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Summer Assignment Please Note: This assignment is a requirement, and is NOT for extra credit! 1. Purchase your own copy of 5 Steps to a 5 on the AP: Chemistry, John T Moore, McGraw Hill, 2008-2009 Edition. 2. Buy a few color highlighters. 3. Read and study Chapter 1 and 2. Highlight material that applies to you. 4. Take the diagnostic test on Page 23. (Go ahead and write in the book, I will make an additional copy of this test for you to take before the AP Exam.) 5. Take a look at the AP and other websites. List the three most useful in the front cover of your book 6. Read and study (highlight, take notes in the margin, etc) and do all the review questions at the end of the chapter for Chapter 3 (Basics) and Chapter 5 (Stoichiometry) 7. Bring your highlighted book, notes and diagnostic test to school the first day of class in August. Points will be assigned to you and then the book will be returned to you for your further enjoyment. NO LATE ASSIGNMENTS WILL BE ACCEPTED!!! AP CHEMISTRY FIRST DAY TEST AP Chemistry is a difficult course. It is not all about memorization; however, having these items memorized is essential for success in learning the concepts covered in the course. Make flashcards, have your friends and family quiz you, take the lists with you on vacation, or do whatever it takes to get this information firmly planted in your head. Do not wait until the night before school begins. The first day test will cover six areas of memorization: 1. Polyatomic Ions (including name, symbol and charge) 2. Variable Valences for Transition Metals 3. Rules for Naming Acids 4. Rules for Naming Ionic Compounds 5. Solubility Rules 6. Determining Oxidation Numbers If this seems like too much work for the summer, please drop the course. Advanced Placement Chemistry is a college level course. You will need to be dedicated and work very hard if you are to be successful. Rules for Naming an Acid 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 Cl- is the Chloride ion so HCl = hydrochloric acid 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 ClO2- is the Chlorite ion so HClO2 = Chlorous acid. 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 ClO3- is the Chlorate ion so HClO3 = Chloric acid. Rules for Naming Ionic Compounds 1. Balance Charges (charges should equal zero) 2. Cation is always written first (in name and in formula) 3. Change the ending of the anion to -ide Solubility Rules 1. All compounds containing alkali metal cations and the ammonium ion are soluble. 2. All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble. 3. All chlorides, bromides, and iodides are soluble except those containing Ag +, Pb2+, or Hg2+. 4. All sulfates are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+. 5. All hydroxides are insoluble except compounds of the alkali metals, Ca2+, Sr2+,and Ba2+. 6. All compounds containing PO43-, S2-, CO32-, and SO32- ions are insoluble except those that also contain alkali metals or NH4+. Rules for Determining Oxidation Number Oxidation Number: A number assigned to an atom in a molecular compound or molecular ion that indicates the general distribution of electrons among the bonded atoms. 1. The oxidation number of any uncombined element is O. 2. The oxidation number of a monatomic ion equal the charge on the ion. 3. The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 4. The oxidation number of fluorine in a compound is always –1 5. Oxygen has an oxidation number of –2 unless it is combined with F, when it is +2, or it is in a peroxide, when it is –1. 6. The oxidation state of hydrogen in most of its compounds is+1 unless it combined with a metal, in which case it is –1. 7. In compounds, the elements of groups 1 and 2 as well as aluminum have oxidation number of +1, +2, and +3, respectively 8. The sum of the oxidation numbers of all atoms in a neutral compound is O. 9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the ion. Examples: (use your periodic table, group #’s are columns) CO: (Sum will equal 0 since it is a neutral molecule) O will have a -2 ox. number. 1C+1O=0 (C?) + (-2) = 0 C? = +2 Oxidation number of C in CO is +2 Oxidation number of O in CO is -2 (known) Check ox. number to see if it falls within range: +2 is in between the maximum value of C, +4, (Group #) and the minimum value of C, 4, (Group # - 8). So okay. Cr2O72-: (Sum of all oxidation numbers will equal -2 since it is an ion.) 2 Cr + 7 O = -2 2(Cr?) + 7(-2) = -2 2(Cr?) + (-14) = -2 2(Cr?) = +12 Cr? = +6 Oxidation number of each Cr in Cr2O72- is +6 Oxidation number of each O in Cr2O72- is -2 (known) Check ox. number to see if it falls within range: +6 is the maximum value that Cr can have (Group#). So okay. CS2: (Sum will equal 0 since it is a neutral molecule) C will have the positive oxidation number since it is less EN than S S will have a -2 charge since it is Gr # 6, (6 - 8 = -2) C+2S=0 (C?) + 2 (-2) = 0 (C?) + (-4) = 0 C? = +4 Oxidation number of C in CS2 is +4 Oxidation number of each S in CS2 is -2 (known) Check ox. number to see if it falls within range: +4 is the maximum value that C can have, (Gr#). So okay. NH4+: (Sum will equal +1 since it is an ion) H will have a +1 ox. number since it is bonded to N, a nonmetal. N + 4 H = +1 (N?) + 4(+1) = +1 N? = -3 Oxidation number of N in NH4+ is -3 Oxidation number of each H in NH4+ is +1 (known) Check ox. number to see if it falls within range: -3 is the minimum value that N can have, (Group # - 8). So okay. H5IO6: (Sum will equal 0 since