課程名稱︰普化丙
課程性質︰系訂必修
課程教師︰張煥宗
開課學院：電資學院
開課系所︰電機系
考試日期（年月日）︰Jan. 15,2007
考試時限（分鐘）：10:20 - 12:10
是否需發放獎勵金：是
（如未明確表示，則不予發放）
試題 :
Final Examination for General Chemistry
Multiple - Choice (2 points each, total 100)
1) The balanced half-reaction in which sulfate ion is reduced to sulfite ion
is a ___________ process.
(A) four-electron (B) one-electron (C)two-electron (D)three-electron
(E) six-electron
2) The half-reaction occurring at the anode in the balanced reaction shown
below is __________.
3MnO4-(aq) + 24H+(aq) + 5Fe(s) → 3Mn2+(aq) + 5Fe3+(aq) + 12H2O(l)
(A) MnO4-(aq) + 8H+(aq) + 5e- → Mn2+(aq) + 4H2O(l)
(B) 2MnO4-(aq) + 12H+(aq) + 6e- → 2Mn2+(aq) + 3H2O(l)
(C) Fe(s) → Fe3+(aq) + 3e-
(D) Fe(s) → Fe2+(aq) + 2e-
(E) Fe2+(aq) → Fe3+(aq) + e-
3) In a voltaic cell, electrons flow from the __________ to the _________.
(A) salt bridge, anode (B) anode, salt bridge (C) cathode, anode
(D) salt bridge, cathode (E) anode, cathode
4) 1V = _____________.
(A) 1 amp*s (B) 1 J/s (C) 96485 C (D) 1 J/C (E) 1 C/J
。
5) The standard cell potential (Ecell) for the reaction below is +0.126V. The
。
value of △G for the reaction is _________ kJ/mol.
Pb(s) + 2H+(aq) → Pb2+(aq) + H2(g)
(A) -24 (B) +24 (C) -12 (D) +12 (E)-50
6) The standard cell potential (Ecell) for the reaction below is +0.63V. The
cell potential for this reaction is _____________ V when [Zn2+] = 1.0 M
and [Pb2+] = 2.0 * 10^-4 M
Pb2+(aq) + Zn(s) → Zn2+(aq) + Pb(s)
(A) 0.52 (B) 0.85 (C) 0.41 (D) 0.74 (E)0.63
7)What is the equilibrium constant for the reaction listed in Question 6 at
。
25 C ?
(A) 2.0 * 10^15 (B) 2.0 * 10^17 (C) 2.0 * 10^19 (D) 2.0 * 10^21
(E) 2.0 * 10^23
8) The lead-containing reactant(s) consumed during recharging of a lead-acid
battery is/are __________.
(A) Pb(s) only (B) PbO2(s) only (C) PbSO4(s) only
(D) both PbO2(s) and PbSO4(s) (E) both Pb(s) and PbO2(s)
9) Corrosion of iron is retarded by ___________.
(A) the presence of salts (B) high pH conditions (C) low pH conditions
(D) both the presence of salts and high pH conditions
(E) both the presence of salts and low pH conditions
10) What is the cell potential of a concentration cell containing AgNO3
。
solutions at the concentrations of 0.1 M and 0.01 M at 25 C?
(A) 0.030 (B) 0.045 (C) 0.059 (D) 0.090 (E)0.12 V
11) Which element is oxidized in the reaction below?
Fe(CO)5(l) + 2HI(g) → Fe(CO)4I2(s) + CO(g) + H2(g)
(A) Fe (B) C (C) O (D) H (E) I
12) What is the coefficient of Fe3+ when the following equation is balanced?
CN- + Fe3+ → CNO- + Fe2+ (basic solution)
(A) 1 (B) 2 (C) 3 (D) 4 (E) 5
13) The purpose of the salt bridge in an electrochemical cell is to _________.
(A) maintain electrical neutruality
(B) provide a source of ions to react at the anode and cathode
(C) provide oxygen to facilitate oxidation at the anode
(D) provide a means for electrons to travel from the anode to cathode
(E) provide a means for electrons to travel from the cathode to anode
14) Which one of the following is the best oxidizing agent?
(A) H2 (B) Na (C) O2 (D) Li (E) Ca
15) Which substance can be oxidized by O2(g) in acidic aqueous solution?
(A) Br2(l) (B) Ag(s) (C) Cu2+(aq) (D) Ni2+(aq) (E) Br-(aq)
16) Which of the following reactions will occur spontaneously as written?
(A) Sn4+(aq) + Fe3+(aq) → Sn2+(aq) + Fe2+(aq)
(B) 3Fe(s) + 2Cr3+(aq) → 2Cr(s) + 3Fe2+(aq)
(C) Sn4+(aq) + Fe2+(aq) → Sn2+(aq) + Fe(s)
(D) 3Sn4+(aq) + 2Cr(s) → 2Cr3+(aq) + 3Sn2+(aq)
(E) 3Fe2+(aq) → Fe(s) + 2Fe3+(aq)
17) Consider an electrochemical cell based on the reaction:
2H+(aq) + Sn(s) → Sn2+(aq) + H2(g)
Which of the following actions would change the measured cell potential?
