Text @Sumapc to 81010 ​ for Quick Links and Info REFERENCES

**Join Remind101: Text @sumapc to 81010 for quick links and info June 4, 2019 ​ ​

Dear Prospective AP Chemistry Students and Parents, Advanced Placement Chemistry is a course designed to be the equivalent of the general chemistry course taken during ​ the first year of college by science majors. For some students, this course enables them to undertake, as freshmen, second year ​ ​ work in the chemistry sequence or to register for courses in other fields where general chemistry is a prerequisite. For other students, the AP Chemistry course fulfills the laboratory science requirement and frees time for other courses. AP Chemistry is a rigorous math-based course, with a strong laboratory component. It is intended for students who have demonstrated a willingness to commit considerable time to studying and completing assignments outside of class, and who have successfully completed a prior course in chemistry, preferably Honors Chemistry. ​ ​ Since passing the AP exam may qualify the student to bypass a first-year college chemistry course, AP Chemistry should not be considered "college prep." Rather, this is a college class, with college level expectations for behavior, participation, and effort.

REQUIRED materials: · Scientific calculator or graphing calculator (must have LOG key) th · TEXTBOOK: Chemistry, 10 ​ edition by Brown, Lemay, & Bursten (You may use the link below if you need for now) ​ ​ ​ ​ ​ · Summer Packet Assignment: The AP Chemistry exam is offered in the beginning of May, so we require that students ​ ​ complete summer review requirements prior to the start of school. This is vital in assuring that our students are guided in the best way possible. *Note: We will be utilizing the WebAssign Online Homework and the billing is applied per class.

RECOMMENDED material: There are so many free online sources ​ AP Chem Course & Exam Description (The best resource provided by the College Board with details of the exam) ​ AP Chem Review of Everything (created by AP Chem teachers) ​ http://blog.prepscholar.com/ap-chemistry-study-guide http://www.sciencegeek.net/APchemistry/APtaters/directory.shtml http://blog.prepscholar.com/best-ap-chemistry-books (Read this blog before you decide to spend money) ​ Textbook: https://drive.google.com/file/d/0B1Zhp01hnSI_WVVqQ1VYZ3hUdE0/view ​ Mrs. Ismail’s website for video links: www.mervetismail.com ​

The SUMMER ASSIGNMENT checklist is typed on the first page of the Basics of Chemistry Packet. This material should be a review of material learned in your prior chemistry course. Please follow those directions carefully. An exam over the material will occur the 3rd full week of class. *The SUMMER PACKET will be collected the FIRST DAY OF SCHOOL.* ​ Please be sure to spend the time to skim through the entire packet very carefully. We hope you are excited to be enrolled in this class. We look forward to meeting all of you in the fall. Have a wonderful summer!

Sincerely,

Mrs. Matynowski & Mrs. Ismail West Bloomfield High School

For questions or problems, please e-mail: [email protected] ​ REFERENCES: (p2-7)

Predicting Chemical Reactions Notes The products of a chemical reaction may often be predicted by applying known facts about common reaction types. Only 5 general types of reactions will be considered: Combustion, Single Displacement, Double Displacement, Synthesis, and Decomposition (Analysis).

A COMBUSTION REACTION occurs when an element/compound reacts with oxygen(O2), often ​ ​ ​ ​ producing energy in the form of heat/light.

Ex: CH4 + 2 O2 → CO2 + 2 H2O + heat/light ​ ​ ​ ​ ​ ​ ​ ​

**Hydrocarbons are compounds made up mainly of carbon and hydrogen (they also may contain oxygen or ​ ​ nitrogen). When hydrocarbons react with oxygen gas, they from CO2 + H2O **A rhyme to help you ​ ​ ​ ​ remember: “Reacting O2 with “CH or CHO” always produces “CO(2) and H(2)O”! ​ ​ ​ ​ ​ ​ ​

A SINGLE DISPLACEMENT REACTION occurs when one element displaces another in a compound. ​ ​ The general form is: element + compound → element + compound A + BC → B + AC ex: Zn + 2HCl → H + ZnCl ​2 ​2 We call this: “SPORTS SUBSTITUTION”

A DOUBLE DISPLACEMENT REACTION occurs when the cations and anions of the two reactants are ​ ​ interchanged. The general form is: compound + compound → compound + compound AB + CD → AD + CB

