7#, K "\\999G<sss .ɭ>xă ʟ̉*̳^9̉ʷ̉̉:̉̉̉̉̉̉ NAME _________________ Chemistry 141 Third Exam Fall, 1994 Constants: c = 2.998 x 108 m sec-1 h = 6.626 x 10-34 J sec To = 273.2 K R = 0.08206 L atm mol-1 K-1 NA = 6.023 x 1023 mol-1 You must show all work for full credit. Please report all answers with the correct number of significant figures and units. Review: What about question 1. on the preexam??? 1. Excited H atoms emit visible light when electrons fall from higher levels to n = 2 (this is called the Balmer series of lines). If green light comes from the transition from n = 4 to n = 2, is the light from the n = 3 to n = 2 transition expected to be: A) red or blue? B) of higher or lower energy? 2. Place the following isoelectronic ions in order of increasing size. K+ , S2- , Cl- 3. Place the following elements in order of increasing first ionization energy. B, O, Al, F 4.. Circle the correct answer for each of the following: a) the least electronegative: F, Cl, P b) would be likely to form a stable (+2) ion: S, Cl, Mg c) is diamagnetic: F, Fe3+, Na+ 5. Write the ground state electronic configuration for the stable ions of: Se K Al 6. List the number and identity of the orbitals involved in hybridization that results in a trigonal bipyramidal geometry. 7. Using a MO diagram, determine the bond order and magnetic properties of the following diatomic molecules: BN, BN+, and BN-. Which molecule is most stable? 8. For each of the following molecules; a) draw a reasonable Lewis dot structure, b) describe the molecular geometry and polarity, and c) give the hybridization on the central atom. a) SCl2 b) NO2- (N is central atom) c) XeOF4 (Xe is central atom) 9. Draw the Lewis dot Structure for the following molecules: a) HONO b) PO43- 10. Indicate the shape and bond angles of each molecule given the following Lewis structures:  11. (Homework 9.75) A compound used to treat AIDS is azidothymidine (AZT). The line structure of AZT is:  a) Identify the hybridization used in bonding by each of the nitrogen atoms. b) What is the bond angle around the oxygen atom in the five-membered ring? c) How many s bonds are there? d) How many p bonds are there? 12. (Homework 9.9) Use average bond energies to estimate the energy change for the reaction of N2 and O2 to give N2O4.  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.667 1 0 rcurveto .135 -.667 .865 -.667 1 0 rcurveto}rp SM st gr}{gs 12 OB np 0 lW 2 dv o o n p M p l bW 2 dv wF m o o p l n p l cp SM lW 0.8 m sl st gr}{P}{4 2 r gs OP/rad x 1 SA DA gr}{P}}o 1 g 1 s g e 2 4 gi al P 5 -1 r xc}{al P 8 ix 1 eq{DD}{DS}ie 5 -1 r 2 eq{DB}{DS}ie P}{DT}}o 0 g g xc}b /SP{/sf x/lW x/bW x/cW x SPn}b/SPn{gs count 9 ge 7 ix 192837465 eq and{7 -1 r P 6 -2 r o o xl 7 -1 r s e 7 -1 r s e 5 -1 r dv neg e 5 -1 r dv neg e sc neg e neg e xl}{xl P P}ie 1 1 S dv D sc CMT currentmatrix P lW sl 4.0 setmiterlimit np}b "cX"gX"_X"a"e"e;"TP "tQ"wN"U "_"v q_idid_d"dqafaffasend %%EndProcSet 40 80 20 20 54 chemdict30 begin/hS x/sf x/lW x/bW x/cW x/sh T d 289 53 58 332 SPn/origstk x 65535 65535 65535 sBg 0 0 0 C np 1750 7100 M 1750 7120 l 1350 7120 l 1350 7100 l cp f np 1750 7172 M 1750 7192 l 1350 7192 l 1350 7172 l cp f np 1750 7028 M 1750 7048 l 1350 7048 l 1350 7028 l cp f np 3410 7064 M 3410 7084 l 3030 7084 l 3030 7064 l cp f np 3410 7136 M 3410 7156 l 3030 7156 l 3030 7136 l cp f np 6290 7140 M 6290 7160 l 5890 7160 l 5890 7140 l cp f np 6721 6805 M 6735 6819 l 6489 7065 l 6475 7051 l cp f np 6750 7446 M 6736 7460 l 6509 7233 l 6523 7219 l cp f np 6700 7496 M 6686 7510 l 6459 7283 l 6473 7269 l cp f np 5410 6834 M 5424 6820 l 5680 7076 l 5666 7090 l cp f np 5460 6784 M 5474 6770 l 5730 7026 l 5716 7040 l cp f np 5459 7495 M 5445 7481 l 5682 7244 l 5696 7258 l cp f 4890 7110 4050 7110 5 Ar gr count origstk sub{P}rp end chemsave restore ,  Helvetica .