Name:______________________ Student number:__________________________
問答題
1) Name each of the following compounds. (12 pts)
(a) KClO4
potassium perchlorate
(b) Ca3(PO4)2
calcium phosphate
(c) K2Cr2O7
potassium dichromate
(d) NH4NO2
ammonium nitrite
(e) SF6
sulfur hexafluoride
(f) BaCrO4
barium chromate
2) Write the formula for each of the following. (12 pts)
3)
(a) sodium dihydrogen phosphate
NaH2PO4
(b) lithium nitride
Li3N
(c) sodium peroxide
Na2O2
(d) diphosphorus pentoxide
P2O5
(e) perbromic acid
HBrO4
(f) mercury (I) sulfide
Hg2S
The reaction of ethane gas (C2H6) with chlorine gas produces C2H5Cl as its
main product (along with HCl). In addition, the reaction invariably produces a
variety of other minor products, including C2H4Cl2, C2H3Cl3, and others.
Naturally, the production of these minor products reduces the yield of the
main product. Calculate the percent yield of C2H5Cl if the reaction of 300. g of
ethane with 650. g of chlorine produced 490. g of C2H5Cl.
(4 pts)
MW(C2H6) = 30.07 g/mol
MW(Cl2) = 70.90 g/mol
MW(C2H5Cl) = 64.51 g/mol
300./30.07 = 9.98 mol C2H6
650/70.90 = 9.17 mol Cl2 (limiting reagent)
C2H6 + Cl2  C2H5Cl + Cl2
So 9.17 x 64.51 = 592 g C2H5Cl (theoretical yield)
490./ 592 = 82.8 % yield
1
4)
Using half-reaction method, balance the following oxidation reduction
reactions that occurs in acidic solution. (4x2 pts)
(a) I-(aq) + ClO-(aq)  I3-(aq) + Cl-(aq)
3I-  I3- + 2e+) 2e- + 2H+ + ClO-  Cl- + H2O
3I-(aq) + 2H+(aq) + ClO-(aq)  I3-(aq) + Cl-(aq) + H2O(l)
(b) CH3OH(aq) + Cr2O72-(aq)  CH2O(aq) + Cr3+(aq)
3 x (CH3OH  CH2O + 2H+ + 2e-)
+)
6e- + 14H+ + Cr2O72-  2Cr3+ + 7H2O
3CH3OH(aq) + 8H+(aq) + Cr2O72-(aq)  2Cr3+(aq) + 3CH2O(aq) + 7H2O(l)
5)
Using half-reaction method, balance the following oxidation reduction
reactions that occurs in basic solution. (4x2pts)
(a) NO2-(aq) + Al(s)  NH3(g) + AlO2-(aq)
6e- + 7H+ + NO2-  NH3 + 2H2O
+)
2 x (2H2O + Al  AlO2- + 4H+ + 3e-)
2H2O + 2Al+ NO2- + OH- NH3 + 2AlO2- + H+ + OH-
H2O(l) + 2Al(s) + NO2-(aq) + OH-(aq)  NH3(aq) + 2AlO2-(aq)
(b) Cr(s) + CrO42-(aq)  Cr(OH)3(s)
2H2O + Cr  Cr(OH)3 + 3H+ + 3e3e- + 5H+ + CrO42-  Cr(OH)3 + H2O
4H2O(l) + Cr(s) + CrO42-(aq)  2Cr(OH)3(s) + 2OH-(aq)
2
6)
Write the expected electron configurations for each of the following atoms.
(8pts)
a)
Sc
1s22s22p63s23p63d14s2
b)
Cr
1s22s22p63s23p63d54s1
c)
Al
1s22s22p63s23p1
d)
O
1s22s22p4
解釋名詞（不可只翻譯）
b)
(2x4 pts)
Pauli exclusion principle
In a given atom no two electrons can have the same set of four quantum
numbers (n, l, ml, ms).
c) Electron affinity
The energy change associated with the addition of an electron to a gaseous
atom.
d) law of multiple proportion
When two elements form a series of compounds, the ratios of the masses of
the second element that combine with 1 gram of the first element can always
be reduced to small whole numners.
e) degeneracy (concerning orbitals)
A group of orbitals have the same energy.
