AP Chemistry Summer Assignment

AP Chemistry Summer Assignment 2015

TEACHER: Mr. Trent Garrison [email protected]

RATIONALE: Since next year’s course is a college-level chemistry course, it is imperative that you begin the year with as much chemistry knowledge as possible. I expect that you will be challenged like no other course you have ever experienced. You will need to devote yourself to regular studying and continual practice of your new skills. Therefore, I are asking you to review the topics you have utilized over the last couple of years, memorize a few key charts, and learn a smattering of new concepts.

TIME: It is estimated that you will need to spend approximately five hours on this assignment, plus time for memorization.

HELP: Some web sites that you may find useful are included at the bottom of this assignment. If you need further assistance on any of these concepts, please feel free to get in touch with me, I will be available these dates and times: August 10-14, 17-21, & 24-28 from 7:30 to 3:00 everyday. You can also email me any day or time at [email protected]. I will also be offering a Chemistry Boot Camp on August 3-5 in the mornings at RHS. I will email you more details soon. I do want to stress to you that I am not your private tutor. Please come prepare to engage in a dialog about your challenges.

THE ASSIGNMENT: You must become familiar with or memorize facts for the following topics: 1. Preparation Materials 2. Mathematics Review 3. Nomenclature 4. Ionic Nomenclature and Oxidation Numbers 5. Strong Acids & Bases 6. Solubility Rules 7. Dimensional Analysis 8. Balancing Equations 9. Stoichiometry

THE ASSESSEMENTS: The first day of class you will have a quiz on the memorized material. You will receive a brief review of the summer assignment and an exam will quickly follow.

TEXTBOOK: Kotz & Treichel, Chemistry & Chemical Reactivity, 5th ed. Thomson, 2003. We may get a new textbook over the summer. You can utilize your textbook’s chapters 1-4 to find additional help on this assignment.

ANSELARY RESOURCES: https://www.khanacademy.org/science/chemistry http://www.brightstorm.com/science/chemistry/ http://chemmybear.com/stdycrds.html http://chemteam.info/ChemTeamIndex.html http://chemtutor.com/ http://chem.tamu.edu/class/majors/tutorialnotefiles http://bozemanscience.com/ap-chemistry/

Have a great summer and get ready to be challenged to greatness.

13 AP Chemistry Summer Assignment 2015

SUMMER ASSIGNMENT PART 1:  Pick up a copy of your Kotz & Treichel’s Chemistry & Chemistry Reactivity (5th edition) from Mrs. Rogucki or Mrs. Dickenson in the front office BEFORE leaving school for the summer.

 Purchase a used copy of Tro’s Chemistry: A Molecular Approach (2nd edition) from Amazon (approximately $15). This is the textbook I am trying to get the school to purchase for you, but it may not arrive before the start of school.  Print out a copy of the Chemistry Cruncher at http://home.comcast.net/~cochranjim/PDFS/CC.pdf. Attach your copy to the materials you turn in on the first day of class.  Download apps to your smart phone, tablet, or computer that are free or you can afford (Chem Solver, Polyatomic Ions, etc.) Create a screenshot of your phone with the app on your desktop. Print out a copy and attach your copy to the materials you turn in on the first day of class.  Visit the AP Central website at http://apcentral.collegeboard.com/apc/public/exam/exam_information/221837.html. Create a screenshot of your phone, tablet or computer with the app on your desktop. Print out a copy and attach your copy to the materials you turn in on the first day of class.

SUMMER ASSIGNMENT PART 2:  Remove pages 27-28 from this summer assignment packet. Finish the math review problems. Attach your copy to the materials you turn in on the first day of class.

SUMMER ASSIGNMENT PART 3:  Remove pages 33-34 from this summer assignment packet. Finish the comprehensive nomenclature problems. Attach your copy to the materials you turn in on the first day of class.

SUMMER ASSIGNMENT PART 4:  Memorize the content of page 36.

