C118 Final Exam

(PE1) Which of the following liquids will exhibit the highest vapor pressure? A) Br2, bp = 58.8°C B) CH3OH, bp = 64.7°C C) H2O, bp = 100°C D) All exhibit the same vapor pressure.

A) Br2, bp = 58.8°C

(E2) What is the most soluble salt of the following set? A) Ca(OH)2with Ksp= 4.7 × 10-6 B) Mg(OH)2with Ksp= 5.6 × 10-12 C) Fe(OH)2with Ksp= 4.9 × 10-17 D) Al(OH)2with Ksp= 1.9 × 10-33

A) Ca(OH)2with Ksp= 4.7 × 10-6

(PE3) Consider the reaction: CuO(s) + H2(g) → Cu(s) + H2O(l) In this reaction, which substance is the oxidizing agent and which substance is the reducing agent? A) CuO (oxidizing agent) and H2 (reducing agent) B) H2O (oxidizing agent) and H2(reducing agent) C) H2(oxidizing agent) and CuO (reducing agent) D) CuO (oxidizing agent) and Cu (reducing agent)

A) CuO (oxidizing agent) and H2 (reducing agent)

(E2) Which of the following is an Arrhenius acid? A) H2CO3 B) LiOH C) NH2CH3 D) CH3CCl3 E) More than one of these substances is an Arrhenius acid.

A) H2CO3

(PE2) Which of the following is an Arrhenius acid? A) H2SO4 B) LiOH C) NH2CH3 D) CH3CCl3 E) More than one of these substances is an Arrhenius acid

A) H2SO4

(PE2) What is the strongest Br∅nsted-Lowry acid in the chemical reaction shown below? 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l) A) HNO3 B) Ba(OH)2 C) Ba(NO3)2 D) H2O

A) HNO3

(E2) Which one of the following will form a basic solution in water? A) NaC2H3O2 B) NaNO3 C) FeCl3 D) NH4Cl E) All of the above will form basic solutions.

A) NaC2H3O2

(PE2) Acid rain consists primarily of ________. A) both nitric and sulfuric acid B) sulfuric acid C) nitric acid D) acetic acid E) carbonic acid

A) both nitric and sulfuric acid

(PE3) Which of the following octahedral complexes would absorb the longest wavelengths of light? Spectrochemical series: CO > CN-> NO2->en > NH3> SCN->H2O > F-> OH->Cl->Br-> I- A)[Cr(H2O)6]{3+} B)[Cr(CN)6]{3-} C)[Cr(SCN)6]{3} D)[Cr(en)3]{3+}(en = ethylenediamine) E)[Cr(NH3)6]

A)[Cr(H2O)6]{3+}

(E3) In the coordination compound K3[Cr(CN)6], how many 3d electrons does chromium have? A. 3 B. 4 C. 5 D. 6 E. 7

A. 3

(E3) Which of the following is a true statement concerning the reaction? 2 Al(s) + 3 Co2+(aq) → 2 Al3+(aq) + 3 Co(s) A. Al(s) is being oxidized. B. Co2+(aq) is the reducing agent C. Al(s) is the oxidizing agent D. Co(s)is the oxidizing agent. E. Al3+(aq)is the reducing agent

A. Al(s) is being oxidized.

(E3) According to the table of standard reduction potentials, which aqueous metal ion will reduce Ag+, but not Cu2+? A. Fe2+ B. Fe3+ C. Mn2+ D. Sn2+

A. Fe2+

(E1) Give the reason that antifreeze is added to a car radiator. A. The freezing point is lowered and the boiling point is elevated. B. The freezing point is elevated and the boiling point is lowered. C. The freezing point and the boiling point are elevated. D. The freezing point and the boiling point are lowered. E. None of the above

A. The freezing point is lowered and the boiling point is elevated.

(E1) Which of the following compounds will be most soluble in ethanol (CH3CH2OH)? A. ethylene glycol (HOCH2CH2OH) B. trimethylamine (N(CH3)3) C. hexane (CH3CH2CH2CH2CH2CH3) D. acetone (CH3COCH3) E. None of these compounds should be soluble in ethanol.

A. ethylene glycol (HOCH2CH2OH)

(E1) Arrange the following molecules from lowest to highest boiling point. H2S, H2O, CH4, SiH4 A.CH4 < SiH4< H2S < H2O B.SiH4< H2S < CH4< H2O C.SiH4< CH4< H2S < H2O D.CH4 < SiH4< H2O < H2S E.H2O < H2S < SiH4< CH4

A.CH4 < SiH4< H2S < H2O

(PE3) Two well-known complex ions containing Ni are [Ni(H2O)6]2+, which is green, and [Ni(en)3]2+, which is purple. Which of these statements is TRUE? A.The crystal field splitting energy (Δ) is greater in [Ni(en)3]2+than in [Ni(H2O)6]2+ B.[Ni(en)3]2+absorbs energy in the red region of the spectrum. C.[Ni(en)3]2+is diamagnetic and [Ni(en)3]2+is paramagnetic. D.Nickel has different oxidation numbers in the two complexes. E.The green complex absorbs green light.

