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-----CHEM 112 EXAM 1

FALL 2008 NAME:Dr Thomas Berg

Total Points - 150Questions 1-30: 5 points eachUSEFUL INFORMATION:No = 6.022 x 1023 morlR =8.314 J . mor l K-I8E=q+w

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1. What is the molar solubility ofCdS when the salt is dissolved in sodium sulfidesolution that has a concentration ofS2-ion of3.0 x 10-3 MAssumed reaction: CdS(s) --+- Cd2+(aq) + S2-(aq) Ksp = 3.6 X 10-29a) 6.0 x 10-15 Mb) 1.2 X 10-26 Mc) 3.4 X 10-15 Md) 1.2 X 10-29 Me) 8.3 x 10-15 M

2. Consider the following information:.6.W = -311 kJ

BE for C-C = 350. kJ / mol BE for H-H = 435 kJ / molBE for C-H =410. kJ / mol

What is the estimated value for the bond dissociation energy for the carbon tocarbon triple bond?a) 1050. kJ / molb) 833 k1 / molc) 807 k1 / mold) 397 k1 / mole) 884 kJ / mol

3. A saturated solution ofAg2Cr04 formed by dissolving ~ C r 0 4 in water has aAg+ ion concentration of 1.6 x 10-4 M. What is the Ksp for Ag2Cr04?

a) 2.0 x 10- 12 b) 2.6 X 10-8 c) 4.1 X 10-12 d) 5.1 X 10-8

e) 1.6 x 10-11

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4. Consider the following data:ilHo (kJ / mol)

Cf2(g) -- 2 c.e(g) 242.3h(g) -- 2 leg) 151.0ICt(g) - - leg) + ct(g) 211.3h(s) -- h(g) 62.8What is the standard heat of formation of the compound ICt(g)

a) 14.7 kJ / mol b) 16.8 kJ / mol c) 72.6 kJ / mol d) -14.7 kJ / mol e) None of these is correct.

5. All of the following are state function except:a) enthalpyb) internal energy.c) heat.d) temperature.e) pressure.

6. Which is the soluble salt of the following se t at identical temperatures?a) Ba(OH)z with Ksp =5.0 X lO-3b) Ca(OH)z with Ksp = 4.7 X 10-0c) Cr(OH)3 with Ksp = 6.7 X 10-31d) Cd(OH)z with Ksp = 5.3 X lO-ISe) Fe(OH)z with Ksp =2.5 X 10-37

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7. The heat of vaporization ofwater at 373 K is 40.7 kJ / mol. When 9.00 g of steamcondense at 373 K, the value for the change in enthalpy ( ~ H ) is:

a) -8.14 x 10 1 kJ

b) 2.04 X 101

c) 8.14x 101 kJd) -2.04 x 101 kJe) None of these is correct.

8. A solution which is 0.65 M is each ofPb2+, Ag+, and Hgl+ has the CCconcentration adjusted to 1.0 x 10-

9M. Which of the following chlorides willprecipitate? Ksp for PbCt2 = 1.6 x 10-5

Ksp for Hg2Ct2= 4.3 X 10-19Ksp for AgCt = 1.7 x 10- 10

a) PbCt2 only b) AgCt only

9. A saturated solution Ag2C03 was fonned by dissolving Ag2C03 in water. lftheKsp ofAg2C03 is 8.2 X 10- 12, what is the concentration of the silver ion?a) 2.6 x 10-4 Mb) 1.6 X 10-8 Mc) 1.3 X 10-4 Md) 3.2 X 10-4 M e) 1.6 x 10-4 M

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10. As a purity check for industrial diamonds, a 10.25 carat (carat 0.2000 g)diamond is heated to 74.21 C and immersed in 26.05 g ofwater (specific heatcapacity of water = 4.184 J ig ' K) in a constant pressure calorimeter . The initialtemperature ofthe water is 27.20 dc. What is the final temperature of the waterand diamond (specific heat capacity of diamond is 0.519 J / g . K? (Assume noheat is lost to the surroundings.)

a) 27.65Cb) 23.51 Cc) 28.85Cd) 28.18 DCe) None of these is correct.

11. A solution is 0.050 M in K2S04 and 0.050 M K2CrO... A solution ofPb(N03)2 isadded slowly without changing the volume appreciably. The Ksp value for PbS04is 1.8 X 10-8 and the Ksp value for PbCr04 is 1.8 x 10- 14 . What is the concentrationofCrOl- when PbS04 just begins to precipitate?

a) 1.3 x 10-4Mb) 5.0 X 10.8 Mc) 1.4 X 10-7 Md) 3.6 X 10- 7 Me) None of these is correct.

12. The Ksp for PbF2 is 2.7 X 10-8 Ifa 0.050 M NaP solution is saturated with PbF2,what is the concentration ofPb2+ is solution?a) 7.4 x 10-4 Mb) 1.1 X 10-5 Mc) 1.6 X 10-4 Md) 5.4 X 10-7 M e) 1.9 x 10-3 M

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13. Consider the following reaction:P4(s) + 10 Ct2(g) - 4 PCtS(s) ~ H =-435.2 Kcal

When 50.00 g ofP4 react with excess Ct2, which of the following statements is true?

a) 175.8 Kcal will be produced. b) 435.2 Kca1 will be produced c) 2.176 X 104 Kcal will be produced. d) 175.8 Kca1 will be consumed. e) 435.2 Kcal will be consumed.

14. When 0.1 mol of solid silver nitrate is added to 1.0 L of clear, saturated solutionof A82Cr04 ( !

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16. Consider the following reaction:

If 10.35 g ofliquid toluene (C7HS) releases 12.12 kcal of heat to the surroundingswhen burned in oxygen, what is the molar heat of combustion, M-Icomb, fortoluene?

a) -11.7 kcal b) 108 kcal c) -108 kcal d) 11.7 kcal e) -12.12 kcal

17. Two metals of equal mass with different heat capacities are subjected to the sameamount of heat. 'Which undergoes the smallest change in temperature?a) the metal with the higher heat capacityb) the metal with the lower heat capacityc) Both undergo the same change in temperature.d) You need to know the initial temperature of the metals.e) None of these is correct.

