South Pasadena · AP Chemistry



Memo

Date: 5/24/2012

To: Members of the AP Chemistry Class of 2012 - 2013

From: Mr. Douglas Arbuckle

RE: Summer Assignment

I am very excited that you have chosen to take AP Chemistry next year. As you know, Chemistry is a subject that requires the student to know a wide and comprehensive range of information. Chemistry also involves a large vocabulary, and requires a student to perform a wide variety of calculations and measurements. In order to prepare each student to sit for the AP Chemistry exam next May, the class will move at a rapid pace. It requires that each student keep up with daily assignments, read and study notes and text, and to ask questions (both in and outside of class). It is also highly recommended that students form study groups, and work together whenever possible. The goal of this class is to prepare the student to be successful on one of the most difficult and demanding tests that is given by the AP College Board. Having taken Honors Chemistry, you already have an excellent foundation, and have already been exposed to many of the concepts that we will tackle at a deeper level in AP.

There are several course requirements/expectations that you should understand, including:

• There is a summer assignment (attached) that must be completed, preferably in mid-late August.

• I am looking into an on-line assignment system (WebAssign) that looks promising. If we move forward on this, there will be a licensing fee of approximately $11.00 per student for the year.

• You need a scientific calculator, preferably TI-83, TI-84, or equivalent.

• You must be able to study independently outside of class at least 5 hours a week.

Please stop by my room (601) this week or next (PRIOR to leaving for the summer) so I may assign you a textbook. Also, so that I may contact you with any additional information, please email me within the next week from the email address you will be using throughout the summer. My school email address is douglas.arbuckle@. As most of you know, my website is Arbuckle., and you should check it regularly.

Have a fun and safe summer!! I look forward to seeing you next year.

AP Chemistry 2012-2013

Summer Assignment

The following assignment needs to be completed by the first day of school.

You should be able to find any information you need in your notes from Honors Chemistry and in your AP Chemistry textbook. This packet contains information which is review of material that has already been covered in Honors - we have worked hard to provide a strong foundation so that we don’t have to cover the basics in detail over again. AP Chemistry is an intense course by nature; it requires a great deal of maturity on your part and time commitment outside of class. We want to have as much time as possible for new content; therefore, it’s important that we move through “review” material quickly.

As in Honors Chemistry, and more importantly in AP Chemistry, you are encouraged to work together this summer on the assignment (consider it training in forming good study groups); however, YOU are responsible for this material. There will be a quiz the first couple of days after we return to school, with a subsequent test in a week or so covering chapters 1, 2, and 3 of the text. Please read/review these chapters thoroughly, keeping in mind that there is nothing new in these!!!

*Reminder: It’s best to wait until towards the end of the summer before completing these problems - if you do them too early in the summer, the point of refreshing your memory will be lost! (

AP Chemistry Name ____________________________________

Summer Work

Matter and Measurement

*Please do all work NEATLY on a separate sheet of paper if necessary!

1. Identify the following changes as physical or chemical changes:

a. Baking soda reacts with vinegar to produce carbon dioxide.

b. The copper sheath on the Statue of Liberty turns green.

c. Addition of salt melts ice on the highway.

d. Steam condenses on the windowpane.

e. Epoxy resin cures and hardens.

f. Sugar dissolves in a cup of coffee.

g. Natural gas burns in a furnace.

2. a. Calculate the density of lead if a 10 kg block has a volume of 885 cm3.

b. What is the volume of a 100 g bar of aluminum if its density is 2.70 g·cm-3?

c. Calculate the mass of 100 cm3 of uranium (density 19.07 g·cm-3).

3. Convert:

a. 25(C to K b. 25(C to oF

4. Define extensive and intensive physical properties.

Which of the following physical properties are extensive?

a. heat of fusion d. viscosity

b. melting point e. conductivity

c. color f. density

5. Write the names of the following elements:

a. N b. Ca c. K d. P e. V

6. Write the symbols for the following elements:

a. silicon b. chlorine c. iron d. sodium e. silver f. sulfur

7. Convert, using dimensional analysis (aka factor labeling): c. 8,768 mg into g

a. 1342 mL into L d. 400 cm3 into m3

b. 3.26 x 10-6 km into mm e. 3600 sq. in. into sq. ft.

8. Write the following numbers in scientific notation showing three significant figures:

a. 1,327 b. 0.00562 c. 2.76 d. 0.166 e. 0.09911

9. Measurements of the boiling point of a liquid were taken by two laboratory technicians (A and B). The actual boiling point was 92.3. Which technician achieved the most accurate result and which technician was the most precise?

A: 92.0 92.1 92.4 92.2

B: 91.9 92.5 92.6 92.0

10. Match the prefix with the correct multiplier:

|milli |mega |kilo |micro |centi |pico |

| | | | | | |

|10-6 |103 |10-2 |106 |10-12 |10-3 |

11. Evaluate the following expressions. Express the answers in scientific notation with the correct number of significant figures and the correct units.

a. 0.0045 in + 1.0098 in + 0.987 in + 23.08 in

b. (3.45 cm3 x 2.70 g·cm-3) + (7.433 cm3 x 1.677 g·cm-3)

c. 2.703 g/(1.376 cm x 2.45 cm x 3.78 cm)

12. A 12.3 g block of an unknown metal is immersed in water in a graduated cylinder. The level of water in the cylinder rose. The level of water in the cylinder rose exactly the same distance when 17.4 grams of aluminum (density 2.70 g·cm-3) was added to the same cylinder. What is the unknown metal’s density?

