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Marketplace > University of St. Thomas > 111/40551 > CHEM 111 FINAL EXAM STUDY GUIDE
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units 1-4; answer key included
General Chemistry I
Study Guide
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This 7 page Study Guide was uploaded by Notetaker on Sunday December 13, 2015. The Study Guide belongs to 111/40551 at University of St. Thomas taught by Uzcategui-White in Summer 2015. Since its upload, it has received 27 views.




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Date Created: 12/13/15
CHEM 111 FINAL EXAM REVIEW A. WORK-OUT PROBLEMS: 1.   Write formulas for the following: calcium nitrate phosphorous pentafluoride aluminum carbonate strontium hydroxide methane potassium oxide lithium chloride barium sulfate phosphate ion dinitrogen tetroxide 2.   Give the complete electron configurations of: S, O , and Mn. 3.   For the following molecules/ions, give the Lewis structure, molecular geometry, and electron pair geometry: - NO 2 SF 4 4.   Write Lewis structures to represent all resonance forms of CO .32- 5. How many joules of heat energy are lost when a 100-gram sample of a metal (with a specific heat of 0.312 J/(gºC) cools from 80.0ºC to 30.0ºC? 6.   Calculate the number of moles in: (a)  4.20 X 10 molecules of SO 2 (b)  240 grams of NaOH (c)  5.00 liters of2H gas at 0ºC and 1.00 atm. (d)  1.7 liters of Ar gas at STP 7. How many grams of AlCl can3be prepared from 50.0 g of Al and 100.0 g of Cl 2 according to the equation: 2 Al + 3 Cl 2 2 AlCl ?3 131 8.   How many neutrons are there in I? 9.   Which bond is the most polar? I-Cl I-Br I-S I-I 10.  Circle the molecules that are polar (have a dipole moment): CCl 4 CH 4 H 2 NH 3 HBr CHCl 3 CCl 2 2 11.  How many unpaired electrons does the Si atom have? 12.  Write the correct Lewis structure for CS2. 2+ 13.  Write the formal charges on each atom in [F-S=F] (lone pairs are not shown). 14.  How many ions are formed when Ca (PO ) dissolves? 3 4 2 19 15.  How many protons, neutrons, and electrons are there in F- ion? 16.  Discuss the properties of molecules used as liquid crystals. (ignore this question) 17.  What is the molarity of the solution made when 1.25 grams of sodium chloride are dissolved in 500 mL of water? 18.   What is the hybridization of the carbon atom C H ?2 2 19.  What is the molecular formula of a compound with 30.5% N and 69.5% S, and it has a molar mass of 184 g/mol? 20.  How many electrons are found at the sublevel 1=2? 21.  How many sigma and how many pi bonds does carbon dioxide have? 22.  How many milliliters of 2.5M solution are needed to prepare 500 mL of 0.08M solution? 23.  How many milliliters of 1.25M hydrochloric acid are needed to neutralize 50.0 millimeters of 0.55M barium hydroxide? 24.  The vapor pressure of SiCl i4 100 mmHg at 5.4ºC and the normal boiling point is 56.8ºC. What is ΔHvap for SiCl in k4/mol? B. MULTIPLE CHOICE 1.   A 34.6 g sample of calcium oxide is a. 0.0346 mol b. 0.617 mol c. 1.23 mol d. 34.6 mol 2. When the following equation is balanced, the total number of nitrogen atoms on the reactant side is: BaCl (2q) + AgNO (aq)3 Ba(NO ) (aq) +3 2Cl(s) a. 2 b. 3 c. 4 d. 6 3.   