CHEM 1411 - FINAL EXAM
PART I Multiple Choice (2 points each)
Please DO NOT write or mark on this paper. Mark your answer on your Scantron.
1. The value seven hundred fifty million with four significant figures is written as
A. 7500 x 106
B. 7.500 x 108
C. 750 x 106
D. 750,000,000
E. 7500 x 108
2. Which of the following is NOT an element of the fourth period in the periodic table?
A. Co
B. V
C. Mg
D. Ca
E. Kr
3. To obtain 5.66 x 1021 atoms of nickel, you would weigh
A. 0.552 g
B. 1.81 g
C. 106 g
D. 9.64 x 1019 g
E.1.04 x 10-20 g.
4. How many grams of magnesium contain the same number of atoms as 20.04g of calcium?
A. 12.16 g
B. 20.04 g
C. 24.30 g
D. 40.08 g
E. 48.60 g
5. Which of the following series represents only known stable metal ions?
A. Fe2+, Fe3+, K2+
D. Fe2+, Sr2+, Mg2+
B. Mg2+, Ba3+, Na+
E. Li2+, Ca2+, Al3+
C. Li2+, Na+, Al3+
6. Which formula represents the binary compound formed by sodium and tellurium?
A. Na2Te
B. NaTe
C. Na3Te
D. Na3Te2
E. NaTe2
7. What is the correct name of KClO4?
A. potassium chlorate
D. potassium hypochlorate
B. potassium perchlorite
E. potassium hypochlorite
C. potassium perchlorate
8. Which of the following compounds is 36.4% oxygen by mass?
A. N2O
B. NO
C. N2O3
D. N2O4
E. N2O5
C. 261.35 g/mol.
D. 336.61 g/mol.
E. 398.62 g/mol.
9. The molar mass of barium nitrate is
A. 199.21 g/mol. B. 229.32 g/mol.
10. When 8.00 g of hydrogen reacts with 32.0 g of oxygen to form water, the limiting reagent is __________.
A. H2
B. H2, H2O
C. O , H2O
D. O2 and H2
E. pure H2O.
11. When NaBr dissolves in water, what types of intermolecular forces must be broken?
A. ion-ion forces
D. ion-ion forces and H-bonds
B. H-bonds
E. dipole-dipole
C. ion-dipole forces
12. Copper (II) sulfate pentahydrate , CuSO4.5H2O, is a blue hydrated salt. What is the approximate percentage
of water in this hydrated salt?
A. 32%
B. 64%
C. 56%
D. 46%
E. 7 %
13. Which pairs of reagents (if any) could be used in an aqueous solution to prepare pure manganese(II) sulfide
by a precipitation reaction?
A. MnCO3 and Ag2S
D. MnSO4 and PbS
B. MnCl2 and Na2S
C. MnCl2 and Na2SO4
E. none of these reagents will produce pure manganese(II) sulfide
14. Consider the equation : 2NaI(aq) + Cl2(g) → I2(aq) + 2NaCl(aq). The species undergoing
reduction is
A. sodium.
B. iodide.
C. chlorine.
D. iodine.
E. water.
D. +3
E. +2
15. The oxidation number of sulfur in S2O32A. +8
B. +6
C. +4
16. A solution of sodium carbonate is treated with a solution of nitric acid. Bubbles are observed in the
colorless solution. The balanced equation is
A. Na2CO3(aq) + 2HNO3(aq) → H2O(l) + CO2(g) + 2NaNO3(aq)
B. Na2CO3(aq) + 2HNO3 (aq) → H2CO3(aq) + 2NaNO4(aq)
C. Na2CO3(aq) + 2HNO3 (aq) → H2(g) + CO2(g) + 3 O2(g) + N2(g) + Na2O(aq)
D. Na2CO3(aq)) + 2HNO3 (aq) → H2O(l) + 2CO(g) + 3 O2(g) + NaNO3(aq)
E. 2 Na2CO3(aq)) + 2HNO3(aq) → H2O(l) + 2CO2(g) + N2(g) + 2NaNO3(aq)
17. If 15.0 g water at 28.0 ºC is added to 125.0 g water at 20.0 ºC, what is the final temperature of the
resulting mixture?
A. 20.9 ºC
B. 22.6 ºC
C. 23.1 ºC
D. 24.0 ºC
E. 27.3 ºC
18. Consider the thermal energy transfer during a chemical process. When heat is transferred to the
System from the surroundings, the process is said to be _______ and the sign of q is _______.