Ex: FeS + 2HCl → FeCl2 + H2S ​ ​ ​

A SYNTHESIS REACTION occurs when two or more elements or compounds are combined to form ONE ​ ​ more complex substance. The general form is: element/cmpd + element/cmpd → compound ex: Fe + S → FeS

A DECOMPOSITION (ANALYSIS) REACTION occurs when energy in the form of heat, light, ​ ​ electricity, or mechanical shock is supplied. A compound may decompose to form simpler compounds and/or elements.The general form is: compound → two or more substance. There are six general types: *You do NOT need to memorize the following, just apply the statement. 1. Some oxy-acids, when heated, decompose to form water and non-metal oxide. ​ ​ Ex: H2CO3 → H2O + CO2 ​ ​ ​ ​ ​ ​ ​ 2. Some metallic hydroxides,when heated, decompose to form metal oxide & water. ​ ​ Ex: Ca(OH)2 → CaO + H2O ​ ​ ​ ​ 3. Some metallic carbonates, when heated, decompose to form the metal oxide and carbon dioxide. ​ ​ Ex: Li2CO3 → Li2O + CO2 ​ ​ ​ ​ ​ ​ ​ 4. Some metallic chlorates, when heated, decompose to form the metal chloride and oxygen gas. ​ ​ Ex: 2KClO3 → 2KCl + 3O2 ​ ​ ​ 5. Most metallic oxides are stable, but a few decompose when heated to form the metal and oxygen gas. ​ ​ Ex: 2HgO → 2Hg + O ​2 6. Some compounds may be decomposed by electricity, called electrolysis, into their elements. ​ ​ Ex: 2NaCl → 2Na + Cl ​2

Balancing Equations and Identifying Reactions Synthesis / Combination 2> smaller compounds/elements → 1 compound ​ ​ Decomposition 1 compound → >2 smaller compd / elements ​ Combustion reaction with O2 as a reactant → ​ ​ Single Replacement “Sports Substitution” AB + B → AC + B Double Replacement “Double Dating” AB + CD → AD + CB

Organic Alkane Naming Throughout the year, you will see problems involving compounds made primarily of C and H. These are called hydrocarbons, or alkanes. You should become familiar with the first 10 normal alkanes. ​ ​ ​ ​ Methane CH4 Hexane C6H14 ​ ​ ​ ​ Ethane C2H6 Heptane C7H16 ​ ​ ​ ​ ​ ​ Propane C3H8 Octane C8H18 ​ ​ ​ ​ ​ ​ Butane C4H10 Nonane C9H20 ​ ​ ​ ​ ​ ​ Pentane C5H12 Decane C10H22 ​ ​ ​ ​ ​ ​

A handy way to remember the top 4 is with “Me Eat Peanut Butter!” You may use the “times 2, plus 2” rule to remember the ratio of C to H. e.g. octane: I know “octa-“ refers to 8 carbons, so 8 x 2 = 16 + 2 = 18 H ​ ​ ​ ​

Another interesting fact about hydrocarbons: When you burn (combustion) compounds with H and C

(generally with O also), you always produce CO2 + H2O. ​ ​ ​ ​ ​ ​ ex: CH4(g) + 2O2 (g) → CO2 (g) + 2H2O (g) ​ ​ ​ ​ ​ ​ ​ ​

Mass Percent The equation for the % of anything is: % = “X” (your focus) x 100 ​ ​ ​ TOTAL Know %, want grams: (work backwards): Shift your % decimal 2 loops back, multiply by TOTAL! ​

*If you are given a compound, asked for % of an element: Add up molar masses & use the equation above. *If you are given a reaction and you want to know the % element in an impure substance: (1) Figure out the mass of the element in question in the compound on the product side by finding % element in the compound ((X/total) x 100)). (2) Use the % to find the grams of the element in the given product sample (Shift your % decimal…) (3) Since the grams of the element should be equal on R & P side, grams element x 100 ​ ​ total grams Reactant