SUMMER ASSIGNMENT PART 7:  Remove pages 41-46 from this summer assignment packet. Finish the dimensional analysis problems. Attach your copy to the materials you turn in on the first day of class.

SUMMER ASSIGNMENT PART 8:  Remove page 49 from this summer assignment packet. Finish the balancing equations problems. Attach your copy to the materials you turn in on the first day of class.

SUMMER ASSIGNMENT PART 9:  Remove page 55 from this summer assignment packet. Finish the dimensional analysis problems. Attach your copy to the materials you turn in on the first day of class.

Solubility Rules

Salt Solubility Rules + 1. Salts of ammonium (NH4 ) and Group IA are always soluble.

2. Halogens: - a. All chlorides (Cl ) are soluble except AgCl, Hg2Cl2, and PbCl2 which are insoluble. - b. All bromides (Br ) are soluble except AgBr, Hg2Br2, HgBr2, and PbBr2 which are insoluble. - c. All iodides (I ) are soluble except AgI, Hg2I2, HgI2, and PbI2 which are insoluble.

- - - 3. Chlorates (ClO3 ), nitrates (NO3 ), and acetates (CH3COO ) are soluble.

-2 4. Sulfates (SO4 ) are soluble except CaSO4, SrSO4, BaSO4, Hg2SO4, HgSO4, PbSO4, and Ag2SO4 which are insoluble.

-3 -2 + 5. Phosphates (PO4 ), and carbonates (CO3 ) are insoluble except NH4 and Group IA compounds.

-2 + 6. All metallic oxides (O ) are insoluble except NH4 and Group IA compounds.

- + 7. All metallic hydroxides (OH ) are insoluble except NH4 and Group IA and Group IIA from calcium down.

-2 + 8. All sulfides (S ) are insoluble except NH4 and Groups IA and IIA.

Rules for Naming an Acid

1. When the name of the anion ends in –ide, the acid name begins with the prefix hydro-, the stem of the anion has the suffix –ic and it is followed by the word acid. -ide becomes hydro _____ic Acid

Example: Cl- is the Chloride ion so HCl = hydrochloric acid

2. When the anion name ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by the word acid. -ite becomes ______ous Acid

- Example: ClO2 is the Chlorite ion so HClO2. = Chlorous acid.

3. When the anion name ends in –ate, the acid name is the stem of the anion with the suffix –ic, followed by the word acid. -ate becomes ______ic Acid

- Example: ClO3 is the Chlorate ion so HClO3 = Chloric acid.

TABLE OF STRONG ACIDS Completely Ionized in Water to Give One (or more) Protons per Acid Molecule

HI H+(aq) + I-(aq) HBr H+(aq) + Br-(aq) + - HClO4 H (aq) + ClO4 (aq) HCl H+(aq) + Cl-(aq) + - HClO3 H (aq) + ClO3 (aq) H+(aq) + HSO -(aq) (HSO - is a weak acid that H SO 4 4 2 4 contributes additional protons) + - HNO3 H (aq) + NO3 (aq)

TABLE OF STRONG BASES Completely Ionized in Water to Give One (or more) Hydroxides per Base Molecule

NaOH Na+(aq) + OH-(aq) KOH K+(aq) + OH-(aq) LiOH Li+(aq) + OH-(aq) RbOH Rb+(aq) + OH-(aq) CsOH Cs+(aq) + OH-(aq) 2+ - Ca(OH)2 Ca (aq) + 2OH (aq) (but not very soluble) 2+ - Ba(OH)2 Ba (aq) + 2OH (aq) (but not very soluble) 2+ - Sr(OH)2 Sr (aq) + 2OH (aq) (but not very soluble)

In order for chemists and other scientists to communicate with each other, a system of nomenclature or naming was agreed upon by the International Union of Pure and Applied Chemistry or IUPAC. You'll hear chemicals called their common names (e.g., salt, sugar, and baking soda), but in the lab you would use systematic names (e.g., sodium chloride, sucrose, and sodium bicarbonate). Here's a review of some key points about nomenclature.