18. The Ksp ofAg2C03 is 8.2 X 10- 12. 'What is the molar solubility of silver carbonate? a) lAx 1O-

6M

b) 2.0 x 10-6 M c) 1.3 X 10-4 M d) 2.0 x 1O-4 M e) 1.6 x 10-4 M

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19. A 1.00 gram sample of the rocket fuel hydrazine, N 2 ~ . is burned in a bombcalorimeter containing 1200. grams ofwater. The temperature of the water andthe bomb calorimeter rises from 24.62 e to 28.16 e. Assuming the heatcapacity of the empty bomb calorimeter is 837 J / e, what is the heat ofcombustion of 1mole ofhydrazine in the bomb calorimeter?(The specific heat capacity ofliquid water is 4.184 J / g '0c.)

a) -665 kJ / molb) 20.7 kJ / molc) -152 kJ I mold) 47.4 kJ / mole) -569 kJ I mol

20. At 25C, the heat of fusion of aluminum is 10.6 kJ / mol and the heat ofsublimation is 326.4 kJ / mol. What is the heat ofvaporization of aluminum at25C?

a) 158.2 kJ / molb) 168.5 kJ / molc) 315.8 kJ / mol d) 337.0 kJ / mol e) It cannot be determined without the normal boiling point temperature.

21. The Ksp of AC(OH)3 is 2.0 X 10-33 . At what pH will a 0.20 M At3+ solution beginto show precipitation ofAf(OH)3?a) 3.44b) 4.15c) 10.99d) 2.86 e) 8.30

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22. Solid cadmium cyanide, Cd(CN)2, dissolves in aqueous KCN solutions to fonnCd(CN)l-. Which of the following statements best describes the equilibriumconstant, Keq, for this reaction? (Ksp for Cd(CN)2 ; KJiss for Cd(CN)l).

a) Keq = [ Ksp ][ Kmss ]b) Keq = [ Cd2+ :I [ CN- ]2 c) Keq = [Ksp ] [ 1 / Kmss] d) Keq = [ Cd2+ ] [ C ~ ]4 e) Keq = [ 1 / Ksp] l.K&ss]

23. The solubility product expression for Tb3(P04)4 is Ksp =a) [Tb4+]3 [POl-tb) [3Tb3+] [4POlTc) [3Tb3+]3 [4Pol-td) [Tb3+t [pO/]3.e) None of these is correct.

24. The amount of heat needed to raise the temperature of 1.00 g of copper by 1 C iscalled its:a) molar heat capacity.b) heat capacity.c) specific heat capacity.d) enthalpy. e) work.

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25. For a particular process, q = 20 KJ and w = 15 KJ. Which oftbe followingstatements is true? .a) Heat flows from the system to the surroundings.b) The system does work on the surroundings.c) L\E= 35 KJd) a), b), and c) are all true. e) a), b), and c) are all false.

26. The solubility ofAge. will be greatest in a IM solution of which of thefollowing?a) Hct b) NaCt

d) NaOH

27. The internal energy increases by 20.9 kJ when 1.00 mole of a substance isvaporized at 300 K and 1.00 atmosphere ofpressure. What is the enthalpy ofvaporization for X?

a) 20.9 kJ / molb) -20.9 kJ / molc) 23.4 kJ / mold) 18.4 kJ / mol e) 2.51 kJ / mol

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28. What is the solubility in g I mL ofbarium carbonate, BaCO:J, i f the Ksp for thissalt is 8.1 X 10-9 at 25C?a) 1.6 x 10-3 g/mLb) 1.8 x lO-sg I mLc) 3.5 x lO-sg/mLd) 1.6 x 10-6 g I mL e) 3.2 x 10-6 g I mL

29. Consider the following data:AHOr for CO(g) = -111 kJ I molABorfor C02(g) = -394 kJ / mol

Calculate the AHO for the following process per mole ofFe203(s)'Fe203(s) + 3 CO(g) -+ 2 Fe(s) + 3 C02(g)

a) 321 kJb) 23 kJc) -321 kJd) 1675 kJe) -23 kJ

30. What is the solubility ofCr(OHh, Ksp 6.3 x 10-31 , in a buffer of pH 9.50?a) 2.0 x 10-8 Mb) 2.0 X 10-26 Mc) 2.0 X 10-2 Md) 2.0 X 10- 21 Me) None of these is COlTect.

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PERIO-DrG CHART OF THE ELEMENTS IA - 1 ..-.H VilA VIII

I ~ 1.0079 -7 2HeIIA lilA IVA _ VA V(A 4.00263 4 5 6 7 6 9 10Li Be 8 C N 0 F Ne6.94' 9.01218 10.811 12.011 14.0067 15.9994 10,99U403 20.179

11 12 13 14 15 16 17 18Na Mg -AI Si P 5 CI Ar22.98911 24.305 26.981539 28.0855 30.97376 32.0G6 35.453 39.94819 20 21 22 23 24 25 26 27 28 29 30 JI 32 -J J J4 35 36K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr39.0983 40.078 44.9559 47.88 50.9415 51.996 54.9380 55.847 58.9332( 58.69 63.546 65.39 69.723 72.61 74.9216 18.96 1 9 . ~ 0 4 83.8037 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In- Sn Sb Te I Xe85.4678 87.62 88.9059 91.224 92.9064 95.94 ' (98) 101.01 102.905f 106.42 1 0 7 . B 6 8 ~ 112.41 114.82 118.710 121.75 127.60 26.'1045 131.2955 56 57 72 7J 74 75 76 n 78 79 80 01 82 63 04 . 85 66

Cs Ba *La HI Ta W Re Os Ir -Pt Au ~ J I TI Pb Bi Po At Rn132.!K154 137.33 1 3 1 ~ 9 0 5 5 118.49 160.9479 183.85 186.20' 190.2 192.22 195.09 1 9 6 . 9 6 6 ~ 2 0 4 . 3 8 3 ~ 201.2 208.9804 (209) (210) (ZZZI87 88 89 104 105 106 107 108 109Fr Ra 'Ac Rf Db 89 Bh Hs MtIll3, 226.025-4 221.0171 (261) ,Z62t (Z6JJ (262) (265) ( 2 6 ~58 59 60 61 62 63 64 65 . 66 67 68 69 70 I 71Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb LUJ140,115 140.90n 144.24 ( 1 ~ 5 J ' 150.36 15'.96 157.25 168.9264 1 6 l . ~ O 164.9304 -167.26 168.93421 J7l.1J4 174.%7-

-

-- - - ~ - -

90ThZJZ.03I191Pa231.0359

92U238.02993Np2J7.0482

- 94Pu(244)95Am(243)

.96em(241)97Ok(247)

96Cf(151,99Es

f2521

100Fm(251)101Md

(250'102No

(259)

10JLr(2GO)

-

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~ K

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-;wf)/UILJQ Q IIS A b 1 a v ~ i ~ ~ &(of/Jl. ) ~ ( o J l ) J . . > J ( ) H J ~ ) Fe.(O){jL . (s;;e;.JJ..J1-

G:...(Off),1, (() ~ Sa. K1P J yt';:t ~ (e ~

AJce,j) ~ ~ ~ f ) t r.(!. ~ f J~ p '" . ~ l - J [(I-.J, (o.bJ-) (1.0 )Vo-'fJ :: (,J X/D - /0