A. exothermic, positive
D. endothermic, negative
B. exothermic, negative
E. enthalpic, negative
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C. endothermic, positive
19. Which of the following particles has the largest radius?
A. He
C. O2-
B. F
D. Mg2+
E. N3-
20. State whether each of the following changes would be physical(P) or chemical(C) respectively.
I. painting wood
A. P, P, C
II. burning propane
B. P, C, P
III. breaking glass
C. P, C, P
D. P, P, P
E. C, C, C
21. Which of the following electronic transitions in a hydrogen atom would have the highest energy?
A. n = 4 to n = 1
B. n = 4 to n = 2
C. n = 2 to n = 1
D. n = 4 to n = 3
E. n = 3 to n = 2
D. d
E. s
22. When l = 3, what set of orbitals is designated?
A. g
Bp
C. f
23. What element has the electron configuration 1s22s22p63s23p6?
A. O
B. S
C. Ar
D. Si
E. none of these
24. A measure of the ability of a gaseous atom to acquire an electron to become negatively charged
is called its
A. ionization energy.
D. electronegativity.
B. polarizability.
E. electron density.
C. electron affinity.
25. Which of the following elements has the highest electron affinity?
A. Cl
B. Mg
C. C
D. P
E. Na
26. Which of the following diatomic molecules has the greatest bond strength?
A. F2
B. O2
C. N2
D. HF
E. HCl
27. A hydrocarbon has a molecular weight of 84 g/mol and empirical formula C3H6. Its molecular formula is
A. C6H6
B. C6H8
C. C6H10
D. C6H12
E. C6H14
28. The Lewis structure O = N= O (with 2 double bonds and 2 lone pairs on each O) represents
A. NO2−
B. NO2+
E. NO2+ NO2, and NO2−
D. both NO2+ and NO2−
C. NO2
29. In the combustion of methane, CH4, in an O2 atmosphere, CH4, what change in hybridization (if any) occurs
to the carbon atom?
A. sp3 to sp4
B. sp2 to sp3
E. no change in hybridization occurs
C. sp2 to sp
3
D. sp3 to sp
30. What hybrid orbital set is used by the terminal carbon atoms in the following molecule?
?
H3C - C
A. sp
B. sp2
CH
C. sp3
D. sp3d
E. sp3d2
31. At what temperature (T) and pressure (P) will all three phases of tastegudum coexist at equilibrium?
A. T = -200 oC , P = 10 atm
D. T = 350 oC , P = 100 atm
B. T = 750 oC , P = 90 atm
E. T = 0 o C , P = 1 atm
C. T = 250 oC , P = 35 atm
32. Identify the phase transition that occurs when NH4Cl solid turns to NH3 gas as it is heated.
A. deposition
B. sublimation
C. vaporization
D. freezing
E. melting
33. What volume will a mixture of 0.200 mole N2 and 0.500 mole He occupy at 0.944 atm and
15.0ºC?
A. 0.913 liters
B. 5.00 liters
C. 12.5 liters
D. 15.7 liters
E. 17.5 liters
D. 0.870 g/L
E. 2.09 g/L
34. What is the density of CH4 at 200 ºC and 0.115 atm?
A. 0.0475 g/L
B. 0.0716 g/L
C. 0.542 g/L
35. How many pi bonds are in the following molecule?
H3 C - CH = CH - C
A. 2
B. 3
C. 4
N:
D. 8
4
E. 9
Name_____________________________________
PART II Show Work (5 points each)
Please write your complete work in the space provided. Partial credit will be given.
1. The following questions pertain to lead (atomic mass of 207.2 g/mol) which crystallizes in a facecentered cubic arrangements. Lead has an atomic radius of 1.75 x 10-8 cm. What is the density of
lead in g/cm3?
2. Ammonia gas can be prepared by the reaction of a basic oxide like calcium oxide with ammonium
chloride, an acidic salt, according to the reaction CaO(s) + 2NH4Cl(s)  2NH3(g) + H2O(g) + CaCl2(s)
If 100.0 g of CaO was reacted with excess NH4Cl according to this reaction and 52.8 g of NH3 was obtained,
what is the percentage yield of ammonia?
3. Draw the lewis dot structure for SO42- and determine the hybridization, electron geometry, molecular
geometry, and bond angles for the central atom. Is this ion polar or nonpolar?
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4. Given the heats of the following reactions:
2ClF(g) + O2(g) → Cl2O(g) + F2O(g)
2ClF3(g) + 2O2(g) → Cl2O(g) + 3F2O(g)
2F2(g) + O2(g) → 2F2O(g)
ΔHº = 167.4 kJ
ΔHº = 341.4 kJ
ΔHº = −43.4 kJ
Calculate the heat of the reaction of chlorine monofluoride with F2 according to the equation:
ClF(g) + F2(g) → ClF3(g)
5. What is the chemical formula of a homonuclear diatomic gas if it has a pressure of 1.40 atm and a density of
1.82 g/L at 27 ºC?
6. A sample of an unknown carbon-hydrogen compound was burned in excess oxygen to
form 88.0 g of CO2 and 27.0 g H2O. What is the empirical formula of the hydrocarbon?