Naming Binary Compounds Compounds may be made up of only two elements (binary compounds) or more than two elements. Certain rules apply when naming binary compounds:

 If one of the elements is a metal, it is named first.  Some transition metals can form more than one positive ion. It is common to state the charge on the ion using Ro- man numerals.

. For example, FeCl2 is iron(II) chloride.  If the second element is a nonmetal, the name of the compound is the metal name followed by a stem (abbreviation) of the nonmetal name followed by "ide". . For example, NaCl is named sodium chloride.  For compounds consisting of two nonmetals, the more electropositive element is named first. The stem of the second element is named, followed by "ide". . An example is HCl, which is hydrogen chloride.

Naming Ionic Compounds In addition to the rules for naming binary compounds, there are additional naming conventions for ionic compounds:

 Some polyatomic anions contain oxygen. If an element forms two oxyanions, the one with less oxygen ends in -ite while the one with more oxgyen ends in -ate. . For example: NO2- is nitrite NO3- is nitrate

Dimensional Analysis (also called Factor-Label Method or the Unit Factor Method) is a problem-solving method that uses the fact that any number or expression can be multiplied by one without changing its value. It is a useful technique. The only danger is that you may end up thinking that chemistry is simply a math problem - which it definitely is not.

Unit factors may be made from any two terms that describe the same or equivalent "amounts" of what we are interested in. For example, we know that

1 inch = 2.54 centimeters

Note: Unlike most English-Metric conversions, this one is exact. There are exactly 2.540000000... centimeters in 1 inch.

We can make two unit factors from this information:

Now, we can solve some problems. Set up each problem by writing down what you need to find with a question mark. Then set it equal to the information that you are given. The problem is solved by multiplying the given data and its units by the appropriate unit factors so that only the desired units are present at the end.

(1) How many centimeters are in 6.00 inches?

(2) Express 24.0 cm in inches.

You can also string many unit factors together.

(3) How many seconds are in 2.0 years?

Scientists generally work in metric units. Common prefixes used are the following:

Prefix Abbreviation Meaning Example mega- M 106 1 megameter (Mm) = 1 x 106 m kilo- k 103 1 kilogram (kg) = 1 x 103 g centi- c 10-2 1 centimeter (cm) = 1 x 10-2 m milli- m 10-3 1 milligram (mg) = 1 x 10-3 g micro- 10-6 1 micrometer ( g) = 1 x 10-6 g nano- n 10-9 1 nanogram (ng) = 1 x 10-9 g

(4) Convert 50.0 mL to liters. (This is a very common conversion.)

(5) What is the density of mercury (13.6 g/cm3) in units of kg/m3?

We also can use dimensional analysis for solving problems.

(6) How many atoms of hydrogen can be found in 45 g of ammonia, NH3? We will need three unit factors to do this calculation, derived from the following information:

1. 1 mole of NH3 has a mass of 17 grams. 23 2. 1 mole of NH3 contains 6.02 x 10 molecules of NH3.

3. 1 molecule of NH3 has 3 atoms of hydrogen in it.

There are many, many more examples in your textbook!

Dimensional Analysis: Convert the following. Show ALL work on a SEPARATE SHEET OF PAPER, use dimensional analysis and scientific notation: 1. Convert 0.014 kilograms to centigrams 2. Convert 4.305 L to milliliters 3. Convert 1.76 yards to centimeters 4. Convert 1.8 quarts to cubic centimeters 5. Calculate the displacement (the total volume of the cylinders through which the pistons move) of a 5.70 L automobile engine in cubic inches. 6. How many cubic centimeters are there in 2.11 yd3? 7. The mass of fuel in a jet must be calculated before each flight to ensure that the jet is not too heavy to fly. A 747 is fueled with 173,231 L of jet fuel. If the density of the fuel is 0.7868 g/cm3, what is the mass of the fuel in kilograms? 8. Backpackers often use canisters of white gas to fuel a cooking stove’s burner. If one canister contains 1.45 L of white gas, and the density of the gas is 0.710 g/cm3, what is the mass of the fuel in kilograms? 9. What volume would a 200 gram sample of gold have if its density is known to be 20.5 g/cm3? 10. Light travels at a speed of 3.00 x 1010cm/sec. What is the speed of light in km/hr?