Given that 4 HNO (aq3à 4NO (aq) 2 2 H O(l) + 2 (g), the2amount of NO which could 2 be produced from 3.00 mol HNO is: 3 a. 138 g b. 177 g c. 184 g d. 236 g 4.   Given that 3 CuCl (2q) + 2 Al(s) à 3 Cu(s) + 2 AlCl (aq)3 the amount of Al required to produce 42.4 g of Cu is: a. 12.0 g b. 28.3g c. 40.5 g d. 42.4 g 5.   The type of substance least likely to appear as a product in a net ionic equation is a.   a soluble salt c. a weak electrolyte b.   an insoluble salt d. an insoluble gas 6.   When a solution of NiBr is2mixed with a solution of (NH ) CO th4 2et i3nic equation is: a. NiBr 2aq) + (NH ) 4 2(aq)3à NiCO (s) + 23NH Br(aq) 4 b. Ni (aq) + 2Br- (aq) à 2 NH (aq) 4 CO 32-(aq)à NiCO (s3+ 2 NH (aq) 4 2 Br (aq) - 2+ 2- c. Ni -aq) + CO (aq+à NiCO (s) 3 d. Br (aq) + NH (a4) à NH Br(aq)4 7.   When a sample of chlorine gas at 35º C doubles in volume, its pressure a.   stays the same c. is half as great b.   doubles d. increases fourfold 8.   A 385-mL sample of oxygen gas collected at 747 mm Hg and 27.4ºC would occupy what volume at STP? a. 344 mL b. 356 mL c. 416 mL d. 431 mL 9.   A 9.74 g sample of CO wil2 occupy 6.37 L at 0.829 atm only if the temperature is a. 17.6ºC b. 6.61ºC c. 564ºC d. above 100ºC 10.  A sample of N w2uld obey the ideal gas law most closely at a.   0.68 atm and –68ºC c. 680 atm and –68ºC b.   0.68 atm and 680ºC d. 680 atm and 680ºC 11.  A 50.0 g sample of an unknown substance absorbed 1.64 kJ as its temperature changed from 36ºC to 98ºC. The specific heat of the unknown is: a. 0.53 J/(gºC) b. 0.76 kJ/(gºC) c. 1.3 kJ/(gºC) d. 1.9 kJ/(gºC) 12.  The formation reaction in this list is a. Sn(s) + 2Cl (2) à SnCl (l4 c. 2C2H 5H(l) + 7O (g)2à4CO (g) + 2H O(l) 2 b. 2HNO (l2 + NO(g) à 3NO (g) + 2 O(l) 2 d. 2Cl 2(g)à 2Cl (g2 + O (g) 2 13.  For CH (g)+ 4Cl (g)à CCl (g)+ 4HCl(g), ΔHº=-402 kJ. How much HCl was formed 4 2 4 when 201 kJ were given off? a. 18.2 g b. 72.9 g c. 146 g d. 292 g 14.  Use the thermochemical equations below to calculate the enthalpy of reaction for NOCl(g)+ Cl(g)à NO(g)+ Cl (g) 2 N 2g)+ O (g2+ Cl (g)à2 2NOCl(g) ΔHº=105.2 kJ N 2g) + O (g2 à 2NO(g) ΔHº=180.7 kJ Cl 2g) à 2Cl(g) ΔHº=243.2 kJ a. 529.1 kJ b.264.6 kJ c. -83.85 kJ d. –167.7 kJ 15.  The energy of a photon of electromagnetic radiation is directly proportional to its a. speed in a vacuum c. frequency b. wavelength d. diffraction 16.  The volume in space where an electron with a particular energy is likely to be found is called a.   a wave function c. the spin quantum number b.   a photon d. an orbital 17.  The frequency of a microwave with a wavelength of 12.2 cm is -33 7 a. 8.08 x 10 9 Hz c. 2.46 x 10 9z b. 3.66 x 10 Hz d. 2.46 x 10 Hz 18.  The number of orbitals in the 4p subshell is a. 1 b.3 c. 5 d. 18 19.  The energy difference between the two energy levels responsible for the 451 nm blue- violet line the emission of indium is 5 18 a. 6.65 x 10 5 c. 2.27 x 10 -19 b. 1.50 x 10 J d. 4.40 x 10 J 20.  The maximum number of electrons contained in a 3d subshell is a. 2 b. 6 c. 10 d. 18 21.  The number of valence electrons shown in the Lewis formula for SF is 4 a. 40 b. 34 c. 32 d. 5 22.  The formal charge on O in the compound H O (in2th2 order HOOH) is a. 0 b. –2 c. –1 d. –3 23.  The resonance structures for SO i2clude each of these except a. O=S-O b. O-S=O c. O=S=O d. S-O=O 24.  