Download Chemistry 106: General Chemistry

Chemistry 106: General Chemistry
Syracuse University Project Advance
Final Exam, Fall 2012
Name
Date
__________________
The last page of each examination should be a periodic table.
Rydberg Constant (RH) = 2.18 x 10-18 J
(1) A sample that cannot be separated into two or more substances by physical means is:
(a) A compound
(b) An element
(c) Either a compound or an element
(d) A homogeneous mixture
(e) A heterogenous mixture
(2) Which of the following is not an intensive property:
(a)
(b)
(c)
(d)
(e)
density
temperature
melting point
mass
boiling point
(3) In which of the following are none of the zeros significant?
(a)
(b)
(c)
(d)
(e)
100.0
1065
0.0100
1.003450
0.00001
CHE 106, Fall 2012, Final Exam
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(4) Which combination of protons, neutrons and electrons is correct for the isotope of copper,
63
?
29 Cu
(a)
(b)
(c)
(d)
(e)
29 p+; 34 n°, 29 e29 p+; 29 n°, 63 e63 p+; 29 n°, 63 e34 p+; 29 n°, 34 e34 p+; 34 n°, 29 e-
(5) The element X has three naturally occurring isotopes. The masses (amu) and % abundances
of the isotopes are given in the table shown below. The average atomic masses of the
element is
amu.
Isotope
221
X
220
X
218
X
(a)
(b)
(c)
(d)
(e)
Abundance
74.22
12.78
13.00
Mass
220.9
220.0
218.1
219.7
220.4
220.42
218.5
221.0
(6) Which pair of elements would you expect to exhibit the greatest similarity in their physical
and chemical properties?
(a)
(b)
(c)
(d)
(e)
As, Br
Mg, Al
I, At
Br, Kr
N, O
(7) When the following equation is balanced, the coefficients are
C8H18 + O2 ------> CO2 + H2O
(a)
(b)
(c)
(d)
(e)
2, 3, 4, 4
1, 4, 8, 9
2, 12, 8, 9
4, 4, 32, 36
2, 25, 16, 18
CHE 106, Fall 2012, Final Exam
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.
(8) Calculate the percentage by mass of lead in PbCO3.
(a)
(b)
(c)
(d)
(e)
17.96
22.46
73.05
77.54
89.22
(9) A compound that is composed of carbon, hydrogen and oxygen was determined by
combustion analysis to contain 70.6% carbon, 5.9% hydrogen and 23.5% oxygen, by mass.
The molecular weight of the compound was determined by mass spectroscopy to be 136
amu. What is the compound’s molecular formula?
(a)
(b)
(c)
(d)
(e)
C8H8O2
C8H4O
C4H4O
C9H12O
C5H6O2
(10) How many moles of sodium carbonate contain 1.773 x 1017 carbon atoms?
(a)
(b)
(c)
(d)
(e)
5.890 x 10-7
2.945 x 10-7
1.473 x 10-7
8.836 x 10-7
9.817 x 10-8
CHE 106, Fall 2012, Final Exam
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(11) The net ionic equation for the reaction between nitric acid (HNO3) and aqueous sodium
hydroxide (NaOH) is:
(a)
(b)
(c)
(d)
(e)
H+(aq) + HNO3(aq) + 2OH-(aq) ------> 2 H2O(l) + NO3-(aq)
HNO3(aq) + NaOH(aq) ------> NaNO3(aq) + H2O(l)
H+(aq) + OH-(aq) ------> H2O(l)
HNO3(aq) + OH-(aq) ------> NO3-(aq) + H2O(l)
H+(aq) + Na+(aq) + OH-(aq) ------> H2O(l) + Na+(aq)
(12) Sodium does not occur in Nature as Na(s) because
(a)
(b)
(c)
(d)
(e)
.
It is easily reduced to Na-.
It is easily oxidized to Na+.
It reacts with water with great difficulty.
It is easily reduced to Na+.
It undergoes a disproportionation reaction to Na- and Na+.
(13) Which of the following is an oxidation-reduction reaction?
(a)
(b)
(c)
(d)
(e)
Cu(s) + 2AgNO3(aq) ------> 2Ag(s) + Cu(NO3)2(aq)
HCl(aq) + NaOH(aq) ------> H2O(l) + NaCl(aq)
AgNO3(aq) + HCl(aq) ------> AgCl(s) + HNO3(aq)
Ba(C2H3O2)2(aq) + Na2SO4(aq) ------> BaSO4(s) + 2 NaC2H3O2(aq)
H2CO3(aq) + Ca(NO3)2(aq) ------> 2HNO3(aq) + CaCO3(s)
(14) What are the respective concentrations (M) of Mg2+ and C2H3O2- afforded by dissolving
0.600 mol of Mg(C2H3O2)2 in water and diluting it to 135 mL?