Unknown CH/CHO Assistance Sheet Use this information for #68-73 Before you begin the problem, analyze that you are solving for an EMPIRICAL and MOLECULAR FOR”MOL”A. So, you need to find “MOLES” of C, H, and O to get the answer. 1. Write the equation for the combustion reaction. Then, write the values given below each substance. ​ ​ 2. · Find the %C in the CO2 and multiply this constant value (using the decimal form of the percent) by the ​ ​ ​ ​ total grams of CO2. Underline this value, #g C. ​ ​ ​ ​ · Change #g C→ #moles C and underline your answer. ​ ​ ​ · Repeat this for the H in H2O. ​ ​ 3. Now, you have to deal with the oxygen. The problem is that the O appears in both of the reactants, ​ ​ making it hard to find exactly how much is only in the {CHO}, not in the O2. But, you know by the Law ​ ​ ​ of Conservation of Mass how much C and H are in {CHO}, because the amount present in the products ​ must be equal to what is present in the reactants and each of these only appear in one place on either side. You also were given the amount of {CHO} that you started with; the C+H+O = {CHO}! · #grams of {CHO} - #grams C - #grams H = #grams O ​ · change #grams O → #moles O ​ ​ 4. Write the for”MOL”a. Divide by the lowest number to get whole numbers greater than 1. This whole number, reduced ratio between the atoms is called the EMPIRICAL for“mol”a. ​ ​ ​ 5. For the molecular for”mol”a, use the “ME” equation to find your “multiplier”: Molar mass of MOLECULAR FORMULA = Molar mass of EMPIRICAL FORMULA Multiply the empirical formula by this value to find the molecular formula. YOU ARE DONE!! Sample problem: Vanillin (methyl vanillin) is used in flavorings, fragrances, pharmaceuticals, and ​ ​ ​ perfumes is made of carbon, hydrogen, and oxygen. If 3.00g of the substance is combusted and 6.93 grams of CO2 and 1.42 grams of water are produced, what is the empirical formula for the substance? The molar ​ ​ mass of the molecular formula is 456 g/mol. Find the molecular formula.

AP Chemistry Helpful Equations Guide The following are optional ways to solve particular types of problems. Some are simple rules we will follow when solving problems. Molecular Weights *Using the NEW AP EXAM P.T, use the entire # from the periodic table. (units: g/mol) Mass % % X = grams of element X x 100 (a.k.a. % composition or ​ ​ ​ total molecular weight of compound % by weight) Empirical Formula or Use the following steps. Start at the point of units that you are given. “forMOLa” Step 1: Change % to grams (change the symbol) Step 2: Change grams to moles (divide by molar mass). Step 3: Write the “formola” and divide by the lowest moles. Empirical Formula a. Calculate grams of each element: -when masses of products #g of product mole (MW) #g of element are given (combustion (MW) #g mole process) of product **NEW b. If the compound given contains oxygen, you need to subtract grams of ​ each element from the total mass to find how much oxygen there is. ​ c. Now you know grams of each element. Follow 2&3 under “Empirical Formula”. Molecular Formula “ME Equation” : -when mass of compound M = MW of Molecular Formula (given) = “Multiplier” (whole #) ​ ​ ​ ​ and Empirical Formula E MW of Empirical Formula (use PT) are given Multiply the subscripts in the empirical formula by the multiplier. Grams → Moles # grams mole (Use P.T to find molecular weight in g/mol) ​ (MW)# grams

Moles → Grams # moles (MW)# grams (Use P.T to find molecular weight in g/mol) ​ mole

23 Moles → Molecules # moles 6.02 x 10 ​ molecules ​ mole

Molecules → Moles # molecules mole 23 6.02 x 10 ​ molecules ​

Stoichiometry There are three bridges (ratios) you can use when going from one ​ ​ chemical to another. They are M L M (not M & M ). These stand for: ​ ​ Moles Liters Molecules

Example: Find molecules of A when you know grams of B 23 # grams B mole # mol A 6.02 x 10 ​ molecules ​ ​ ​ (MW)# grams B # mol B mol A ​ ​ (Note: in bold is the ratio of the formulas from the chemical equation.) Remember, the only time you can use 22.4 liters = 1 mole is for a gas at STP. ​ ​ ​ ​

*NEW: You will use the following AP Periodic Table for the molar masses. **DO NOT ROUND THEM ANYMORE!