~ (/1(e.. QJ,o,.) k4p , ",pi ~ t:J

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'i1..C'3(.() ~ ~ ~ ~ f ) 4" ('03 ~ I ! ~ / O ~ (iJl; ~ + J CS0cf.2..J -- [ f ' . 6 ~ t i [o.OJ-oj

[tobl+J 3 faXI D-1' fJ1. /fee. [JOJ, ~ t J wf,Jt ;Cb -S0lAtJ tv!+b

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il94KS,o ;: [ t ? h ~ + J (f:]2.C ~ - 6 ~ u S L )

';;'/lx/tJ-/r-= (So ) ( ~ S + ( ) . o ~ ~ o ) : l - ~ (s) (.OJ?J)'

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t,HS(..1o ;: (lH.f.w. t Lvlrrr.6!-11R1f 6J./jub - dHJ.w :: 326, -I K f J H ! ~ - /0.6, I

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--JW Q/4f()0 < 1 It H = E - ~ i /~ J I :: 4E1- *)

~ j l = I J E - r P A I J (CCMJt to)= A.Et /M/?j.:: ,;({).9 I

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CHEM 112EXAM 2

FALL 2008 NAME: Dr Thomas Berg

Total Points == 150Questions 1-30: '5 points eachUSEFUL INFORMATION:AG=AGO + RTlnQ k= 1.381 X 10-23 J IK In [K2/K1 ] =-[mo/R] [(lJT2) -(l /T l ) ] In [ k2 I k) ] = - [Ea I R] [(1IT2) - (1 I T1)] k = A e-(Ea/RnR = 8.315 J I (mol K)

(1 /[] )=kt + (1/[ ]0)[ ] = -kt + [ ]0In[ ] = -kt + In[ ]0

MirO:::::E n ' BE(R)-:E m ' BE (P)~ s = nCpln(T 2 I T 1)

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1. Consider a bimolecular reaction in the gas phase. Which of the following changesin condition will cause an increase in the rate of the reaction.a) increase the temperature at constant volumeb) increase the volume at constant temperaturec) add a catalystd) both a) and c) e) both b) and c)

2. Hydroquinone, H O C 6 ~ O H , can be formed by the reaction with acetylene below:3 HCCH + 3 CO + 3 H20 ~ 2 HOC6RtOH + CO2

How is the rate of disappearance of acetylene, HCCH, related to the appearanceofhydro quinone (Hq)? - ~ [ H C C H ] / ~ T =

a) ~ [ H q ] / ~ Tb) -2/3 ~ [ H q ] / ~ Tc) 3/2 ~ [ H q ] / ~ Td) -3/2 [ H q ] / ~ Te) 2/3 ~ [ H q ] / ~ T

3. Which part of the Arrhenius equation contains a term which measures the numberofmolecules that have the correct orientation for the reaction?

a) activation energy e-(Ea I RT)b)

c) frequency factor d) e Ea

e-(Ea/T)e)

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4. Which statement regarding the half-life of a second-order reaction is true?a) Each half-life is half as long as the preceding one.b) Each half-life is twice as long as the preceding one.c) Each half-life varies in a unpredictable way.d) Each half-life is four times as long as the preceding one.e) The length of the half-life remains unchanged throughout the course ofthe reaction.

5. Which of the following is in accord with the three laws of thermodynamics?I. The entropy of the universe never decreases.II. A nonspontaneous process can occur if it is coupled to aprocess that is sufficiently spontaneous.

a) I and II are both false.b) I is false and II is true.c) I is true and II is false.d) I and n are both true. e) I is unknown but II is true.

6. When a stable diatomic molecule spontaneously forms from its atoms, what arethe signs ofmo, ~ S O , and ~ G ~

a) + + + b) + c) - + + d) - + e)

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7. For which of the following processes is ASsystem negative?a) H2O(s) ~ H2O(t)b) S8(s) ~ 8 S(g)c) Ct2(t) ~ Ct2(g)d) H.B(t) ~ H.B(s)e) NaCt(s) ~ NaCt(aq)

8. For a particular process, AG AH at a particular temperature and pressure. Thus:a) L\S is positive ifAH is positive and negative i fAH is negative.b) L\S is negative i fAH is positive and positive i fAH is negative.c) L\S is zero.d) AS =AG/T.e) L\S could be either positive or negative.

9. For the reaction, H2(g) + h(g) ~ 2 HI(g) the proposed mechanism is:h(g) ~ 2 leg) ( fast)

(slow)What is a rate law consistent with the above mechanism?

a) Rate = k[h]b) Rate = k[H2] [12]c) Rate = k[H2] [hfd) Rate = ke) Rate =k[H2] [h] \/2

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13. Consider the following data:2 HC.t(g) + A ~ O ( s ) - + 2 AgCt(s) + H20(t) ~ G o = 61.00 Kcal

2 HCt(g) + A ~ C 0 3 (s) - + H20() + 2 AgCt(s) + CO2 (g) ~ G o = -53.37 KcalWhat is the standard free energy, ~ G o , for the following reaction?

Ag2C03(S) - + A ~ O ( s ) + C02 (g)a) 7.63 kcalb) -7.63 kcalc) -114.37 kcald) -68.63 kcale) 114.37 kcal

14. For a particular reaction, the equilibrium constant is 1.50 x 10-2 at 370. c and~ o is 16.0 kJ I mol. Assuming ~ H O and 88 are temperature independent,calculate 8 for the system at 370. c.

a) -18.8ll(Kmol) b) 18.8l l (Kmol) c) -10.0l l (Kmol) d) 10.Oll(Kmol) e) 0.00 J I ( K . mol)

15. For the process CHCt3(s) +-+ CHCt3 ([) , ~ H o 9.2 kJ I mol and ~ 8 43.9 J I(mol K). What is the melting point of chloroform?

a) -63Cb) 210Cc) 5.0 Cd) 63C e) -5.0C

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16. If S u n i v is positive for a process, the process is , if flSuniv for a process isnegative, the process is - - ' and if the flSuniv accompanying a process is zero,the process is__.a) at equilibrium, spontaneous, impossible b) impossible, spontaneous, at equilibrium c) impossible, spontaneous, impossible d) spontaneous, at equilibrium, impossible e) spontaneous, impossible, at equilibrium

17. The free energy of formation of gaseous nitric oxide, NO, is equal to86.57 kJ I mol. What is the value of Kp at 25C for the reaction below?N2(g) + 02(g) -+ 2 NO(g)

a) 6.7 x 10-16 b) 9.3 X lO-11 c) 7.7 X 10-27d) 4.3 X 10-29e) N one of these is correct.