(a)
(b)
(c)
(d)
(e)
0.444 and 0.889M
0.0444 and 0.0889M
0.889 and 0.444 M
0.444 and 0.444 M
4.44 and 8.89M
(15) The __________ subshell contains only one orbital.
(a) 5d
(b) 6f
(c) 4s
(d) 3d
(e) 1p
CHE 106, Fall 2012, Final Exam
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H corresponds to an
(16) A
(a)
(b)
(c)
(d)
(e)
process
negative, endothermic
negative, exothermic
positive, exothermic
zero, exothermic
zero, endothermic
(17) The reaction below is
, and therefore heat is
4Al(s) + 3O2(g) ------> 2Al2O3(s)
(a)
(b)
(c)
(d)
(e)
by the reaction.
H° = -3351kJ
endothermic, released
endothermic, absorbed
exothermic, released
exothermic, absorbed
thermoneutral, neither released nor absorbed
(18) The temperature of a 12.58 g sample of calcium carbonate [CaCO3(s)] increases from
23.6°C to 38.2C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of
heat are absorbed?
(a)
(b)
(c)
(d)
(e)
0.82
5.0
7.5
410
151
(19) Given the following thermochemical equations:
Fe2O3(s) + 3 CO(g)
3 Fe(s) + 4 CO2(g)
2 Fe(s) + 3 CO2(g)
4 CO(g) + Fe3O4(s)
H° = -28.0 kJ
H° = +12.5 kJ
What is the value of H° for the reaction
3 Fe2O3(s) + CO(g)
CO2(g) + 2 Fe3O4(s)
(a) -59.0 kJ
(b) +40.5 kJ
(c) -15.5 kJ
(d) -109.0 kJ
(e) -85 kJ
CHE 106, Fall 2012, Final Exam
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(20) Use the table of bond dissociation energies to calculate H (in kJ) for the following gasphase reaction (balance equation).
Bond
C-C
C=C
CCtriple bond
C-H
H-Cl
C-Cl
(a)
(b)
(c)
(d)
(e)
Dissociation Energy (in kJ/mol)
348
614
839
413
431
328
-44
38
-129
2134
none of the above
(21) Of the following transition in the Bohr hydrogen atom, the
the emission of the highest-energy photon.
(a)
(b)
(c)
(d)
(e)
transition results in
n =1 to n = 6
n = 6 to n = 1
n = 6 to n = 3
n = 3 to n = 6
n = 1 to n = 4
(22) According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both
the position and the
of an electron simultaneously.
(a)
(b)
(c)
(d)
(e)
mass
direction
momentum
charge
velocity
(23) An electron in an atom cannot have the quantum numbers where n =___, l =___,
and ml =___.
(a)
(b)
(c)
(d)
(e)
6, 1, 0
3, 2, 3
3, 2, -2
1, 0, 0
3, 2, 1
CHE 106, Fall 2012, Final Exam
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(24) The lowest orbital energy is reached when the number of electrons with the same spin is
maximized. This is a statement of the
.
(a)
(b)
(c)
(d)
(e)
Pauli Exclusion Principal
Planck’s constant
de Broglie’s hypothesis
Heisenberg Uncertainty Principle
Hund’s Rule
(25) In molecular orbital theory, the σ1s orbital is _________ and the σ*1s orbital is__________
in the H2 molecule.
(a) filled, filled
(b) filled, empty
(c) filled, half-filled
(d) half-filled, filled
(e) empty, filled
(26) The ground state electronic configuration of fluorine is
(a)
(b)
(c)
(d)
(e)
(27)
(a)
(b)
(c)
(d)
(e)
[He]2s22p2
[He]2s22p3
[He]2s22p4
[He]2s22p5
[He]2s22p6
Choose the electron configuration that corresponds to an excited state
[Ar]3d34s2
[Ne]5s1
[Ar]3d54s1
[Ar]3s13p6
[Xe]4f145d106s2
(28) Screening of the nuclear charge by core electrons in atoms is
(a)
(b)
(c)
(d)
(e)
..
.
less efficient than that by valence electrons.
more efficient than that by valence electrons.
essentially identical to that by valence electrons.
responsible for a general decrease in atomic radius going down a group.
both essentially identical to that by valence electrons and responsible for a general
decrease in atomic radius going down a group.
