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CHM 2045C Final Exam Spring 2007

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 

According to the kinetic-molecular theory of matter, particles in a liquid
a.
are packed closely together in a regular array.
b.
move slower as the temperature increases.
c.
expand to fill their container.
d.
vibrate back and forth about an average position.
e.
are packed closely together, but are not confined to specific positions.
 

 2. 

A pure substance composed of two or more different elements is
a.
a homogeneous mixture.
b.
a heterogeneous mixture.
c.
a polyelement.
d.
an atom.
e.
a chemical compound.
 

 3. 

What is the correct symbol for lead?
a.
L
b.
Ld
c.
Pb
d.
Sn
e.
Pd
 

 4. 

The molecular model below depicts a molecule composed of carbon (black), oxygen (gray), and hydrogen (white) atoms. What is the correct molecular formula?

45finals07online_files/i0050000.jpg
a.
CHO
b.
C6H6O2
c.
C6H7O
d.
C7H6O
e.
C7H6O2
 

 5. 

When 24 copper pennies are submerged in water, the pennies displace 8.26 cm3 of water. If the combined mass of the pennies is 73.86 g, what is the density of copper?
a.
0.112 g/cm3
b.
1.34 g/cm3
c.
8.94 g/cm3
d.
32.8 g/cm3
e.
107 g/cm3
 

 6. 

At 0 °C, a bottle contains 325 mL of water in its liquid state. What is the volume of the water after it freezes (at 0 °C)? The densities of liquid water and ice at 0 °C are 1.000 g/mL and 0.917 g/mL, respectively.
a.
27.0 mL
b.
298 mL
c.
325 mL
d.
354 mL
e.
391 mL
 

 7. 

All of the following are examples of chemical change EXCEPT
a.
the tarnishing of silver.
b.
the rusting of iron.
c.
the combustion of butane gas.
d.
the condensation of steam.
e.
the decomposition of water to hydrogen gas and oxygen gas.
 

 8. 

Which of the following observations are examples of chemical changes to aluminum?

1.
When aluminum reacts with hydrochloric acid, hydrogen gas is evolved.
2.
Aluminum melts at 660 °C.
3.
A cube of aluminum with a volume of 4.0 cm3 has a mass of 10.8 g.
4.
Aluminum is a good electrical conductor.
a.
1 only
b.
2 only
c.
1 and 2
d.
3 and 4
e.
1, 2 and 4
 

 9. 

Thermostats are often set to 68 °F. What is this temperature in Celsius?
a.
2.0 ´ 101 °C
b.
25 °C
c.
38 °C
d.
56 °C
e.
7.0 ´ 102 °C
 

 10. 

The boiling point of liquid helium is 4 K. What is this temperature in Celsius?
a.
-294 °C
b.
-277 °C
c.
-269 °C
d.
-255 °C
e.
-169 °C
 

 11. 

What is a correct method for converting Celsius to Kelvin?
a.
45finals07online_files/i0120000.jpg
b.
45finals07online_files/i0120001.jpg
c.
45finals07online_files/i0120002.jpg
d.
45finals07online_files/i0120003.jpg
e.
45finals07online_files/i0120004.jpg
 

 12. 

Two electronic balances are tested using a standard weight. The true mass of the standard is 1.3111 g. The results of 5 individual measurements on each balance are recorded below.

 
Balance A
Balance B
 
0.8888 g
1.3110 g
 
0.9959 g
1.3109 g
 
1.1182 g
1.3111 g
 
1.0033 g
1.3110 g
 
0.9938 g
1.3110 g
average mass =
1.0000 g
1.3110 g

Which statement best describes the results?
a.
A: good precision, good accuracy. B: good precision, good accuracy.
b.
A: good precision, good accuracy. B: poor precision, poor accuracy.
c.
A: poor precision, good accuracy. B: good precision, good accuracy.
d.
A: poor precision, poor accuracy. B: good precision, good accuracy.
e.
A: poor precision, poor accuracy. B: good precision, poor accuracy.
 

 13. 

