課程名稱︰普通化學甲
課程性質︰必修
課程教師︰林泱蔚
開課學院：
開課系所︰地質系、農化系、大氣系
考試日期（年月日）︰98/12/4
考試時限（分鐘）：160
是否需發放獎勵金：是
（如未明確表示，則不予發放）
試題 :
I.名詞解釋(20%)
1. Covalent bond and Coordinate covalent bond
2. Sigma bond and Pi bond
3. Dipole-dipole interaction and Dipole-induced dipole interaction
4. Adhesion and Cohesion
5. Crystalline solid and Amorphous solid
II.選擇題(40%)
2-
1. The Lewis dot symbol for the S ion is
.. ..2- 2- . 2- ..
A. : S : B. : S : C. S D. —S— E. :S—
.. .. . .
2. Which one of the following ionic solids would have the largest lattice
energy?
A. NaCl B. NaF C. CaBr2 D. CsI E. CaCl2
3. Which of the following solids would have the lowest melting point?
A. KI B. KBr C. KCl D. KF
4. Calculate the energy change for the reaction
+ -
K(g)+Br(g)→K (g)+Br (g)
given the following ionization energy(IE) and electron affinity(EA) values
────────────────────────
IE EA
────────────────────────
K 419 kJ/mol 48 kJ/mol
Br 1140 kJ/mol 324 kJ/mol
────────────────────────
A. -1,092 kJ/mol
B. -95 kJ/mol
C. 95 kJ/mol
D. 1,092 kJ/mol
E. 1,187 kJ/mol
5. Which of the elements listed below has the greatest electronegativity?
A. Mg B. Ga C. Si D. Ba E. Pb
6. Which one of these polar covalent bonds would have the greastest percent
ionic character?
A. H─Br B. H─Cl C. H─F D. H─I
7. The electron dot structure for AsCl3 shows
A. a total of 84 electron dots
B. three single bonds and 10 lone pairs
C. two single bonds,one double bond,and 9 lone pairs
D. one single bond,two double bonds,and 8 lone pairs
E. three single bonds and one lone pair
8. The total number of bonding electrons in a molecule of formaldehyde(H2CO)
is
A. 3 B. 4 C. 6 D. 8 E. 18
9. The number of resonance structures for the sulfur dioxide molecule that
satisfy the octet rule is
A. 1 B. 2 C. 3 D. 4 E. None of these
-
10. The azide ion,N3,is very reactive although it is isoelectronic with the
very stable CO2 molecule. This reactivity is reasonable inasmuch as
A. a Lewis structure cannot be written for the azide ion that has nitrogen
formal charges of zero.
B. there is no valid Lewis structure possible for the azide ion.
C. there are resonance structures for azide ion but not for carbon dioxide
D. nitrogen cannot form multiple bonds.
E. charged species always decompose in solution.
3-
11. How many covalent bonds will be drawn to phosphorous in PO4 for the dot
structure that expands the octet to minimize formal charge and if
necessary places negative formal charges on the most electronegative
atom(s)
A. 4 B. 5 C. 6 D. 7 E. 8
12. What is the formal charge on sulfur in the best Lewis structure for the
-
SCN (thiocyanate) ion?
A. +2 B. -2 C. +1 D. -1 E. 0
13. Which of the following substances will display an incomplete ocet in its
Lewis structure?
A. CO2 B. Cl2 C. ICl D. NO E. SO2
14. Give the number of lone pairs around the central atom and the molecular
geometry of CBr4.
A. 0 lone pairs,square planar
B. 0 lone pairs,tetrahedral
C. 1 lone pair,square pyramidal
D. 1 lone pair,trigonal bipyramidal
E. 2 lone pairs,square planar
15. Give the number of lone pairs around the central atom and the molecular
geometry of SeF4.
A. 0 lone pairs,tetrahedral
B. 1 lone pair,distorted tetrahedron (seesaw)
C. 1 lone pair,square pyramidal
D. 1 lone pair,tetrahedral
E. 2 lone pairs,square planar
-
16. The bond angle in ICl2 is expected to be
A. a little less than 109.5度
B. 109.5度
C. a little more than 109.5度
D. 120度
E. 180度
17. Complete this sentence: The PCl5 molecule has
A. nonpolar bonds,and is a nonpolar molrcule
B. nonpolar bonds,but is a polar molecule
C. polar binds,and is a polar molecule
D. polar bonds,but is a nonpolar molrcule
18. N,N-diethy1-m-tolumide (DEET) is the active ingredient in many mosquito
repellents. What is the hybridization state of carbon indicated by the
arrow in the structure of DEET shown below?
