Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO

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1 AP Chemistry Summer Review Packet 2018 Section 1: Names and Formulas of ionic compounds. Name: Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + 2 NH 4 Cr 4 H Cl 3 H 2 P 4 CN Cl P 4 3 HS HC 3 HS 3 Mn 4 C 2 H 3 2 Cr C Cl 4 P 3 3 CH 3 C Cl 2 HP N 2 S 4 2 Si 3 2 C 3 2 S 3 2 SCN N 3 HS 4 Section 2: For each of the following compounds, write A) the correct name (include a roman numeral if applicable) B) the number of each ion in one molecule of that compound. 11. CaI calcium iodide, each molecule has 1 Ca +2 ion and 2 I ions 12. Na 2 C Ga(Cl 3 ) CuF (NH 4 ) 3 P FeS Mg(N 3 ) NH 4 N KC 2 H Na 2 Cr

2 Section 3: Ionic Formulas (Binary, Polyatomic, Transition Metals Write the formula for each of the following compounds. 1. sodium hydroxide mercury (II) sulfate lead (II) phosphate ammonium sulfide aluminum chlorate copper (I) carbonate manganese (IV) oxide manganese (II) sulfate iron (III) oxide magnesium nitrate calcium sulfide potassium oxide magnesium chloride chromium (III) oxide gold (III) bromide beryllium fluoride yttrium (III) sulfide rubidium oxide aluminum dichromate iron (II) phosphide iron (III) nitrate chromium (III) sulfate tin (IV) nitride lead (II) permanganate niobium (V) oxalate 25. 2

3 Section 4: Write the correct name for each of the following compounds. *Some of these compounds are acids use the correct acid name) 1. Na 2 S NH 4 Cl Cu 3 N CuF PbS Cr(N 3 ) Al N H 2 S HCl H 2 S H 3 P HBr H 2 C HN Write the chemical formula for each of the following compounds. 16. nickel (II) chloride cuprous nitrate ammonium sulfate magnesium nitride copper (I) sulfide carbon monoxide iron (II) oxide diphosphorus pentoxide hydrogen sulfate sulfur dioxide 25. 3

4 Section 5: Chemical Word Equations Directions : Write the UNBALANCED chemical equation for each of the word equations below. Include states of matter (s,l,g,aq) after each of the chemical formulas. Don t forget about the 7 diatomic elementsbrinclhf! ** ACIDS are always aqueous. a. Aqueous sodium chloride reacts with aqueous lead (II) nitrate to yield solid lead (II) chloride and aqueous sodium nitrate. b. Aqueous barium nitrate reacts with sulfuric acid to yield solid barium sulfate and nitric acid c. Silver nitrate reacts in solution with aqueous potassium chromate to yield solid silver chromate and aqueous potassium nitrate d. Solid calcium carbonate reacts with hydrochloric acid to yield aqueous calcium chloride, carbon dioxide gas, and liquid water e. Aqueous zinc chloride reacts with dihydrogen monosulfide gas to yield solid zinc sulfide and hydrochloric acid f. Magnesium nitrate reacts in solution with potassium hydroxide to yield solid magnesium hydroxide and aqueous potassium nitrate g. Solid aluminum hydroxide reacts with nitric acid to yield soluble aluminum nitrate and liquid water h. Aqueous lead (IV) nitrate reacts with aqueous sodium sulfate to yield solid lead (IV) sulfate precipitate and aqueous sodium nitrate 4

5 i. Aqueous sodium hydroxide reacts with carbon dioxide gas to yield aqueous sodium carbonate and liquid water j. Solid magnesium oxide reacts with hydrochloric acid to yield a solution of magnesium chloride and liquid water k. Solid zinc metal reacts with sulfuric acid to yield aqueous zinc sulfate and hydrogen gas l. Solid iron (III) oxide reacts with aluminum metal to yield solid aluminum oxide and iron metal Section 6: Balancing Chemical Equations Directions : First, balance each of the chemical equations below. Then, classify each reaction as synthesis, decomposition, singlereplacement, or doublereplacement. Balance the equation and classify it. a. Sb + Cl 2 SbCl 3 b. SrBr 2 + (NH 4 ) 2 C 3 SrC 3 + NH 4 Br c. Al + Pb(N 3 ) 2 Al(N 3 ) 3 + Pb d. NaCl 3 NaCl + 2 e. Fe + HCl FeCl 2 + H 2 f. Cu + H 2 Cu + H 2 f. Al + H 2 S 4 Al 2 (S 4 ) 3 + H 2 5

