Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this exam. 3. Use the spaces provided to write down your answers. To receive full credit, you must show all work. Do not write answers on any other pieces of paper. If you need more room, write on the back of the exam and be sure to include a note describing where the work is located. 4. When solving numerical problems, make sure you include the proper units in your final answer as well as the proper number of significant digits. 5. If a question asks for a response in sentence or paragraph form, make sure you respond in that format. 6. Useful data for the exam and a periodic table are provided on the last page of the exam. Carefully tear out these sheets if you wish. Page # Points possible Points awarded 2-5 (MC) 39 5 10 6 22 7 15 8 10 Attendance 4 In-Class EC 4 Total 100 1
Multiple Choice Unless otherwise directed, choose the single best answer for each question. When balancing chemical equations, use the smallest whole number coefficients. 1. Which of the following is the correct name for V(NO 2 ) 2? a. vanadium nitrate b. vanadium nitrite c. vanadium(ii) nitride d. vanadium(ii) nitrate 2. Which of the following is/are ionic compounds? I.) NH 4 IO IV.) NH 3 II.) HCl V.) AlN III.) CF 4 a. I, V b. II, III, IV c. I, II, V d. I, II, IV, V 3. Use the unbalanced chemical equation shown below to answer the following question. If one molecule of O 2 reacts, how many molecules of SO 2 will react? SO 2 (g) + O 2 (g) SO 3 (g) a. 1 molecule of SO 2 b. 2 molecules of SO 2 c. 3 molecules of SO 2 d. 4 molecules of SO 2 4. When Ba(BrO 3 ) 2 (aq) is mixed with Li 3 PO 4 (aq) a reaction occurs. What is the sum of all the coefficients for the balanced chemical equation for this reaction? Hint: If the balanced chemical equation was 2A + B 3C, the sum of the coefficients would be 6. a. 12 b. 10 c. 7 d. 4 2
5. What is the oxidation state/number of chromium in H 2 Cr 2 O 7? a. +2 b. +3 c. +5 d. +6 6. When C 5 H 12 O(l) is combusted, what is the sum of all of the coefficients in the balanced chemical equation? Hint: If the balanced chemical equation was 2A + B 3C, the sum of the coefficients would be 6. a. 38 b. 13 c. 27 d. 39 7. When NaOH(aq) is mixed with H 3 PO 4 (aq) a reaction occurs. What is the sum of all the coefficients for the balanced chemical equation for this reaction? Hint: If the balanced chemical equation was 2A + B 3C, the sum of the coefficients would be 6. a. 4 b. 6 c. 8 d. 10 8. Which of the following is the correct name for P 2 O 5? a. diphosphorus pentoxide d. phosphorus oxide b. potassium oxide c. potassium(v) oxide 3
9. How many grams of silver are contained in a 0.0556 mole sample of silver? a. 1.78 g b. 0.000515 g c. 1.56 g d. 6.00 g 10. Which of the following would you expect to be strong electrolytes when placed in deionized water? I.) LiF IV.) HCN II.) HNO 3 V.) Ca(OH) 2 III.) FeS a. I, II, III, IV, V b. I, II, III, V c. I, II, IV, V d. I, II, V 11. A sample of 2.00 moles of Al 2 (Cr 2 O 7 ) 3 contains how many moles of chromium? a. 3.00 moles b. 12.0 moles c. 6.00 moles d. 2.00 moles 12. How many SO 2 molecules are there in a 115 g sample of SO 2? a. 5.58x10 23 molecules b. 3.01x10-24 molecules c. 6.02x10 23 molecules d. 1.08x10 24 molecules 4
13. When N 2 gas reacts with H 2 gas, NH 3 gas is formed. What is the sum of all the coefficients for the balanced chemical equation for this reaction? Hint: If the balanced chemical equation was 2A + B 3C, the sum of the coefficients would be 6. a. 3 b. 4 c. 5 d. 6 e. 7 End of Multiple Choice 14. a. When aqueous lead(ii) nitrate reacts with aqueous nickel(i) iodide, what is the formula of the precipitate that is formed? (3 points) b. For the reaction above, what are the formulas of the spectator ions? (3 points) 15. What is the molar mass of PtMnO 4? (4 points) 5
16. In the table below, the name or formula for a chemical compound is given. Fill in the table with the corresponding name or formula of the chemical compound. (16 points) NAME FORMULA lithium oxalate BrF 5 HCl(aq) ammonium acetate HIO 2 (aq) CoN silver thiosulfate barium hypochlorite 17. What are the complete, total ionic, and net ionic equations for the reaction that occurs when an aqueous solution of HClO 4 reacts with an aqueous solution of Ba(OH) 2? Assume the reaction takes place in a beaker of deionized water. (6 points) Complete Total Ionic Net-Ionic 6