A.The crystal field splitting energy (Δ) is greater in [Ni(en)3]2+than in [Ni(H2O)6]2+

(E3)Which of the following octahedral complexes would absorb the longest wavelengths of light? Spectrochemical series: CO > CN-> NO2->en > NH3> SCN->H2O> F-> OH->Cl->Br-> I- A.[Ni(H2O)6]3+ B.[Ni(SCN)6]3- C.[Ni(NH3)6]3+ D.[Ni(CN)6]3- E.[Ni(en)3]3+(en = ethylenediamine)

A.[Ni(H2O)6]3+

(E3) Which one of the following complexes can exhibit geometrical isomerism? A.[Pt(NH3)2Cl2](square planar) B.[Zn(NH3)2Cl2](tetrahedral) C.[Cu(NH3)4]2+(square planar) D.[Co(NH3)5Cl]2+(octahedral) E.[Cu(CN)2]-(linear)

A.[Pt(NH3)2Cl2](square planar)

(PE2) Which is the best acid to use in the preparation of a buffer with pH = 7.4? A) CH3COOH (Ka= 1.8 x 10-5) B) H2PO4-(Ka= 6.3 x 10-8) C) HBrO (Ka= 2.3 x 10-9) D) HClO4

B) H2PO4-(Ka= 6.3 x 10-8)

(E2) Write a balanced equation for the dissociation of the Bronsted-Lowry acid HSO4-in water. A) HSO4-(aq) + H2O(l) ⇌H2SO4(aq) + OH-(aq) B) HSO4-(aq) + H2O(l) ⇌SO42-(aq) + H3O+(aq) C) HSO4-(aq) + H2O(l) ⇌SO32-(aq) + OH-(aq) D) HSO4-(aq) + H2O(l) ⇌SO3(g) + OH-(aq) + H2O(l)

B) HSO4-(aq) + H2O(l) ⇌SO42-(aq) + H3O+(aq)

(PE1) Which cation in each set is expected to have the larger (more negative) hydration energy? Set I. Mg2+or Ca2+ Set II.Li+or Al3+ A) Mg2+in set I and Li+in set II B) Mg2+in set I and Al3+in set II C) Ca2+in set I and Li+in set II D) Ca2+in set I and Al3+in set II

B) Mg2+in set I and Al3+in set II

(PE1) Which of the following should most favor the solubility of an ionic solid in water? A) a small lattice energy for the solid and a low hydration energy for its ions B) a small lattice energy for the solid and a high hydration energy for its ions C) a high lattice energy for the solid and a low hydration energy for its ions D) a high lattice energy for the solid and a high hydration energy for its ions

B) a small lattice energy for the solid and a high hydration energy for its ions

(PE1) One reason ionic compounds do not dissolve well in nonpolar solvents is that A) ion-dipole interactions are too large for effective solvation to occur. B) ion-solvent interactions are not strong enough to solvate the ions in solution. C) not all cations and anions have the same magnitude of charge and therefore do not form neutral ion pairs. D) there are no forces of attraction between ions and nonpolar molecules.

B) ion-solvent interactions are not strong enough to solvate the ions in solution.

(E3) Why is Zn2+colorless? A. d-orbitals are completely empty B. d-orbitals are completely filled C. ∆ is large and the ion absorbs light in the UV (which we can't see) D.∆ is small and the ion absorbs light in the IR (which we can't see)

B. d-orbitals are completely filled

(E3) Select the correctname for: [Co(NH3)6]2+ A. hexammoniacobaltate(II) ion B. hexaamminecobaltate(II) ion C. hexammoniacobalt(II) ion D. hexaamminecobalt(II) ion E. hexammoniacobalt ion

B. hexaamminecobaltate(II) ion

(E3) Consider the violet-colored compound, [Cr(H2O)6]Cl3and the yellow compound, [Cr(NH3)6]Cl3. Which of the following statements is false? A. Both chromium metal ions are paramagnetic with 3 unpaired electrons. B. ∆ for [Cr(H2O)6]Cl3is calculated directly from the energy of yellow light. C. ∆ for [Cr(H2O)6]3+is less than ∆ for [Cr(NH3)6]3+. D. A solution of [Cr(H2O)6]Cl3transmits light with an approximate wavelength range of 400 -420 nm. E. The two complexes absorb their complementary colors.