(h;N)N)4O)O+sN)N(TPO*+O(TO*+O,Times (ht+dFCHMDSTRGL:[  x (XP6H$jDk hm npqPsuPwylortvx zNNOONNOOO O `  {, `  |  ` HX}pB ` H~B@ ` P ` Nl ` Ndl ` dP `   ,  `  f      + HelveticaTimesChemistry 142FirstSpring, 1995 R = 8.314 J mol-1K-1 1) Define: State Function 2) Define:Standard State 3) Define:The First Law of Thermodynamics 4) Define:The Second Law of Thermodynamics 5) The combustion of 1.1 grams of propane, C3H8, with excess O2 in a calorimeter ?wg*f86 61#?@JKLYZ`bderv}~<&',.56z| kln D F G I @9t @    $$    J   (IJSsxz}\ '()*45ABLM     @ @ @p@   M)4?@K<=EFopX8>?@[\[\]^_`a  hhh$$$$ $ $ PTUV`abcdopqrs E F H I    ( ) HItuyz{|} RW$ $ $  $'$hhhHhhhJ   produced enough heat to increase the temperature of 1000. g of water in the calorimeter by 12.2 oC. The calorimeter has a heat capacity of 65. J/K. The water has a specific heat of 4.18 J/K g. C3H8 (g) + 5 O2 (g) = 3 CO2 (g) + 4 H2O(g) Calculate the standard enthalpy of formation for propane given the following standard enthalpies of formation: DHfo [CO2 (g)] = -393.5 kJ/mole; and DHfo [H2O(g)] = -241.8 kJ/mole. CH142:Exam Iinitials ______5) Under what condition(s) is the enthalpy change of a chemical reaction equal to the heat of the reaction (q)? YY) A 65 gram block of silver metal (sp. ht. = 0.234 J/g oC) with an initial temperature of 89.5 oC is immersed in an insulated beaker of water with an initial temperature of 20.2 oC. If the final temperature of the silver and the water is 22.6 oC, what is the mass of the water? (sp. ht. water = 4.18 J/g oC). ZZ) Determine DHorxn for #24IJKL"VWgh !$*,./0134578;EOPQRST\]`a @      SFG]k{|}~*+VW @vx`abc0=KLMNOUVrͻ͵$ $$ $$ $$$$ $hh$ $G the following reaction: 5 PbO2 (s)+ 4 P (s,w) P4O10 (s)+ 5 Pb (s) element DHof (kJ/mol) PbO2 (s) -277 P4O10 (s) -2984 XX) (mwt. 44.0)perfect A) molar heat of combustion for propane (DHrxn). B) Calculate the (DHfo) CH142:Exam Iinitials ______6) Fill the boxes in the following table. DH DS DG(low T) DG (high T) Spont.? - + X( ) X( ) X( ) + X( ) + + X( ) X( ) + - X( ) - - - abefjklmnpqtuz{|} #$()*+,/23678BCWZ]_abegklwyz} 00     RX( ) X( ) CH142:Exam Iinitials ______+789 10) Label the three regions of the phase diagram and  CH142:Exam Iinitials ______!"#$%&( !SXd$ $ $ $$$$$$$$$$$$$$ $$$$$$$$$$$$$$$$$$$ $'$ $ $ $$ $ $  ,;<=>?@uvwx  @  @ 00 00Vd WORD  ##! ,Times .+ P (atm) +T (K)`}ZZ"`7ZZ"E#"v# (K1.0 (}0.5""}"D +4C100 (s200 )8300 (ZPhase Diagram for Br2 continued next page9 A). B) Using the diagram, describe what would happen to a sample of Br2 at 1.0 atm and 25 oC if it were introduced into a large vacuumm chamber. 11) Calculate the free enery change associated with the following reaction: N2(g) + O2(g) 2 NO(g) The pressure of N2 = O2 = 0.2 (atm) and the pressure of NO = 1.2 (atm). S0 (J/mol K)N2 0 191 O2 0 205 NO 90. 211 12) CH142:Exam Iinitials ______ Define: Standard Define: The Define: The vacuumenergymollFind the DS for the system, surroundings, and the universe when 25.0 grams of CH4)*`c $%&(/1259<?JOTUVbqr    Y (l) (mwt. 16.0) is evaporated at 112 K, if the heat required is provided by a room at 298 oC. (DHvap (CH4) = 9.2 kJ/mol) 13) Cu(I) is oxidized to Cu(II) by hydrogen peroxide according to the following two step mechanism. Cu+ + H2O2 Cu2+ + OH + OH- (1) {slow}Cu+ + OH Cu2+ + OH- (2) {fast} A) What is the overall reaction? B) Write the rate law for the rate limiting step. C) What is the rate of H2O2 consumption compared to Cu2+ formation? 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