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| Chem 110, Dr. Paselk |
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Name |
| Fall 2002 |
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Lab |
This examination is scheduled for fifty (50) minutes. At the end of this fifty minute period you will have five (5) minutes to bring your examination to the front of the examination room.
1. (10 @ 2 ea) True/False. Indicate whether the following statements are True (T) or False (F).
Diamagnetism is due to paired electrons in an atom or molecule. _______________
An atom with dsp3 hybridization will have a trigonal bipyramidal electronic geometry. _______________
Hybrid orbital theory is based on a localized electron model. _______________
The Group VA elements are an excellent example of the trend of increasing metallicity with increasing atomic size in a group. _______________
The inert pair effect may explain the behavior of Group VIIIA elements. _______________
2. (21 @ 3 ea) Answer the following in the spaces provided.
How many allotropes exist for carbon under normal conditions? _______________
Give the formula of the strongest of the chlorine oxyacids _______________
Would you expect the oxide of Sn or Sb to be the stronger base? _______________
What is the formula for white phosphorus? _______________
Would you expect a Te oxide to be acidic, basic, or amphoteric? _______________
List two properties typical of metals generally. _______________
Give an oxidation state for Sb explained by the inert pair effect. _______________
3. (8) Sketch a molecular orbital diagram for lithium fluoride showing how the MO's arise from the orbitals of the bonded atoms, including all bonding electrons from each atom before and after bond formation.
4. (10) a. Draw a Molecular Orbital Energy-level diagram for molecular oxygen, including all valence electrons from each atom.
b. What is the bond order for oxygen? Indicate your reasoning or show a calculation based on your diagram for credit.
c. Based on your diagram, is this molecule diamagnetic or paramagnetic? Explain (short sentence or phrase).
5. (12) Fill in the table below to describe the hybridization and bonding seen for the central atom in each structure.
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6. (12) In one of our demonstrations the instructor heated a yellow powder in a test tube over a Bunsen burner. As the contents were heated a yellowish, watery liquid appeared at the bottom of the tube as the powder melted. With continued heating the liquid gradually turned orange and them reddish as the liquid became very viscous. When poured into cold water the viscous liquid turned to a light yellow elastic solid.
a. Explain the change at the molecular level which gives rise to the viscosity change.
b. What will happen to the elastic material obtained at the end? Why?
c. During the demonstration an acrid odor was noted as the experiment proceeded. What is the odiferous gas likely to be? Write an equation for its formation.
7. (7) Why do the elements of the second period tend to differ so markedly from the other elements of their groups?
8. (20) Write the NET ionic equation for the reaction which occurs when the following are mixed. (If there is no reaction, indicate by "NR." )
a. Tin(IV) sulfide is treated with a large excess of sodium hydroxide.
b. Bismuth(III) chloride is mixed with hydrogen sulfide in a moderately acidic solution.
c. Aluminum metal is added to a solution of tin(IV) in 6M hydrochloric acid (SnCl62-).
d. Sulfuric acid is added to a solution of barium chloride.
e. Sulfur trioxide is added to water.
| Syllabus/Schedule |
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© R A Paselk
Last modified 30 October 2006