CHE 106, Fall 2012, Final Exam
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(29) Of the choices below, which gives the order for the first ionization energies?
(a)
(b)
(c)
(d)
(e)
Kr > Se > Br > Ga > Ge
Kr > Br > Se > Ge > Ga
Ga > Br > Ge > Kr > Se
Ga > Ge > Se > Br > Kr
Br > Se > Ga > Kr > Ge
(30) Of the following elements,
(a)
(b)
(c)
(d)
(e)
has the most negative (highest) electron affinity.
S
Cl
Se
Br
I
(31) Which of the following has eight valence electrons?
(a)
(b)
(c)
(d)
(e)
Ti4+
Kr
ClNa+
all of the above
(32) If 4 mol of Neon gas and 6 mol of Krypton gas are contained in a flask whose total pressure
is 1000 mmHg, the partial pressure of Neon gas is:
(a) greater than the partial pressure of the Krypton gas
(b) less than the partial pressure of the Krypton gas
(c) the same as the partial pressure of the Krypton gas
(33) The types of compounds that are most likely to contain covalent bonds is
(a)
(b)
(c)
(d)
(e)
.
one that is composed of a metal from the far left of the periodic table and a nonmetal
from the far right of the periodic table.
a solid metal.
one that is composed of only nonmetals.
held together by the electrostatic forces between oppositely charged ions.
There is no general rule to predict covalency in bonds.
CHE 106, Fall 2012, Final Exam
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(34) The molecular geometry of the BrO3- ion is
(a)
(b)
(c)
(d)
(e)
trigonal pyramidal
trigonal planar
Sbent
tetrahedral
T-shaped
(35) Of the following, only
(a)
(b)
(c)
(d)
(e)
(36)
.
has sp2 hybridization of the central atom.
PH3
CO32ICl3
I3PF5
What mass of nitrogen dioxide would be contained in a 4.32 L vessel at 48° C and 1062
torr?
5.35 x 104 g
53.5 g
10.5 g
105.0 g
none of the above
(a)
(b)
(c)
(d)
(e)
(37)
Which of the following statements is/are incorrect?
(a)
(b)
(c)
(d)
(e)
I. Sodium (Na), has a larger atomic radius than Cesium (Cs).
II. The first ionization energy of an atom generally increases moving left to right
across a period because the effective nuclear charge, Zeff, increases in that direction.
III. An atom of Phosphorus (P), releases more energy (becomes more stable) when it
adds an electron (i.e. has a more negative electron affinity value) than Chlorine
(Cl).
III
II
I
I and III
I and II
(38) In the Lewis structure for CIF3, the number of lone pairs of electrons around the central
atom is
(a)
(b)
(c)
(d)
(e)
0
1
2
3
4
CHE 106, Fall 2012, Final Exam
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(39) A sample of nitrogen gas at 18°C and 760 mm Hg has a volume of 2.67 mL. What is the
volume at 0°C and 1 atm of pressure?
(a)
(b)
(c)
(d)
(e)
2.85 mL
1.42 mL
1.50 mL
2.00 mL
2.50 mL
(40) Ammonium sulfate, used as a fertilizer, is produced by reacting ammonia with sulfuric acid,
according to: 2NH3(g) + H2SO4(aq)  (NH4)2SO4(aq). What volume of ammonia gas at
15°C and 1.15 atm is required to produce 150.0 g of ammonium sulfate? Molar masses:
NH3, 17.0 g/mol; H2SO4, 98.0 g/mol, (NH4)2SO4, 132.0 g/mol.
(a)
(b)
(c)
(d)
(e)
11.7 L
20.5 L
23.4 L
40.6 L
46.7 L
(41) A gas from a certain volcano was a mixture of CO2 (mole fraction 0.650), H2 (mole fraction
0.250), HCl (mole fraction 0.054), HF (mole fraction 0.028), and “other gases.” The total
pressure is 760 mm Hg. What is the sum of partial pressures of the “other gases”?
(a)
(b)
(c)
(d)
(e)
13.7 mm Hg
18 mm Hg
21.3 mm Hg
137 mm Hg
152 mm Hg
CHE 106, Fall 2012, Final Exam
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(42)
Using the phase diagram shown below, in which phase does this substance exist at 25°C
and at pressures 1.0 atm?
(a)
(b)
(c)
(d)
(e)
w
x
y
z
not enough information provided
CHE 106, Fall 2012, Final Exam
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KEY
CHE 106, Fall 2012 Final Exam
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CHE 106, Fall 2012, Final Exam
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