18. I f flO is small and positive:a) the forward reaction is spontaneous and the system is far fromequilibrium.b) the forward reaction is spontaneous and the system is near equilibrium.c) the reverse reaction is spontaneous and the system is near equilibrium.d) the reverse reaction is spontaneous and the system is far fromequilibrium. e) None of these need be true.

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19. For a spontaneous process:a) . energy and entropy are conserved.b) energy is conserved and the entropy of the system and surroundingsincreases.c) the energy of the system and the :surroundings decreases and the entropy ofthe system and surroundings increases.d) both the energy and the entropy of the system and surroundings decrease.e) the energy of the system and the surroundings increases and the entropy ofthe system and surroundings decreases.

20. On a plot of concentration versus time for a reaction, the average rate of a reactionover a particular time interval is the:

a) slope of the tangent to the curve at the point where the rate is half theoriginal rate.b) slope of the tangent to the curve at the point where a reactionconcentration is half its original value.c) slope of the straight line connecting the concentration at the limits of thetime interval.d) All of these should yield equivalent results. e) None of these is correct.

21. Chlorine reacts with chloroform according to the reaction below:

When the initial concentration ofCf2 is doubled the reaction rate increases by afactor of 1.41. What is the order of the reaction with respect to Cf2?a) - ~b) -1c) ~d) 1e) 2

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22. The decomposition of ozone in the stratosphere can occur by the follo\\-lng twostep mechanism:

Step 1: Br + 03 - j . BrO + O2Step 2: BrO + 0 - j . Br + O2

Which species is an intermediate in this mechanism? a) Br b) BrO c) 0

23. Compounds A an B react in such a why that it was found to be second-orderoverall and second-order in A. The rate constant at 30C is 0.622 M- l min-1What is the half-life of A when 4.10 x 10-2 M A is mixed with excess B?a) 0.0330 min b) 1.11 min c) 47.3 min d) 23.9 min e) None of these is correct.

24. The decomposition of nitric oxide, NO, to N2 and O2 is second-order with a rateconstant of 0.0150 M-

l . S-l at 543C and 0.0515 M- J S-I at 715C. What is theactivation energy for the reaction?a) 48 kJ I mol b) 11 kJ ! mol c) 23 kJ! mol d) 17 kJ ! mole) None ofthese is correct.

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25. Consider the following reaction energy profile:

Reaction pathwayhich step is the fastest?a) step 1b) step 2c) step 3d) step 4e) Insufficient information to answer the problem.

26. Consider the following data for the decomposition of according to theequation:

Time, s [ A X ~ ] , Mo 0.05002.0 0.04486.0 0.03008.0 0.024910.0 0.020920.0 0.0088

What is the approximate rate constant for the decomposition reaction at thisparticular temperature.

a) 0.0625 SIb) 0.087 SIc) 2.5 Sld) 0.0031 SIe) None of these is correct.

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27. Consider the following data:

p ( H ~ ) = 2.5 atmWhat is the value of b.G for the above reaction at 25C?

a) -163.7 kJ I mol'b) -152.1 kJ I molc) -168.9 kJ I mold) -159.4 kJ I mole) None of these is correct.

28. The decomposition of a certain insecticide in water follows tirst-order kineticswith a rate constant of 1.45 y{l. How long will it take for the insecticide to reach0.15 of its initial value? a) 0.76 yr b) 0.93 yr c) 1.3 yr d) 1.1 yr e) None of these is correct.

29. What is the overall reaction order that corresponds to a rate constant with the unitsofM-5/2 min-I?a) I-orderb) 3/2-orderc) 5/2-orderd) 712-ordere) None of these is correct.

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30. Which of the folloVving show a correct prediction for the sign of L'l.SO?3 NO(g) -+ N20(g) + N02(g) L'l.SO = (+)2 N2H4(g) + 2 N02(g) -+ 3 N2(g) + 4 H20(g) L'l.SO (+)3 N02(g) + H20(l) -+ 2 HN03(l ) + NOq ) L'l.SO =(-)

a) I onlyb) II onlyc) I, II onlyd) II, III onlye) I, II, and III

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PERIO'orc CHART OF THE ELEMENTSVilA villA

2I IA l i lA IVA. VA V(A He4.0026

IA ~ _ t . ~ , r - - . ~3 4 5 6 7 0 9 10Li Be B C N () F Ne6.941 9.01218 10.811 12.011 14.0067 15.9994 18,990403 20.179

11 12 13 14 15 16 17 10Na Mg AI. Si P S CI Ar22.91917 24.305 26.981539 28.0855 30,91316 32.066 35.453 39.94819 20 21 22 23 24 25 26 27 20 29 30 31 32 33 J4 35 36K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Dr Kr39.U983 40.078 44.9559 47.88 50.9415 51.996 54.9380 55.847 58.9332( 58.69 63.546 65.39 69.723 72.61 74.9216 78.96 7 9 . ~ 0 4 83.8037 38 39 40 41 42 43 44 45 46 47 40 49 50 51 52 53 54Rb Sr Y Zr Nb Mo Tc Ru Rh Pd A9 Cd In Sn Sb Te I Xe85.4678 87.62 88.9059 91.224 92.9064 95.94 ) (98) 101.07 1 0 2 . 9 0 5 ~ 106.42 1 0 7 . 8 6 8 ~ 112.41 114.82 118.710 121.75 127.60 20.'045 131.2955 56 57 72 73 74 75 76 n 78 79 00 81 02 03 84 . 85 86Cs 8a *La HI Ta W Re Os Ir .p t Au ~ f I TI Pb Bi Po At Rn132.9054 137.33 1 3 8 ~ 9 0 5 5 178.49 180.9419 183.85 186.207 190.2 192.22 195.09 1 9 6 . 9 6 G ~ 2 0 4 . 3 8 3 ~ 207.2 208..9804 (209, (ZIO) (2ZZ,87 88 89 104 105 106 107 108 109Fr Ra lAc Rf Db S9 Bh Hs Mt(223) 226.0Z5-4 221.021' (2'1) fZIl) (26J) (2'2) (2'5) (266)

60 61 62 63 64 65 ' 66 67 68 69 70 718 59Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb , ~ ~ j40,115 140.90n 144.24 ~ { 1 4 5 J _ 150.36 1151.9& 151.25 168.9264 16Z.5U 164.9304 . 161.26 168.un 173.0490Th

732.0381

91Pa231.0359

92U234.02993Np

IJ1.D481

. 94Pu-.!?44)95Am(243) c7n(247) 97Bk(247) 96Cf{lSI''----" -99EsLJ2Sn 100Fm(257) 101Md(2SD) 102No(259J to3Lr~ J 2 ( 0 )

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~ ' ~ ~ ~ 1.-(... TtoIl4()-(jf19-'5I;' :tJi ...:l /loCyHyJ)H 1- (()..

