Nomenclature 1. Name these binary compounds of two nonmetals. IFy N204_ PCl3_ N205_ .As40io_ - S2Cl2_ XeF2. SF6_ 2. Name these binary compounds with a fixed charge metal. AICI3. KI CaF2_ MgO_ SrBr2. AhOs. Bal2_ Na2S. 3. Name these binary compounds of cations with variable charge. CuCh. PbCl4_ Aul3_ Fe203_ . CU2S_ SnO HgS_ CoP 4. Name these compounds with polyatomic ions. Fe(N03)3_ Ca(C103)2_ NH4N02_ NaOH . KNO2 CU2SO4 _NaHC03_ Cu2Cr207 5. Name these binary acids HC1 HI. HF 6. Name these acids with polyatomic ions. HC104_ H3P04_ H2C204_ H2S04_ . HN02_ . H2C03_ HC2H302_ H2Cr04_ 7. Name these compounds appropriately. CO_ Nl3_ LiMn04_ SO2 FeFs NH4CN _ A1P_ _HC10 CuCr207_ KCzHaOz. 8. Write the formulas for the following compounds. Tin (IV) phosphide copper (II) cyanide. HI03_ OF2__ HF_ K20_ . MnS_ Magnesium hydroxide Sulfurous acid Potassium nitride Gallium arsenide Zinc fluoride sodium peroxide, lithium silicate chromium (III) carbonate. cobalt (II) chromate dichromic acid Solubility rules 9. Review solubility rules and identify each of the following compounds as soluble or insoluble in water. Na2C03 K2S Agl FeS Li20 AgClOs C0CO3 BaS04 Ni(N03)2 PbCh Mn(C2H302)2 Sn(S03)4 Pb(N03)2 (NH4)2S KI CuS04_ Cr(OH)3, FeF2 10. Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the products. If yes, identify the precipitate. silver nitrate and potassium chloride magnesium nitrate and sodium carbonate strontium bromide and potassium sulfate cobalt (III) bromide and potassium sulfide ammonium hydroxide and copper (II) acetate. lithium chlorate and chromium (III) fluoride _ Balancing Equations 11. Balance the following equations with the lowest whole number coefficients. Ss + 02^ SO3 C10H16 + C b ^ Fe + O2 -> C+ HC1 Fe203 C7H6O2 + O2 -> CO2 + H2O KCIO3 -» H3ASO4 -> KC1 + O2 AS2O5 + H2O V205 + H C l ^ VOCI3 + H2O Hg(OH)2 + H3PO4 "> Hg3(P04)2 + H2O Stoichiometrv and Limiting Reactants 12. Given the equation below, what mass of water would be needed to react with lO.Og of sodium oxide? Na20 + H2O -> 2NaOH 13. ZNaClOs -> 2NaCI + 3O2 What mass of sodium choride is formed along with 45.Og of oxygen gas? 14. 4NH3 + 502 -> 4NO + 6 H2O What mass of water will be produced when 100.Og of ammonia is reacted with excess oxygen? 15. If the reaction in #14 is done with 25.Og of each reactant, which would be the limiting factor? 16. Na2S + 2AgN03 -> Ag2S + ZNaNOs If the above reaction is carried out with 50.Og of sodium sulfide and 35.Og of silver nitrate, which is the limiting factor? What mass of the excess reactant remains? What mass of silver sulfide would precipitate? 17. 6NaOH + 2A1 -> ZNasAlOs + 3H2 What volume of hydrogen gas (measured at STP) would result from reacting 75.Og of sodium hydroxide with 50.Og of aluminum? •J&<\c{r . Round the following numbers to three significant figures, a. 4325 b. 6.873 xlO 3 , c. 0.17354 7 . Perform the indicated operations and round your answers to the proper .number i. of significant figures. Assume that all answers were obtained from measurements. a. (2.11 xl0"3) + (1.54 xlO"3) c. (4.56 + 18.7)/(1.23 x 102) ~ 3 2 2 b. (1.54 xl0" ) +(2.11 xlO" ) d. (1.23 x 10" )(4.56 + 1.87) ^ . Make the following conversions: a. 0.75 kg to milligrams c. 2390 g to kg b. 1500 millimeters to km d. 0.52 km to metersIf „ How many cubic meters (m3) are there in 4312 cubic centimeters (cm3)? The helium gas stored inside a large weather balloon weighs 13.558 grams. What is the volume of this balloon if the density of helium is 0.1786 g/L? j Write the electron configuration (long way) for krypton. {/ Write the orbital notation (boxes) for t A o A ^ c v ^ ^ . 7 Write the electron configuration using the Noble Gas core method for nickel. <f. Write a balanced equation and indicate the reaction type (single or double replacement, decomposition, or synthesis/composition) for each of the following: a. Magnesium nitrate (aq) + sulfuric acid (aq) —> magnesium sulfate (aq) + nitric acid (aq) b. Potassium carbonate (aq) + barium chloride (aq) —> potassium chloride (aq) + barium carbonate (aq) c. Aluminum chloride (aq) + sulfuric acid (aq) —> aluminum sulfate (aq) + hydrogen chloride (aq) d. Cadmium phosphate (s) + ammonium sulfide (aq) —• cadmium sulfide (s) + ammonium phosphate (aq) ^f. Calculate the percentage of water in the following compounds: a. Calcium chloride dihydrate b. Calcium chloride hexahydrate \o. Determine the moles of NaiS that can be prepared by the reaction of 0.2240 moles of sodium with 0.1320 moles of sulfur. Which reactant in the limiting reactant? 16 Na + Sg -> 8 Na2S , A zinc sample, which has a mass of 40.0 grams, reacts with 20.0 grams of pure HC1. Zinc chloride and hydrogen gas are produced. Calculate the moles of H2 gas produced. 11". How many molecules of ammonia would be produced if 12.4 grams of hydrogen gas reacted with«12.0 grams of nitrogen gas at STP? I 3-" ^ 46.2 grams of sulfiir trioxide gas decompose into oxygen and sulfur dioxide, how many liters of oxygen gas will be produced at STP? ? ^ How many liters are required to form a 5.00 M solution of PbCh if 48.00 grams the solid are dissolved? AP Chemistry 2013-2014 Summer Review Short Answer Problems from Previous AP Exams 1. The reaction between silver ion and solid zinc is represented by the following equation: 2Ag+ (aq) + Zn (s) -> Zn 2+ (aq) + 2Ag (s) A 1.50g sample of Zn is combined with 250mL of 0.110M AgNOa at25 0 C. a. Identify the limiting reagent. Show calculations to support your answer. b. On the basis of the limiting reactant that you identified in part a, determine the value of [Zn2+] after the reaction is complete. 2. Consider the hydrocarbon pentane, C5H12 (molar mass 72.15g). a. Write the balanced equation for the combustion of pentane to yield carbon dioxide and water. b. What volume of dry carbon dioxide, measured at 250C and 785mmHg, will result from the complete combustion of 2.50g pentane? 3. Find the mass percent of nitrogen in each of the following compounds: a. NO b. NO2 C. N2O4 d. N2O 4. Benzene contains only carbon and hydrogen and has a molar mass of 78.1g/mol. Analysis shows the compound to be 7.74%H by mass. Find the empirical and molecular formulas of benzene. 5. 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 12.25g of calcium carbonate is completely decomposed? c. What volume of carbon dioxide gas is produced form this amount of calcium carbonate, at STP? 6. Hydrogen gas and bromine gas react to form hydrogen bromide gas. a. Write a balanced chemical equation for this reaction.