLE NO3-

All nitrates are soluble.

CH3COO- or C2H302 -

All acetates are soluble except AgCH 3COO*.

3-

C10

All chlorates are soluble. All chlorides are soluble except AgCI, Hg 2C12 PbC12*.

Cl-

All bromides are soluble except AgBr, PbBr 2*, Hg2Br2 and HgBr2 *.

Br I-

All iodides are soluble except AgI, Hg 2I2 , HgI2 and Pb12,

SO 4 2-

•

All sulfates are soluble except BaSO 4, PbSO4, Hg2SO4, CaSO4, Ag2SO4* and SrSO 4*.

Alkali metal cations All are soluble. (Group IA) and NH 4+ ,H+

All common inorganic acids and low molecular mass organic acids are soluble.

MAINLY WATER INSOLUBLE

.

.

CO 3 2-

All carbonates are insoluble except those of the IA elements and NH4+.

Cr() 4 2-

All chromates are insoluble except those of of the IA elements, NH 4+, CaCrO4* and SrCrO4*.

OH -

All hydroxides are insoluble except those of the IA elements, NH 4+, Ba(OH)2, Sr(OH)2 *, and Ca(OH) 2*.

PO 4 3-

All phosphates are insoluble except those of the IA elements and NH 4+.

32-S0 2-

S

All sulfites are insoluble except those of the IA elements and NH 4+. All sulfides are insoluble except those of the IA and IIA elements and NH4+.

*Soluble compounds dissolve to the extent of at least 10 g/L at 25 °C. Slightly soluble compounds (marked with an') dissolve in the range of from 1 g/L to 1C g/L at 25 ''C. Those compounds that have a solubility of less than 1 g/L are considered to be insoluble. These standards are common but arbitrary.

Steric Number --, Lone Pairs

5

6

3

4

sp 3d

sp'

sip'

sp

4/

90°

90°,(129 °

109.5 °

120 °

tao°

0

Octahedral

Trigonal Bipyramidal

Tetrahedral

Togonal Planar

Linear

. • •

AD

0-0-0

Q Non-Polar

Non-Polar

SquarePyramidal

Seesa 114

(distorted

•

.-

2

NOn-Polar

Non-Polar

Non-Polar

Trigenal Pyramidal

Bent

Linear

..•

••

Q(Cl°

0):::INO

Polar

Polar

Polar

Square Planar

T-Shaped

Bent

linear

.. ••!

...

Non-Polar

Po1ar

Polar

T-Shaped

Linear

Linear

Non-Polar

Linear

Linear

,. 7. . .;

1

.1'4.

U

Non-Polar

5

...„...0. Pole

C, ,emistri

•

NI

Geometries

i• Polar

is

w

ybridIzatIons

Polar

4/

0 0

Linear •!.......t.

REM E

Polar

w

••

0 Polar

MI

.;:c)—4-3

. 0/19..,...

Polar

A

0

.•

. .4 _L P:

Linear

Polar

...

0.4?:..!. 46 ''

undefined

Advance

A POlar

3 4

•

1

2

sp3d 2

And Angi Es

,

0—

0

0- 0

N

Period

Name

NET IONIC EQUATIONS WORKSHEET #1 For each of the following reactions, which are understood to be conducted in water, write A) the complete and balanced conventional (aka "molecular") equation, B) the "total ionic" equation, still balanced, and C) the net ionic equation, still balanced.

1. potassium + water --> potassium hydroxide + hydrogen A) B) C) 2. zinc + hydrochloric acid

zinc chloride + hydrogen

A)

B) C) 3. copper(II) sulfate + iron --* iron(III) sulfate + copper A) B) C) 4. ammonia(aq) + sulfuric acid ammonium sulfate A) B) C) 5. iron(III) sulfate + barium nitrate -› A) B) C)

-

6. iron(III) nitrate + barium chloride -) A)

B) C) 7. lead(II) acetate + hydrogen sulfide

lead(II) sulfide + acetic acid

A) B) C) 8. sodium hydroxide + ammonium sulfate A) B) C) e 9. potassium iodide + chlorine 4 potassium chloride + iodin A) B) C) 10. iron(II) chloride + ammonium sulfide —> A) B)