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C w u ; f ~ ,~ Q . d /I- ---... . [ . I J ~( q ( U k ~ ) F ~ ~ I ; K

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t:..G-=. - ~ ~ K:eq ) 66 0 ~ ~ tA. ~ ~ 'II' J ~ ~

C. 13 ~ ~ ~ + . z C O J ( , I " ) ~ t . . ( ~ I t (O;

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UfUL/{

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C d W ~~ J L( ~ & , Cut,ftiLus2)

0,& = t.6 + ~ /Q r l Q _ ~ N ~ ) & ~=: -JsCr. 'I ~ u + . O u l - 3 I Y ~ (2yJ-kJ ~ ( ( ; , ~ ~ . :.J) J:;' -/f9, Y ~ u t t .QOJ-31$l;1fo("i< (ZyJ-/:: ) ..

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------

CHEM 112 EXAM 3


Total Points == 150Questions 1-25: 6 points eachUSEFUL INFORMATION:amp =coulomb I s11 = 96,486 CS=SO - (0.0592 V I n) log QS = SO - (0.0257 V I n) In Q

2 HzO(t) ---+ OZ(g) + 4 ~ ( a q ) + 4 e2 HzO(r) + 2 e- ---+ H 2(g) + 20H-(aq) Sred ::::: -1.0 V2 SO/-(aq) ---+ .S20l-(aq) + 2 e- SO ox = -2.00 Vkwh =3.6 x 106 J

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1. For the galvanic cell: Pt(s) ISn2+(aq). Sn4+(aq) II Pb2+(aq) IPb(s) , what is the functionof the Pt metal?

a) Pt is the anode and is a reactant in the overall cell reaction.b) Pt is the anode and does not appear in the overall cell reaction.c) Pt is the cathode and is a product in the overall cell reaction.d) Pt is the cathode and does not appear in the overall cell reaction.e) None ofthese is correct.

2. A galvanic cell consists of a La3+ILa half-cell and a standard Cu2+ ICu electrode.I f the La3+ILa standard half-cell functions as the anode, the reduction potentialfor Cu2+ is 0.34 V, and the standard cell potential is 2.52 V, what is the standardreduction potential for the La3+ ILa half-cell?

a) 2.S6V b) -2.S6 V c) -2.1S V d) 2.1SV e) 0.73 V

3. According to the standard reduction table, which aqueous metal ion will reduceAg+, but not Cu2+?a) H822+b) Cu+c) Fe3+d) Fe2+ e) Hi+

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4. Consider the cell reaction represented by the following notation:

What is the quantitative change in the cell voltage on increasing the ionconcentration in the anode compartment by a factor of 10?

a) 0.06 Vb) 0.03 Vc) -0.03 Vd) -0.06 Ve) None of these is correct.

5. The equivalent mass ofMn04- ion in the following unbalanced reaction in basicaqueous solution is:Mn04-(aq) + r(aq) -- MnO(s) + 12 (s)

a) 118.93 g.b) 59.47 g.c) 39.64 g.d) 29.73 g. e) 23.79 g.

6. What is the relationship betw"een the standard cell potentials, Z;0, for the followingtwo cell reactions?

a) Z;(l) = Z;(2)b) Z;(l) =2 o ( 2 )c) Z;(l) = -2 Z;(2)d) ~ o ( l ) = -( ~ o ( 2 ) l e) ~ o ( l ) = _ ~ o ( 2 )

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7. An electrochemical cell is constructed to operate with the following reaction,

for which = 0.34 V. Which of the following changes will result in an increase inthe cell potential?

1. increasing the dichromate concentration2. increasing the pH3. increasing the mercuric ion concentration4. increasing the amount of liquid mercury

a) 1 only b) 2 onlyc) 1 and 2 onlyd) 1 and 3 onlye) 1,2 and 4 only

8. What is the oxidation number of the element As in the compound Na3As04?a) +8b) +2c) +1d) +5e) +7

9. Which of the following statements is true about the electrolysis of aqueous CuC C2?a) Ct2g) is produced at the anode.b) H2(g) is produced at the cathode. c) 02(g) is produced at the cathode. d) Cll(s) is produced at the anode. e) None of these is correct.

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10. What volume of S02 gas at STP is produced by the reduction of SOi- in acidic solution i3.50 A of current is passed through the solution for 45.0 min? a) 2.19 L b) 0.0895 L c) 0.358 L d) 4.39 L e) None of these is correct.

11. How many seconds does it take to deposit 1.35 g ofNi on a decorative plate when 10.5 Ais passed through a Ni(N03)2 solution?a) 423 sb) 106sc) 211 sd) 2.22 X 103 s e) None of these is correct.

12. The pH of an unknown If" ion solution was determined using glass and calomelelectrodes with a reference value of0.4 7 V. If the cell potential for the unknown solutionis 0.93 V, what is the pH?

a) 4.35 b) 3.17 c) 6.39 d) 7.77 e) None of these is correct.

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13. A salt bridge:a) is typically a tube containing a solution or a gel of a salt such as NfuN03or Kce that connects the two half cells of an electrochemical cell.b) allows for ion flow between the half cells of an electrochemical cell.c) helps provide for the maintenance of electrical neutrality in an

electrochemical celL d) Only two of the above are correct. e) All (a,b, and c ) of the above are correct.

14. A ~ a l v a n i c cell is constructed from two (CU2+(aq) ICll(s) half-cells, one having aeu + concentration of 0.03 59 M and the other a concentrat ion of 8.17 x 10-4 M.At 25C, this cell will exhibit a voltage o f ~ _ , and the anode will be the cellhaving the __ Cu2+ concentration.

a) 0.049 V smaller b) 0.097 V larger c) 0.097 V smaller d) 0.049 V larger e) 0.00 V larger

15. During a galvanic cell reaction, electrons move through the external circuittoward the _ which has a __ sign and positive ions in the cell move towardthe-

a) anode (-) anode b) anode (-) cathode c) cathode; (-) anode d) c.athode ; (+) anode e) cathode; (+) cathode

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16. Which of the following statements is true when the following half reaction is properlybalanced in aqueous acid solution?

a) There are 2 e- on the left. b) There are 3 e- on the left. c) There are 6 e- on the left. d) There are 4 e- on the left. e) None of these is correct.

17. When the following equation is properly balanced in aqueous basic solution, what is thecoefficient in front ofH20?3 ) 4- Fe(CN)6 -(aq) + Re{s) --+ Fe(CN 6 (aq) + Re04 (aq) (NOTE: CN-)

a) 1b) 2c) 3d) 4e) None ofthese is correct.