Which method is correct for determining the liters of gas required to fill an automobile's 15 gallon tank? (1.000 L = 1.057 quarts, 4 quarts = 1 gallon)
a.
15 gallons 45finals07online_files/i0140000.jpg
b.
15 gallons 45finals07online_files/i0140001.jpg
c.
15 gallons 45finals07online_files/i0140002.jpg
d.
15 gallons 45finals07online_files/i0140003.jpg
e.
none of the above
 

 14. 

The wavelength of light emitted from a green laser pointer is 5.32 ´ 102 nm. What is the wavelength in meters?
a.
5.32 ´ 10-9 m
b.
5.32 ´ 10-7 m
c.
5.32 ´ 10-5 m
d.
5.32 ´ 10-3 m
e.
5.32 ´ 10-1 m
 

 15. 

How many protons, neutrons, and electrons are in an oxygen-18 atom?
a.
6 protons, 8 neutrons, 4 electron
b.
6 protons, 10 neutrons, 8 electrons
c.
8 protons, 8 neutrons, 8 electrons
d.
8 protons, 10 neutrons, 8 electrons
e.
8 protons, 10 neutrons, 18 electrons
 

 16. 

What is the atomic symbol for an element that has 30 neutrons and a mass number of 55?
a.
Cs
b.
At
c.
Zn
d.
Hg
e.
Mn
 

 17. 

How many elements are in the first period of the periodic table?
a.
2
b.
7
c.
8
d.
10
e.
18
 

 18. 

What alkali metal is in the fourth period?
a.
Ca
b.
K
c.
Na
d.
Sr
e.
Sc
 

 19. 

A nitride ion has ____ electrons.
a.
2
b.
4
c.
7
d.
8
e.
10
 

 20. 

For a nonmetal in Group 5A of the periodic table, the most common monatomic ion will have a charge of ____.
a.
3-
b.
2-
c.
1-
d.
1+
e.
2+
 

 21. 

Sodium sulfate has the chemical formula Na2SO4. Based on this information, the formula for chromium(III) sulfate is ____.
a.
Cr3(SO4)2
b.
Cr2(SO4)3
c.
Cr(SO4)2
d.
Cr2SO4
e.
CrSO4
 

 22. 

What is the charge on the copper ion in Cu2O?
a.
2-
b.
1-
c.
1+
d.
2+
e.
4+
 

 23. 

What is the correct formula for potassium dihydrogen phosphate?
a.
K2H2PO4
b.
KH2PO4
c.
KH2PO3
d.
K2H2P
e.
KH2P
 

 24. 

All of the following are named correctly EXCEPT
a.
LiClO4; lithium perchlorate.
b.
CaHPO4; calcium hydrogen phosphide.
c.
NaCN; sodium cyanide.
d.
Mg(OH)2; magnesium hydroxide.
e.
CaSO3; calcium sulfite.
 

 25. 

What is the molar mass of ammonium sulfate?
a.
110.0 g/mol
b.
114.1 g/mol
c.
132.1 g/mol
d.
144.6 g/mol
e.
168.9 g/mol
 

 26. 

What is the mass percent of each element in dichloromethane, CH2Cl2?
a.
10.06% C, 60.24% H, 29.70% Cl
b.
20.00% C, 20.00% H, 60.00% Cl
c.
24.10% C, 3.11% H, 72.79% Cl
d.
33.87% C, 0.22% H, 65.91% Cl
e.
14.14% C, 2.37% H, 83.48% Cl
 

 27. 

Nitrogen and oxygen form an extensive series of oxides with the general formula NxOy. What is the empirical formula for an oxide that contains 46.68% nitrogen?
a.
N2O
b.
NO
c.
NO2
d.
N2O3
e.
N2O5
 

 28. 

The combustion of propane produces carbon dioxide and steam.

C3H8(g) + 5 O2(g) ® 3 CO2(g) + 4 H2O(g)

All of the following statements concerning this reaction are correct EXCEPT
a.
three molecule of carbon dioxide are formed per one molecule of propane consumed.
b.
five molecules of oxygen are consumed per one molecule of propane consumed.
c.
four moles of steam are formed per five moles of oxygen consumed.
d.
the combined mass of reactants consumed equals the mass of products formed.
e.
three grams of carbon dioxide are formed per five grams of oxygen consumed.
 