POLYATOMIC IONS TO MEMORIZE 1- Charged Ions 2- Charged Ions 3- Charged Ions 1- 2- 3- dihydrogen phosphate H2PO4 hydrogen phosphate HPO4 phosphate PO4 ​ ​ ​ ​ ​ ​ ​ ​ 1- 2- 3- hydrogen sulfite HSO3 sulfite SO3 phosphite PO3 ​ 1​ - ​ 2​ - ​ 3​ - hydrogen sulfate HSO4 sulfate SO4 borate BO3 ​ ​ ​ ​ ​ ​ 1- 2- bicarbonate HCO3 carbonate CO3 ​ ​ ​ ​ (hydrogen carbonate) 1- 2- nitrite NO2 chromate CrO4 ​ 1​ - ​ ​ 2- nitrate NO3 dichromate Cr2O7 ​ ​ ​ ​ ​ ​ 1- 2- hypochlorite ClO silicate SiO3 1​ - ​ ​ 2- chlorite ClO2 oxalate C2O4 ​ ​ 1- ​ ​ ​ ​ chlorate ClO3 ​ 1​ - perchlorate ClO4 ​ ​ cyanide CN1- ​ thiocyanate SCN1- ​ hydroxide OH1- 1- ​ 1- ​ acetate C2H3O2 / CH3COO ​ ​ ​ ​ ​ ​ ​ ​ ​ 1- permanganate MnO4 ​ ​ - bromate BrO3 ​ -​ + azide N3 ammonium NH4 ​ ​ ​ ​

Nomenclature Tip Sheet

Diatomics: H2 N2 O2 F2 Cl2 Br2 I2 Use the “Triple 7 Rule” or “H-I O-N F-Cl-Br” ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ Molecular: The prefixes tell you how many, just write the formula and do not reduce. ​ Ionic: If there is a metal, you must “REDUCE CRISS-CROSS ABSOLUTE”. Remember to put polyatomic ions in ​ ​ ​ parentheses when there’s more than 1. Tips that have helped in the past to memorizing some of these: 1. First of all, notice the bolded borders. These ions have been grouped according to similarities. 2. Choosing –ite versus –ate: “After I –ate, I gained an O”. Notice that the –ate version contains an extra oxygen atom ​ ​ compared to the –ite. **Please also note, -ite and –ate do not tell how many O atoms, just whether there are more or less. -3 -2 1- + ​ ​ ​ ​ 3. Compare PO4 to HPO4 to H2PO4 . Notice that each time you add a H , the overall charge increases. (that’s what happens ​ ​ ​ ​ ​ ​ ​ ​ ​ when you add + charges.) This works for others on the list. 2- ​ 4. Silicate: SiO3 “Silly Kate rides a tricycle, not a bicycle”. Don’t ask!! Silicate has -O3. The charge is –2. ​ ​2- ​ ​ ​ ​ ​ ​ 2- ​ ​ 5. Oxalate: C2O4 “A COw (or an Ox) has 2 eyes, 4 legs, 2 ears.” Again, don’t ask. Oxalate is C2O4 (all evens.) ​ ​ ​ ​ ​ ​ 2- ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ 6. Carbonate: CO3 Have some “carbonated” COke in your car(3 letters); it’s better with 2 people: 1- ​ ​ rd ​ ​ ​ ​ ​ ​ 1- ​ ​ ​ ​ ​ 7. Nitrate: NO3 Night is the 3 part of the day and there is one moon, so NO3 is nitrate. ​ ​ 2- ​ 2-​ ​ ​ 8. Chromate: CrO4 Chrome wheels come in 4’s and then think “24’s” CrO4 ​ ​ 1- ​ ​ 9. Permanganate: MnO4 ​ “I per-four(prefer) one mango” ​ ​

Nick the Camel ATE a Clam & Crepes Supper in Phoenix ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ Nitrate Carbonate Chlorate Chromate Sulfate Phosphate 1- 2- 1- 2- 2- 3- NO3 CO3 ​ ClO3 ​ CrO4 ​ SO4 PO4 ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ 1-​ ​ - Example: Nick has 3 consonants and 1 vowel, so NO3 ​ ​ ​ ​ ​ ​ - The –ite version is just one less oxygen, with the same charge ​ + ​ 2- 2- ​ 3-​ 1- - Add H ​ to CO3 ,​ SO4 ,​ or PO4 ​ and the charge just goes UP by one. Ex: HCO3 ​ ​ ​ ​ ​ ​ ​ ​ ​ ​

THE PACKET: AP Chemistry Name______Basics of Chemistry Packet

The material included in this packet covers approximately the first 3 chapters of AP Chemistry. You may use your textbook to help you review the material. The following material should be review ​ for most of you and we recommend that you begin this packet a couple weeks before school resumes. (Not too early - so it stays fresh)! Please initial and check off the following DUE the FIRST DAY of school: ◻ Complete Basics Packet Initials______◻ Memorize Polyatomic Ion Sheet (see Ref’s) Initials ______(*Poly Ion Qz –Class Day 3) ◻ Need to Review? Go to www.mervetismail.com & click “Class Lecture Videos” ​ ​

rd Plan for the first test to be the beginning of the 3 ​ week of school. Prior to the test, it is ​ ​ ​ ​ recommended that you SKIM (read) Chapters 1-3 of Chemistry (BLB): ​ https://drive.google.com/file/d/0B1Zhp01hnSI_WVVqQ1VYZ3hUdE0/view *See Ref’s for link. ​ ​ Ch.1: Matter & Measurement (pdf p46) ​ ​ Ch.2: Atoms, Molecules & Ions (pdf p82) ​ ​ Ch.3: Stoichiometry: Calculations with Chemical Formulas & Equations (pdf p120) ​ ​