B. ∆ for [Cr(H2O)6]Cl3is calculated directly from the energy of yellow light.

(E1)Determine the type of intermolecular forces that are present in CH2F2. A.Dispersion B.Dispersion and dipole-dipole C.Dipole-dipole D.Dispersion, dipole-dipole, and hydrogen bonding E.Dipole-dipole and hydrogen bonding

B.Dispersion and dipole-dipole

(E3) Which of the following is the strongest oxidizing agent? Refer to the table of standard potentials at the front of the exam. A.Au (s) B.O2(g) C.Zn2+(aq) D.Mg (s) E.No oxidizing agents are listed because this is a table of reduction potentials.

B.O2(g)

(PE1) Which of the following is expected to have the greatest viscosity? A) C5H12 B) C6H14 C) C5H11OH D) CH4

C) C5H11OH

(E2) Which of the following is a Bronsted-Lowry base, but not an Arrhenius base? A) H2SO4 B) LiOH C) NH2CH3 D) CH3CCl3 E) More than one of these is a Bronsted-Lowry base.

C) NH2CH3

(PE2)Which of the following is aBronsted-Lowry base, but not an Arrhenius base? A) H2SO4 B) LiOH C) NH2CH3 D) CH3CCl3 E) More than one of these is a Bronsted-Lowry base.

C) NH2CH3

(PE3) Which complex is optically active? A) [CoCl4en]{2-} B) trans-[CrCl2(en)2]{+} C) cis-[CrCl2(en)2]{+} D) [PtCl2(NH3)2]

C) cis-[CrCl2(en)2]{+}

(PE1) Which of the intermolecular forces is the most important contributor to the high surface tension shown by water (H2O)? A) dipole-dipole forces B) dispersion forces C) hydrogen bonding D) ion-dipole forces

C) hydrogen bonding

(PE1) The change in the Gibbs free energy (ΔG) for dissolving more solute in a saturated solution is: A) negative. B) zero. C) positive. D) negative at low temperatures and positive at high temperatures.

C) positive.

(E1) Which of the following best explains why ΔHvap is usually higher than ΔHfusion? A. Vaporization occurs at high temperature. B. Vaporization involves the breaking of bonds within molecules. C. Vaporization involves the breaking of all intermolecular forces between molecules. D. Vaporization increases the entropy of molecules.

C. Vaporization involves the breaking of all intermolecular forces between molecules.

(PE2) What is the pH at the equivalence point of a weak acid-strong base titration? A. pH < 7 B. pH = 7 C. pH > 7 D. pH = 14.00

C. pH > 7

(PE3) Doubling all the coefficients in the equation for the cell reaction A.doubles both E° and ΔG°. B.doubles E°, but does not change ΔG°. C.doubles ΔG°, but does not change E°. D.does not change E° or ΔG°.

C.doubles ΔG°, but does not change E°.

(PE2) Which one of the following salts, when dissolved in water, produces the solution with the lowest pH? A) RbCl B) NH4Cl C) SrCl2 D) AlCl3

D) AlCl3

(PE2) Arrange the following 0.10 M aqueous solutions in order of increasing pH(ie lowest pH on left...highest on the right: NaOH, HBr, NaCH3CO2, KBr, NH4Br. A) HBr, KBr, NH4Br, NaCH3CO2, NaOH B) NaOH, NaCH3CO2, NH4Br, KBr, HBr C) NaOH, NaCH3CO2, KBr, NH4Br,HBr D) HBr, NH4Br, KBr, NaCH3CO2, NaOH

D) HBr, NH4Br, KBr, NaCH3CO2, NaOH

(E2) Barium hydroxide is slightly soluble in water, with a Ksp of 5.00 × 10-4at 298K. The dissolution of barium hydroxide in water is an endothermic process. Ba(OH)2(s) -->/<-- Ba+2(aq) + 2OH-(aq) Which of the following will increase the solubility of Barium hydroxide? A) Barium hydroxide is added to the solution. B) Sodium hydroxide (NaOH) is added to the solution. C) The temperature is decreased. D) HCl is added to the mixture.

D) HCl is added to the mixture.