 29. 

Ammonia is prepared by reacting nitrogen and hydrogen gases at high temperature according to the unbalanced chemical equation below.

__ N2(g) + __ H2(g) ® __ NH3(g)

What are the respective coefficients when the equation is balanced with the smallest whole numbers?
a.
1, 1, 1
b.
1, 3, 1
c.
1, 3, 2
d.
2, 1, 2
e.
2, 3, 2
 

 30. 

The products of the complete combustion of a hydrocarbon are carbon dioxide and water. Write a balanced chemical equation for the combustion of pentane, C5H12.
a.
C5H12(g) + 8 O2(g) ® 5 CO2(g) + 6 H2O(g)
b.
C5H12(g) ® 5 C(s) + 6 H2(g)
c.
C5H12(g) + 9 O2(g) ® 4 CO2(g) + 5 H2O(g)
d.
C5H12(g) + 11 O2(g) ® C5O10(g) + 6 H2O(g)
e.
C5H12(g) + 11 O2(g) ® 5 CO2(g) + 12 H2O(g)
 

 31. 

The complete combustion of 0.40 moles of butane gas, C4H10, will
a.
consume 0.40 mol O2 and produce 0.20 mol CO2.
b.
consume 0.80 mol O2 and produce 0.40 mol CO2.
c.
consume 1.3 mol O2 and produce 0.80 mol CO2.
d.
consume 2.6 mol O2 and produce 1.6 mol CO2.
e.
consume 5.2 mol O2 and produce 3.2 mol CO2.
 

 32. 

The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced chemical equation is shown below.

P4S3(s) + O2(g) ® P4O10(s) + SO2(g)

What mass of O2 will react with 0.641 grams of P4S3?
a.
0.0466 g
b.
0.0932 g
c.
0.186 g
d.
0.372 g
e.
0.746 g
 

 33. 

What is a correct method for determining how many grams of oxygen react with 1.00 gram of pentane?

C5H12(g) + 8 O2(g) ® 5 CO2(g) + 6 H2O(g)
a.
1.00 g C5H12 45finals07online_files/i0340000.jpg45finals07online_files/i0340001.jpg45finals07online_files/i0340002.jpg=
b.
1.00 g C5H12 45finals07online_files/i0340003.jpg45finals07online_files/i0340004.jpg45finals07online_files/i0340005.jpg=
c.
1.00 g C5H12 45finals07online_files/i0340006.jpg45finals07online_files/i0340007.jpg45finals07online_files/i0340008.jpg=
d.
1.00 g C5H12 45finals07online_files/i0340009.jpg45finals07online_files/i0340010.jpg45finals07online_files/i0340011.jpg=
e.
1.00 g C5H12 45finals07online_files/i0340012.jpg45finals07online_files/i0340013.jpg45finals07online_files/i0340014.jpg=
 

 34. 

Sulfur trioxide is made from the reaction of sulfur dioxide and oxygen. How many grams of SO3 can be made from the reaction of 3.00 g SO2 with 2.02 g O2?

2 SO2(g) + O2(g) ® 2 SO3(g)
a.
2.53 g
b.
3.75 g
c.
5.02 g
d.
5.05 g
e.
10.1 g
 

 35. 

Under certain conditions the reaction of ammonia with excess oxygen will produce a 38.2% yield of NO. How many grams of NH3 must be reacted with excess oxygen to yield 17.5 g of NO?

4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6 H2O(g)
a.
3.79 g
b.
9.93 g
c.
26.0 g
d.
32.2 g
e.
45.8 g
 

 36. 

A 2.000 g mixture of CaCO3 and CaO is heated. The CaCO3 decomposes to CaO and CO2. What was the mass percentage of CaCO3 in the mixture if the mass after heating is 1.809 g?
a.
17.8%
b.
21.7%
c.
43.4%
d.
78.3%
e.
95.5%
 

 37. 

If 0.10 mole of each of the following compounds is dissolved to a volume of 1.0 L in water, which one will have the highest concentration of dissolved ions?
a.
HF
b.
NaOH
c.
MgSO4
d.
Al(NO3)3
e.
CaI2
 

 38. 