it is neutral species.) H will have a +1 ox. number since it is combined w/ nonmetals Iodine will have a + charge since it is less EN than Oxygen 5H+I+6O=0 5(+1) + (I?) + 6(-2) = 0 (+5) + (I?) + (-12) = 0 (I?) + (-7) = 0 I? = +7 Oxidation number of I in H5IO6 is +7 Oxidation number of each H in H5IO6 is +1 (known) Oxidation number of each O in H5IO6 is -2 (known) Check ox. number to see if it falls within range: +7 is the maximum value that I can have, (Gr#). So okay. NaBH4: (Sum will equal 0 since it is neutral species.) H will have a -1 ox. number since it is combined w/ metals Na will have a +1 charge (+ Gr# = +1) Na + B + 4 H = 0 (+1) + (B?) + 4(-1) = 0 (+1) + (B?) + (-4) = 0 (B?) + (-3) = 0 B? = +3 Oxidation number of B in NaBH4 is +3 Oxidation number of each Na in NaBH4 is +1 (known) Oxidation number of each H in NaBH4 is -1 (known) Check ox. number to see if it falls within range: +3 is the maximum value that B can have, (Gr#). So okay. H2MnO4: (Sum will equal 0 since it is neutral species.) H is a +1 ox. number since it is combined w/ nonmetals (ignore metal) Mn will have a + charge since it is less EN than Oxygen 2 H + Mn + 4 O = 0 2(+1) + (Mn?) + 4(-2) = 0 (+2) + (Mn?) + (-8) = 0 (Mn?) + (-6) = 0 Mn? = +6 Oxidation number of Mn in H2MnO4 is +6 Variable Valences For Transition Metals Name Chromium Cr +2 Stock Name Chromium (II) Manganese Mn +3 +2 Chromium (III) Manganese (II) Iron Fe +3 +2 Manganese (III) Iron (II) Co +3 +2 Iron (III) Cobalt (II) Copper Cu +3 +1 Cobalt (III) Copper (I) Lead Pb +2 +2 Copper (II) Lead (II) Mercury Hg +4 +1 Lead (IV) Mercury (I) Sn +2 +2 Mercury (II) Tin (II) Gold Au +4 +1 Tin (IV) Gold (I) Silver Ag +3 +1 Gold (III) Silver Bismuth Bi +3 Bismuth (III) Antimony Sb +5 +3 Bismuth (V) Antimony (III) Cadmium Cd +5 +2 Antimony (V) Cadmium Zinc Zn +2 Zinc Cobalt Tin Symbol Charge Polyatomic Ions Name ammonium acetate bromate chlorate chlorite cyanide dihydrogen phosphate hypochlorite hydrogencarbonate(bicarbonate) hydrogen sulfate (bisulfate) hydrogen sulfite (bisulfite) hydroxide iodate nitrate nitrite perchlorate permanganate thiocyanate carbonate chromate dichromate oxalate selenate silicate sulfate sulfite phosphate phosphite Symbol NH4 C2H3O2 BrO3 ClO3 ClO2 CN H2PO4 ClO HCO3 HSO4 HSO3 OH IO3 NO3 NO2 ClO4 MnO4 SCN CO3 CrO4 Cr2O7 C2O4 SeO4 SiO3 SO4 SO3 PO4 PO3 Charge +1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -1 -2 -2 -2 -2 -2 -2 -2 -2 -3 -3 1. Write formulas for the following: 2. Name each of the following: a. barium sulfate ________________ a. CuSO4 ______________________ b. ammonium chloride ___________ b. PCl3 _______________________ c. chlorine monoxide ____________ c. Li3N ______________________ d. silicon tetrachloride ___________ d. BaSO3 _____________________ e. magnesium fluoride ___________ e. N2F4 _______________________ f. sodium oxide ________________ f. KClO4 ______________________ g. sodium peroxide _____________ g. NaH _______________________ h. copper(I) oxide ______________ h. (NH4)2Cr2O7 _________________ i. zinc sulfide _________________ i. HNO2 _______________________ j. potassium carbonate __________ j. Sr3P2 ________________________ k. hydrobromic acid ____________ k. Mg(OH)2 ____________________ l. perchloric acid _______________ l. Al2S3 ________________________ m. lead(II) acetate ______________ m. AgBr _______________________ n. sodium permanganate _________ n. P4O10 _______________________ o. lithium oxalate _______________ o. HC2H3O2 ____________________ p. potassium cyanide ____________ p. CaI2 ________________________ q. iron (III) hydroxide ___________ q. MnO2 _______________________ r. silicon dioxide _______________ r. Li2O ________________________ s. nitrogen trifluoride ___________ s. FeI3 ________________________ t. chromium(III) oxide __________ t. Cu3PO4 _____________________ u. calcium chlorate _____________ u. PCl3 _______________________ v. sodium thiocyanate ___________ v. NaCN ______________________ w. nitrous acid _________________ w. HF _______________________ 2. Find the mass percent (percent compostion) of nitrogen in each of the following compounds: a. NO b. NO2 c. N2O4 d. N2O 3. Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the compound to be 7.74 % by mass. Find the empirical and molecular formulas of benzene. 4. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide. a. Write a balanced chemical equation for this reaction. b. How many grams of calcium oxide will be produced after 12.25 grams of calcium carbonate are completely decomposed? c. What is the volume of carbon dioxide gas produced 12.25 grams of calcium carbonate at STP? d. What is the volume of carbon dioxide in (c) if the pressure is pressure is 785mm Hg and the temperature is 30oC? (R =62.4 mm x L/mol x K) 5. Hydrogen gas and bromine gas react to form hydrogen bromide gas. a. Write a balanced equation for this reaction. b. 3.2 grams of hydrogen react with 9.5 grams of bromine. Which is the limiting reagent? c. How many grams of hydrogen bromide gas can be produced using the amounts in (b)? d. How many grams of excess reactant are left unreacted? e. What volume of HBr, measured at STP is produced in (b)? 6. When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products are hydrogen cyanide gas and water. a. Write a balanced chemical equation for this reaction. b. Calculate the mass of each product produced when 225 grams of oxygen gas is reacted with an excess of the other two reactants. c. If the actual yield of the experiment in (b) is 105 grams of HCN, calculate the percent yield.