Chemistry 106: General Chemistry
Syracuse University Project Advance
Final Exam, Fall 2005
Name
Date
The last pages of this examination are reference tables.
c = 3.00 x 108 m/sec, h = 6.63 x 10-34 Js, mp = 1.67 x 10-24 g (mass of proton)
Rydberg Constant (RH) = 2.18 x 10-18 J
1. The balanced net ionic equation for precipitation of PbSO4 when aqueous solutions of
lead nitrate, Pb(NO3)2, and sodium sulfate, Na2SO4 are mixed is:
a)
b)
c)
d)
e)
Pb2+(aq) + 2NO3-(aq) + 2Na+(aq) + SO42-(aq)  PbSO4(s) + 2NO3- + 2Na+
Pb2+(aq) + SO42-(aq)  PbSO4(s)
Pb2+(aq) + 2NO3-(aq)  Pb(NO3)2(aq)
Pb(NO3)2(aq) + Na2SO4(aq)  PbSO4(s) + 2NaNO3(aq)
Pb(NO3)2(aq) + Na2SO4(aq)  PbSO4(aq) + 2NaNO3(aq)
2. If 19.36 mL of NaOH is needed to exactly neutralize 90.00 mL of 0.6600 M HCl, the
concentration of the NaOH is
a)
b)
c)
d)
e)
0.1278 M
0.1420 M
1.278 M
2.640 M
3.068 M
3. What is the formula of the compound formed between calcium ions and phosphorus
ions?
a)
b)
c)
d)
e)
CaP2
Ca3P2
Ca2P2
CaP
Ca2P3
4. Which of the following statements is/are correct?
I. CoCl2 is copper chloride
II. ClO- is chloride ion.
III. NaNO2 is sodium nitrate.
IV. KClO4 is potassium chlorate.
V. Mg2SO4 is magnesium sulfate.
a)
b)
c)
d)
e)
All are correct.
Only I and IV are correct.
II, III, and V are correct.
I, III, and V are correct.
None of the statements is correct.
5. How many moles of ethanol, C2H5OH, are contained in 6.14 g of ethanol?
a)
b)
c)
d)
e)
0.133 mol
25.3 mol
0.319 mol
282.4 mol
3.13 mol
6. The hormone adrenalin contains 56.79% C, 6.56% H, 28.37% O, and 8.28% N. Its
empirical formula is
a)
b)
c)
d)
e)
C5H7O2N
C9HO4N
C9H13O4N2
C8H11O3N
C6H8O3N
7. To prepare 300.0 mL of 0.200 M KNO3, what volume of 0.800 M KNO3 must be
diluted with water?
a)
b)
c)
d)
e)
500 x 10-2 L
7.5 x 10-2 L
1.80 x 10-1 L
6.00 x 10-1 L
1.20 L
8. What is the molarity of a solution that contains 32.0 g of sulfuric acid, H2SO4, in 2.50
L of solution?
a)
b)
c)
d)
e)
0.0128 M
0.123 M
0.131 M
0.818 M
12.8 M
9. Under constant volume conditions, the heat of combustion of propane, C3H8, is 2220
kJ/mol. When a 2.500 g sample of propane was burned in a calorimeter, the
temperature changed from 20.55° C to 28.25°C. The total heat capacity of the
calorimeter, in kJ/°C, is
a)
b)
c)
d)
e)
126.1
16.4
720.8
6.55
No answer is correct within 10%
10. Passing steam over hot charcoal at 1000°C produces water gas which is a mixture of
CO and H2, according to the following reaction:
C(s) + H2O(g)  CO(g) + H2(g); H°reax
The H°reax for this reaction can be calculated from the thermodynamic data for the
following reactions:
2H2(g) + O2(g)  2H2O(g)
C(s) + O2(g)  CO2(g)
2CO(g) + O2(g)  2CO2(g)
a)
b)
c)
d)
e)
H°1
H°2
H°3
;
;
;
H°reax = H°2 + 1/2H°1 + 1/2H°3
H°reax = H°2 - H°1 - H°3
H°reax = H°3 - H°1 - H°2
H°reax = H°2 - 1/2H°1 - 1/2H°3
H°reax = H°1 - H°2 + H°3
11. Which of the following combinations of quantum numbers are not possible for an
electron in an atom.
N
L
Ml
S
(a)
3
2
-2
-1/2
(b)
3
3
-2
-1/2
(c)
2
1
0
-1/2
(d)
1
0
0
+1/2
(e)
3
1
0
+1/2
12. What values of ml are possible for a 4f electron?
a)
b)
c)
d)
e)
4, 3, 2, 1, 0, -1, -2, -3, -4
3, 2, 1, 0, -1, -2, -3
2, 1, 0, -1, -2
1, 0, -1
3, 2, 1, 0
13. Which of the following electronic configurations is that of a vanadium atom in its
ground state?
a)
b)
c)
d)
e)
1s22s22p63s23p63d5
1s22s22p63s23p63d54s2
1s22s22p63s23p63d34s2
1s22s22p63s23p63d44s1
1s22s22p63s23p64s24p3
14. Which of the following statements is/are correct?
I. The second ionization energy of Na is greater than that for Mg.
II. Na is more metallic than Al.
III. O atoms are smaller than F atoms.
IV. Cl is more electronegative than B.
V. O is less reactive than Ne.
a)
b)
c)
d)
e)
I, II and IV are correct.
Only I and II are correct.
Only III and IV are correct.
Only II and III are correct.
No statement is correct.