Which of the following compounds is a weak acid?
a.
H3PO4
b.
HI
c.
HBr
d.
HClO4
e.
H2SO4
 

 39. 

What are the spectator ions in the reaction between aqueous perchloric acid and aqueous potassium hydroxide?
a.
H+, ClO4-, K+, and OH-
b.
H+ and OH-
c.
K+ and ClO4-
d.
H+ and ClO4-
e.
K+ and OH-
 

 40. 

Write a net ionic equation for the reaction of aqueous acetic acid and aqueous potassium hydroxide.
a.
CH3CO2H(aq) + KOH(aq) ® K+(aq) + CH3CO2-(aq) + H2O(l)
b.
CH3CO2H(aq) + KOH(aq) ® KCH3CO2(aq) + H2O(l)
c.
H+(aq) + OH-(aq) ® H2O(l)
d.
CH3CO2H(aq) + OH-(aq) ® CH3CO3H2-(aq)
e.
CH3CO2H(aq) + OH-(aq) ® CH3CO2-(aq) + H2O(l)
 

 41. 

Write a balanced equation for the reaction of aqueous solutions of baking soda and acetic acid.
a.
NaHCO3(aq) + CH3CO2H(aq) ® NaCH3CO2(aq) + H2O( l) + CO2(g)
b.
2 NaHCO3(aq) + CH3CO2H(aq) ® 2 Na2CO3(aq) + CH4(aq) + 2H2O( l) + CO2(g)
c.
NaHCO3(aq) + CH3CO2H(aq) ® H2CO3(s) + NaCH3CO2(aq)
d.
NaHCO3(aq) + CH3CO2H(aq) ® NaOH(aq) + CH3CO2H(aq) + CO2(g)
e.
NaHCO3(aq) + CH3CO2H(aq) ® CH4(aq) + 2 CO2(g) + O2(g) + NaOH(aq)
 

 42. 

Which of the following are oxidation-reduction reactions?

1.
Zn(s) + CuSO4(aq) ® ZnSO4(aq) + Cu(s)
2.
Pb(ClO4)2(aq) + 2 KI(aq) ® PbI2(s) + 2 NaClO4(aq)
3.
CaCO3(s) ® CO2(g) + CaO(s)
a.
1 only
b.
2 only
c.
1 and 2
d.
1 and 3
e.
2 and 3
 

 43. 

If 5.00 mL of 0.314 M KOH is diluted to exactly 125 mL with water, what is the concentration of the resulting solution?
a.
5.02 ´ 10-4 M
b.
1.26 ´ 10-2 M
c.
0.127 M
d.
0.281 M
e.
7.85 M
 

 44. 

What is the pH of 0.27 M HNO3?
a.
0.57
b.
1.31
c.
1.86
d.
2.70
e.
13.43
 

 45. 

A 25.00 mL sample of NaOH is titrated with 17.13 mL of 0.3150 M HCl. What is the concentration of the NaOH solution?
a.
0.001360 M
b.
0.1233 M
c.
0.2158 M
d.
0.4597 M
e.
0.7356 M
 

 46. 

Assuming the following reaction proceeds in the forward direction,

Ni2+(aq) + Cr(s) ® Ni(s) + Cr2+(aq)
a.
Ni2+(aq) is oxidized and Cr(s) is reduced.
b.
Ni2+(aq) is oxidized and Ni(s) is reduced.
c.
Ni(s) is oxidized and Ni2+(aq) is reduced.
d.
Cr(s) is oxidized and Cr2+(aq) is reduced.
e.
Cr(s) is oxidized and Ni2+(aq) is reduced.
 

 47. 

The following reaction occurs spontaneously.

3 Cu2+(aq) + 2 Fe(s) ® 2 Fe3+(aq) + 3 Cu(s)

Write the balanced oxidation half-reaction.
a.
2 Fe(s) ® 2 Fe3+(aq) + 6 e-
b.
2 Fe(s) + 6 e- ® 2 Fe3+(aq)
c.
3 Cu2+(aq) + 6 e- ® 3 Cu(s)
d.
3 Cu2+(aq) ® 3 Cu(s) + 6 e-
e.
3 Cu(s) ® 3 Cu2+(aq) + 6 e-
 

 48. 