單選題（共30題，每題2分）
1) Which of the following is an example of a quantitative observation?
a)
b)
c)
d)
e)
The piece of metal is longer than the piece of wood
Solution 1 is much darker than solution 2.
The liquid in beaker A is blue.
The temperature of the liquid is 60°C.
At least two of these (a-d) are quantitative observations.
3
2) A titration was performed to find the concentration of hydrochloric acid with the
following results:
Trial
Molarity
1
1.25 ± 0.01
2
1.24 ± 0.01
3
1.26 ± 0.01
The actual concentration of HCl was determined to be 1.000 M; the results of
the titration are:
a) both accurate and precise.
b)
c)
d)
e)
accurate but imprecise.
precise but inaccurate.
both inaccurate and imprecise.
accuracy and precision are impossible to determine with the available
information.
3) A scientist obtains the number 0.045006700 on a calculator. If this number actually
has four (4) significant figures, how should it be written?
a)
0.4567
b)
0.4501
c)
0.045
d)
0.04500
e)
0.04501
d)
1  109
e)
1  1015
4) One second contains this many picoseconds.
a)
1  1012
b)
1  10–12 c)
1  10–9
5) In a recent accident some drums of uranium hexafluoride were lost in the English
Channel. The melting point of uranium hexafluoride is 64.5°C. What is the
melting point of uranium hexafluoride on the Fahrenheit scale? (TF = TC 
(9°F/5°C) + 32°F)
a)
1.35°F
b)
82.3°F
c)
116°F
d)
122°F
e)
148°F
6) What are substances with constant composition that can be broken down into
elements by chemical processes.
a)
d)
Solutions b)
Quarks
e)
Mixtures c) Compounds
Heterogeneous mixtures
7) Which of the following statements from Dalton’s atomic theory is no longer true,
according to modern atomic theory?
a)
b)
c)
Elements are made up of tiny particles called atoms.
Atoms are not created or destroyed in chemical reactions.
All atoms of a given element are identical.
4
d)
e)
Atoms are indivisible in chemical reactions.
All of these statements are true according to modern atomic theory.
8) Rutherford’s experiment was important because it showed that:
a)
b)
c)
d)
e)
9)
40
20
radioactive elements give off alpha particles.
gold foil can be made to be only a few atoms thick.
a zinc sulfide screen scintillates when struck by a charged particle.
the mass of the atom is uniformly distributed throughout the atom.
an atom is mostly empty space.
Ca2+ has
a)
b)
c)
d)
e)
20 protons, 20 neutrons, and 18 electrons.
22 protons, 20 neutrons, and 20 electrons.
20 protons, 22 neutrons, and 18 electrons.
22 protons, 18 neutrons, and 18 electrons.
20 protons, 20 neutrons, and 22 electrons.
10) Which metals form cations with varying positive charges?
a)
c)
transition metals
Group 2 metals
b)
d)
Group 1 metals
Group 3 metals
e)
metalloids
11) Gallium consists of two isotopes of masses 68.95 amu and 70.95 amu with
abundances of 60.16% and 39.84%, respectively. What is the average atomic
mass of gallium?
a)
69.95
b)
70.15
c)
71.95
d)
69.75
e)
69.55
12) Iron is biologically important in the transport of oxygen by red blood cells from
the lungs to the various organs of the body. In the blood of an adult human,
there are approximately 2.60  1013 red blood cells with a total of 2.90 g of
iron. On the average, how many iron atoms are present in each red blood
cell? (molar mass (Fe) = 55.85 g)
a)
d)
8.33  10–10
2.60  1013
b)
e)
1.20  109
5.19  10–2
c)
3.12  1022
13) Roundup, an herbicide manufactured by Monsanto, has the formula C3H8NO5P.
How many moles of molecules are there in a 500.-g sample of Roundup?
a)
0.338
b)
1.75 c) 2.96
d) 84.5
e)
none of these
5
14) What is the coefficient for water when the following equation is balanced?
