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CHEMISTRY– 2nd SEMESTER EXAM REVIEW
STRATEGY: Start by reading through your notes to refresh your memory on these topics. Then, use this
review sheet as a starting point to identify the areas on which you need to spend more study time. For those
areas, go back to homework assignments, quizzes, and reviews to practice more problems. These questions are
only samples and do not include specific examples of how vocabulary and other conceptual information might
appear in a multiple-choice or other format. More recent material will be represented in a greater number of
questions. Nomenclature is a component of the exam that is not covered on this review sheet. Please consult
your notes.
FORMAT:
 Questions will include multiple-choice and matching. (100 questions)
 A Chemistry Helper and one 3 x 5 index card (double sided) may be used on the final.
 Please complete these questions on a separate sheet of paper (15 pts.)
Bonding and Molecular Geometry
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The shape of the methane molecule (CH4) is called ____.
What is a typical characteristic of an ionic compound?
Experimental evidence suggests that the H-C-H bond angles in ethene, C2H4, are ____ degrees.
What causes hydrogen bonding?
According to the VSEPR theory, molecules adjust their shapes to keep ____ as far apart as possible.
Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen:
a) carbon, or
b) oxygen?
A molecule with a single covalent bond is: a) CO2, or b) Cl2?
A bond formed between a silicon atom and an oxygen atom is likely to be a(n) ____ bond.
Which of the following diatomic molecules is joined (seemingly) by a double covalent bond:
a) O2, or b) N2?
What causes water molecules to have a bent shape, according to the VSEPR theory?
Which of these elements does not exist as a diatomic molecule: a) Ne, or b) F?
Which of the following elements can form diatomic molecules held together by triple covalent bonds:
a) fluorine, or b) nitrogen?
Which of the following covalent bonds is the most polar:
a) H-F, or b) H-N?
What is thought to cause the disperson forces?
What are the weakest attractions between molecules called?
Why do atoms share electrons in covalent bonds?
What is the shape of a molecule with a triple bond?
Which of the forces of molecular attraction is the weakest:
a) hydrogen bonding, or
b)
dispersion forces?
In which of the following compounds is the octet expanded to include 12 electrons: a) PCl5, or b) SF6?
What causes dipole interactions?
How many electrons does carbon need to gain in order to obtain a noble-gas electron configuration?
How many covalent bonds are in a covalently bonded molecule containing 1 phosphorus atom and 3
chlorine atoms?
How many unshared pairs of electrons does the nitrogen atom in ammonia possess?
Gases
24.
25.
26.
27.
28.
Charles’s law states that ____.
As the temperature of a fixed volume of a gas increases, the pressure will ____.
Which gas law can be used to calculate the number of moles of a contained gas?
If a sealed syringe is plunged into cold water, in which direction will the syringe piston slide?
An ideal gas CANNOT be ____.
29. Boyle’s law states that ____.
30. Which of the following atoms would have the greatest velocity if each atom had the same kinetic energy?
a) ammonia, or b) hydrogen
31. The tendency of molecules to move from high concentration toward areas of lower concentration is called
____.
32. What happens to the pressure of a gas inside a container if the temperature of the gas decreases?
33. Which of the following gases will effuse the most rapidly?
a) chlorine, or b) hydrogen
34. Under what conditions of temperature and pressure is the behavior of a real gas most like that of an ideal
gas?
35. The volume of a gas is doubled while the temperature is held constant. So, how does the gas pressure
change?
36. What does the ideal gas law allow a scientist to calculate that the other gas laws do not?
37. How is the ideal gas law usually written?
38. The combined gas law relates which items together?
39. If a balloon is squeezed, what happens to the pressure of the gas inside the balloon?
40. Which of the following gases is the best choice for inflating a balloon that must remain inflated for a long
period of time: a) argon, or b) hydrogen?
41. At low temperatures and pressures, how does the volume of a real gas compare with the volume of an ideal
gas under the same conditions?
42. If the volume of a container of gas is reduced, what will happen to the pressure inside the container?
43. In general, for a gas at a constant volume, the pressure of the gas is ____ proportional to its Kelvin
temperature.