Write a balanced half-reaction for the reduction of ClO3-(aq) to Cl2(g) in an acidic solution.
a.
2 ClO3-(aq) + 6 H+(aq) + 10 e- ® Cl2(g) + 6 OH-(aq)
b.
2 ClO3-(aq) + 12 H+(aq) + 5 e- ® Cl2(g) + 6 H2O(l)
c.
2 ClO3-(aq) + 10 e- ® Cl2(g) + 6 H2O(l) + 3 O2(g)
d.
2 ClO3-(aq) + 12 H+(aq) + 10 e- ® Cl2(g) + 6 H2O(l)
e.
2 ClO3-(aq) + 18 H+(aq) ® Cl2(g) + 6 H3O+(aq)
 

 49. 

Write a balanced half-reaction for the reduction of permanganate ion, MnO4-, to MnO2 in a basic solution.
a.
MnO4-(aq) + 4 OH-(aq) + 3 e- ® MnO2(s) + 2 H2O(l) + 2 O2(g)
b.
MnO4-(aq) + 2 OH-(aq) + 3 e- ® MnO2(s) + 2 HO2(aq)
c.
MnO4-(aq) + 3 e- ® MnO2(s) + O2(g)
d.
MnO4-(aq) + 2 H+(aq) + 3 e- ® MnO2(s) + 2 OH-(aq)
e.
MnO4-(aq) + 2 H2O(l) + 3 e- ® MnO2(s) + 4 OH-(aq)
 

 50. 

Write a balanced chemical equation for the following reaction in an acidic solution.

Cr2O72-(aq) + Br-(aq) ® Cr3+(aq) + Br2(aq)
a.
Cr2O72-(aq) + 2 Br-(aq) ® 2 Cr3+(aq) + Br2(aq)
b.
Cr2O72-(aq) + 6 Br-(aq) + 14 H+(aq) ® 3 Br2(aq) + 2 Cr3+(aq) + 7 H2O(l)
c.
Cr2O72-(aq) + 2 Br-(aq) + 14 H+(aq) ® 2 Cr3+(aq) + Br2(aq) + 7 H2O(l)
d.
Cr2O72-(aq) + 2 Br-(aq) + 7 H+(aq) ® 2 Cr3+(aq) + Br2(aq) + 7 OH-(aq)
e.
Cr2O72-(aq) + 6 Br-(aq) + 7 H+(aq) ® 2 Cr3+(aq) + 3 Br2(aq) + 7 OH-(aq)
 

 51. 

Of the following types of energy, which are classified as kinetic energy?

1.
thermal energy
2.
mechanical energy
3.
electrical energy
a.
1 only
b.
2 only
c.
3 only
d.
2 and 3
e.
1, 2, and 3
 

 52. 

Specific heat capacity is
a.
the quantity of heat needed to change 1.00 g of a substance by 1.00 K.
b.
the mass of a substance that 1.00 J of energy will heat by 1.00 K.
c.
the mass of a substance that 1.00 cal of energy will heat by 1.00 K.
d.
the temperature change undergone when 1.00 g of a substance absorbs 4.184 J.
e.
the quantity of heat required to melt 4.184 g of a substance.
 

 53. 

If the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will experience the smallest temperature change?

Metal
Specific Heat Capacity (J/g·K)
Al
0.897
Au
0.129
Cu
0.385
Fe
0.449
K
0.753
a.
Al
b.
Au
c.
Cu
d.
Fe
e.
K
 

 54. 

How much energy is required to change the temperature of 21.5 g Cu from 27.0 °C to 88.1 °C? The specific heat capacity of copper is 0.385 J/g·K.
a.
223 J
b.
506 J
c.
641 J
d.
729 J
e.
3.41 ´ 103 J
 

 55. 

If 50.0 g H2O at 13.6 °C is combined with 85.0 g H2O at 93.7 °C, what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g·K.
a.
26.1 °C
b.
40.0 °C
c.
56.1 °C
d.
64.0 °C
e.
80.1 °C
 

 56. 