YOU ARE ONLY REQUIRED TO COMPLETE THE CIRCLED(OR *) PROBLEMS. A. Significant Figures. Review Significant Figures Video. Complete the following questions. ​

*1. How many significant figures are in each of the following measurements? ​ a. 35.409 grams ______b. 100.0 ml ______23 c. 0.044 grams ______d. 4.260 x 10 ​ molecules ______​

*2. Compute the correct answer using significant figures. *Use “Place Rule” for + & -. ​ a. 23.01 grams + 7.7 grams + 9.110 grams = ______a. 23. 1 cm x 7.71 cm x 9.100 cm = ______

*3. Compute the correct answer using significant figures. ​ a. What is the density of a hydrochloric acid solution that has a mass of 17.84 grams and occupies 14.0 milliliters? (density= g/ml)

b. What is the volume, in L, required of nitric acid if the mass of the acid is 32.0 grams? The density of nitric acid is 1.251 g/ml.

4. Name the following compounds. *Mentally label it as Molecular or Ionic first. (See Ref’s for help)

*a. BO3 *b. Ca3P2 ​ ​ ​ ​ ​ ​

*c. SeO4 *d. Cl3O2 ​ ​ ​ ​ ​ ​

*e. TeI5 *f. Se2N4 ​ ​ ​ ​ ​ ​

*g. OF8 *h. As4Te7 ​ ​ ​ ​ ​ ​

*i. Ba(CH3COO)2 *j. Ti(CN)3 ​ ​ ​ ​ ​ ​ k. K2S l. CoCO3 ​ ​ ​

m. Co3N2 n. NaClO3 ​ ​ ​ ​ o. LiNO p. MgSO ​3 ​4

q. Mn(PO4)2 r. RbMnO4 ​ ​ ​ ​

s. CsOH t. Pd(ClO4)4 ​ ​ ​

u. Fe2S3 v. Sn(OH)2 ​ ​ ​ ​

w. Ni(NO2)2 x. K2Cr2O7 ​ ​ ​ ​ ​ ​ ​ ​

y. In(NO3)3 z. YI3 ​ ​ ​ ​

5. Name the following Acids

*a. H2S *b. H2CrO4 ​ ​ ​ ​ ​ ​ ​ c. HCl d. H3P ​ ​

*e. HMnO *f. HBr ​4 ​ ​ g. H2SO4 h. HClO4 ​ ​ ​ ​

*i. HC2H3O2 *j. HNO2 ​ ​ ​ ​ ​ ​ ​ ​

*Answers to select problems will be posted on www.mervetismail.com ​ → CALENDARS → AP Chem Cal → Sept 4, 2018 *Join Remind101 AP Chem Summer: Text @sumapc to 81010

6. Write the formulas for these names. a. tetrasilicon triarsenide b. diselenium hexabromide

*c. diphosphorus monoxide *d. octasulfur trioxide ​ ​ *e. carbon monoxide *f. sodium azide ​ ​ g. silicon heptaiodide h. pentaboron triselenide

*i. nickel(II) nitrite *j. aluminum perchlorate ​ ​ *k. copper(II) carbonate *l. cadmium sulfate ​ ​ *m. mercury(I) nitrite *n. hafnium selenide ​ ​ o. ruthenium(III) sulfate p. yttrium carbonate q. gallium(III) selenide r. osmium(IV) chromate s. niobium(V) sulfate t. ruthenium(IV) phosphate u. hexaoxygen difluoride v. magnesium sulfide w. calcium phosphide x. tetra-arsenic hexaoxide y. lead(IV) chloride z. ruthenium(VI) sulfate

Write the formulas for the following acids. *a. phosphorous acid *b. nitric acid ​ ​ c. sulfuric acid *d. oxalic acid ​ *e. hydrofluoric acid *f. boric acid ​ ​ g. hydrocyanic acid h. hypochlorous acid