The O-S-O bond angle in SO is 2losest to a. 90º b. 109.5º c. 120º d. 180º 25.  Of the following substances, the least polar bonds are those found in a. H2 b. H 2 c.H 2 d.CH 4 26.  Matter is said to be transparent to those wavelengths it a. absorbs b. diffracts c. cycles d. transmits 27.  In formaldehyde (H C2) the electron pairs are located about the central atom in which type of arrangement? a. pyramidal b. tetrahedral c. trigonal planar d. bent 28.  The molecular geometry of SO is best described as 3 a. linear b. trigonal planar c. tetrahedral d.bent 2- 29.  The molecular geometry of CO 3 is best described as a. linear b. trigonal planer c. tetrahedral d. bent 30.  Of the following, which has a molecular geometry that is not planar? a. CH 4 b. H 2O c. C 2 4 d. SO 3 31.  When a solution of sodium chloride and a solution of lithium nitrate are mixed a.   a precipitate forms b.   a new salt is formed c.   a gas is evolved d.   no reaction occurs 32.  When solutions of barium chloride and sodium sulfate are mixed, the spectator ions in the resulting reaction are a. only Ba 2+ b. only SO 42- c. Only Na + d. both Na and Cl- 33.  Which of the following ionic compounds is insoluble in water? a. NH 4l b. AgNO 3 c.KI d. Na2S 34.  Given that Fe 2 (3) + 3CO(g) à 2Fe(s) + 3CO (g), 2hen 45.3 g of CO reacts quantitatively with 79.8 g of Fe O , the amount of Fe formed is 2 3 a. 45.3 g b. 55.8 g c. 60.2 g d. 79.8 g 35.  For the above reaction, when 45.3 g of CO reacts quantitatively with 79.8 g of Fe O , 2he3 amount of leftover reactant is a. 34.5 g b. 24.0 g c. 17.8 g d. 3.2 g 36. The oxidation numbers of P, S and Cl in H PO ,2H S2and 2ClO are, resp4ctively a) -1, -1, +3 b) +1, -2, +7 c) +1, +2, +7 d) -1, -2, +7 e) -1, -2, +3 37. Identify the oxidizing agent in the following redox reaction. Hg (aq) + Cu(s) → Cu (aq) + Hg(l) 2+ 2+ 2+ 2+ a) Hg (aq) b) Cu(s) c) Cu (aq) d) Hg(l) e) Hg (aq) and Cu (aq) ANSWER KEY: A. WORK-OUT PROBLEMS: 1. Ca(NO ) PF 3 2 5 Al2(CO ) 3 3 Sr(OH) 2 CH 4 K 2 LiCl BaSO 4 PO 43- N 2 4 2. S: 1s 2s 2p 3s 3p 4 2- 2 2 6 O : 1s 2s 2p Mn: 1s 2s 2p 3s 3p 4s 3d2 5 - 3. NO :2 Electron Pair Geomentry = trigonal planar Molecular Shape/Geometry = bent SF : 4 Electron Pair Geometry = trigonal bipyramid Molecular Shape/Geometry = see-saw 4. (three resonance structures; all trigonal planar) 5. -1560 J 6. 6.98 moles SO 2 6.0 moles NaOH 0.223 moles H 2 0.070 moles Ar 7. 125 g AlCl (3imiting regent is Cl ) 2 8. 78 n 9. I-Cl 10. Polar: H 2, NH , 3Br, CHCl , CCl3F 2 2 11.2 12. S=C=S 2+ 13. [F-S=F] 0, +1, +1 14. Five 15. 9p, 10n, 10e (16. You can ignore this question.) 17. 0.0428 M 18. Both carbon atoms are sp hybridized 19. S 4 4 20. 1 = 2 describes a d sub shell which can contain a maximum of 10 electrons. 21. Two sigma and two pi bonds 22. You will need 16.0 mL of 2.5M solution 23. (Note that in the stoichiometic equation there are 2 moles hydrochloric acid for each mole of barium hydroxide). You need 44.0 mL of HCl. 24. 30.12 kJ/mol B. Multiple Choice 1.   b 16. d 31. d 2.   a 17. d 32. d 3.   a 18. b 33. d 4.   a 19. d 34. b 5.   a 20. c 35. d 6.   c 21. b 36. b 7.   c 22. a 37. a 23. d 8.   a 24. c 9.   b 25. a 10.  a 26. d 11.  a 27. c 12.  b 28. b 13.  c 29. b 14.  c 30. a


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