Download Spring 2004 Final Exam Review Problems

Academic Chemistry Spring 2009 Final Exam Review Problems
Chapter 8
1. How many moles are there in a 9.6 x 1022 formula unit sample of NaCl?
A 1.6 moles
B 58 moles
C
D
0.16 moles
5.8 moles
2. Determine the number of molecules of CO2 in a 1.75 mole sample of CO2.
A 1.05 x 1023 molecules CO2
B 2.91 x 10-22 molecules CO2
C
D
1.05 x 1024 molecules CO2
2.91 x 1022 molecules CO2
3. How many moles of H2 gas are there in a 4.3 x 1023 molecules sample of H2 at STP?
A 0.71 mol H2
B 1.4 mol H2
C
D
7.1 mol H2
14 mol H2
4. How many atoms of neon gas are present in a 15.7 L sample of neon at STP?
A 4.22 x 1024 atoms Ne
B 4.22 x 1023 atoms Ne
C
D
4.68 x 1023 atoms Ne
4.68 x 1024 atoms Ne
5. Which of the following is not an empirical formula?
A Na2SO4
B C6H5Cl
C
D
N2H4
Sn3(PO4)4
6. A compound has the empirical formula C2H3O and a molar mass of 172.0 g/mol. What is its molecular
formula?
A C6H9O3
B C8H12O4
C
D
C9H16O3
C7H8O5
7. What is the percent of aluminum in Al2(SO4)3?
A 28.1%
B 54.0%
C
D
15.8%
56.7%
8. What is the empirical formula of a compound that is 3.05% carbon, 0.26% hydrogen, and 96.96% iodine?
A C2HI7
B CH2I5
C
D
C3H2I11
CHI3
Chapters 6 & 7
9. When the equation Fe2O3  Fe + O2 is balanced, the coefficient for O2 is:
A 4
B 3
C
D
2
1
10. The reaction in question 9 is an example of a(n):
A decomposition
B synthesis
C
D
single displacement
combustion
11. In a double displacement reaction:
A
B
C
D
one of the products is always a gas
one of the products must be an element
positive ions are exchanged between two compounds
all of the above
12. A double displacement reaction takes place when aqueous K2SO4 reacts with aqueous Pb(NO3)2. You
would expect one of the products of this reaction to be:
A K2S
B NaPb
C
D
PbSO4
CNO3
C
D
single-displacement reactions
decomposition reactions
13. Water is always a product in:
A combustion reactions
B decomposition reactions
14. The following would be classified as which type of reaction?
CH4 + 2 O2  CO2 + 2 H2O
A
C
synthesis
single displacement
B
D
combustion
double displacement
15. Which of the following describes the products of a synthesis reaction?
A
C
carbon dioxide and water
an element and a compound
B
D
a single product
two ionic compounds
16. Predict the products from the following reactants:
MgSO4 + Na 
A
C
Mg +Na2SO4
MgSO4 + Na
B
D
MgNa + SO4
Mg + NaSO4
17. When the following equation is balanced, what is the coefficient that goes with water?
_____ Mn(OH)3 + _____ H2SO3  _____ Mn2(SO3)3 + _____ H2O
A
C
2
6
B
D
3
12
18. O2, N2, Cl2, and I2 are examples of—
A
C
diatomic molecules
ionic compounds
B
D
compounds
atoms
19. Which compound will be a precipitate (solid) in the following equation?
_____ (NH4) 2SO4 + _____ Pb(NO3) 2  _____ PbSO4 + _____ NH4NO3
A
C
(NH4)2SO4
PbSO4
B
D
Pb(NO3) 2
NH4NO3
20. Which of the following compounds will be soluble in water?
A
C
AgCl
MgCO3
B
D
KOH
AlPO4
Chapter 9
21. How many moles of oxygen gas will react with excess sulfur according to produce 1.25 mol of sulfur
trioxide according to the following equation?
__1__ S8 + __12__ O2  __8__SO3
A
C
0.833 mol
1.88 mol
B
D
1.25 mol
10.0 mol
22. What is the molar mass of iron (III) sulfate, Fe2(SO4)3?
A
C
104.0 g/mol
335.7 g/mol
B
D
312.0 g/mol
400.1 g/mol
23. How many grams of CO2 will be produced when 7.82 liters of O2 reacts with excess CH4 according to the
following equation at STP?
CH4 + 2 O2  CO2 + 2 H2O
A
C
7.66 grams CO2
2.74 grams CO2
B
D
5.36 grams CO2
5.47 grams CO2
24. How many moles of H2O will be produced when 3.7 x 1023 molecules of NH3 react with excess O2
according to the following equation?