6 h. MgBr 2 + Cl 2 MgCl 2 + Br 2 i. Ba(H) 2 Ba + H 2 j. Pb(N 3 ) 2 + H 2 S PbS + HN 3 k. NH 4 N 2 N 2 + H 2 l. KCl 3 KCl + 2 m. Fe H 2 Fe + H 2 Section 7: Stoichiometry, Percent Composition and determining Empirical/Molecular Formulas Complete these questions on lined paper. You MUST SHW ALL WRK CLEARLY AND CMPLETELY for each of the following questions to receive credit. No work, no credit! Also, where applicable, round your answers to the correct number of significant figures. 1. Find the mass percent of nitrogen in each of the following compounds: a. N b. N 2 c. N 2 4 d. N 2 2. Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the compound to be 7.44% hydrogen by mass. Find the empirical and molecular formula of benzene. 3. 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 grams of calcium carbonate are completely decomposed? c. What volume of carbon dioxide gas is produced from grams of calcium carbonate at STP? d. What is the volume of carbon dioxide in L if the pressure is 785 mmhg and the temperature is 30.0 C? (R= ). Hint The ideal gas law is helpful here! 4. 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 reacts with 9.5 grams of bromine. Which is the limiting reactant? 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)? 5. When ammonia gas, oxygen gas and methane gas (CH 4 ) are combined, the products are hydrogen cyanide gas and water. a. Write a balanced equation for this reaction. b. Calculate the mass of each product produced when 225 grams of oxygen gas reacts 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. 6. Sodium sulfate has the formula Na 2 S 4. 6

7 a) What is the mass percent of each element in sodium sulfate? b) How many grams of this compound contain 2.00 grams sulfur? c) How many grams of oxygen are in 15.0 g of the compound? d) How many grams of the compound contain grams of sodium? 7. A sample of tin (Sn) is heated in air to form a tin oxide. Assuming all of the tin is converted to the oxide, use the data table below to determine the empirical formula of the tin oxide formed. mass of crucible = g mass of crucible + tin (before heating) = g mass of crucible + product (after heating) = g 8. ctane undergoes complete combustion to form carbon dioxide and water. a) Balance the following chemical equation for the combustion of octane: C 8 H 18 ( l ) + 2 ( g ) C 2 ( g ) + H 2 ( l ) b) How many moles of oxygen are required to burn 1.00 mole of octane? c) How many grams of octane are needed to produce 6.63 moles of water? d) How many moles of C 2 are produced from the combustion of 101 grams of octane? e) What mass of C 2 is produced when 4.77 grams of oxygen gas are used up? f) How many molecules of water are produced by the combustion of 2.1 grams of octane? g) What mass of C 2 is produced starting from 5.00 g 2 and 1.62 g C 8 H 18? h) What is the percent yield if 3.70 g of C 2 are produced starting from 1.62 g C 8 H 18? 10. A gram piece of magnesium metal is heated and reacts with oxygen. The magnesium oxide product weighed grams. Determine the percent composition of each element in the compound. 11. A compound contains 21.6% sodium, 33.0% chlorine, 45.1% oxygen. Determine the empirical formula of the compound. 12. A gram sample of uranium was heated in air. The resulting uranium oxide product weighed gram. Determine the empirical formula of the oxide. {Hint: Carry out the calculations to four decimal places}. 13. When g of zinc is burned in air, grams of the oxide is produced. (a) What elements are present in the oxide? (b) Determine the percent composition of each element in the oxide. (c) Determine the empirical formula of the compound. 14. A gaseous compound has the empirical formula of CH 3 Br and a density of 6.00 g/l, at 375 K and.983 atm. Using these data, determine the following: (a) The molar mass of the compound. (P=DRT/MM). R= ) (b) The molecular formula of the compound. Stoichiometry Part II MassMass, MassVolume. Complete work on a separate sheet of paper. MATHEMATICALLY JUSTIFY YUR ANSWER T RECEIVE FULL CREDIT and round your answers to the correct number of significant figures. 1. Given the balanced chemical equation 2 Ag + I 2 > 2 AgI (a) How many grams of silver metal (Ag) are required to react completely with 51.8 g of iodine (I 2 ) to produce silver iodide (AgI)? (bi) How many grams of silver iodide will be formed? 2 ZnS(s) (g) > 2 Zn(s) + 2 S 2 (g) 2. If 500. g of lithium oxide (Li 2 ) are required to be produced according to the unbalanced equation: Li + 2 > Li 2 Calculate the mass of lithium and volume of oxygen (at STP) needed to react. 7

