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Chemistry Final Exam - Spring 2000, Exams of Chemistry

A final exam for a college-level chemistry course, including questions on various topics such as radioactive decay, coordination compounds, electron configurations, isomerism, and thermodynamics.

Typology: Exams

Pre 2010

Uploaded on 08/06/2009

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CH 126 B NAME:
FINAL EXAM
Spring 2000
1) Match the term in column A to the one term or statement in column B that best
describes it. Notice that there will be two definitions from column B that will not be
used. (2 points each)
Column A Column B
Paramagnetism 1) The number of ligands attached to a metal.
Diamagnetism 2) The nucleus of a helium atom.
Chiral 3) Enantiomer.
Coordination Number 4) An electron.
Gangue 5) A proton or neutron.
Alpha Particle 6) Weak repulsion by a magnetic field.
Beta Particle 7) Impurities associated with ores.
Nucleon 8) Species bonded to central metal atoms in a coordination
complex.
Fission 9) Weak attraction to a magnetic field.
High Spin 10) Superimposable mirror images
Low Spin 11) Nonsuperimposable mirror images.
Fusion 12) The electron configuration for a coordination complex with
the maximum number of unpaired electrons.
Optical isomer 13) The electron configuration for a coordination complex with
the minimum number of unpaired electrons.
Ligand 14) Cis-Trans or Fac-Mer Isomer
Geometric isomer 15) The highly exothermic process by which light nuclei
combine to form heavier nuclei.
16) The highly exothermic process by which heavy nuclei split
to form lighter nuclei.
17) “Bubbling” associated with metal dissolution.
2) The first four steps of the radioactive decay series of 235U are , , , and
emission respectively. Write balanced nuclear equations for each of these four
steps. (8 points)
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CH 126 B NAME:

FINAL EXAM

Spring 2000

  1. Match the term in column A to the one term or statement in column B that best describes it. Notice that there will be two definitions from column B that will not be used. (2 points each)

Column A Column B

Paramagnetism 1) The number of ligands attached to a metal. Diamagnetism 2) The nucleus of a helium atom. Chiral 3) Enantiomer. Coordination Number 4) An electron. Gangue 5) A proton or neutron. Alpha Particle 6) Weak repulsion by a magnetic field. Beta Particle 7) Impurities associated with ores. Nucleon 8) Species bonded to central metal atoms in a coordination complex. Fission 9) Weak attraction to a magnetic field. High Spin 10) Superimposable mirror images Low Spin 11) Nonsuperimposable mirror images. Fusion 12) The electron configuration for a coordination complex with the maximum number of unpaired electrons. Optical isomer 13) The electron configuration for a coordination complex with the minimum number of unpaired electrons. Ligand 14) Cis-Trans or Fac-Mer Isomer Geometric isomer 15) The highly exothermic process by which light nuclei combine to form heavier nuclei.

  1. The highly exothermic process by which heavy nuclei split to form lighter nuclei.
  2. “Bubbling” associated with metal dissolution.
  3. The first four steps of the radioactive decay series of 235 U are , , , and  emission respectively. Write balanced nuclear equations for each of these four steps. (8 points)
  1. Name the following coordination compounds. (3 points each) a) [Co(NH 3 ) 5 Cl]Cl 2 b) K 4 [PtCl 6 ] c) [Co(en) 2 (CN)Cl]Br
  2. Give formulas for the following. (3 points each) a) Pentaammineiodochromium (III) b) Potassium tetracyanonickelate (II) c) Trisethylenediaminenickel (II) bromide
  3. Jordi Roach, the future Miss America and 2015 Wimbledon Champion, requires 5.00 mg of 47 Ca, a radioactive nuclide with a half-life of 4.5 days, for a junior high science project. What mass of 47 Ca must she order if it takes exactly 48 hrs for delivery from the supplier? (8 points)
  1. Name the following transition metal complexes. (4 points each) a) b)

Co

NH

H

N

H

N

NH

Cl

Cl

Co

NH

H

N

H

N

Cl

Cl

Cl

  1. Depict the electron configurations for each of the following complexes, determine the number of unpaired electrons present in each, and describe each as paramagnetic or diamagnetic. (4 points each) a) Low-spin [Co(NH 3 ) 6 ]3+ b) High-spin [CoF 6 ]3-
  2. Which of the following complexes can have fac or mer isomers? You may circle more than one of the following. (6 points) a) Co(H 2 O) 3 Cl 3 b) [Pt(NH 3 ) 3 Br 3 ]- c) Fe(NH 3 ) 4 Cl 2 c) [Ni(Cl) 2 (Br) 2 ]2-

Comprehensive Part

  1. A solution contains 9.06 g of sucrose (C 12 H 22 O 11 ) in 400.0 g of water. Answer the following questions about this solution at 25.0 0 C. (3 points each) a) What is the molality of this solution? b) What is the vapor pressure of the solution? c) What is the freezing point of the solution? d) What is the boiling point of the solution?
  2. How will an equilibrium system described by the exothermic reaction below be affected by the following stresses? Respond with shift to the left, shift to the right, or no change. (3 points each) CO(g) + H 2 O(g) = H 2 (g) + CO 2 (g) a) Pressure is increased by decreasing the volume. b) Addition of CO(g). c) Temperature is increased.
  1. For the reaction : 2I-(aq) + S 2 O 8 2-(aq)  2SO 4 2-(aq) + I 2 (aq) The following data were obtained. Experiment [I-]initial (M) [S 2 O 8 2-]initial (M) Initial Rate 1 0.04 0.04 6.25x10- 2 0.08 0.04 1.25x10- 3 0.08 0.02 6.25x10- 4 0.32 0.04 5.00x10- a) What is the rate law for this reaction? (6 points) b) What is the value of the rate constant? (4 points)
  2. Calculate [H+], [Cl-], and pH for a 0.205 M HCl solution. (6 points) [H+]: [Cl-]: pH:
  1. Consider the following exothermic reaction, N 2 (g) + 3 H 2 (g) = 2 NH 3 (g). a) Is this reaction more product-favored at high or low temperatures? (3 points) b) Is this reaction enthalpy- or entropy- driven? (3 points)
  2. Consider the galvanic cell described by the line notation below. Zn  Zn2+(1.0 M)  Cu2+(1.0 M)Cu Determine the overall cell reaction, E^0 cell , and G^0. (6 points)
  3. Determine the concentrations of all the chemical species (HOCl, OH-, H+, OCl-) present in a 0.155 M HOCl solution. Ka = 3.0 x 10-8. ALSO, determine the pH of this solution. (10 points)
  1. Balance the following reaction using the half-reaction method. This reaction occurs in acidic solution. Identify the reduction half-reaction, the oxidation half-reaction, the oxidizing agent, and the reducing agent. (8 points) Cr 2 O 7 2-(aq) + SO 2 (g)  Cr3+(aq) + SO 4 2-(aq)
  2. Identify all species in the following reaction as either an acid or a base (conjugate acid or conjugate base) using Bronsted-Lowry theory. (4 points) HSO 4 - (aq) + NH 3 (aq)  SO 4 2-(aq) + NH 4 +(aq)
  3. Write the equilibrium constant expression, K, for the following reaction. (3 points) 2H 2 O(g) + 4KO 2 (s) = 4KOH(s) + 3O 2 (g)
  4. For the equilibrium reaction below K = 170. Determine the “direction” of reaction if the reaction mixture contains [NO 2 ] = 0.0800 mol/L and [N 2 O 4 ] = 0.550 mol/L. (4 points)

2NO 2 (g) = N 2 O 4 (g)