(A) increasing the pH in the cathode compartment
(B) lowering the pH in the cathode compartment
(C) increasing the [Sn2+] in the anode compartment
(D) increasing the pressure of hydrogen gas in the cathode compartment
(E) Any of the above will change the measured cell potential
18) Consider an electrochemical cell based on the reaction:
2H+(aq) + Sn(s) → Sn2+(aq) + H2(g)
Which of the following actions would not change the measured cell potential?
￣￣￣￣
(A) lowering the pH in the cathode compartment
(B) addition of more tin metal to the anode compartment
(C) increasing the tin(II) ion concentration in the anode compartment
(D) increasing the pressure of hydrogen gas in the cathode compartment
(E) Any of the above will change the measured cell potential
19) What is the anode in an alkaline battery _________?
(A) MnO (B) KOH (C) Zn powder (D) Mn2O3 (E) Pt
20) Cathodic protection of a metal pipe against corrosion usually entails
(A) attaching an active metal to make the pipe the anode in an
electrochemical cell
(B) coating the pipe with another metal whose standard reduction potential
is less negative than that of the pipe
(C) attaching an active metal to make the pipe the cathode in an
electrochemical cell
(D) attaching a dry cell to reduce any metal ions which might be formed
(E) coating the pipe with a fluoropolymer to act as a source of fluoride ion
(since the latter is so hard to oxidize)
21) One of the differences between a voltaic cell and an electrolytic cell is
that in an electrolytic cell __________.
(A) an electric current is produced by a chemical reaction
(B) electrons flow toward the anode
(C) a nonspontaneous reaction is forced to occur
(D) O2 gas is produced at the cathode
(E) oxidation occurs at the cathode
22) What is the reduction potential of AgCl saturated with 0.1 M NaCl if the
reduction potential of Ag is 0.799 V and the Ksp of AgCl is 1.8 * 10^-10 ?
(A) 0.111 (B) 0.222 (C) 0.333 (D) 0.910 (E) 1.022 V
23) The coordination numbers of cobalt(III) and of chromium(III) in their
complexes are always __________.
(A) 4 (B) 5 (C) 2 (D) 3 (E) 6
24) The "dentation" of a ligand is definded by ___________.
(A) how many "dents" or "deceptions" there are in the coordination sphere
of a complex species it forms
(B) how many electron donor atoms it utilizes to form coordinate bonds to
the central metal ion
(C) the total number of lone pairs of electrons it possesses
(D) how many metal ions it can sequester from solution
(E) none of the above
25) How many iron atoms are coordinated ina hemoglobin molecule ________?
(A) 1 (B) 2 (C) 3 (D) 4 (E) 5
26) The correct name for Na3[CoF6] is _________.
(A) trisodium hexakisfluorocobalt(III)
(B) trisodium hexakisfluorocobalt(II)
(C) trisodium hexakisfluorocobalt(IV)
(D) sodium hexafluorocobaltate(III)
(E) sodium hexafluorocobaltate(IV)
27) The correct name for [Ni(NH3)6](NO3)3 is ___________.
(A) dinitrohexaamminenickel(II)
(B) hexaamminenickel(III) trinitrate
(C) dinitrohexaamminenickelate(III)
(D) hexaamminenickel(II) nitrate
(E) hexaamminenickel(III) nitrate
28) In _________, the bonds are the same but the spatial arragement of the
atoms is different.
(A) structual isomers (B) linkage isomers (C) coordination-sphere isomers
(D) stereo isomers (E) resonance structures
29) The complex [Zn(NH3)2(Cl)2]2+ does not exhibit cis-trans-isomerism. The
geometry of this complex must be _____________.
(A) tetrahedral (B) trigonal bipyramidal (C) octahedral (D) square planar
(E) either tetrahedral or square planar
30) How many isomers exist for the octahedral complex ion [Co(NH3)4(F)2]+ ?
(A) 1 (B) 2 (C) 3 (D) 4 (E) 5
31) Linkage-isomerism can only occur ____________.
(A) in cis-isomers of octahedral complexes (B) with cobalt complexes
(C) with coordination number 6 (D) with tetrahedral complexes
(E) with ligands that have more than one possible donor atom
32) Metals with _________ electron configurations characteristically form
diamagnetic, square planar complexes
0 9 6 8 10
(A) d (B) d (C) d (D) d (E) d
n+
33) Formation of a complex species of M metal ion with ligands often ______.
n+
(A) "masks" original chemical properties of both the M ion and the ligands
n+
(B) reduces availability of the free M ions in solution
n+
(C) may cause changes in the ease iwth which M is reduced or oxidized
n+
(D) alters original physical properties of M
(E) all of the above
34) Changes in the coordination sphere of a complex compound may lead to
changes in _____________.