8 3. The solid fuel in the booster stage of the space shuttle is a mixture of ammonium perchlorate and aluminum powder, which react as follows: 6 NH 4 Cl 4 (s) + 10 Al(s) > 5 Al 2 3 (s) + 3 N 2 (g) + 6 HCl(g) + 9 H 2 (g) a. What mass of aluminum is required to react with g of ammonium perchlorate? b. Determine the volume (assume STP) of each of the gases produced. Limiting/Excess Reagent: MATHEMATICALLY JUSTIFY YUR ANSWER T RECEIVE FULL CREDIT and round your answers to the correct number of significant figures. 1. A solution containing 5.0 g of silver nitrate was mixed with another containing 5.0 g of potassium chloride. (i) Determine the 2 products of the reaction and write a balanced chemical equation. (ii) Determine which substance is the limiting reagent silver nitrate or potassium chloride. (iii) Calculate the mass of each of the products formed. 2. If 36.5 g of HCl and 73 g of Zn are reacted according to the equation: 2 HCl + Zn > ZnCl 2 + H 2 (i) Determine which reactant is the limiting reactant, (ii) Find the mass of ZnCl 2 formed, (iii) Find the volume of H 2 (@ STP) formed, (iv) Determine which reactant is in excess and by how much. 3. According to the balanced chemical equation below: (i) (ii) Cu(s) + 2 AgN 3 (aq) > Cu(N 3 ) 2 (aq) + 2 Ag(s) How many grams of silver will be produced from combining 100 g of copper with 200 g of silver nitrate? If the reaction is 65% efficient, determine the actual yield of silver produced. Section 8 Solutions and Molarity Mathematically justify your answer and round your answers to the correct number of significant figures. Determine the molarity of the following solutions. (a) 50.0 grams of Na 2 C 3 is dissolved in enough water to make liters of solution. (b) grams of (NH 4 ) 2 C 3 is dissolved in enough water to make 250 ml of solution. (c) 1.25 grams of PbCl 2 is dissolved in enough water to form 45.0 ml of solution. Determine the mass of solute required to make each of the following solutions. (d) 500. ml of a 2.75 M NaF solution. (e) 1.5 L of a 1.00 M KCl solution. (f) 750 ml of a 3.50 M CaCl 2 solution Determining the volume of solution: (g) What volume (in ml) of 2.0 M NaCl is needed to contain 5.00 g NaCl? (h) What volume (in ml) of 6.0 M HCl is needed to contain 1.5 g of HCl? Dilutions Use the formula M 1 V 1 = M 2 V 2 to solve each of the following problems. (i) 40.0 ml of M NaH solution is diluted to a final volume of ml, calculate the new concentration. (j) A M solution is concentrated by evaporation to a reduced final volume of ml and a molarity of M. Calculate the original volume. (k) 85.0 ml of a solution of NaH is diluted to a final volume of ml and the new molarity is M. Calculate the original molarity of the base. 8

9 Section 9: Mini Home Inquiry Lab Measure the amount of sodium bicarbonate in an AlkaSeltzer tablet by measuring the amount of carbon dioxide that is produced. Think of how to do this, try it, recording your data and analysis. You may work with someone else on this, but everyone must have a general procedure, data & analysis. Section 10: Gas Laws Mathematically justify your answer and round your answers to the correct number of significant figures. 1) Calculate the density of ammonia, NH3 in grams per liter at 752 torr and 550C. 2) What is the volume occupied by g HCl(g) at 678 torr and 25 o C? 3) A 2.0 L soda bottle contains 2.37 g air at a pressure of 1.0 atm and a temp.of 25 o C. What additional mass of air must be added to the bottle to raise the pressure to just below the point where it will burst, 7.0 atm? (The avg. molar mass of air is 29.0 g/mol.) 4) Using the information from STP conditions determine the value of the ideal gas constant. 5) The density of a certain gas at 27.0 C and kpa is 2.53 g/l. Calculate its molecular mass. 9

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