7. Relax and do well.

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1 CHEM 1215 Exam II John II. Gelder October 7, 1998 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. You will receive 2 points for knowing your TA s name AND laboratory section number in which you are officially enrolled. 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 (16) 1. Complete the following table by inserting the name of a compound or a formula. Compound Name hydrosulfuric acid Formula H 2 S iron(iii) oxide Fe 2 O 3 iodine heptafluoride IF 7 lithium sulfite Li 2 SO 3 barium hydroxide Ba(OH) 2 lead acetate or lead(ii) acetate Pb(C 2 H 3 O 2 ) 2 potassium cyanide KCN sodium nitrite NaNO 2 (8) 2. When gaseous hydrogen fluoride is used to etch solid glass, CaSiO 3, at room temperature, gaseous silicon tetrafluoride, liquid water and aqueous calcium fluoride are formed. Write the balanced chemical equation for the following description. Be sure to include the phase for each substance. CaSiO 3 (s) 6HF(g) SiF 4 (g) 3H 2 O(l) CaF 2 (aq) (12) 3. Predict the solubility of the following compounds in water. For those compounds that are soluble write the formula for the cation and anion that exists in aqueous solution. a) PbSO 4 c) HCl insoluble soluble H and Cl b) Mg(ClO 4 ) 3 d) (NH 4 ) 3 PO 4 soluble Mg 2 and ClO 4 soluble NH 4 and PO 4 3

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) Fe(s) 2HCl(aq) FeCl 2 (aq) H 2 (g) or 2FeCl 3 (aq) 3H 2 (g) b) MgSO 4 (aq) 2AgNO 3 (aq) Mg(NO 3 ) 2 (aq) Ag 2 SO 4 (s) c) 2H 3 PO 4 (aq) 3Ba(OH) 2 (aq) Ba 3 (PO 4 ) 2 (s) 6H 2 O(l) d) Pb(NO 3 ) 2 (aq) K 2 CrO 4 (aq) PbCrO 4 (s) 2KNO 3 (aq) e) H 2 SO 4 (aq) 2KOH(aq) K 2 SO 4 (aq) 2H 2 O(l) f) 2C 6 H 14 (l) 19O 2 (g) 12CO 2 (g) 14H 2 O(l) g) S 8 (s) 8O 2 (g) 8SO 2 (g) h) 2Cs(s) Br 2 (l) 2CsBr(s) h) 2C 4 H 10 O 2 (l) 11O 2 (l) 8CO 2 (g) 10H 2 O(l) (12) 5. Write the balanced ionic and balanced net ionic chemical equations for 1d) and one other choosing from 1a, 1b or 1c. (Remember to include the correct charges on all ions and the phase of each species.) 1d) Ionic equation: Pb 2 (aq) 2NO 3 (aq) CrO 4 (aq) 2K (aq) 2K (aq) 2NO 3 (aq) PbCrO 4 (s) Net Ionic equation: 1a, 1b or 1c) Ionic equation: Pb 2 (aq) CrO 4 (aq) PbCrO 4 (s) Fe(s) 2H (aq) 2Cl (aq) Fe 2 (aq) 2Cl (aq) H 2 (g) Net Ionic equation: Fe(s) 2H (aq) Fe 2 (aq) H 2 (g)

4 CHEM 1215 EXAM II PAGE 4 (8) 6a. Solubility is defined as the maximum amount of a solute that will dissolve in a given amount of solvent at a given temperature. Provide a brief explanation of the meaning of solute and solvent when discussing solubility. The solute is the component in the solution present in the smallest amount. The solvent is the component in the largest amount, or the component whose phase is the same as the phase of the solution, or water. b) What does it mean when it is stated that the solubility of a substance depends on temperature? The amount of solute which will dissolve in a given amount of solvent depends on the temperature. The amount of solute which will dissolve in a given amount of solvent may increase or decrease with an increase or decrease of temperature. (8) 7. Describe what happens, at the atomic level, when a soluble ionic compound dissolves in water. You may use a diagram with your explanation if you want. When an ionic solute, such as NaCl, dissolves in water the compound is separated into its component ions (cation and anion) and each ion is surrounded by water molecules. For cations the oxygen atom of the water molecule orients itself so it is closest to the cation. For anions the hydrogen atoms of water orient themselves so they are closest to the anion. Since the ionis are now free to move in the solution this explains why solutions of soluble ionic compounds are good conductors of electricity.

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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