Calculate the amount of heat required to change 50.0 g ice at -20.0 °C to steam at 135 °C. (Heat of fusion = 333 J/g; heat of vaporization = 2260 J/g; specific heat capacities: ice = 2.09 J/g·K, liquid water = 4.18 J/g·K, steam = 1.84 J/g·K)
a.
4.18 kJ
b.
32.4 kJ
c.
78.8 kJ
d.
135 kJ
e.
156 kJ
 

 57. 

45.0 g of ice at -12.0 °C is mixed with 256 g of water at 31.4 °C. What is the final temperature of the mixture? (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.09 J/g·K, liquid water = 4.184 J/g·K)
a.
-1.6 °C
b.
0.0 °C
c.
13.9 °C
d.
21.0 °C
e.
25.8 °C
 

 58. 

The heat of vaporization of benzene, C6H6, is 30.8 kJ/mol at its boiling point of 80.1 °C. How much heat is required to vaporize 128 g benzene at its boiling point?
a.
4.04 kJ
b.
18.8 kJ
c.
19.3 kJ
d.
50.5 kJ
e.
4.04 ´ 103 kJ
 

 59. 

Calculate DE for the system in which a gas absorbs 31 J of heat and does 18 J of work on the surroundings?
a.
-49 J
b.
-13 J
c.
+13 J
d.
+31 J
e.
+49 J
 

 60. 

Determine DH for the following reaction,

N2(g) + 3 H2(g) ® 2 NH3(g)

given the thermochemical equations below.

N2(g) + O2(g) ® 2 NO(g) DH = +180.8 kJ
4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6 H2O(g) DH = -906.2 kJ
2 H2(g) + O2(g) ® 2 H2O(g) DH = -483.6 kJ
a.
-1209.0 kJ
b.
-1189.0 kJ
c.
-756.5 kJ
d.
-241.8 kJ
e.
-91.5 kJ
 

 61. 

Calculate 45finals07online_files/i0620000.jpg for sulfur dioxide,

S(s) + O2(g) ® SO2(g)

given the thermochemical equations below.

2 S(s) + 3 O2(g) ® 2 SO3(g) DH° = -791.5 kJ
2 SO2(g) + O2(g) ® 2 SO3(g) DH° = -197.9 kJ
a.
-296.8 kJ/mol
b.
-395.7 kJ/mol
c.
-494.7 kJ/mol
d.
-593.6 kJ/mol
e.
-989.4 kJ/mol
 

 62. 

Which of the following chemical equations corresponds to the standard molar enthalpy of formation of N2O?
a.
NO(g) + 1/2 N2(g) ® N2O(g)
b.
N2(g) + 1/2 O2(g) ® N2O(g)
c.
2N(g) + O(g) ® N2O(g)
d.
N2(g) + O(g) ® N2O(g)
e.
2 N2(g) + O2(g) ® 2 N2O(g)
 

 63. 

The standard enthalpy change for the combustion of 1 mole of benzene is -3267.4 kJ.

C6H6(l) + 15/2 O2(g) ® 6 CO2(g) + 3 H2O(l)

Calculate 45finals07online_files/i0640000.jpg for benzene based on the following standard molar enthalpies of formation.

molecule
45finals07online_files/i0640001.jpg (kJ/mol)
CO2(g)
-393.5
H2O(l)
-285.8
a.
-6485.8 kJ
b.
-3946.7 kJ
c.
-3218.4 kJ
d.
+49.0 kJ
e.
+2588.1 kJ
 

 64. 

The standard molar enthalpy of formation of ClF3 is -405 kJ.

1/2 Cl2(g) + 3/2 F2(g) ® ClF3(g)

The bond energies of Cl2 and F2 are 242 kJ and 155 kJ/mol, respectively. Calculate the energy of an Cl-F bond.
a.
8 kJ/mol
b.
87 kJ/mol
c.
207 kJ/mol
d.
253 kJ/mol
e.
802 kJ/mol
 

 65. 

When heated, azomethane decomposes into nitrogen gas and ethane gas.