Stoichiometry: Complete the following problems SEPARATE SHEET OF PAPER using dimensional analysis. Balance all of the equations that need to be balanced. The answers are given in parenthesis at the end of each problem. Show ALL of your work, balance all of the equations that need to be balanced, and use dimensional analysis.

1. In the decomposition of sodium hydroxide, how many moles of sodium hydroxide are needed to produce 30.0 moles of water? (60.0 moles NaOH) 2. In the single replacement reaction of lithium and magnesium nitrate, what mass of lithium combines with 75.o grams of magnesium nitrate (7.02 g Li) 3. How many grams of lead(II)nitrate are needed to produce 60.0 grams of potassium nitrate in the double replacement reaction of potassium iodide and lead(II)nitrate. (98.3 g lead(II)nitrate) 4. When methane and oxygen react (complete combustion reaction) how many grams of water would be pro- duced from 25.0 grams of methane? (56.1 g water) 5. If 7.40 grams of calcium hydroxide react with nitric acid to produce 2.01 grams of water, what is the percent yield? (55.8%)

Putting it together: ON A SEPARATE SHEET OF PAPER Write the balanced chemical equations and then solve the problem.

6. If you begin with 1250 g of N2 and 225 g of H2 in the reaction that forms ammonia gas (NH3), how much ammonia will be formed? What is the limiting reagent? How much of the non-limiting reagent is left when the maximum amount of ammonia is formed? 7. A 0.941 gram piece of magnesium metal is heated and reacts with oxygen. The resulting oxide weighed 1.560 grams. Determine the percent composition of each element in the compound. 8. A compound contains 21.6% sodium, 33.0% chlorine, 45.1% oxygen. Determine the empirical formula of the compound.

Sample Formula Sheets Provided on AP Exam

Write the name for the following compounds.

1. N3O6______16. CoBr2______

2. KCl______17. Ni(NO3)2______

3. Ca(NO3)2______18. NaPO4______

4. Na2SO4______19. Si2I______

5. Fe3(PO4)2______20. TiCl4______

6. CuSO4 * 5H2O______21. Mn(OH)2 * 6H2O______

7. Ba3 (PO4)2______22. KClO3______

8. H2CO3______23. CaF2______

9. (NH4)2CO3______24. FeBr3______

10. Hg2O______25. VCO3______

11. N8F4______26. NF4______

12. Sr3As2______27. Li3N______

13. NH4NO3______28. S4N7______

14. S6I2______29. CoS______

15. V2O5______30. NH4NO3______

Write the formula for the following compounds.

31. ammonium chromate______46. ammonium phosphate______

32. cobalt (II) oxide______47. iron (II) oxide______

33. sulfur nonoxide______48. carbon monoxide______

34. sodium hydride______49. calcium chloride______

35. potassium sulfate______50. potassium nitrate______

36. aluminum hydroxide______51. magnesium hydroxide______

37. cesium sulfate______52. aluminum sulfate______

38. tungsten (II) 53. copper (II) carbonate______sulfate______

39. titanium (IV) 54. iron (III) phosphide______phosphide______

40. tin (IV) chromate______55. lead (IV) carbonate______

41. tetraphosphorus heptoxide______56. diphosphorus pentoxide______

42. potassium 57. potassium hydroxide______hydroxide______

43. sodium 58. sodium telluride______carbide______

44. rhenium (VI) 59. zinc (II) nitrate______nitrate______

45. indium sulfite______60. aluminum sulfate______