4 NH3 + 7 O2  4 NO2 + 6 H2O
A
C
0.922 mol H2O
16.6 mol H2O
B
D
0.410 mol H2O
3.68 mol H2O
25. In the following reaction, which reactant could be the limiting reactant?
2 MgCl2 + Pb(OH)4  PbCl4 + 2 Mg(OH)2
A
C
PbCl4
Mg(OH)2
B
D
MgCl2
none of these could be the limiting reactant
26. 1 mole is equal to which of the following?
A
C
22.4 L at STP
molar mass of an element
B
D
6.02 x 1023 atoms, molecules or formula units
all of the above are correct
27. Given the reaction 2 NO + O2  2 NO2, if 6.5 L of O2 react at STP, how many liters of NO2 are produced?
A
C
6.5 L
26 L
B
D
3.2 L
13 L
28. Given the reaction Zn + 2 HCl  ZnCl2 + H2, if 2.0 mol Zn and 5.0 mol of HCl are allowed to react:
A
C
Zn is the limiting reactant
1.0 mol of ZnCl2 is produced
B
D
HCl is the limiting reactant
5.0 mol of H2 is produced
29. Given the reaction CaCO3  CaO + CO2, if 50.0 g of CaCO3 react to produce 20.0 g of CO2, what is the
percent yield of CO2?
A
C
66.7%
90.9%
B
D
40.0%
250%
Chapter 10
30. What is the frequency of radiation whose wavelength is 5.89 x 10 - 9 m?
A
C
1.96 x 10 – 17 s-1
5.09 x 10 16 s-1
B
D
1.77 x 10 1 s-1
1.77 x 10 18 s-1
31. Which of the following is not a type of electromagnetic radiation?
A
C
X-rays
Radiowaves
B
D
Gamma rays
Alpha waves
32. How many electrons can be held in the 2nd energy level?
A
C
2
18
B
D
8
32
33. Which element is represented by the following electron configuration?
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p4
A
Thallium
B
Polonium
C
Bismuth
D
Astatine
34. Which of the following is the correct noble gas configuration for Barium?
A
C
[Kr]5s2
[Xe]6s1
B
D
[Xe]5s2
[Xe]6s2
35. Which element is represented by the following noble gas configuration?
[Kr]5s24d105p4
A
C
Tellurium
Selenium
B
D
Bromine
Indium
36. What part of the following electron configuration is not in the correct order?
1s22s22p63s13p64s24d104p6
A
C
3p6
4p6
B
D
4d10
4s2
37. How many orbitals does each “d” sublevel contain?
A
C
1
5
B
D
3
7
38. What is the maximum number of electrons that each “p” sublevel can hold?
A
C
2
10
B
D
6
14
39. Put the following elements in order of decreasing atomic radii: Fe, S, F, Ba, Cl, Ca
A
C
F, Cl, S, Fe, Ba, Ca
F, Cl, S, Fe, Ca, Ba
B
D
Ba, Ca, Fe, S, Cl, F
Cl, Ca, F, Fe, Ba, S
40. Put the following elements in order of increasing electronegativity: Rb, O, Ca, Sr, Mn
A
C
Rb, Sr, Ca, Mn, O
O, Mn, Ca, Sr, Rb
B
D
Rb, O, Ca, Sr, Mn
Rb, Ca, Sr, Mn, O
41. Which of the following elements has the smallest ionization energy: C, Se, K, or Sc?
A
C
C
K
B
D
Se
Sc
42. What is the electron configuration for Arsenic?
A
B
C
D
1s22s22p63s23p64s23d104p3
1s22s22p63s23p64s23d94p4
1s22s22p63s23p64s13d104p4
1s22s22p63s23p64s23d104p6
43. Put the following in order of decreasing ionic radii: N - 3, F - 1, Na + 1, Mg + 2, O - 2.
A
B
C
D
N - 3, F - 1, Na + 1, Mg + 2, O - 2
N - 3, O - 2, F - 1, Na + 1, Mg + 2
Mg +2, Na + 1, F - 1, O - 2, N - 3
N - 3, O - 2, Mg + 2, F - 1, Na + 1
44. How many unshared electrons will Silicon have in its orbital notation?
A
C
0
2
B
D
1
3
Chapter 11
45. How many valence electrons does C2ClO3-3 contain?
A
C
32
33
B
D
36
29
46. What is the electron configuration for sulfide ion, S-2?
A
C
1s22s22p63s23p3
1s22s22p63s23p6
B
D
1s22s22p63s23p4
1s22s22p63s23p1
47.
