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1 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) Attendance 4 In-Class EC 4 Total 100 1

2 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

3 5. What is the oxidation state/number of chromium in H 2 Cr 2 O 7? a. +2 b. +3 c. +5 d 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 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 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

4 9. How many grams of silver are contained in a mole sample of silver? a g b g c g d 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 moles b moles c moles d 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

5 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

6 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

7 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

8 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

9 9

10 10

11 Conversion Factors, Constants, and Periodic Table Avogadro s Number: Mass of Proton: Mass of Neutron: Mass of Electron: Mass of 1 amu: Temperature conversion: x particles/mole amu amu x 10-4 amu 1.66 x g T [K] = 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 Li Na K Rb Cs Fr (223) 4 Be Mg Ca Sr Ba Ra Sc Y La Ac Ti Zr Hf Rf (261) 23 V Nb Ta Db (262) 24 Cr Mo W Sg (263) 25 Mn Tc (98) 75 Re Bh (262) 26 Fe Ru Os Hs (265) 27 Co Rh Ir Mt (266) 28 Ni Pd Pt Uun (269) 29 Cu Ag Au Uuu (272) 30 Zn Cd Hg Uub (277) 5 B Al Ga In Tl C Si Ge Sn N P As Sb O S Se Te F Cl Br I He Ne Ar Kr Xe Pb Bi Po At Rn (209) (210) (222) Ce Th Pr Pa Nd U Pm (145) 93 Np (237) 62 Sm Pu (244) 63 Eu Am (243) 64 Gd Cm (247) 65 Tb Bk (247) 66 Dy Cf (251) 67 Ho Es (252) 68 Er Fm (257) 69 Tm Md (258) 70 Yb No (259) 71 Lu Lr (260) 11

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