<p> Advanced Placement Chemistry – Review Packet</p><p>Name______</p><p>Date______Advanced Placement Chemistry requires the student to be responsible for the information taught in the Honors or Academic Chemistry class. Included in this packet are 5 assignments which emphasize important chemistry concepts.</p><p>Assignment #1: Formula Writing and Nomenclature Memorize each formula, name and charge of the following common ions. </p><p>Positive Ions (cations) Negative Ions (anions) +1 -1 + - Ammonium (NH4) Acetate (C2H3O2) Cesium, Cs+ Bromide, Br- + - Copper (I) or cuprous, Cu Chlorate (ClO3) Hydrogen, H+ Cyanide (CN)- Lithium, Li+ Dihydrogen phosphate - (H2PO4) Potassium, K+ Fluoride, F- Silver, Ag+ Hydride, H- Sodium, Na+ Hydrogen carbonate or - bicarbonate (HCO3) +2 Hydrogen sulfite or bisulfite - (HSO3) Barium, Ba+2 Hydroxide (OH)- Cadmium, Cd+2 Iodide, I- +2 - Chromium (II) or chromous, Cr Nitrate (NO3) +2 - Copper (II) or cupric, Cu Perchlorate (ClO4) +2 - Iron (II) or ferrous, Fe Permanganate (MnO4) Lead (II) or plumbous, Pb+2 Thiocyanate (SCN)- Magnesium, Mg+2 -2 +2 -2 Manganese (II) or Manganous, Mn Carbonate (CO3) +2 -2 Mercury (I) or mercurous (Hg2) Chromate (CrO4) +2 -2 Mercury (II) or mercuric, Hg Dichromate (Cr2O7) +2 - Strontium, Sr Hydrogen Phosphate (HPO4) 2 Nickel, Ni+2 Oxide, O-2 +2 -2 Tin (II) or stannous, Sn Peroxide, (O2) -2 +3 Sulfate (SO4) Aluminum, Al+3 Sulfide, S-2 +3 -2 Chromium (III) or chromic, Cr Sulfite (SO3) Iron (III) or ferric, Fe+3 -3 -3 Arsenate (AsO4) -3 Phosphate (PO4)</p><p>Assignment #2: Nomenclature and Writing Formulas You will be expected to be able to write the formula of a compound, if given the name. You will also be expected to name the compound if given the formula. Review the rules for naming compounds. The rules were given to you during your Chemistry Class and are also in any basic chemistry textbook. 1. Name the following ionic compounds: Ca(NO3)2, SnO, Cu2CrO7, Al(CN)3, HCl, (NH4)2SO4, CrCO3, NiF2, NaH, BaO2, Fe(OH)3, Ag2(CrO4), Cr2(HPO4)3, KClO4, Ba(SCN)2. 2. Write the correct chemical formula for the following compounds: cadmium bicarbonate, plumbous chloride, aluminum oxide, copper(I) cyanide, mercury(I) acetate, sodium hydrogen sulfite, chromium(III) sulfate, silver dichromate, cesium peroxide, magnesium chlorate, nickel nitrate, manganese(II) hydroxide, cobaltous chloride, stannous dihydrogen phosphate, ammonium phosphate. 3. Name the following binary molecular compounds: Cl2O7, N2O5, P2O5, SbCl3, SF6, CO2, CO, N2H4, P4O10. 4. Write the formulas for the following binary molecular compounds: nitrogen dioxide, sulfur trioxide, chlorine pentafluoride, bromine trifluoride, boron trifluoride and phosphorus pentachloride. Answers: 1. calcium nitrate, tin(II) oxide or stannous oxide, copper(II) dichromate or cupric dichromate, aluminum cyanide, hydrochloric acid, ammonium sulfate, chromium(II) carbonate, nickel fluoride, sodium hydride, barium peroxide, iron(III) hydroxide or ferric hydroxide, silver chromate, chromium(III) hydrogen phosphate or chromus hydrogen phosphate, potassium perchlorate, barium thiocyanate.</p><p>2. Cd(HCO3)2, PbCl2, Al2O3, CuCN, Hg2(C2H3O2)2, NaHSO3, Cr2(SO4)3, Ag2Cr2O7, Cs2O2, Mg(ClO3)2, Ni(NO3)2, Mn(OH)2, CoCl2, Sn(H2PO4)2, (NH4)3PO4. 