According to the Lewis diagram above, a nitrogen molecule has a –
A
B
C
D
bent structure and a double bond
polar structure and a triple bond
linear structure and a triple bond
circular structure and an ionic bond
48. Which of the following elements is not an exception to the octet rule?
A
C
Hydrogen
Boron
B
D
Beryllium
Carbon
49. Which of the following compounds is considered ionic?
A
C
CO
NaCl
B
D
H2O
F2
50. The bond between carbon and chlorine is polar. Carbon tetrachloride is a molecule
with a tetrahedral shape. This molecule is
A
C
polar
ionic
B
D
nonpolar
metallic
51. Methane, CH4, contains what type of intermolecular forces?
A
C
hydrogen bonding
dispersion forces
B
D
dipole-dipole interactions
nonpolar covalent bonding
52. The bond that exists between nitrogen and fluorine is
A
C
ionic
polar covalent
B
D
covalent
nonpolar ionic
53. When drawing structural formulas, two lines between atoms (as in O = C = O)
represents
A
B
C
D
2 electrons in a single bond
2 electrons in a double bond
4 electrons in a double bond
4 electrons in a single bond
54. The bond in the molecule hydrogen bromide, HBr, is considered to be
A
C
nonpolar covalent
ionic
B
D
polar covalent
metallic
55. How many valence electrons would an atom of aluminum gain or lose when forming a bond?
A
C
gain 3
gain 5
B
D
lose 3
lose 5
56. What is the VSEPR shape for SO3-2?
A
C
trigonal planar
tetrahedral
B
D
bent
trigonal pyramidal
Chapter 12
57. The average kinetic energy of water molecules is greatest in:
A
C
steam at 200oC
liquid water at 273 K
B
D
liquid water at 90oC
ice at 0oC
58. An increase in the temperature of a contained liquid:
A
causes the vapor pressure above the liquid to increase.
B
decreases the vapor pressure above a liquid.
C
causes fewer particles to escape the surface of the liquid
D
has no effect on the kinetic energy of the liquid
59. A pressure of 2.5 atm is equivalent to
A
C
41 kPa
3.0 x 102 torr
B
D
1900 mm Hg
2.5 kPa
60. A 1.0 mol sample of gas is at a temperature of 20oC and a pressure of 1.2 atm. What
is the volume occupied by the gas? (R = 0.0821 L atm/K mol)?
A
C
20 L
40 L
B
D
30 L
50 L
61. Increasing the volume of a given amount of gas at constant temperature causes the
pressure to decrease because:
A
B
C
D
the molecules are striking a larger area with the same force
there are fewer molecules
the molecules are moving more slowly
there are more molecules
62. A gas occupies a volume of 2.50 L at a pressure of 350.0 kPa. If the temperature
remains constant, what volume would the gas occupy at 1750 kPa?
A
C
5.00 L
12.5 L
B
D
0.500 L
1.40 x 102 L
63. If a sample of oxygen occupies a volume of 2.15 L at a pressure of 58.0 kPa and a
temperature of 25oC, what volume would this sample occupy at 101.3 kPa and
0.0oC?
A
C
1.35 L
4.10 L
B
D
1.13 L
3.44 L
Spring Final Exam Review Problems Part II
1. A compound is composed of 25.46% N, 9.09% H and 65.45% C. What is the empirical formula for this
compound? If the molar mass of the molecular formula is 165.0 g/mol, what is the molecular formula for
this compound?
2. Predict the products from the following reactants and determine if any of the products are insoluble (form a
solid).
AgNO3(aq) + K2SO4 (aq) 
Zn (s) + CuSO4 (aq) 
3. Predict the products of the following equations given their reactants along with the type of reaction for each
equation.
C2H5OH + O2 
Type:
Pb(NO3)2 + K2CrO4 
Type:
Zn + H2CO3 
Type:
Na + FeBr3 
Type:
4. Determine the number of valence electrons in NO3-1. Draw the Lewis dot structure for this ion. Determine
if it is polar or nonpolar, and also determine the VSEPR shape for this ion. Tell the strongest type of
intermolecular forces that exist in this ion.
5. How many grams of hydrogen gas, H2, will be produced when 1.6 x 1022 atoms of magnesium metal react
with excess ammonia, NH3?
3 Mg (s) + 2 NH3 (g)  Mg3N2 (s) + 3 H2 (g)
6. How many grams of dinitrogen tetrafluoride, N2F4, can be produced by the reaction of 5.8 grams of
ammonia, NH3, and 9.5 grams of fluorine gas, F2? What is the limiting reactant? What is the excess
reactant? Don’t forget to balance the equation first though!
_____ NH3 + _____ F2  _____ N2F4 + _____ HF
7. How much energy would be produced when a particle of light has a wavelength of 8.23 x 10-8 m? (Hint:
you must use the c = wf equation and the E = hf equations).
8. Draw the orbital notation for silicon. Be sure to label each sublevel appropriately. Also, determine the
number of shared and unshared pairs of electrons in silicon.
9. Write out the electron configuration and the noble gas configuration for Francium (Fr, atomic # 87).