*i. carbonic acid j. chlorous acid ​

C. Balance the following equations and identify the type of reaction.

*11. ____Fe2O3 (s) → ____Fe(s) + ____O2 (g) ​ ​ ​ ​ ​ ​ ​

*12. ____C3H8 + ____O2 → ____CO2 + ____H2O ​ ​ ​ ​ ​ ​ ​ ​ *13. ____NaCl + ____Br → ____NaBr + ____Cl ​2 ​2 ​

D.Predicting Products of a Chemical Reaction REFER to PREDICTING PRODUCTS GUIDE ​ Predict the products for the following chemical equations. Classify each reaction as (C) Combustion, (SD) Single Displacement, (DD) Double displacement, (D1-6) Decomposition, or (S) Synthesis. Then, write the balanced chemical equation. Indicate the type of reaction on the line.

14. __DD___ aluminum sulfate + calcium phosphate → ​ ​ Al2(SO4)3 + Ca3(PO4)2 → 2Al(PO4) + 3CaSO4 ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​

*15. ______magnesium chloride + silver nitrate → ​

*16. ______potassium chlorate → ​

*17. ______hydrogen gas + oxygen gas → ​

*18. ______silver metal + copper (II) nitrate → ​

*19. ______sulfurous acid → ​

*20. ______copper (I) oxide + sulfuric acid → ​

*21. ______nitrogen gas + hydrogen gas → ammonia gas ​

22. ______sodium iodide + chlorine gas →

23. ______copper (II) hydroxide →

24. ______ammonia gas (NH3) + hydrochloric acid → (Single product) ​ ​

+ - 25. ______potassium metal + water (H OH​ )→​ ​ ​

+3 26. ______iron + oxygen gas → (will form Fe )​ ​

27. ______aluminum metal + sodium acetate →

28. ______gallium hydroxide + calcium sulfate →

29. ______calcium chlorate →

30. ______tungsten (V) chlorate + silver nitride →

31. ______barium chloride + sodium hydroxide →

4+ 32. ______tin metal + fluorine gas→ (Sn )​ ​

33. ______potassium iodide + bromine gas →

34. ______octane(C8H18) + oxygen gas → (remember octane is a hydrocarbon) ​ ​ ​ ​

35. ______sodium chloride + sulfuric acid →

36. ______glucose(C6H12O6) + O2 → (glucose reacts as a hydrocarbon) ​ ​ ​ ​ ​ ​ ​ ​

37. ______potassium hydroxide + phosphoric acid →

38. ______iron (II) sulfide + hydrochloric acid →

39. ______magnesium + nitrogen gas →

*40. Write the balanced equation for the combustion of: ​ a) propane

b) butane

Limiting Reagents: Think about a “Grilled Cheese Party” ​ ​ 1 Cheese + 2 Bread → 1 Grilled Cheese Sandwich You went to Costco and bought one of those 100 singles of American Cheese. You’re all going to get the party started and you notice that you FORGOT TO BUY LOAVES OF BREAD. You only have a pack of bread with 6 slices of bread. a) How many grilled sandwiches can you make?______(3) b) In a sense, 100 moles of cheese were allowed to react with 6 moles of bread, so how many moles of grilled cheese sandwiches could you produce?______(3 moles) c) What is the limiting reagent? ______. (bread) d) What’s the excess reagent? ______(cheese) How much is in excess? ____ (97)

ANSWER THE FOLLOWING CIRCLED PROBLEMS, # 42 – 72 ON SEPARATE PAPER!! YOU MUST SHOW WORK ON SEPARATE PAPER FOR FULL CREDIT!!

**USE THE AP PERIODIC TABLE FOR ALL MOLAR MASSES. DO NOT ROUND! *Use your sig fig rules for all of the following.

*42. If I began with 11.0 g AgNO3 and 10.0 g Na2SO4, how many grams of Ag2SO4 can I make? ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ Na2SO4 + 2AgNO3 → 2NaNO3 + Ag2SO4 ​ ​ ​ ​ ​ ​ ​ ​

43. Find the molecular weight (molar mass) of each of these compounds. ↓add, not multiply ​ *a. RbOH b. Na2Cr2O7 c. AlBr3 d. Ba3(PO4)2 *e. Fe(NO3)2 · 4H2O ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ 44. Determine the molecular weight of each of the following. ↓add, not multiply ​ *a. Ga(NO3)3 b. Y2(CO3)3 *c. CoCl2 · 6H2O ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ 45. Determine the % of chlorine in each of these compounds. ​ ​ *a. LiCl b. HClO4 c. AlCl3 *d. Mg(ClO2)2 ​ ​ ​ ​ ​ ​ ​ 46. Determine the mass percent (% composition)