13. If one pound is 453.59 grams, how many grams are there in one ounce? How many ounces are there in one kilogram? Use dimensional analysis (factor labeling).

14. A sample of gold alloy contains 5.6% silver by mass. How many grams of silver are there in 1 kilogram of the alloy?

15. List the number of protons, neutrons, and electrons in carbon-13.

16. What is the frequency of ultraviolet light with wavelength 2.94 10-8 m? (c = 3.00 × 108 m/s)

17. What is the energy of a microwave photon that has a frequency of 1.12 × 1012 Hz? (h = 6.63 × 10-34 J∙s)

18. Describe the two types of mixtures, and the different ways mixtures can be separated into pure substances.

Writing Formulas and Naming Compounds

Writing formulas and naming compounds can be confusing because there are different types of compounds that follow different rules. Additionally, some compounds (H2O, NH3, CH4, etc.) simply have common names that must be memorized.

The two types of compounds we will focus on first are ionic compounds (formed from positive and negative ions) and binary nonmetal compounds (molecular compounds). Later we will add acids. So… you must recognize the type of compound before you try to name it. [Note: + ion = “cation” and – ion = “anion”.]

| |Ionic |Binary Nonmetal |

|Formula |+ ion before – ion |usually the less electronegative atom is first |

| |ex: NaCl (NH4)2SO4 Al2S3 |ex: CO CO2 N2O |

|Naming |Name of cation + name of anion |Indicate the number (mono, di, tri, and kind of atoms. First element is simply |

| | |name of element. Second element name ends with “ide” |

| |sodium chloride | |

| |ammonium sulfate |carbon monoxide |

| |aluminum sulfide |carbon dioxide |

| | |dinitrogen monoxide |

I. Naming Ionic Compounds

|Cation |Anion |Formula |Name |

|Cu2+ |OH− | | |

|Ba2+ |SO42− | | |

|NH4+ |Cr2O72− | | |

|Ag+ |C2H3O2− | | |

|Fe3+ |S2− | | |

II. Writing Formulas of Binary Nonmetal Compounds

|Name |Formula |Name |Formula |

|nitrogen trifluoride | |phosphorus trichloride | |

|nitrogen monoxide | |phosphorus pentachloride | |

|nitrogen dioxide | |sulfur hexafluoride | |

|dinitrogen tetroxide | |disulfur decafluoride | |

|dinitrogen monoxide | |xenon tetrafluoride | |

III. Naming Binary Nonmetal Compounds

|Name |Formula |Name |Formula |

| |CCl4 | |HBr |

| |P4O10 | |N2F4 |

| |ClF3 | |XeF3 |

| |BCl3 | |PI3 |

| |SF4 | |SCl2 |

IV. Practice for Both Types of Compounds

|Formula |Name | |Formula |Name |

|HCl | | | |carbon dioxide |

|PCl5 | | | |ammonium carbonate |

|K2S | | | |sulfur dichloride |

|NiSO4 | | | |calcium iodide |

|ClF3 | | | |boron trifluoride |

|OF2 | | | |phosphorus triiodide |

|Al(OH)3 | | | |magnesium perchlorate |

|NCl3 | | | |potassium permanganate |

|(NH4)3PO4 | | | |aluminum phosphate |

|S2Cl2 | | | |dioxygen difluoride |

Chemical Equations and Stoichiometry

BALANCING EQUATIONS

1. __LaCl3 + __Na2CO3 ( __La2(CO3)3 + __NaCl

2. __NH4Cl + __Ba(OH)2 ( __BaCl2 + __NH3 + __H2O

3. __Ca(OH)2 + __H3PO4 ( __Ca3(PO4)2 + __H2O

4. __C4H10 + __O2 ( __CO2 + __H2O

5. __C7H6O2 + __O2 ( __CO2 + __H2O

6. __P4O10 + __H2O ( __H3PO4

Stoichiometry:

1. How many moles of potassium hydroxide are needed to completely react with 3.47 moles of aluminum sulfate according to the following BALANCED equation?

6 KOH + Al2(SO4)3 ( 2 Al(OH)3 + 3 K2SO4

2. Calcium carbonate and sodium chloride react to produce sodium carbonate and calcium chloride according to the following BALANCED equation. How many moles of calcium chloride will be produced if 13.0 g of calcium carbonate are reacted?

CaCO3 + 2 NaCl ( Na2CO3 + CaCl2

3. When mercury (II) nitrate is heated, it decomposes to form mercury (II) oxide, nitrogen dioxide, and oxygen gas according to the following BALANCED equation.

2 Hg(NO3)2 ( 2 HgO + 4 NO2 + O2

a. How many grams of mercury (II) oxide will be produced if 27.0 g of mercury (II) nitrate react?

b. How many moles of oxygen gas will be produced if 3.5 g of nitrogen dioxide are produced?

c. When 12.0 g of mercury (II) nitrate are decomposed in the lab, it is found that 7.56 g of mercury (II) oxide are produced. What is the actual yield, the theoretical yield, and the percent yield?

4. If 5.6 g of copper (II) oxide are reacted with 8.6 g of hydrogen according to the following BALANCED reaction, how many grams of copper metal will be produced?

CuO + H2 ( Cu + H2

The limiting reactant is __________, and the excess reactant is __________. The amount of excess reactant that remains when the reaction stops is _______.

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