15. For which of the following pairs is the first ion larger than the second?
I. Sr2+ and Rb+
II. I- and ClIII. Tl3+ and Tl+
IV. Se2- and Bra)
b)
c)
d)
e)
II and IV
I, III, and IV
Only II
Only IV
None of the above.
16. For which of the following pairs does the second element have the greater metallic
character?
I. Be, B
II. Li, Na
III. P, Ga
IV. Sn, In
V. As, S
a)
b)
c)
d)
e)
For all pairs
II and III only
II, III, and IV
I and V only
For no pairs
17. For which of the following pairs does the first listed element have the larger second
ionization energy?
a)
b)
c)
d)
e)
Cs, Ba
Mg, Al
P, S
K, Na
Mg, Be
18. The octet rule is violated by which of the following?
I. NO2
II. SF4
III. H2CO
IV. CH3
V. PCl3
a)
b)
c)
d)
e)
All of them.
III and IV only
I, II, III, and V
I, II, and IV
IV only
19. The formal charge on boron in BF3 is
a)
b)
c)
d)
e)
0
+1
+4
+3
+5
20. In which of the following pairs is/are the atoms or ions isoelectronic with each other?
I. Kr, Br+
II. Te, I+
III. Ca2+, Ti
IV. S, Se
V. K+, Ar
a)
b)
c)
d)
e)
In all pairs
I and III only
II and V only
I, II, and III
In no pairs
21. Which of the Lewis structures below is/are correct?
Cl
I.
H
C
II.
H
N
N
H
Cl
H
III.
O
IV.
C O
O
H
H
C
V.
C
C
H
H
a)
b)
c)
d)
e)
N C C
All are correct.
Only I is correct.
I, III and IV are correct.
All except II are correct.
All except I are correct.
22. Bromine reacts with alkenes by adding to the carbon-carbon double bond, according
to the equation shown below:
H
H
C
H
Bond
Bond dissociation
energy (kJ/mol)
+
C
Br2
H
Br Br
H C C H
H H
;
H°reax
C-C
C=C
C-H
C-O
C-Br
Br-Br
348
614
413
358
276
193
From the information given above, determine the value of H°reax (in kJ/mol) for the
reaction shown.
a)
b)
c)
d)
e)
-276
+54
-183
+183
No answer is correct within 10%.
23. For which of the following molecules or ions is the given molecular geometry
correct?
I. XeF2, linear
II. SF6, octahedral
III. BrF5, square pyramidal
IV. ICl2-, linear
V. BeCl2, linear
a)
b)
c)
d)
e)
All are correct.
Only I is correct.
Only I, II, and III are correct.
Only IV and V are correct.
All except IV are correct.
24. Which of the following statements is/are correct?
I. If only one bond is formed between two atoms, it is a  bond.
II. If three bonds are formed between two atoms, one is a  bond and two are 
bonds.
III. When two or more equivalent Lewis structures can be drawn for a molecule or
ion, they are called resonance structures.
IV. The nitrate ion, NO3-, is represented by two resonance structures.
V. The acetylene molecule, C2H2, is represented by two resonance structures.
a)
b)
c)
d)
e)
All except I are correct.
I, II, and III are correct.
Only III is correct.
Only II and III are correct.
II, III, and IV are correct.
25. A 275.0-mL sample of oxygen gas is collected over water at 60.0°C. The total
pressure is 755 torr. What is the volume of the O2 at STP? (the vapor pressure of
water at 60°C is 149 torr.)
a)
b)
c)
d)
e)
180 mL
224 mL
244 mL
333 mL
none of these.
26. 131I-1 has
a)
b)
c)
d)
e)
131 protons, 53 neutrons, and 54 electrons
131 protons, 53 neutrons, and 52 electrons
53 protons, 78 neutrons, and 54 electrons
53 protons, 131 neutrons, and 52 electrons
78 protons, 53 neutrons, and 72 electrons
27. How many molecules of glycerol, C3H5(OH)3, dissolved in 750.0 g of water are
needed to make a 1.50 m solution?
a)
b)
c)
d)
e)
9.03 x 1023 molecules
1.20 x 1024 molecules
6.75 x 1023 molecules
4.01 x 1023 molecules
Not enough information to determine answer.
28. What is the boiling point change for a solution containing 0.328 mole of naphthalene
(a nonvolatile, nonionizing compound) in 250 g of liquid benzene? (The freezing
point of pure benzene is 5.44°C. The Kb for benzene = 2.53°C/m)
a)
b)
c)
d)
e)
3.32°C
6.27°C
6.75°C
5.86°C
8.76°C
29. When 1.50 g of glutamic acid is dissolved in 100.0 g H2O, the resulting solution
freezes at -0.190°C. (Kf for water is 1.86°C-kg/mol). The molar mass of glutamic
acid is
a)
b)
c)
d)
e)
14.7 g/mol
1.50 g/mol
189 g/mol
28.0 g/mol
147 g/mol
30. The decomposition of potassium chlorate is used to produce oxygen in the laboratory.
2KClO3 (s)  2KCl (s) + 3O2 (g)
How many liters of O2 (g) at 25oC and 1 atm pressure can be produced by the
decomposition of 7.5 g of KClO3 (s)?
a)
b)
c)
d)
e)
4.5
7.5
2.3
3.7
6.5
Metal Activity Table
(easiest to oxidize at top)
Lithium
Potassium
Barium
Calcium
Sodium
Magnesium
Aluminum
Manganese
Zinc
Chromium
Iron
Cobalt
Nickel
Tin
Lead
HYDROGEN
Copper
Silver
Mercury
Platinum
Gold