H O CH3
︳ ↘∥ ︳
H3C C C CH2
╲ ／ ＼＼ ／ ＼ ／
C C N
∥ ︳ ︳
C C H3C
／＼ ／／＼ ＼
H C H CH3
︳
H
2 3 3 3 2
A. sp B. sp C. sp D. sp d E. sp d
19. What is the hybridization state of carbon indicated by the arrow in the
structure of DEET shown below?
H O CH3
︳ ∥ ↘ ︳
H3C C C CH2
╲ ／ ＼＼ ／ ＼ ／
C C N
∥ ︳ ︳
C C H3C
／＼ ／／＼ ＼
H C H CH3
︳
H
2 3 3 3 2
A. sp B. sp C. sp D. sp d E. sp d
20. What is the hybridization state of the nitrogen atom in the structure
of DEET shown above?
2 3 3 3 2
A. sp B. sp C. sp D. sp d E. sp d
21. Indicate the type of hibrid orbitals use by the central atom in SF6.
2 3 3 3 2
A. sp B. sp C. sp D. sp d E. sp d
22. What is the hybridization of the iodine atom in the IF5 molecule?
2 3 3 3 2
A. sp B. sp C. sp D. sp d E. sp d
23. Which of the following species have the same geometries?
-
A. NH2 and H2O
-
B. NH2 and BeH2
C. H2O and BeH2
-
D. NH2,H2O,and BeH2
24. The number of pi bonds in the molecule below is
H─C﹦C—C≡N
︳ ︳
H H
A. 1 B. 2 C. 3 D. 5 E. 9
+ -
25. Consider the species Cl2,Cl2,and Cl2. Which of these species will be
paramagnetic?
A. only Cl2
+
B. Cl2 and Cl2
-
C. Cl2 and Cl2
+ -
D. Cl2 and Cl2
E. all tree are paramagnetic
26. Consider the species Cl2,Cl2,and Cl2. Which of these species will be
paramagnetic?
-
A. N2 and N2
+
B. N2 and N2
+ -
C. N2 and N2
-
D. only N2
E. none are paramagnetic
27. Which of the following is not true of molecular orbitals?
A. The number of molecular orbitals formed is always equal to the number
of atomic orbitals combined.
B. A molecular orbital can accommodate up to two electrons.
C. When electrons are added to orbitals of the same energy, the most
stable arrangement is predicted by Hund's rule
D. Low-energy molecular orbitals fill before high-energy molecular
orbitals fill
E. For any substance,the number of electrons in moleculae orbitals is
equal to the sum of all te valence electrons on the bonding atoms.
28. The electrons in the delocalized molecular orbitals of benzene (C6H6)
A. are confined between two adjacent bonding atoms.
B. are free to move around the six-membered ring.
C. form the electron pairs in the C—H bonds of the compound.
D. are unevenly distributed through the molecule.
E. are responsible for the fact that the bonds between three pairs of
carbon atoms in the ring are longer and stronger than the bonds
between the other three pairs of carbon atoms.
29. Which of the following correctly list species in oder of increasing
bond length?
- +
A. C2<C2<C2
+ -
B. C2<C2<C2
- +
C. C2<C2<C2
+ -
D. C2<C2<C2
+ -
E. C2<C2<C2
30. Which of the following correctly list species in oder of increasing
bond order?
A. C2<Li2<Be2<N2
B. Be2<Li2<C2<N2
C. N2<Be2<Li2<C2
D. N2<C2<Li2<Be2
E. Be2<C2<N2<Li2
31. Which one of the folloeing substance will have both dipersion force and
dipole-dipole forces?
A. HCl B. BCl3 C. Br2 D. H2 E. CO2
32. Which of the following liquid would have the highest viscosity at 25度C?
A. CH3OCH3 B. CH2Cl2 C. C2H5OH D. CH3Br E. HOCH2CH2OH
33. Each of the following substaneces is a liquid at -50度C. Place these
liquids in order of increasing vapor pressure:dimethyl ether (CH3OCH3),
propane (C3H8),and ethanol (CH3CH2OH)
A. ethanol<propane<dimethyl ether
B. ethanol<dimethyl ether<propane
C. propane<dimethyl ether<ethanol
D. dimethyl ether<ethanol<propane
E. propane<ethanol<dimethyl ether
34. Arrange the following in order of increasing boiling point: RbCl,CH3Cl,
CH3OH,CH4
A. CH3OH<CH3Cl<RbCl<CH4
B. CH3OH<CH4<CH3Cl<RbCl
C. RbCl<CH3Cl<CH3OH<CH4
D. CH4<CH3OH<CH3Cl<RbCl
E. CH4<CH3Cl<CH3OH<RbCl
35. Which one of the following substances should exhibit hyfrogen bonding in
the liquid state?