18. Electrolysis of a molten salt with formula MCt4 required 20.5 min for a currect of 3.50to plate out 1.32 g of the metal. What is the identity of the metal?a) Ti

b) Snc) Pbd) Rh e) None ofthese is correct.

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19. Which of the following statements is true when the following half reaction is properlybalanced in aqueous basic solution?

a) There are 2 e- on the right.b) There are 3 e- on the left.c) There are 3 e- on the right.d) There are 5 e- on the right.e) None of these is correct.

20. Calculate the number of kilowatt-hours of electricity required to produce 1.00 x 105 kg oMg from molten MgCt2 by electrolysis if the applied voltage is 6.50 V. Assume 100%efficiency.

a) 7.17 x 105 KWh b) 3.45 X 105 KWh c) 7.94 X 1011 KWh d) 6.92 x 107 KWhe) None of these is correct.

21. When the following equation is properly balanced in aqueous acid solution, what is thecoefficient in front of H20?Zn(s) + NO) (aq) ---+ Zn(OH)/-(aq) + NH3(g)

a) 8b) 11c) 13d) 15e) None of these is correct.

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22. If pHz 0.100 atm, [Cd2+] = 0.200 M, and [H+l = 1.00 x 10-5 M, what is the valueof ; at 25C for the cell based on the following reaction?

+ d7+C ~ s ) + 2 H (aq) -+ H 2 (g) + C - (aq) 0.40 V a) -0.90 V b) 0.12 V c) 0.15 V d) 0.23 V e) 0.30 V

23. Using standard reduction potentials, what is the standard emf fo r the followingreaction?2+ 2Hg2 (aq) + C + ,u (aq) -+ .., H "\ C 7+L. g(O + L. U- (l1q)

a) 1.00 V b) -1.00 V c) -0.70 V

d) 0.70 V e) None of these is correct.

24. Calculate the equilibrium constant for the following reaction at 298 K. 7+4 Hg- H + 2 H 2+ N - +(aq) + N2 5 (aq) -+ g2 (ag) + 2(g} + .) H (aq)

a) 4.2 x 1046

b) 2.0x 1023 c) 5.0 X 1077 d) 7.1 X 1038 e) None of these is correct.

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25. Consider the following reduction half-reactions: F 3+ F 2+ e (aq) + -+ e (aq) ~ o r e d 0.77 V

red -1.77 V What is the value of A G o for the oxidation of Fe2-(aq} by N:;O(aq) at 298 K?

a) -193 kJ I mol b) 193 kJ 111101 c) 490. kJ I mol d) -490. kJ I mol e) 245 kJ I mol

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Standard Electrode (Half-t::ell) Potentials (298 K)*HALF-REACTION

F (9) + 2e- ~ 2F-(aq)z03(9) + 2H+(aq) + 2e- ~ O'},(g) + H'},O(l)Co3+(aq) + e- ~ Col+(aq)H'},O'},(aq) + 2H+(aq) + 2e- ~ 2H 0(l)zPbO'},(s) + 4H+(aq) + SO/-(aq) + 2e- ~ PbS0 4 (s) + 2H'},O(l)Ce4+(aq) + e- ~ Ce3+(aq)Mn0 4 -(aq) + BH+(aq) + 5e- Mn2+(aq) + 4H 2 0(l)Au3+(aq) + 3e- ~ Au(s)C12 (a) + 2e- ~ 2Cl-(aq)Cr 0 Z-(aq) + 14H+(aq) + 6e- ~ 2Cr3+(aq) + 7H 0(l)2 7 2Mn02(s) + 4H+(aq) + 2e - ~ Mn2+(aq) + 2H 0(l)z02(9) + 4H+(aq) + 4e- ~ 2H20(l) Br2 (l) + 2e- ~ 2BC(aq) NO) -(aq) + 4H+(aq) + 3e- ~ NO(S) + 2Hp(l) 2Hg2+(aq) + 2e- ~ Hg/+(aq) Hg/+(aq) + 2e- ~ 2Hg(l) Ag+(aq) + e- ~ Ag(s) Fe3+(aq) + e- ~ Fe2+(aq) 02(&) + 2H+(aq) + 2e- ~ H20z(aq) Mn0 4 (aq) + 2H20(l) + 3e- ~ Mn01(s) + 40H-(aq) 12 (s) + 2e- ~ 21-(aq)02(&) + 2H20(l) + 4e- ~ 40H-(aq)Cu2+(aq) + 2e- ~ Cu(s)AgCl(s) + e- ~ Ag(s) + 'Cl-(aq)S04'},-(aq) + 4H+(aq) + 2e - ~ S02(g) + 2H1Cu2+(aq) + e- ~ Cu+(aq)Sn4+(aq) + 2e - ~ Sn2+(aq)2H+(aq) + 2e- ;:=': Hz(a)Pb2 +(aq) + 2e- ~ Pb(s)Sn2+(aq) + 2e- ~ Sn(s)N (a) + 5H+(aq) + 4e- ~ N H/(aq)2 2Ni2+(aq) + 2e Co2+ (aq) + 2ePbS04(s) + 2eCd2+(aq) + 2eFe2+(aq) + 2eCr3+(aq) + 3eZn2+(aq) + 2e

~~

~~

~~

~

Ni(s)Co(s)Pb(s) + SO/-(aq)Cd(s)Fe(s)Cr(s)Zn(s)

2H20(l) + 2e- ~ H2 (g) + 20H-(aq) Mn2+(aq) + 2e- ~ Mn(s) AP+(aq) + 3e- ~ Ai(s) Mg2+ (aq) + 2e- ~ Mg(s) Na+(aq) + e- ~ Na(s) Ca2+(aq) + 2e Sr2+(aq) + 2eBa2+(aq) + 2eK+(aq) + e- ~ U+(aq) + e- ~

~ Ca(s)~ Sr(s)

~ Ba(s)K(s)Li(s)

0(l)

+2.87+2.07+1.82+1.77+1.70+1.61+1.51+ 1.50+1.36+ 1.33+1.23+1.23+1.07+0.96+0.92+0.85+0.80+0.77+0.68+0.59+0.53+0.40+0.34+0.22+0.20+0.15+0.13

0.00-0.13-0.14-0.23-0.25-0.28-0.31-0.40-0.44-0.74-0.76-0.831.18

1.66-2.37-2.71-2.87-2.89-2.90-2.93-3.05

Written as reductions; 0 value refers to all components in [hei r standard states: 1 M fordissolved spedes; I atm pressure for gases; the pure sllbstance for solids and liquids.