*a. % C in Al2(CO3)3 b. % O in Na2Cr2O7 ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ 47. How many moles are represented in each of these samples? ​ ​ *a. 150. molecules of H2O b. 200.0 grams of H2O ​ ​ ​ ​ c.​ 500. atoms of Cu d. 500.00 grams of Fe

*48. a. How many moles are in 58.6 g of AgNO3? b) How many formula units is this? ​ ​ ​ 49. Determine the mass in grams of each of the following. ​ ​ 20 *a. 3.00 x 10 ​ molecules of O2 b. 4.66 moles of O2 ​ ​ ​ 21 ​ c. a single molecule of O d. 4.50 x 10 formula​ units of KOH ​2 ​ *e. 0.00255 moles of KOH ​

50. Ascorbic acid (vitamin C), C6H8O6, is an essential vitamin. It cannot be stored by the body and therefore must be ​ ​ ​ ​ ​ ​ present in the diet. a. *What is the molecular weight of ascorbic acid? ​ b. *If you were to take a vitamin C tablet every day, with 1500. g of ascorbic acid, how many moles would you ingest?​

c. *How many molecules of C6H8O6 are you taking? ​ ​ ​ ​ ​ ​ ​ 51. Aspartame is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when it dissolves in water. It is marketed as “Nutra-Sweet”. The molecular formula of aspartame is C14H18N2O5. ​ ​ ​ ​ ​ ​ ​ ​ a. What is the molecular weight of aspartame? b. How many molecules of aspartame are present in 15.0 grams of the compound? c. Calculate the mass of 3.56 moles of aspartame. d. How many molecules are in 5.900 mg of aspartame? 15 e. What is the mass in grams of 21.66 x 10 ​ molecules of aspartame? ​ f. What is the mass in grams of one molecule of aspartame?

*52. A compound contains 22.1% Al, 25.4 % P, and 52.4 % O. What is the empirical formula? ​ 53. A particular compound contains 25.93% N and 74.07 % O. What is the empirical formula?

*54. An organic compound containing 8.28 g C and 1.72 g H is analyzed. What is the empirical formula? If the molecular​ weight is 58.0 g/mol, what is the molecular formula?

55. A compound that contains only carbon, hydrogen, and oxygen is 48.38% C, 8.12 % H, and 43.50 % O. What is the empirical formula for this compound?

56. The active ingredient in photographic fixer solution contains sodium, sulfur, and oxygen. Analysis of this sample shows that the sample contains 0.979 g Na, 1.365 g S, and 1.021 g O. What is the empirical formula for this compound?

57. A compound that contains only nitrogen and oxygen is 30.4% by mass of nitrogen. The molar mass of the compound is 92 grams/mole. What is the empirical formula? What is the molecular formula?

*58. A sample of urea contains 1.1211 g N, 0.161 g H, 0.480 g C, and 0.640 g O. What is the empirical formula for this​ compound? If the compound is found to have a molecular weight of 180. g/mol, what is the molecular formula?

59. A compound containing only sulfur and nitrogen is 69.6% S by mass. It also has a molar mass of 184 g/mol. What are the empirical and molecular formulas?

60. Acrylic acid, used in the manufacture of plastic has a composition of 50.0% C, 5.60% H, and 44.4% O. The molar mass of the compound is 288 g/mol. What are the empirical and molecular formulas of this compound?

*61. Over the years, the thermite reaction has been used for welding railroad rails, for incendiary (combustible) bombs,​ and to ignite solid fuel rocket motors. The reaction is:

Fe2O3 (s) + 2 Al (s) ←→ 2 Fe (s) + Al2O3 (s) ​ ​ ​ ​ ​ ​ ​ ​ What mass of iron III oxide must be used to produce 515.0 g of iron?