C)

Name: Homework

Date:

AP Chemistry Summer

1. A method of separation that employs a system with two phases of matter, a mobile phase and a stationary phase, is called A) filtration B) chromatography C) distillation D) vaporization E) homogenization 2.

are substances with constant composition that can be broken down into elements by chemical processes. A) Solutions B) Mixtures C) Compounds D) Quarks E) Heterogeneous mixtures

3. Express the volume 641.4 cm3 in liters. A) 641.4 L B) 64.14 L C) 6.414 L D) 0.6414 L E) 0.06414 L 4. Convert 7616.7 g to mg. A) 7.6167 mg B) 76.167 mg C) 761.67 mg D) 7.6167 x 103 mg E) 7.6167 x 106 mg

Page 1

5. Which of the following has 61 neutrons, 47 protons, and 46 electrons? A)

80 pm 61

B)

108Ag+ 47

C)

108 46

D)

108 cd 47

pd+

E) 108 A• g 1 47

6. All of the following are characteristics of metals except: A) good conductors of heat B) malleable C) ductile D) often lustrous E) tend to gain electrons in chemical reactions 7. Which of the following pairs is incorrect? A) NI-1413r, ammonium bromide B) K2CO3, potassium carbonate C) BaPO4, barium phosphate D) CuCI, copper(I) chloride E) Mn02, manganese(IV) oxide 8. Which of the following is incorrectly named? A) Pb(NO3)2, lead(II) nitrate B) NH4C1O4, ammonium perchlorate C) P043-, phosphate ion D) Mg(OH)2, magnesium hydroxide E) NO3-, nitrite ion

9. What is the best answer to report for A) B) C) D) E)

3. 478 g x 1.164 g 2.00 mL

1.6700 g/mL 1.670 g/mL 1.67 g/mL 1.7 g/mL 2 g/mL

Page 2

0.350 g/mL?

10. How many significant figures should be reported for the difference between 18.7073 mL and 18.57 mL? A) 1 B) 2 C) 3 D) 4 E) 6 11. How many significant figures are there in the number 3.1400? A) 1 B) 2 C) 3 D) 4 E) 5 12. How many significant figures are there in the number 0.0005417? A) 7 B) 3 C) 8 D) 4 E) 0 13. How many significant figures are there in the number 0.04560700? A) 4 B) 5 C) 7 D) 8 E) 9 14. Using the rules of significant figures, calculate the following: 6.167 +59 5.10 A) 12.8 B) 14 C) 13 D) 71 E) 12.78

Page 3

15. Consider the numbers 23.68 and 4.12. The sum of these numbers has figures, and the product of these numbers has significant figures. A) 3, 3 B) 4, 4 C) 3, 4 D) 4, 3 E) none of these

significant

16. The beakers shown below have different precisions as shown.

Suppose you pour the water from these three beakers into one container. What would be the volume in the container reported to the correct number of significant figures? A) 78.817 mL B) 78.82 mL C) 78.8 mL D) 80 mL E) 79 mL 17. We generally report a measurement by recording all of the certain digits plus uncertain digit(s). A) no B) one C) two D) three E) four

Page 4

18. Express the number 1.82 x 10 4 in common decimal form. A) 182000 B) 0.0000182 C) 0.000182 D) 18200 E) 1820 19. Express 165,000 in exponential notation. A) 1.65000 x 105 B) 1.65 x 105 C) 1.6500 x 10-5 D) 1.65 x 10-5 E) 165 x 103 20. A scientist obtains the number 0.045006700 on a calculator. If this number actually has four (4) significant figures, how should it be written? A) 0.4567 B) 0.4501 C) 0.0450 D) 0.04500 E) 0.04501 21. The amount of uncertainty in a measured quantity is determined by: A) both the skill of the observer and the limitations of the measuring instrument B) neither the skill of the observer nor the limitations of the measuring instrument C) the limitations of the measuring instrument only D) the skill of the observer only E) none of these 22. A solution is also called a A) homogeneous mixture B) heterogeneous mixture C) pure mixture D) compound E) distilled mixture

