7. Relax and do well.

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1 CHEM 1215 Exam II John II. Gelder October 13, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility table. All work should be done in this booklet. 2. PRINT your name, TA's name and your lab section number now in the space at the top of this sheet. DO NOT SEPARATE THESE PAGES. 3. Answer all questions that you can and whenever called for show your work clearly. Your method of solving problems should pattern the approach used in lecture. You do not have to show your work for the multiple choice (if any) or short answer questions. 4. Point values are shown next to the problem number. 5. Budget your time for each of the questions. Some problems may have a low point value yet be very challenging. If you do not recognize the solution to a question quickly, skip it, and return to the question after completing the easier problems. 6. Look through the exam before beginning; plan your work; then begin. 7. Relax and do well. Page 2 Page 3 Page 4 TOTAL SCORES (36) (48) (16) (100)

2 CHEM 1215 EXAM II PAGE 2 (18) 1. Complete the following table by inserting the name of the compound or the formula. Compound Name sulfuric acid Formula H 2 SO 4 (aq) Dinitrogen trioxide N 2 O 3 Hydrobromic acid HBr(aq) Hydrogen peroxide H 2 O 2 Acetic acid HC 2 H 3 O 2 Sodium hydrogen carbonate NaHCO 3 Potassium chlorate KClO 4 Tetraphosphorus decaoxide P 4 O 10 FePO 4 (7) 2. When solid barium hydroxide is added to solid ammonium chloride and mixed a wet slush containing aqueous barium chloride and water, and smelling of ammonia is produced. Write a balanced chemical equation from this description. Be sure to include the phase for each substance. Ba(OH) 2 (aq) 2NH 4 Cl(aq) BaCl 2 (aq) 2NH 3 (g) 2H 2 O(l) (11) 3. Predict the solubility of the following compounds in water. For those soluble compounds write the formula for the cation and anion that exists in aqueous solution. a) CuCl 2 soluble c) HNO 3 soluble Cu 2 Cl H NO 3 b) KMnO 4 soluble d) BaSO 4 insoluble K MnO 4

3 CHEM 1215 EXAM II PAGE 3 (36) 4. Write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as, (l)iquid, (s)olid or (aq)ueous. a) 2Na(s) 2H 2 O(l) 2NaOH(aq) H 2 (g) b) HCl(aq) Ba(OH) 2 (aq) BaCl 2 (aq) 2H 2 O(l) c) NH 3 (aq) H 2 SO 4 (aq) (NH 4 ) 2 SO 4 (aq) d) 2Fe(NO 3 ) 3 (aq) 3Na 2 S(aq) Fe 2 S 3 (s) 6NaNO 3 (aq) e) 2H 2 (g) O 2 (g) 2H 2 O(g) f) 2C 4 H 10 (l) 13O 2 (g) 8CO 2 (g) 10H 2 O(l) g) 2K(s) Br 2 (l) 2KBr(s) h) Mg(s) 2HNO 3 (aq) Mg(NO 3 ) 2 (aq) H 2 (g) i) Na 2 CO 3 (s) HCl(aq) 2NaCl(aq) H 2 O(l) CO 2 (g) (12) 5. Write the balanced ionic and balanced net ionic chemical equations for 1d) and one other choosing from 1a, 1b or 1i. (Remember to include the correct charges on all ions and the phase of each species.) 1d) Ionic equation: 2Fe 3 (aq) 6NO 3 (aq) 3S 2 (aq) 6Na (aq) 6Na (aq) 6NO 3 (aq) Fe 2 S 3 (s) Net Ionic equation: 2Fe 3 (aq) 3S 2 (aq) Fe 2 S 3 (s) 1a, 1b or or 1i) Ionic equation: 2Na(s) 2H 2 O(l) Net Ionic equation: 2Na(s) 2H 2 O(l) 2Na (aq) 2OH (aq) H 2 (g) 2Na (aq) 2OH (aq) H 2 (g)

4 CHEM 1215 EXAM II PAGE 4 (8) 6a. Briefly define a chemical reaction. List at least three 'driving forces' which are common to chemical reactions. A chemical reaction involves the conversion of one or more reactants to products which are chemically different, i.e., substances with differnet combinations of elements. Driving Forces; 1. formation of a precipitate, 2. formation of a gas, 3. formation of water, 4. color change. b) When a soluble ionic solid is added to water it dissolves. Is this 'process' a chemical reaction? Yes or No. Briefly defend your answer. NO. The process of a solid dissolving in water is not a chemical reaction. Ionic solids are composed of ions, when dissolved in water the ions are only hydrated. Allowing the water to evaporate, the original solid will reform. In a chemical reaction the reactants can not be obtained from a simple physical change in the system. (8) 7. When an ionic compound like NaCl(s) is added to water we observe it dissolving. The same thing happens when HCl(g) is added to water, it dissolves. Use the space below to sketch two diagrams one depicting at the atomic level the NaCl(aq) solution and the other depicting at the atomic level the HCl(aq) solution. Clearly label the important species in your diagrams.

5 CHEM 1215 EXAM II PAGE IA 1 H Li IIA 4 Be Na Mg K Ca Rb Sr Cs Ba Fr (223) Ra IIIA IVA VA VIA VIIA B C N O F 9 10 Ne IIIB IVB VB VIB VIIB VIII IB IIB Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe (98) La Periodic Table of the Elements Hf Al Si P S Cl VIIIA 2 Ta W Re 75 Os Ir Pt Au Hg 80 Tl Pb Bi Po At Rn (209) (210) Ac Rf Db Sg Bh Hs Mt (261) (262) (263) (262) (265) (266) He Ar (222) Lanthanides Actinides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (145) Th Pa U Np Pu AmCm Bk Cf Es Fm Md No Lr (244) (243) (247) (247) (251) (252) (257) (258) (259) (260) Solubility Table Ion Solubility Exceptions NO 3 ClO 4 soluble soluble none none Cl soluble except Ag, Hg 2 2, *Pb 2 SO 4 2 CO 3 2 PO 4 3 CrO 4 2 soluble except Ca 2, Ba 2, Sr 2, Hg 2, Pb 2, Ag insoluble except Group IA and NH 4 insoluble except Group IA and NH 4 insoluble except Group IA, IIA and NH 4 - OH insoluble except Group IA, *Ca 2, Ba 2, Sr 2 S 2 insoluble except Group IA, IIA and NH 4 Na soluble none NH 4 soluble none K soluble none *slightly soluble

6 CHEM 1215 EXAM II PAGE 6

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