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CHEM 1411 GENERAL INFORMATION
Soluble Compounds
Compounds containing NO3
Compounds containing C2H3O2
Compounds containing Cl
Compounds containing Br
Compounds containing I
Compounds containing SO42
Important Exceptions
none
none
Salts of Ag+, Hg22+, Pb2+
Salts of Ag+, Hg22+, Pb2+
Salts of Ag+, Hg22+, Pb2+
Salts of Ca2+, Sr2+, Ba2+, Hg22+, Pb2+
Insoluble compounds
2
Compounds containing S
Compounds containing CO32
Compounds containing PO43
Compounds containing OH
Important Exceptions
Salts of ammonium, alkali metal cations and
Ca2+, Sr2+, Ba2+
Salts of ammonium, alkali metal cations
Salts of ammonium, alkali metal cations
Salts of ammonium, alkali metal cations and
Ca2+, Sr2+, Ba2+
Constants
Activity series
1 amu = 1.6605 X 1024 g
Avogadro's number = 6.022 X 1023
Gas constant = R = 0.08206 L atm / mol K
Planck's constant = h = 6.626 X 1034 J s
Speed of light = c = 2.998 X 108 m/s
RH = 2.18 X 1018 J
Conversion Factors and Relationships
1 mi = 1.6093 km
1 Å = 1010 m
1 cal = 4.184 J
E = h
1 gal = 4 qt = 3.7854 L
1 L = 1.0567 qt
PV = nRT
K = oC + 273.15
o
C = 5/9( oF  32)
o
F = 9/5 oC + 32
Heat = q = m X T X c
E = q + w
En = – RH (1/nf2  1/ni2)
c = 
d = h / mv
1 atm = 760 torr = 101.325 kPa
d = MP/RT
Pi = Xi Pt
r1/r2 =  M2/M1
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Li
K
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Co
Ni
Sn
Pb
H
Cu
Ag
Hg
Pt
Au
Answers –
Multiple Choice: Part I
1. B
2. C
3. A (5.66 x 1021 x 58.7g)/ 6.022 x 1023 .
4. A (20.04g/40g) X 24.3g
5. D
6. A
7. C
8. A
9. C barium nitrate = Ba(NO3)2 => 261.35 g/mol
10. D
11. E
12. A (90/ 249.5) x 100 = 36% closest to 32 % ******
13. B
14. C
15. E -2 = 2S + 3(-2) ; S = +2
16. A
17. A 15g( 28 – Tf ) = 125g( Tf – 20 ) ; Tf = 20.9 ºC
18. C
19. E
20. B
21. A
22. C
23. C
24. C
25. A
26. C
27. D
28. PENDING
29. D
30. A
31. C
32. B
33. E
34. A (density = PM/ RT )
35. B
PART II
1.
Fcc => 4 Pb atoms in unit cell
Mass = 4 atoms x 207.2 (amu/atom) x 1.66 x 10-24g/ amu = 1.38 x 10-21 g
Fcc => a = (√8) r = 1.75 x 10-8 cm x 2.83 = 4.95 x 10-8 cm
Volume = a3 = (4.95 x 10-8cm)3 = 1.21 x 10-22 cm3
Density = Mass / Volume = 11.4 g/ cm3
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2.
Moles of CaO = 100.0 g / 56.08 g/mol = 1.783 mol
Theoretical moles of NH3 = 2 X 1.783 mol = 3.566 mol
Theoretical grams of NH3 = 3.566 mol X 17.034 g/mol = 60.74 g
Percent yield = 52.8 g / 60.74 g = 86.93%
3.
SO4-2 = 6e + 4(6e) + 2e = 32 e = 16 pairs of electrons
O
2-
O -S- O
O
electron domain geometry: tetrahedral molecular geometry: tetrahedral
bond angle: 109.5o
hybridization: sp3
4.
½( 2ClF(g) + O2(g) → Cl2O(g) + F2O(g) )
½(ΔHº = 167.4 kJ )
-½(2ClF3(g) + 2O2(g) → Cl2O(g) + 3F2O(g) )
-½(ΔHº = 341.4 kJ )
½(2F2(g) + O2(g) → 2F2O(g) )
½(ΔHº = −43.4 kJ )
__________________________________________________________
ClF(g) + F2(g) → ClF3(g)
ΔHº = −108.7.4 kJ
5.
Density = D = (PM)/ (RT)
Molar mass = M = (DRT)/ P = (1.82 x 0.0821 x 300) / 1.4
= 32 g/mol
For a homonuclear diatomic gas => O2 .
6.
Moles of CO2 = moles of C = 88.0 g / 44.01 g/mol = 2.00 mol
Moles of H2O = 27.0 g / 18.02 g/mol = 1.50 mol
Moles of H = 2(moles of H2O) = 2(1.50 mol) = 3.00 mol
Empirical formula is C2H3
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