CH3N=NCH3(g) ® N2(g) + C2H6(g)

Bond
Bond Energy (kJ/mol)
Bond
Bond Energy (kJ/mol)
C-H
413
N-N
163
C-N
305
N=N
418
C-C
346
N45finals07online_files/i0660000.jpgN
945

Using average bond energies, calculate the enthalpy of reaction.
a.
-611 kJ
b.
-527 kJ
c.
-429 kJ
d.
-313 kJ
e.
-263 kJ
 

 66. 

What shell contains a total of 9 orbitals?
a.
n = 1
b.
n = 2
c.
n = 3
d.
n = 4
e.
n = 5
 

 67. 

How many nodal planes exist for a 2p orbital?
a.
0
b.
1
c.
2
d.
3
e.
4
 

 68. 

Which of the following diagrams represent d-orbitals?

45finals07online_files/i0690000.jpg
a.
(I) only
b.
(II) only
c.
(III) only
d.
(IV) only
e.
(I) and (IV)
 

 69. 

How many electrons can be described by the following quantum numbers: n = 4, l = 3, ml = -2, ms = +1/2?
a.
0
b.
1
c.
2
d.
3
e.
6
 

 70. 

Which element has the electron configuration [Ar]3d104s1?
a.
Cu
b.
Zn
c.
Ga
d.
Ag
e.
Co
 

 71. 

What is the electron configuration for a lead atom?
a.
[Xe]6s26p2
b.
[Kr]5d106s26p2
c.
[Xe]4f145d106s26p2
d.
[Xe]5d106s26p2
e.
[Kr]4d104f145d2
 

 72. 

Which element has the following electron configuration?

45finals07online_files/i0730000.jpg
a.
Br
b.
Se
c.
S
d.
Cl
e.
Ge
 

 73. 

What 3- ion has the following ground state electron configuration?

45finals07online_files/i0740000.jpg
a.
oxide ion
b.
nitride ion
c.
sodium ion
d.
aluminum ion
e.
phosphide ion
 

 74. 

What 2+ ion has the following ground state electron configuration?

45finals07online_files/i0750000.jpg
a.
Ni2+
b.
Co2+
c.
Ca2+
d.
Cu2+
e.
Mn2+
 

 75. 

Which group of the periodic table of elements forms only 2+ ions?
a.
group 1A
b.
group 2A
c.
group 7B
d.
group 7A
e.
group 8A
 

 76. 

For an atom of a main group element, the number of valence electrons is equal to
a.
its number of core electrons.
b.
the principle quantum number of its outer shell.
c.
its period number.
d.
its group number.
e.
eight minus its group number.
 

 77. 

A silicon atom has ____ valence electrons.
a.
0
b.
2
c.
4
d.
6
e.
10
 

 78. 

Which of the following statements are CORRECT?

1.
Ionic bonds form when one or more valence electrons are transferred from one atom to another.
2.
Covalent bonds involve sharing of electrons between atoms.
3.
Ionic bond formation is always exothermic; covalent bond formation is always endothermic.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
1, 2, and 3
 

 79. 

How many lone-pair electrons are on the carbon atom in CO2?
a.
0
b.
1
c.
2
d.
3
e.
4
 

 80. 

Use VSEPR theory to predict the molecular geometry of H3O+.
a.
trigonal-pyramidal
b.
trigonal-planar
c.
bent
d.
T-shaped
e.
linear
 

 81. 

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of the nitrite ion, NO2-.
a.
The electron-pair geometry is linear, the molecular geometry is linear.
b.
The electron-pair geometry is trigonal-planar, the molecular geometry is bent.
c.
The electron-pair geometry is trigonal-planar, the molecular geometry is linear.
d.
The electron-pair geometry is tetrahedral, the molecular geometry is bent.
e.
The electron-pair geometry is tetrahedral, the molecular geometry is linear.
 

 82. 

Which of the following is a correct Lewis structure for ozone, O3?

45finals07online_files/i0830000.jpg
a.
1
b.
2
c.
3
d.
4
e.
5
 

 83. 

Which of the following is a correct Lewis structure for N2O?

45finals07online_files/i0840000.jpg
a.
1
b.
2
c.
3
d.
4
e.
5
 

 84. 