62. The reusable booster rocket of the U.S. space shuttle employs a mixture of aluminum and ammonium perchlorate for fuel. A possible equation for the reaction is:

3 Al (s) + 3 NH4ClO4 (s) ←→ Al2O3 (s) + AlCl3 (s) + 3 NO (g) + 6 H2O ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ What mass of aluminum must be used to produce 67 grams of AlCl3? ​ ​

63. Alka-Seltzer uses the reaction of sodium bicarbonate with citric acid to produce a fizz. The reaction is:

3 NaHCO3 (aq) + C6H8O7 (aq) ←→ 3CO2 (g) + 3 H2O (l) + Na3C6H5O7 (aq) ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ What mass of C6H8O7 must be used in the tablet to produce 1.558 g of CO2? ​ ​ ​ ​ ​ ​ ​ ​

*64. White phosphorus, P4, burned in excess oxygen forms diphosphorus pentaoxide, P2O5. ​ ​ ​ ​ ​ ​ ​ a. Write a balanced equation for the reaction that occurs (remember oxygen is O2). ​ ​ b. How many grams of P2O5 are formed if 3.40 g of P4 react? ​ ​ ​ ​ ​ ​ c. How many grams of oxygen would be consumed using 16.00 g of P4? ​ ​

*65. When a mixture of silver metal and sulfur is heated, silver sulfide is formed: ​ 16 Ag (s) + S8 (s) ←→ 8 Ag2S (s) ​ ​ ​ ​ How many grams of Ag2S are produced if 2.00 g of silver reacts with 2.00 g of sulfur? ​ ​

66. Aluminum burns in bromine to produce aluminum bromide:

2 Al (s) + 3 Br2 (l) ←→ 2 AlBr3 (s) ​ ​ ​ ​ In a certain experiment, 6.00 g of aluminum is burned in 24.0 g of bromine. What is the maximum amount of aluminum bromide that can be produced?

67. Acid-base neutralization reactions are very common in industrial processes. This is the reaction of sulfuric acid with sodium hydroxide:

H2SO4 (aq) + 2 NaOH (aq) ←→ Na2SO4 (aq) + 2H2O (l) ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ What is the maximum amount of Na2SO4 that can be produced if you use 26.5 g of H2SO4 and 25.4 g of NaOH? ​ ​ ​ ​ ​ ​ ​ ​

Some higher thinking problems…SEE REF’s ABOVE FOR “Mass %” & “UNKNOWN CH/CHO” ​ *68. Impure nickel can be purified by first forming the compound Ni(CO)4, which is then decomposed by heating to ​ ​ yield​ very pure nickel. The metallic nickel in the sample reacts with carbon monoxide as follows: Ni (s) + 4 CO ​ (g) ←→ Ni(CO)4 (s) ​ ​ The other metals in the ore do not react with carbon monoxide. If 94.2 g of a metal mixture produced 98.4 g of

Ni(CO)4 , what is the mass percent of nickel in the original sample? ​ ​ **The following are new problems. ☺ *SEE “Unknown CH/CHO Assistance Sheet” ​ ​ 69. Alcohols burn rapidly in oxygen. A chemist is burning an alcohol in an attempt to determine its identity. She knows the possibilities are: CH3OH, C2H5OH, C3H7OH, C4H9OH, or C5H11OH. In the combustion of 5.00 grams of an ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ ​ alcohol the chemist produced 11.89 grams of CO2 and 6.09 grams of H2O. What is the identity of the alcohol? ​ ​ ​ ​

*70. Many people take a little ascorbic acid every day to keep from getting sick (remember it’s vitamin C). The ​ compound contains C, H, and O. During the combustion of 2.00 g of ascorbic acid, 3.09 g CO2 and 0.818 g H2O are ​ ​ ​ ​ produced. What is the empirical formula for the compound? What is the molecular formula if the molar mass is found to be 176 g/mol?

71. Menthol, a strong smelling substance used in cough drops is a compound of carbon, hydrogen, and oxygen.

When 15.96 grams menthol was subjected to combustion analysis, it produced 44.9 g CO2 and 18.4 g H2O. The ​ ​ ​ ​ molecular weight of the compound is 156 g/mol. What is the molecular formula?

*72. Hydrocarbons are compounds that contain only H and C. Most of these compounds are used as organic solvents or​ the building blocks of larger molecules. 7.00 g of one such hydrocarbon undergoes combustion and produces

23.69 g CO2 and 4.846 g H2O. What is the empirical formula for this hydrocarbon? What is the molecular formula if ​ ​ ​ ​ the molar mass is found to be 78 g/mol? (Remember only C and H).

73. The combustion of 10.0 g of a compound containing C, H, and O produced 20.0 g CO2 and 8.18 g H2O. What is ​ ​ ​ ​ the empirical formula? If the MW = 176 g/mol, what is the molecular formula?