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PERfO'ore CHART OF THE ELEMENTS1 10-IA - VilA VIIH1.0079 2~ HeIA ilIA IVA. VA V(A 4.0026

7 6 8 10 ()i C Fe B Ne10.011.01218 12.011 14.0067 15.9994 18,998403 20.17.9.'11 12 143 16 17 165Mg Si 5 CI Ara PAI 30.97316 35.453 39.948.0855 32.0662.98911 26.9815394.30519 20 21 24 21 362 25 26 28 293 30 31 353 342V Coa Sc Ti Cr Mn Fe Bru Zni Ga Ge As Se Kr83.804.9559 47.88 51.9960.9415 58.9332( 58.69 65.390.018 63.546 69.723 72.61 14.9216 78.96 7 9 . ~ O 49.0983 54.9380 55.841381 41 44 489 40 42 45 47 49 513 46 50 S32 54Agdb Sr Y Cd Sn Sb Iu Rh Te Xer Nb Mo Tc In'87.62 121.755.4678 88.9059 ' (98) 118.71006.42 114.82 131.292.9064 95.94 101.071.224 102.905f 112.41 127.60 ~ 2 6 . ' 0 4 50 7 . 8 6 8 ~ . 8585 56 51 72 74 76 793 75 00 81 82 863 64

p tLa W IrI Au TI Bi At Rns Ba Ta Re Os Pb Po~ J I9 6 . 9 6 6 ~ ! 2 0 4 . 3 8 3 ~83.85 186.207 190.2 192.22 207.23 8 ~ 9 0 5 5 178.49 180.9479 208.9804 (210)32.90S4 137.33 195.09 1222,209J108 109077 898 10604 105lAcr Ra Db Bh Hs Mtf 59(261 ) (.262) (265) (266)26.025-4 221.0111 (Z62) (Z63)J 2 2 3 )

58Ce140,11559Pr'.0.90n

60Nd144.2461Pm

{145J '62Sm150.36

63Eu151.9664Gd151.25

65Tb168.926-4

. 66Dyt f i l . ~ O

67Ho164.9304

68Er167.2669Tm

HMl.9J.42

70Vb173.0471LuI14.1Jf.7

90ThpZ.0J8191Pa

2 J 1 ~ ~

92U238.02993 .Np231.0482

94Pu(244)95Am(243) C ~(247) 97Ok(247) 96Cf(lSI)

,99Es{25Z1

100Fm(257)

101Md(l!inl102No

(259)

103Lr(260)

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B ,c .2 .c,O

? o ~ -f ' ~ - - 6 , 3 ~ L I

f ~ ~ , .:;; ;;';t 3'1 t/ :: 1 J ~ l./FaJ( ,(11f- v

f ('e(.l(J =- o. tYo ) /r ~ J . Ot 77 V

f ~ ;: 0.3

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A 1

E lD

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~ + . 2+C ("11 .03f9111J -) Co. ("f I .0008-/1A')f -!' (fL- 1- 310dto..nr -+! -') -/ j c.JJ.. 6e- 011 S2ef!

Ioe.-+ bJ-/+ r (JZoj - -:> aL- 1- J / - ~ o

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1Ii(c/U);,- t ; ( ~ - ) I) Fe (c.oJ(c '1- t- t { ~ ( J tjdu:tYVfi!.: -t:11 -) ~ 9 ;"(c.J,) f- O i l - ~ ,.Qeffi ~ J J . 411t.O un TI}"t

g.aU- t I) Fe.(ou)b!J -T (rOy J..

( O H - t A ~ J

t - , J . . ~ ()(cJ1fA."'V ; -r -) -.;. l-

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C ;)./

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/0= ' D ~ ; ' V 9 d K ~aL ,,(),f4).V :: R1 kr?jlj,(/,ISV) ::. ~ . Ke : ?1l1x/c Ii D ' { C , ~ l / a r

. r .. 11key = J . () i X-ID~ f f e . ~ 7 ) -) fe3r:r) +Je-J h:>D.

I [ t J ) . O ( ! t ~ ) T ) . ) I { ~ , ) -;-;.e--) t U ~ / ~ ) + o teli { r c ~ ~ -/).Fe. < J . ~ r t iJ.A",) +).;/ iufJ -) ..

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CHEM 112 EXAM 4


Total Points == 150Questions 1-30: 5 points eachUSEFUL INFORMATION:

rn = 0 21Z 30om = 10.9 m

30= 0.529 Ame =9.109 x 10-31 kgh =6.626 X 10.34 J S

. 2 2 mp =1.673 x 10.27 kgJ =kgom S Ry = 2.180 X 10.18 J e = 1.602 x 10.19 CNA =6.022 X 1023 mOr l A=hc/eV th r

~ ( p o s i t i o o ) ~ ( v e l o c i t y ) ~ h I ( 47tm ) A= h I (2meV)YzEn = _Z2 I 0 2 (Ry) A= h I mv

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1. The Pauli exclusion principle requires that:a) both the position of an electron and its momentum cannot simultaneouslybe known very accurately.b) no two electrons in the same atom can have the same set of four quantumnumbers.c) an electron can have either particle character or wave character.d) the wavelength and mass of a subatomic particle are related byA h/mv.e) the wavelength of a photon of light times its frequency is equal to thespeed of light.

2. What is the wavelength of light formed in the He+ ion when an electron movesfrom the n = 4 level to the n = 2 level?a) 91.14 nmb) 45.57 nmc) 145.5 nmd) 121.6 nm e) None of these is correct.

'" Which of the following sets of quantum numbers is not permissible?).n t D1t ms a) 1 0 0 liz

b) 4 0 0 Y;z c) 3 3 -3 -% d) 2 1 1 -Y2 e) 2 0 0 Y2

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4. Which of the following represents the shape of the d/ . / orbital?y

a) c) .:.x

,d)

5. Which of the following statements about a gaseous sulfur atom in its lowestenergy state is true?a) It is paramagnetic with 2 unpaired electrons.b) It is paramagnetic with 3 unpaired electrons.c) It is diamagnetic with no unpaired electrons.d) It is diamagnetic with 2 unpaired electrons.e) It is paramagnetic with no unpaired electrons.

6. What is the maximum electron capacity for the sixth energy level(shell)?a) 18b) 32c) 36d) 50e) 72

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7. The greater the energy ofa photon, the:a) longer the wavelength and the bigher the frequency.b) longer the wavelength and the lower the frequency.

,.c) shorter the wavelength and the bigher the frequency.d) shorter the wavelength and the lower the frequency.e) greater the speed of light in a vacuum.