Page 5

Use the following to answer questions 23-25: Consider the following choices when answering questions 86-89. c) b) 0

e0

0 0

0

0 0

0

d)

0

•

00

SA 0.0.0 is walo 0.00.00.0.111.0.0.0 elpjuicovao e IsA10.0:40 ■ 11 *SALO*

• •141:•• • "vi If

0

•• 01•••• 0:0:0:0:0:0

1

cC

InliVIPIAMILVIL11.11 1 ginfwe.• !A • c.•,0 lic•f•::.• o esofooes•ArAmm:o

1•101•2111111111110,410,0,••21KK•AJDAPPAPP,

e) CO ❑ CO ❑ CO

❑ CO ❑ CO ❑

❑ co

CO ❑ co ❑

ce ❑

❑ CO CO ❑ ❑ CO 03 ❑

❑ CO ❑ CO

❑ co co co ❑

❑

23. Which best represents a heterogeneous mixture of two elements? A) option a B) option b C) option c D) option d E) option e 24. Which best represents a solid element? A) option a B) option b C) option c D) option d E) option e 25. Which best represents a gaseous compound? A) option a B) option b C) option c D) option d E) option e

Page 6

cC cC

26. You are given a compound with the formula MC12, in which M is a metal. You are told that the metal ion has 24 electrons. What is the identity of the metal? A) Cr B) Al C) Ni D) Mn E) Fe 27. If the Thomson model of the atom had been correct, Rutherford would have observed: A) Alpha particles going through the foil with little or no deflection. B) Alpha particles greatly deflected by the metal foil. C) Alpha particles bouncing off the foil. D) Positive particles formed in the foil. E) None of the above observations is consistent with the Thomson model of the atom. 28. Rutherford's experiment was important because it showed that: A) Radioactive elements give off alpha particles. B) Gold foil can be made to be only a few atoms thick. C) A zinc sulfide screen scintillates when struck by a charged particle. D) The mass of the atom is uniformly distributed throughout the atom. E) An atom is mostly empty space. 29. All of the following are characteristics of nonmetals except: A) poor conductors of electricity B) often bond to each other by forming covalent bonds C) tend to form negative ions in chemical reactions with metals D) appear in the upper left-hand corner of the periodic table E) do not have a shiny (lustrous) appearance

Page 7

Use the following to answer question 30: Consider the following choices when answering questions 86-89. c) b) a) 0 0

(20

c0

0 0

O

0

0

c0

0

• • OA IDA • • •••• 01•100:•100 0.0 eirmirsoes....: ■•• :elm we* • weirowe ciimme 0,4:0,1„41LIA•0941 .0.00:00.41 le•C•21,10

0 0

d)

0

F

01•00:•.• • • • • co* cce•••• 0101•1•11010t0p,•20p2M011:•210111

0

e)

cC

cC

co ❑ co co ❑ co co ❑ co ❑ ❑

co ❑

CO ❑ ❑ CO CO ❑

OD ❑ CO

30. Which best represents a homogeneous mixture of an element and a compound? A) option a B) option b C) option c D) option d E) option e

Page 8

2007 AP® CHEMISTRY FREE-RESPONSE QUESTIONS

6. Answer the following questions, which pertain to binary compounds. (a) In the box provided below, draw a complete Lewis electron-dot diagram for the IF 3 molecule.

(b) On the basis of the Lewis electron-dot diagram that you drew in part (a), predict the molecular geometry of the IF3 molecule. (c) In the SO2 molecule, both of the bonds between sulfur and oxygen have the same length. Explain this observation, supporting your explanation by drawing in the box below a Lewis electron-dot diagram (or diagrams) for the SO 2 molecule.

(d) On the basis of your Lewis electron-dot diagram(s) in part (c), identify the hybridization of the sulfur atom in the SO2 molecule. The reaction between S0 2(g) and 02(g) to form SO3(g) is represented below. 2 S02(g) + 02(g)