44. At high pressures, how does the volume of a real gas compare with the volume of an ideal gas under the
same conditions?
45. Why does the pressure inside a container of gas increase if more gas is added to the container?
46. Why is a gas easier to compress than a liquid or a solid?
47. The gaseous product of a reaction is collected in a 25.0 L container at 27 oC. The pressure in the container
is 300.0 kPa and the gas has a mass of 96.0 g. How many moles of the gas are in the container?
48. A balloon filled with helium has a volume of 30.0 L at a pressure of 100 kPa and a temperature of 15.0 oC.
What will the volume of the balloon be if the temperature is increased to 80.0 oC and the pressure remains
constant?
49. The volume of a gas is 250 mL at 340.0 kPa pressure. What will the volume be when the pressure is reduced
to 50.0 kPa, assuming the temperature remains constant?
50. A gas occupies a volume of 140 mL at 35.0 oC and 97 kPa. What is the volume of the gas at STP?
51. A gas has a volume of 590 mL at a temperature of -55.0 oC. What volume will the gas occupy if the
temperature changes to 30.0 oC?
52. What is the pressure exerted by 32 g of O2 in a 22.0 L container at 30.0 oC?
53. A gas has a pressure of 710 kPa at 227 oC. What will its pressure be at 27 oC, if the volume does not
change?
54. Use Graham’s law to calculate how much faster fluorine gas (F2) will effuse than chlorine gas (Cl2). Use the
molar mass of F2 = 38.0; the molar mass of Cl2 = 70.9.
55. A gas storage tank has a volume of 3.5 x 105 m3 when the temperature is 27 oC and the pressure is 101 kPa.
What is the new volume of the tank if the temperature drops to -10 oC and the pressure drops to 95 kPa?
56. A 10 g mass of krypton occupies 15.0 L at a pressure of 210 kPa. Find the volume of the krypton when the
pressure is increased to 790 kPa.
57. How many moles of N2 are in a flask with a volume of 250 mL at a pressure of 300.0 kPa and a temperature
of 300.0 K?
Thermochemistry
58. What would likely happen (how would it feel) if you were to touch the flask in which an endothermic
reaction were occurring?
59. Standard conditions of temperature and pressure for a thermochemical equation are __ and __kPa.
60. What is the definition for heat of solution?
Hess’s law makes it possible to ___.
If heat is released by a chemical system, an equal amount of heat will be ____.
By what quantity must the heat capacity (J/oC) of an object be divided to obtain the specific heat (J/goC) of
that material?
64. When energy is changed from one form to another, ____.
65. What happens to the energy produced by burning gasoline in a car engine?
66. How can the enthalpy change be determined for a reaction in an aqueous solution?
67. A process that absorbs heat is called a(n) ____ process.
68. What does the symbol ΔH stand for?
69. During a phase change, the temperature of a substance ____.
70. The amount of heat needed to melt one mole of a solid at a constant temperature is called ____.
71. Using a table that lists standard heats of formation, you can calculate the change in enthalpy for a given
chemical reaction. The change is equal to ____.
72. A piece of metal is heated, then submerged in cool water. The temperature of the water ____ and the
temperature of the metal ____.
73. The amount of heat released by the complete burning of 1 mole of a substance is the ____.
74. The ΔHsoln is a value that is ____.
75. In an exothermic reaction, the energy stored in the chemical bonds of the reactants is ____ than the energy
stored in the bonds of the products.
76. The amount of heat involved in the synthesis of 1 mole of compound from its elements, with all substances
in their standard states at 25 oC, is called ____.
77. Which of the following substances has the highest specific heat:
a) alcohol, or b) water?
78. On what principle does calorimetry depend?
79. The specific heat capacity of graphite is 0.71 J/g oC. Calculate the energy required to raise the temperature
of 450 g of graphite by 16 oC.