8. Arrange the following spectral regions in order of increasing wavelength?Infrared(]R) ultraviolet(uv) visible!vis) microwavea) microwave < VIS < IR < uv b) nncrowave < IR < VIS < uv c) uv < vis < IR < microwave d) uv < IR < vis < nncrowave e) IR < VIS < uv < microwave

9. Consider the portion of the energy level diagram for the hydrogen atom. Forwhich of the following transitions does the light emitted have the longestwavelength?a) n=4ton=3 b) n=4ton=2 c) n 4ton 1 d) n=3ton=2 e) n 2 to n 1

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10. Which of the following statements is false?a) A 4d orbital can accommodate at most tw o electrons. b) The elect ron density at a particular point in space is proportional to the

wave function squared ( \l' 2 ) at that point.c) The spin quantum number ofan electron must be either +% or -%.d) A 2p orbital is more penetrating than a 2s; i.e., it has higher electron

density near the nucleus and inside the charge cloud of a 1s orbital.e) In the usual order of filling, the 6s orbital is filled before the 4f orbital.

11. The gaseous Cr atoms follow a rule that makes it an exception to the normal principlesfor prediction of electronic structure. Its ground state electronic configuration is:

a) [Ar] 4s2 3d4b) [Ar] 3p3 4s2 3d7c) [Ar] 4so 3d6d) [Ar] 4S1 3ds e) [Ar] 4s2 3d4

12. Which orbitals do not have a node at the nucleus?a) all beyond the first shellb) all beyond the second shellc) all but sd) nonee) only s

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13. To eject an electron from the surface of a particular metal requires a minimumenergy of 4.85 x 10,19 J. When 333 nm photons shine on the surface. what is themaximum velocity of the ejected electrons?

a) 1.25 x 106 m I sb) 1.14 X 106 m / sc) 1.03 X 106 m / sd) 4.95xl0sm/s e) None ofthese is correct.

14. What is the power output of a laser in watts (J'S'I) whose pulse emits 6.50 x 1018photons per second with a wavelength of 475 nm?a) 7.17 wattsb) 5.13 wattsc) 2.72 wattsd) 1.05 watts e) None of these is correct.

15. What is the number of orbitals in a 7f subshell?a) 1b) 3c) 5d) 7e) 14

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16. Which of the following statements i s ~ ?I Atomic radii increase in a group from bottom to topII Ionization potential increases in a period from left to right.III Electron affinity becomes increasing negative in a period from left to right.a) I only b) II only c) III only d) I and II only e) II and III only

17. What is the ionization energy for a mole ofLi2+ ions?a) 3.94 x 103 kJ I molb) 1.18 x 104 kJ I molc) 2.18 x 104 kJ / mold) 1.31 x 103 kJ / mole) None of these is correct.

18. That energy is discontinuous and comes in discrete units was first proposed by:a) Bohr. b) Schrodinger. c) Plank. d) Einstein. e) deBroglie.

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19. How many electrons may be accommodated with the quantum numbersn 3; {, := 2, m[ O?

a) 0b) 2c) 6d) 10e) 18

20. Which ofthe following quantum numbers is often designated by the letters s, p, d,f,and g instead of numbers?a) nb) t c) Illt d) Ills

21. What is the valence shell electron configuration of the ion formed from an atomof the halogen family?

a) ns2b) ns2 np5c) ns2 np6d) ns2 np7 e) ns2 np8

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22. What is the ground state configuration for a gaseous arsenic atom?lOa) [Ar] 4s24p34d

b) Is22s22p63s23p64s23dlo4p3 c) [Zn] 4p3 d) Both b) and c) are correct. e) N one of these is correct.

23. What is the energy of a photon from an JiM radio station at a frequency of 101.1MHz?

a) 6.699 x 10-32 Jb) 3.451 X 10-30 Jc) 6.699 X 10-26 Jd) 3.451 X 10- 24 Je) None of these is correct.

24. How many unpaired electrons are there in a gaseous Fe3+ ion? a) 0 b) 2 c) 3 d) 4e) 5

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25. What is the smallest increment of energy (a quantum) that can be emitted orabsorbed at a wavelength of 435 run?

a) 3.69 x 10- 18 Jb) 5.71 X 10-17 Jc) 9.31 X 10- 19 Jd) 5.11 X 10-19 Je) None of these is correct.

26. If one plots the radial probability density for a 1s orbital:a) a maximum occurs at a distance r from the nucleus.b) a maximum occurs at the nucleus.c) a node exists at a distance r from the nucleus.d) Both a) and b) are true.e) Both a) and c) are true.

27. For n and t = 3, how many possible values are there for m(? a) 0 b) 1c) 3 d) 5 e) 7

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- - -

28. Among the elementary subatomic particles of physics is the muon, which decayswithin a few nanoseconds after formation. It has a rest mass 206.8 times that ofan electron (me 9.1 09 X10 -28 g). What is the wavelength associated with amuon traveling at a velocity of 8.85 x 10 5cm! s?a) 8.22 x 1O-J2 mb) 8.22 x 10- 15 mc) 3.97 x 10- 14 md) 3.97 x 10- 17 me) None of these is correct.

29. The hydrogenic transition between n = 3 and n 1 belong to the series.a) Lymanb) Balmer c) Brackett d) Paschen e) Pfund

30. What is the uncertainity in the speed of a beam of protons \:vhose position isknown with the unceliainity of 24 nm?a) 1.31 111! sb) 0.753 m/sc) 3.51 m I sd) 10.3 m! s e) None of these is correct.

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PERIO'OlG GHART OF THE ELEMENTS1IA H VilA VillA

1.0U79 "" 2IIA filA IvA VA V(A He4.00260

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I 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe85.4678 87.62 88.9059 91.224 92.9064 95.94 ' (98) 101.07 102.905f 106.42 ~ O 7 . 8 6 8 ~ 112.41 114.82 118.110 121.15 127.60 26_'045 131.2955 56 57 72 73 74 75 76 n 78 79 80 01 02 03 84 05 86Cs Ba *La HI Ta W Re Os Ir 'Pt Au ~ J I TI Pb Bi Po At Rn132.90504 137.33 1 3 1 ~ ! J 0 5 5 178.49 180,9419 183.85 18&.207 190.2 192.22 195.09 ~ 9 6 . 9 6 6 ~ 2 0 4 . 3 8 3 ~ 207.2 208.9804 {2091 {ZIO' (ZZZI87 88 89 104 105 106 107 108 109Fr Ra lAc Rf Db 59 Bh Hs Mt_JZZ3L 126.025-4 217..077. (261) 1262) (263) (262) (265) (266)58 59 60 61 62 63 64 65 . 66 67 68 . 69 70 71Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er. Tm Vb L ~40,115 l ~ O . 9 0 n 144.24 ( 1 ~ 5 ' . 150.36 151.96 151.25 168.9264 t6l.!)U 1 G 4 . 9 ~ . 167.26 1 6 3 . ~ 2 173.1)4 J ! ~ . ~ 7

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Berg Fall 2008 T1-4