As(OH)3(s) + H2SO4(aq)  As2(SO4)3(aq) + H2O(1)
a)
1
b)
2
c)
4
d)
6
e)
12
15) A compound is composed of element X and hydrogen. Analysis shows the
compound to be 80% X by mass, with three times as many hydrogen atoms as
X atoms per molecule. Which element is element X?
a)
He
b)
C
c)
F
d)
S
e)
none of these
16) You heat 3.970 g of a mixture of Fe3O4 and FeO to form 4.195 g Fe2O3. The mass
percent of FeO originally in the mixture was:
a)
12.1%
b)
28.7%
c)
71.3%
d)
87.9%
e)
none of these
17) The empirical formula of a group of compounds is CHCl. Lindane, a powerful
insecticide, is a member of this group. The molar mass of lindane is 290.8.
How many atoms of carbon does a molecule of lindane contain?
a)
2
b)
3
c)
4
d)
6
e)
8
18) Iron is produced from its ore by the reactions:
2C(s) + O2(g)  2CO(g)
Fe2O3(s) + 3CO(g)  2Fe(s) + 3CO2(g)
How many moles of O2(g) are needed to produce 1 mole of Fe(s)?
a)
d)
0.5 mole O2
1.5 mole O2
b)
e)
0.75 mole O2 c)
none of these
1 mole O2
19) What mass of solute is contained in 256 mL of a 0.895 M ammonium chloride
solution?
a)
d)
12.3 g
53.5 g
b)
e)
13.7 g
c) 47.9 g
none of these
20) Which of the following is a strong acid?
a)
d)
HF
b) KOH
c)
HclO
e) HBrO
HClO4
6
21) The interaction between solute particles and water molecules, which tends to
cause a salt to fall apart in water, is called
a)
d)
hydration.
coagulation.
b)
e)
polarization. c)
conductivity.
dispersion.
22) The following reactions
2K(s) + Br2(l)  2KBr(s)
AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)
HCl(aq) + KOH(aq)  H2O(l) + KCl(aq)
are examples of
a)
b)
c)
d)
e)
precipitation reactions.
redox, precipitation, and acid-base, respectively.
precipitation (two) and acid-base reactions, respectively.
redox reactions.
none of these
23) Sulfamic acid, HSO3NH2 (molar mass = 97.1 g/mol), is a strong monoprotic acid
that can be used to standardize a strong base:
HSO3NH2(aq) + KOH(aq)  KSO3NH2(aq) + H2O(l)
A 0.179-g sample of HSO3NH2 required 19.4 mL of an aqueous solution of
KOH for complete reaction. What is the molarity of the KOH solution?
a)
d)
9.25 M
0.194 M
b)
e)
9.50  10–5 M c)
none of these
0.0950 M
24) The following reaction occurs in aqueous acid solution:
NO3– + I–  IO3–+ NO2
The oxidation state of iodine in IO3– is:
a)
0
b)
+3
c)
–3
d)
+5
e)
–5
25) When the following reaction is balanced in acidic solution, what is the coefficient
of I2?
IO3– + I–  I2
a)
1 b) 2
c)
3
d)
4
e)
none of these
7
26) The wavelength of light associated with the n = 2 to n = 1 electron transition in
the hydrogen spectrum is 1.216  10–7 m. By what coefficient should this
wavelength be multiplied to obtain the wavelength associated with the same
electron transition in the Li2+ ion?
a)
1/9
b)
1/7
c) 1/4
d) 1/3
e) 1
27) Which of the following is not determined by the principal quantum number, n, of
the electron in a hydrogen atom?
a)
b)
c)
d)
e)
the energy of the electron
the minimum wavelength of the light needed to remove the electron
from the atom.
the size of the corresponding atomic orbital(s)
the shape of the corresponding atomic orbital(s)
All of these are determined by n.
28) How many electrons in an atom can have the quantum numbers n = 3, l = 2?
a)
2
b)
5 c)
10
d)
18
e)
6
29) Which of the following atoms or ions has 3 unpaired electrons?
a)
N
b)
O
c)
Al
d)
S2– e)
Zn2+
30) The statement that "the lowest energy configuration for an atom is the one
having the maximum number of unpaired electrons allowed by the Pauli
principle in a particular set of degenerate orbitals" is known as
a)
b)
c)
d)
e)
the aufbau principle.
Hund’s rule.
Heisenberg uncertainty principle.
the Pauli exclusion principle.
the quantum model.
8