18. a. In the space below, write the balanced chemical equation for what happens to H 2 SO 4 (aq) when it is in deionized water. (2 points) b. Is the process above referred to as ionization or dissociation? (1 points) c. A sample of H 2 SO 4 is placed in a beaker of deionized water. In the diagram below, show the best representation of what will exist in the water if two H 2 SO 4 particles are placed in the beaker. (2 points) Beaker Full of Deionized Water 19. In a reaction, phosphorus starts with an oxidation state of -3. During the reaction, 5 electrons are transferred and phosphorus is oxidized. Use this information to fill out the half-equation below. Show what the phosphorus starts as and what it is converted into and put the transferred electrons on the correct side of the equation. (4 points) 20. What are the complete, total ionic, and net ionic equations for the reaction that occurs when an aqueous solution of Al 2 (SO 4 ) 3 reacts with an aqueous solution of Cs 2 S? Assume the reaction takes place in a beaker of deionized water. (6 points) Complete Total Ionic Net-Ionic 7
21. A sample of H 5 IO 6 contains 9.25 grams of H. How many molecules of H 5 IO 6 are contained in the sample? (4 points) 22. Use the balanced oxidation reduction reaction below to answer the following question. (6 points) 6HBr(aq) + 2In(s) 2InBr 3 (aq) + 3H 2 (g) a. Which element is reduced? b. Which element is oxidized? c. Which element is the reducing agent? d. Which element is the oxidizing agent? e. How many electrons are transferred? f. Which element are the electrons transferred to? 8
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Conversion Factors, Constants, and Periodic Table Avogadro s Number: Mass of Proton: Mass of Neutron: Mass of Electron: Mass of 1 amu: Temperature conversion: 6.022 x 10 23 particles/mole 1.0073 amu 1.0087 amu 5.486 x 10-4 amu 1.66 x 10-24 g T [K] = 273.15 + T [ C] Solubility Rules for Common Ionic Compounds SOLUBLE COMPOUNDS group I cations + any anion soluble ammonium ion + any anion soluble Any cation + nitrate, perchlorate, soluble or acetate ions Mostly Soluble Compounds Any cation + chloride, bromide, soluble or iodide ions (except lead(ii), silver, mercury(i) insoluble) Any cation + sulfate ions soluble (except strontium, calcium barium, lead(ii), mercury(i) insoluble) Insoluble Compounds Any cation + hydroxide ions insoluble (except group I, ammonium, calcium*, barium*, strontium* soluble Any cation + sulfide ions Insoluble (except group I, ammonium, group II* soluble) Any cation + carbonate or phosphate ions (except group I, ammonium soluble) Insoluble * slightly solube (for Chem 130 = soluble) 1 H 1.0079 3 Li 6.941 11 Na 22.9898 19 K 39.0983 37 Rb 85.4678 55 Cs 132.905 87 Fr (223) 4 Be 9.0122 12 Mg 24.3050 20 Ca 40.078 38 Sr 87.62 56 Ba 137.327 88 Ra 226.025 21 Sc 44.9559 39 Y 88.9059 57 La 138.906 89 Ac 227.028 22 Ti 47.88 40 Zr 91.224 72 Hf 178.49 104 Rf (261) 23 V 50.9415 41 Nb 92.9064 73 Ta 108.948 105 Db (262) 24 Cr 51.9961 42 Mo 95.94 74 W 183.85 106 Sg (263) 25 Mn 54.9380 43 Tc (98) 75 Re 186.207 107 Bh (262) 26 Fe 55.847 44 Ru 101.07 76 Os 190.2 108 Hs (265) 27 Co 58.9332 45 Rh 102.906 77 Ir 192.22 109 Mt (266) 28 Ni 58.693 46 Pd 106.42 78 Pt 195.08 110 Uun (269) 29 Cu 63.546 47 Ag 107.868 79 Au 196.967 111 Uuu (272) 30 Zn 65.409 48 Cd 112.411 80 Hg 200.59 112 Uub (277) 5 B 10.811 13 Al 26.9815 31 Ga 69.723 49 In 114.82 81 Tl 204.383 6 C 12.011 14 Si 28.0855 32 Ge 72.61 50 Sn 118.710 7 N 14.0067 15 P 30.9738 33 As 74.9216 51 Sb 121.757 8 O 15.9994 16 S 32.066 34 Se 78.96 52 Te 127.60 9 F 18.9984 17 Cl 35.4527 35 Br 79.904 53 I 126.904 2 He 4.0026 10 Ne 20.1797 18 Ar 39.948 36 Kr 83.80 54 Xe 131.29 82 83 84 85 86 Pb Bi Po At Rn 207.2 208.980 (209) (210) (222) 114 116 118 58 Ce 140.12 90 Th 232.038 59 Pr 140.908 91 Pa 231.036 60 Nd 144.24 92 U 238.029 61 Pm (145) 93 Np (237) 62 Sm 150.36 94 Pu (244) 63 Eu 151.96 95 Am (243) 64 Gd 157.25 96 Cm (247) 65 Tb 158.925 97 Bk (247) 66 Dy 162.50 98 Cf (251) 67 Ho 164.930 99 Es (252) 68 Er 167.26 100 Fm (257) 69 Tm 168.934 101 Md (258) 70 Yb 173.04 102 No (259) 71 Lu 174.967 103 Lr (260) 11