Download (1) Dissolves, accompanied by evolution of flammable gas (2

1995
.
PartD
(45 percent)
.
Spend about 40 minutes on this part of the examination. Answering these questions provides an opportunity to
demonstrate
uciuuiiMicuc your
yum ability
auiuiy to
iu present
picsciu your
yum material
maiei jal in logical, coherent, and convincing English. Your responses wiu
will be
judged
judged on the basis of accuracy and importance
importance of the detail cited and on the aoorooriateness
appropriateness of the descriptive
descHntivp
material used. Specific answers are preferable to broad diffuse responses. Illustrative examples and equations may be
helpful.
ANSWER THE FOLLOWING ESSAY QUESTION.
|_
The conductivity of several substances was tested using the apparatus represented by the diagram below. The
results of the tests are summarized in the following data table.
AgNO, Sucrose
Melting
Point
212e
Liquid
(fused)
•f +
185"
Water
Solution
Solid
Na
H2S04
(98%)
99°
Liquid at
Room Temp
Light
Bulb
+(2)
Not
Tested
<— Sample to
—-1 be tested
Key: + + Good conductor
+ Poor conductor
- Nonconductor
(1) Dissolves, accompanied by evolution
of flammable gas
(2) Conduction increases as the acid is added
slowly and carefully to water
Using models of chemical bonding and atomic or molecular structure, account for the differences in conductivity
between the two samples in each of the following pairs.
(a) Sucrose solution and silver nitrate solution
(b) Solid silver nitrate and solid sodium metal
(c) Liquid (fused) sucrose and liquid (fused) silver nitrate
(d) Liquid (concentrated) sulfuric acid and sulfuric acid solution
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1994
For each of the following, use appropriate chemical principles to explain the observation.
(a) Sodium chloride may be spread on an icy sidewalk, in order to melt the ice; equimolar amounts of calcium
chloride are even more effective.
(b) At room temperature, NH3 is a gas and H2O is a liquid, even though NH3 has a molar mass of 17 grams and
H2O has a molar mass of 18 grams.
(c) C (graphite) is used as a lubricant, whereas C (diamond) is used as an abrasive.
(d) Pouring vinegar onto the white residue inside a kettle used for boiling water results in a fizzing/bubbling
phenomenon.
Use principles of atomic structure and/or chemical bonding to answer each of the following.
(a) The radius of the Ca atom is 0.197 nanometer; the radius of the Ca2+ ion is 0.099 nanometer. Account for
this difference.
(b) The lattice energy of CaO(s) is -3,460 kilojoules per mole; the lattice energy for K2O(s) is -2,240 kilojoules
per mole. Account for this difference.
lonization Energy
(kJ/mol)
First
Second
K
419
3,050
Ca
590
1,140
(c) Explain the difference between Ca and K in regard to
(i) their first ionization energies,
(ii) their second ionization energies.
(d) The first ionization energy of Mg is 738 kilojoules per mole and that of Al is 578 kilojoules per mole.
Account for this difference.
Explain each of the following observations in terms of the electronic structure and/or bonding of the compounds
involved.
(a) At ordinary conditions, HF (normal boiling point = 20°C) is a liquid, whereas HC1 (normal boiling
point = -114°C) is a gas.
(b) Molecules of AsF3 are polar, whereas molecules of AsF5 are nonpolar.
(c) The N-O bonds in the NO2~ ion are equal in length, whereas they are unequal in HNO2.
(d) For sulfur, the fluorides SF2, SF4, and SF6 are known to exist, whereas for oxygen only OF2 is known to
exist.
5. Consider the molecules PF3 and PF5.
(a) Draw the Lewis electron-dot structures for PF3 and PF5 and predict the molecular geometry of each.
(b) Is the PF3 molecule polar, or is it nonpolar? Explain.
(c) On the basis of bonding principles, predict whether each of the following compounds exists. In each case,
explain your prediction.
(i)
(ii)
NF5
AsF5
6. Explain each of the following observations using principles of atomic structure and/or bonding.
(a) Potassium has a lower first-ionization energy than lithium.
(b) The ionic radius of N3" is larger than that of O2~.
(c) A calcium atom is larger than a zinc atom.
(d) Boron has a lower first-ionization energy than beryllium.
-7
'•
Account for each of the following in terms of principles of atomic structure, including the number, properties, and
arrangements of subatomic particles.
(a) The second ionization energy of sodium is about three times greater than the second ionization energy of
magnesium.
(b) The difference between the atomic radii of Na and K is relatively large compared to the difference between the
atomic radii of Rb and Cs.
(c) A sample of solid nickel chloride is attracted into a magnetic field, whereas a sample of solid zinc chloride is
not.
(d) Phosphorus forms the fluorides PF3 and PF5, whereas nitrogen forms only NF3.
I2 in Water
TTE
(£) A water solution of I2 is shaken with an
equal volume of a nonpolar solvent such
as TTE (trichlorotrifluoroethane). Describe
the appearance of this system after shaking.
(A diagram may be helpful.) Account for this
observation.
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8y Explain each of the following in terms of atomic and molecular structures and/or intermolecular forces.
(a)
(b)
(c)
(d)
Solid K conducts an electric current, whereas solid KNO3 does not.
SbCl3 has a measurable dipole moment, whereas SbCl5 does not:
The normal boiling point of CC14 is 77°C, whereas that of CBr4 is 190°C.
Nal(j) is very soluble in water, whereas I 2 (j) has a solubility of only 0.03 gram per 100 grams of water.
9.
NO,
N02
NO,+
Nitrogen is the central atom in each of the species given above.
(a)
(b)
(c)
(d)
Draw the Lewis electron-dot structure for each of the three species.
List the species in order of increasing bond angle. Justify your answer.
Select one of the species and give the hybridization of the nitrogen atom in it.
Identify the only one of the species that dimerizes and explain what causes it to do so.
END OF EXAMINATION
| O. Experimental data provide the basis for interpreting differences in properties of substances.
TABLE 1
Melting
Point
Compound
CO
BeCl2
MgCl2
405
714
SiCl4
-70
MgF 2
1,261
TABLE 2
Electrical Conductivity
of Molten State
(ohm'1)
0.086
>20
0
>20
Substance
Bond Length
(angstroms)
1.42
F2
Br2
2.28
N2
1.09
Account for the differences in properties given in Tables 1 and 2 above in terms of the differences in structure and
bonding in each of the following pairs.
(a) MgCl 2 and SiCl4
(b) MgCl 2 andMgF 2
(c) F2 and Br2
(d) F 2 a n d N 2
1995
SELECT TWO OF THE FOUR ESSAY QUESTIONS, NUMBERED 6 THROUGH 9.
(Additional essays will not be scored.)
1.0
Temperature (°C)
The phase diagram for a pure substance is shown above. Use this diagram and your knowledge about changes of
phase to answer the following questions.
(a) What does point V represent? What characteristics are specific to the system only at point V ?
(b) What does each point on the curve between V and W represent?
(c) Describe the changes that the system undergoes as the temperature slowly increases from X to Y to Z at
1.0 atmosphere.
(d) In a solid-liquid mixture of this substance, will the solid float or sink? Explain.
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