A. PH3 B. He C. H2S D. CH4 E. CH3OH
36. Which of the following is not true with regard to water?
A. Water has a high heat capacity.
B. Water has an usually high boiling point.
C. Water can form hydrogen bonds.
D. Ice is more densc than liquid water.
E. Water is a polar molecu;e.
37. Use the graph of vapor pressure to determine the normal boiling point
of CHCl3.
蒸 900 ┌─┬─┬─┬─┬─┬─┬●┬─┬─┬─┬─┬─┐
氣 │ │ │ │ │ │ │ │ │ │ │ │ │
壓 800 ├─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┤
(mmHg) │ │ │ │ │ │ │ │ │ │ │ │ │
700 ├─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┤
│ │ │ │ │ │ │ │ │ │ │ │ │
600 ├─┼─┼─┼─┼─┼─●─┼─┼─┼─┼─┼─┤
│ │ │ │ │ │ │ │ │ │ │ │ │
500 ├─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┤
│ │ │ │ │ │ │ │ │ │ │ │ │
400 ├─┼─┼─┼─┼─┼●┼─┼─┼─┼─┼─┼─┤
│ │ │ │ │ │ │ │ │ │ │ │ │
300 ├─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┤
│ │ │ │ ● │ │ │ │ │ │ │ │
200 ├─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┼─┤
│ │ │ │ │ │ │ │ │ │ │ │ │
100 ├─┼─●─┼─┼─┼─┼─┼─┼─┼─┼─┼─┤
● │ │ │ │ │ │ │ │ │ │ │ │
0 └─┴─┴─┴─┴─┴─┴─┴─┴─┴─┴─┴─┘
0 10 20 30 40 50 60 70 80 90 100 110 120
T(度C)
(圖是一個拋物線，請自己在點之間做連線)
A. 19度C B. 52度C C. 60度C D. 64度C E. 70度C
38. The vapor pressure of a liquid in a closed container depends upon
A. the amount of liquid.
B. the volume of the container.
C. the surface area of the liquid
D. the temperature
E. None of the above
39. Which of the following is not an endothermic process?
A. melting of a aolid
B. vaporization
C. raising the temperature of a gas
D. condensation of water vapor
E. sublimation of dry ice
40. The number of atoms in a face-centered cubic unit cell is
A. 1 B. 2 C. 3 D. 4 E. 8
III.計算題(45%)
1. Use the Born-Haber cycle to caculate the lattice energy of MgO(s) given
the following data: 5%
△H(sublimation) Mg=130 kJ/mol;I1(Mg)=738.1 kJ/mol;I2(Mg)=1450 kJ/mol;
Bond energy(O=O)=498.7 kJ/mol;EA(O)=141 kJ/mol; EA(O-)=-780 kJ/mol;
。
△H f(MgO(s))=-601.8 kJ/mol
2. Use bond energues to wstimate the enthyalpy change for the reaction of
one mole of CH4 with chlorine gas to give CH3Cl and hydrogen chloride. 5%
BE(C—H)=414 kJ/mol;BE(C—Cl)=326 kJ/mol; BE(H—Cl)=432 kJ/mol;BE(Cl—Cl)=
243 kJ/mol
3. Write the Lewis structure of boron trifluorid,ammonia and the product that
forms when boron trifluoride combines with ammonia. 6%
4. Palladium crystallizes in a face-centered cubic unit cell. Its density is
12.0g/cm^3 at 27度C.Caculate the atomic radius of Pd.(Atomic weight of Pd:
106.4 g/mole) 5%
5. The atomic planes in a graphite crystal are separated by 335 pm. At what
angle would you find the first-order (n=1) diffraction of 0.154 nm X-rays
from a graphite crystal? 3%
6. The molar enthalpy of vaporization of boron tribromide is 30.5 kJ/mol,and
its normal boiling point is 91度C. What is the vapor pressure(torr) of
BBr3 at 20度C? 5%
7. Give possible Lewis structures for XeO3,an explosive compound of xenon.
Determine the formal charges of each atom in the various Lewis structure.8%
8. Write the ground-state electron configurations and magnetic properties foe
(a) oxygen atom and (b) oxygen molecule. 8%
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