Which of the following are possible Lewis structures for C2H6O?

45finals07online_files/i0850000.jpg
a.
1
b.
2
c.
3
d.
2 and 3
e.
1, 2, and 3
 

 85. 

Which of the following is a correct Lewis structure for the phosphate ion?

45finals07online_files/i0860000.jpg
a.
1
b.
2
c.
3
d.
4
e.
5
 

 86. 

What is the bond angle in N2O?
a.
90°
b.
107°
c.
109.5°
d.
120°
e.
180°
 

 87. 

How many sigma (s) bonds and pi (p) bonds are in acetic acid?

45finals07online_files/i0880000.jpg
a.
six s and one p
b.
six s and two p
c.
seven s and one p
d.
eight s and zero p
e.
eight s and one p
 

 88. 

How many sigma (s) bonds and pi (p) bonds are in formaldehyde, H2CO?
a.
one s, one p
b.
two s, two p
c.
three s, one p
d.
three s, two p
e.
four s, one p
 

 89. 

What is the hybridization of the central oxygen atom in ozone, O3?
a.
sp
b.
sp2
c.
sp3
d.
sp3d
e.
sp3d2
 

 90. 

What is the hybridization of the central atom in a molecule with a trigonal-planar geometry?
a.
sp
b.
sp2
c.
sp3
d.
sp3d
e.
sp3d2
 

 91. 

What is the molecular geometry around a central atom that is sp3 hybridized and has one lone electron-pair?
a.
bent
b.
linear
c.
trigonal-planar
d.
trigonal-pyramidal
e.
trigonal-bipyramidal
 

 92. 

Which of the underlined atoms (C1, C2, N, and O) are sp2 hybridized?

45finals07online_files/i0930000.jpg
a.
C1 and C2
b.
C1, N, and O
c.
N and O
d.
O and C2
e.
O only
 

 93. 

If the volume of a confined gas is quadrupled while its temperature remains constant, what change will be observed?
a.
The pressure of the gas will decrease to 1/4 its original value.
b.
The pressure of the gas will quadruple.
c.
The density of the gas will decrease to 1/2 its original value.
d.
The average velocity of the molecules will quadruple.
e.
The average velocity of the molecules will double.
 

 94. 

Avogadro's hypothesis states that equal volumes of gases under the same conditions of temperature and pressure have equal ____.
a.
densities
b.
particle velocities
c.
molar masses
d.
numbers of particles
e.
masses
 

 95. 

Which of the following relationships are true for gases?

1.
The number of moles of a gas is directly proportional to its volume (at constant pressure).
2.
The pressure of a gas is inversely proportional to its temperature in Kelvins (at constant volume).
3.
The volume of a gas is directly proportional to its pressure (at constant temperature).
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
2 and 3
 

 96. 

The pressure in a 20.0 L flask is 0.512 atm at 72 °C. How many moles of gas are in the flask? (R = 0.08206 L·atm/mol·K)
a.
0.0297 mol
b.
0.142 mol
c.
0.276 mol
d.
0.362 mol
e.
1.73 mol
 

 97. 

At 453 K and 755 mm Hg, what volume of N2 will react completely with 22.2 L H2 to produce NH3?

N2(g) + 3 H2(g) ® 2 NH3(g)
a.
7.40 L
b.
14.8 L
c.
22.2 L
d.
44.4 L
e.
66.6 L
 

 98. 

Which of the following are postulates of kinetic-molecular theory of gases?

1.
The distance between gas molecules is large in comparison to their size.
2.
Gas molecules are in constant, random motion.
3.
The kinetic energy of gas particles is proportional to the Kelvin temperature.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
1, 2, and 3
 

 99. 

If a gas effuses 1.618 times faster than Kr, what is its molar mass?
a.
18.02 g/mol
b.
28.01 g/mol
c.
32.01 g/mol
d.
51.79 g/mol
e.
65.88 g/mol
 

 100. 

Non-ideal behavior for a gas is most likely to be observed under conditions of
a.
high temperature and low pressure.
b.
high temperature and high pressure.
c.
low temperature and low pressure.
d.
standard temperature and pressure.
e.
low temperature and high pressure.
 



 
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