(A) color (B) physical properties (C) chemical properties (D) stability
(E) all of the above
35) What are the respective central-metal oxidation state, coordination number
and overall charge on the complex ion in Na2[Cr(NH3)2(NCS)4] ?
(A) +3 ; 6 ; -1 (B) +3 ; 6 ; +1 (C) +2 ; 6 ; -2 (D) +2 ; 4 ; -1
(E) +1 ; 6 ; -2
36) Which of the following is not a chelating agent ?
(A) thiocyanate (B) EDTA (C) porphine (D) ethylenediamine
(E) oxalate anion
37) What is the purpose of adding EDTA to prepared foods ?
(A) to keep ions such as Ca2+ in solution so the food looks good
(B) to complex trace metal ions that catalyze decomposition reactions
(C) to complex iron(III) ions so they can catalyze protien decomposition
on cooking
(D) to aid in browning of the surface during cooking
(E) to prevent dissolution of the container in the food when stored for
long periods of time
38) What are the donor atoms in a porphine molecule?
(A) N (B) O (C) S (D) Br (E) F
39) How many bonds can ethylenediamine form to a metal ion?
(A) 1 (B) 2 (C) 3 (D) 4 (E) 6
40) Which homogeneous aqueous equilibrium would be expected to lie to
the right?
(A) [AgI2]- + 2Br- ←→ [AgBr2]- + 2I-
(B) [Ni(H2NC2H4NH2)3]2+ + 6NH3 ←→ [Ni(NH3)6]2+ + 3 H2NC2H4NH2
(C) [CoCl4]2+ + 6H2O ←→ [Co(H2O)6]2+ + 4Cl-
(D) [Fe(NH3)6]2+ + (C20H10N4)2- ←→ Fe(NH3)2(C20H20N4) + 4NH3
(E) [Cu(NH3)4]2+ + 6H2O ←→ [Cu(H2O)6]2+ + 4NH3
41) The chelate effect is best attributed to considerations of which type?
(A) hydration (B) enthalpy (C) entropy (D) hydrogen bonding (E) resonance
42) Which of the following will display optical isomerism?
(A) square-planar [Rh(CO)2(Cl)2]- (B) square-planar [Pt(H2NC2H4NH2)2]2+
(C) octahedral [Co(NH3)6]3+ (D) octahedral [Co(NH3)5(Cl)]2+
(E) octahedral [Co(H2NC2H4NH2)3]3+
43) Which one of the following complexes can exhibit geometrical isomerism?
(A) [Pt(NH3)2(Cl)2]2- (square planar) (B) [Zn(NH3)2(Cl)2] (tetrahedral)
(C) [Cu(NH3)4]2+ (square planar) (D) [Cu(NH3)5(Cl)]2+ (octahedral)
(E) All of above can exhibit geometrical isomerism
44) A racemic mixture is
(A) an equal mixture of both enantiomers of an optically active species
(B) a mixture of an optically active species with an optically inactive
species
(C) an equal mixture of cis- and trans-isomers
(D) a mixture of metal ions and ligands in equilibrium
(E) a mixture of structural isomers
45) Based on electron configuration, which is most likely colorless?
(A) [Cu(NH3)4]2+ (B) [Cd(NH3)4]2+ (C) [Ni(NH3)6]2+ (D) [Cr(NH3)5(Cl)]2+
(E) [Cu(NH3)6]2+
46) Which one of the following complex ions will be paramagnetic?
(A) [Fe(H2O)6]2+ (low spin)
(B) [Fe(H2O)6]3+ (low spin)
(C) [Co(H2O)3]3+ (low spin)
(D) [Zn(H2O)4]2+
(E) [Zn(NH3)4]2+
47) Which Co(III) complex is most likely high-spin?
(A) [Co(NH3)6]3+ (B) [Co(NO2)6]3- (C) [Co(CN)6]3- (D) [CoF6]3-
(E) [Co(CH3CN)6]3+
48) Which complex below has 2 unpaired electrons?
(A) square-planar [Ni(CN)4]2- (B) low-spin octahedral [Fe(CN)6]3-
(C) tetrahedral [CoCl4]2- (D) octahedral [Ni(NH3)6]2+
(E) tetrahedral [FeI4]2-
49) Which octahedral Ti(III) complex below has its d-d electronic transition
at shortest wavelength?
(A) [Ti(NH3)6]3+ (B) [Ti(H2NC2H4NH2)3]3+ (C) [Ti(H2O)6]3+
(D) [TiCl6]3- (E) [TiF6]3-
50) Which one of the following coordination compounds would be paramagnetic?
(A) [Zn(NH3)4]Cl2 (B) K[FeCl4] (low spin) (C) [Cu(H2O)4]Br
(D) Na[CoCl6] (low spin) (E) [Cd(H2O)6]SO4
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