3. dichlorine heptoxide, dinitrogen pentoxide, diphosphorus pentoxide, antimony trichloride, sulfur hexafluoride, carbon dioxide, carbon monoxide, dinitrogen tetrahydride, tetraphosphorus decoxide.</p><p>4. NO2, SO3, ClF5, BrF3, BF3, PCl5</p><p>Assignment #3: The Mole You will be expected to use the mole concept in various contexts. You should know Avogadro’s number, the molar volume of a gas at STP, the meaning of STP and molar mass. All work and units should be shown. The use of dimensional analysis (conversion factors) is strongly encouraged. 1. Given 2.50 grams of SO3(g), calculate: a. The number of moles of SO3. b. The number of SO3 molecules. c. The number of sulfur and oxygen atoms present. d. The volume occupied by the gas at STP. e. The density of the gas at STP. 2. Given 2.80 x 1022 molecules of carbon dioxide gas, calculate: a. The number of moles of CO2. b. The mass of the sample. c. The number of carbon and oxygen atoms present. d. The volume of carbon dioxide gas at STP. e. The density of the gas at STP. 3. Given a volume of 250.0 mL of fluorine gas at STP, calculate: a. The mass of the fluorine gas. b. The number of fluorine molecules in the sample. c. The number of fluorine atoms in the sample. d. The density of the gas at STP.</p><p>Answers: 1. 0.0313 mol, 1.88x1022 molecules, 1.88x1022 S atoms, 5.64x1022 atoms O, 700.0 mL, 3.57 g/L. 2. 0.0465 mol, 2.05 g, 2.80x1022 atoms C, 5.60x1022 atoms O, 1.04 L, 1.96 g/L. 21 22 3. 0.424 g, 6.72x10 molecules F2, 1.34x10 atoms F, 1.70 g/L.</p><p>Assignment #4: Balancing Equations and Stoichiometry You will be expected to understand basic chemical equations and stoichiometry. 1. Balance the following equations: a. C2H6O + O2  CO2 + H2O</p><p> b. Al(OH)3 + H2SO4  Al2(SO4)3 + H2O</p><p> c. Na2CO3 + C + N2  NaCN + CO</p><p>2. Calculate the mass of carbon dioxide formed when 2.60g of C2H6O is burned in excess oxygen gas. Refer to equation 1a. 3. Calculate the mass of sulfuric acid that would react with 3.50g of aluminum hydroxide. Refer to equation 1b. 4. Calculate the volume of carbon monoxide gas, which would form when 2.80g of nitrogen reacts with excess reactants. Refer to equation 1c. 5. Identify the limiting reagent and excess reagent when 5.0g of Al(OH)3 reacts with 5.0g of H2SO4 as in equation 1b. Calculate the amount (in grams) of the excess reagent that remains at the completion of the reaction. 6. Assuming that reaction 1a has a 95% yield, calculate the volume of carbon dioxide that will be produced from 2.50g of oxygen gas is completely consumed.</p><p>Answers: 1. a.1,3,2,3 b. 2,3,1,6 c. 1,4,1,2,3 2. 4.97g 3. 6.60g 4. 47.0L</p><p>5. H2SO4 is the LR. 2.35g of Al(OH)3 remain after the reaction is complete.</p><p>6. 1.11 L CO2 Assignment #5: Molarity You will be expected to be familiar with the definition of molarity (M) and to be able to perform molarity related calculations. 1. Calculate the molarity of a solution prepared by dissolving 4.52g of Na2SO4 in enough water to prepare 350 mL of solution. 2. Calculate the mass of lead(II) nitrate present in 200.0mL of 0.50M Pb(NO3)2(aq). 3. Calculate the volume of 0.25M Ba(OH)2 that contains 15.0g of the solute. Answers: 1. 0.091M 2. 33.1g Pb(NO3)2 3. 35.03 mL of solution</p>