(PE2) What is the conjugate base of the Br∅nsted-Lowry acid HPO4{2-}? A) H3PO4 B) H2PO4{-} C) HPO4{2-} D) PO4{3-}

D) PO4{3-}

(PE1) For a particular compound, which is expected to be the largest in general? A) the heat required to raise the temperature of one mole of the gas 10.0°C B) the heat required to raise the temperature of one mole of the liquid 10.0°C C) the molar heat of fusion at the normal melting point D) the molar heat of vaporization at the normal boiling point

D) the molar heat of vaporization at the normal boiling point

(PE1) Determine the type of intermolecular forces that are present in CH3CH2CH2OH. A)dispersion B)dispersion and dipole-dipole C)dipole-dipole D)dispersion, dipole-dipole, and hydrogen bonding E)dipole-dipole and hydrogen bonding

D)dispersion, dipole-dipole, and hydrogen bonding

(PE1) Commercial cold packs often contain solid NH4NO3and a pouch of water. The temperature of the pack drops as the NH4NO3dissolves in water. Therefore, for the dissolving of NH4NO3in water A)ΔHsoln is negative and ΔSsoln may be negative or positive. B)ΔHsoln is negative and ΔSsoln is positive. C)ΔHsoln is positive and ΔSsoln may be negative or positive. D)ΔHsoln is positive and ΔSsoln is positive.

D)ΔHsoln is positive and ΔSsoln is positive.

(PE3) In K4[Fe(CN)6], how many 3d electrons does iron have? A. 3 B. 4 C. 5 D. 6 E. 7

D. 6

(PE3) From the Table of Standard Reduction Potentials given at the front of the test, what is the strongest reducing agent. A. F2 B. F- C. Li+ D. Li E. H2 F. H+

D. Li

(E3) In a galvanic cell, the half-reaction: MnO4-(aq) + 8 H+(aq) + 5 e-→ Mn2+(aq) + 4 H2O(l) is A. an oxidation half-reaction and occurs at the anode. B. an oxidation half-reaction and occurs at the cathode. C. a reduction half-reaction and occurs at the anode. D. a reduction half-reaction and occurs at the cathode.

D. a reduction half-reaction and occurs at the cathode.

(PE3) The compound K4[Fe(CN)6] is used in calico printing and wool dyeing. Give its systematic name. A. potassium iron(III) hexacyanate B. potassium hexacyanideferrate C. tripotassium iron(III) hexacyanate D. potassium hexacyanoferrate(II) E. None of these choices is correct.

D. potassium hexacyanoferrate(II)

(E1) Commercial cold packs often contain solid NH4NO3 and a pouch of water. The temperature of the pack drops as the NH4NO3dissolves in water. Therefore, for the dissolving of NH4NO3in water, A. ΔHsoln is negative and ΔSsoln may be negative or positive. B. ΔHsoln is negative and ΔSsoln is positive. C. ΔHsoln is positive and ΔSsoln may be negative or positive. D. ΔHsoln is positive and ΔSsoln is positive.

D. ΔHsoln is positive and ΔSsoln is positive.

(PE2) An important buffer in the blood is a mixture of ________. A) HCl and NCl B) HCl and NaOH C)CH3COOH and HCO3{-} D) H2CO3 and NH3 E) H2CO3 and HCO3{-}

E) H2CO3 and HCO3{-}

(E2) What is the conjugate acid of H2AsO4{-}? A) HAsO42{-} B) AsO43{-} C) H2O D) H3O{+} E) H3AsO4

E) H3AsO4

(E2) Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M concentration at 25∘C. A) HF, Ka= 3.5 × 10-4 B) HCN, Ka= 4.9 × 10-10 C) HNO2, Ka= 4.6 × 10-4 D) HCHO2, Ka= 1.8 × 10-4 E) HClO2, Ka= 1.1 × 10-2

E) HClO2, Ka= 1.1 × 10-2

(PE3) Refer to the table of standard reduction potentials given on the exam. Which of the following metals can be oxidized by H+ under standard conditions? Cu, Zn, Ag, Sn A) All of them B) Ag only C) Ag, Sn, and Cu D) Zn only E) Zn and Sn

E) Zn and Sn

(E3) Consider the coordination compound, Na2[Pt(CN)4]. The Lewis base is A. [Pt(CN)4]2- B. Na+ C. Pt D. Pt2+ E. CN-

E. CN-

(E1) Place the following solutions in order of increasing osmotic pressure. I. 0.15 MHOCH2CH2OH II. 0.15 M BaCl2 III. 0.15 M NaI A. III < I < II B. II < III < I C. I < II < III D. II < I < III E. I < III < II

E. I < III < II

(PE3) Cisplatin complexes are A.used in the extraction of silver and gold. B.effective antidotes for heavy metal poisoning (e.g., Pb2+and Hg2+). C. used to provide nutrients for plants. D. used to prevent oxygen depletion of lakes. E. effective antitumor agents.

E. effective antitumor agents.

(E3) Which response gives the correct coordination number (C.N.) and oxidation number (O.N.) of the transition metal atom in [Co(NH3)2(H2O)2Cl2]+ ? A.C.N. = 2; O.N. = +3 B.C.N. = 3; O.N. = +1 C.C.N. = 4; O.N. = +2 D.C.N. = 6; O.N. = +1 E.C.N. = 6; O.N. = +3

E.C.N. = 6; O.N. = +3