80. Consider a 79 g chunk of ice (ΔHfus = 6.0 kJ/mol) in a beaker immersed in a water bath. To produce just
enough heat to melt the ice, how many moles of solid NaOH (ΔHsoln = -445.1 kJ/mol) must you dissolve in
the water bath?
81. How much heat is required to raise the temperature of 6.5 x 102 g of aluminum by 30 oC? (specific heat of
aluminum = 0.21 cal/g oC)
82. How many joules are there in 125 calories? (1 cal = 4.184 J)
83. How much heat is required to melt 4.6 mol of NaCl (ΔHfus = 30.2 kJ/mol) at its melting point?
84. A substance releases 296 kJ of heat as 1.60 mol condenses from a gas into a liquid. What is the molar heat
of vaporization of the substance?
85. When 34.0 g of methanol (CH3OH) is burned, 954 kJ of energy is produced. What is the heat of combustion
(in kJ/mol) for methanol?
86. If 150 g of iron absorbs 2,000 cal of heat, what will be the change in temperature? (specific heat of iron =
0.11 cal/g oC)
87. If you supply 36 kJ of heat, how many moles of ice at 0 oC can be melted, heated to its boiling point, and
completely boiled away?
Use the following information:
ΔHvap = 40.5 kJ/mol
Specific heatwater = 0.0753 kJ/mol oC
ΔHfus = 6.0 kJ/mol
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States of Matter
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According to the kinetic theory, collisions between molecules in a gas ____.
Compared to the melting points of ionic compounds, the melting points of molecular solids tend to be ____.
What is the key difference between a liquid and a gas?
How does the atmospheric pressure at altitudes below sea level compare with atmospheric pressure at sea
level?
92. Which are the first particles to evaporate from a liquid?
93. The average kinetic energy of the particles of a substance is directly proportional to ____.
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What causes gas pressure in a container, such as a helium balloon?
When the vapor pressure of a liquid is equal to the atmospheric pressure, the liquid ____.
The escape of molecules from the surface of a liquid is known as ____.
What is the value of one standard atmosphere of pressure in kilopascals?
Which of the following will evaporate the fastest: a) water at 20 oC, or b) water at 40 oC?
Which statement is NOT true, according to the kinetic theory:
a) there is no attraction between
particles of a gas, or
b) only particles of matter in the gaseous state are in constant motion?
100.
Which states of matter can flow?
101.
Which of the following statements is part of the kinetic theory: a) the particles in a gas move rapidly, or
b) the particles in a gas are relatively far apart?
102.
What instrument is normally used to measure atmospheric pressure?
103.
If energy is added to a boiling liquid, what happens to the temperature of the liquid?
104.
The average kinetic energy of water molecules is greatest in: a) steam at 110 oC, or b) liquid water at
373 K?
105.
Standard conditions when working with gases are defined as ____ oC and ____ kPa.
106.
What is the pressure (in kPa) when a liquid is boiling at its normal boiling point?
107.
What happens to the rate of evaporation of a liquid as the liquid is cooled?
108.
What is the SI unit of pressure?
109.
Which of the following best describes the motion of the particles in a piece of steel: a) none are moving,
or b) all are moving?
110.
With which temperature scale is temperature directly proportional to average kinetic energy?
111.
Water could be made to boil at 105 oC instead of 100 oC by ____.
112.
Why does a liquid’s rate of evaporation increase when the liquid is heated?
113.
What happens to the temperature of a liquid as it evaporates?
114.
The smallest group of particles in a crystal that retains the shape of the crystal is called ____.
115.
What happens to the average kinetic energy of the particles in a sample of matter as the temperature of
the sample is increased?
116.
The temperature at which the motion of particles theoretically ceases is ____.
117.
Particles in a gas are best described as ____ spheres with ____ volume.
118.
At what temperature (in K) do particles theoretically have no kinetic energy?
119.
What is the pressure (in atm) at the normal boiling point of water?
120.
What is a pressure of 622 mm Hg equal to in atmospheres?
121.
The vapor pressure of 10 mL of ethanol at 20 oC is 5.85 kPa. What is the vapor pressure of 20 mL of
ethanol at the same temperature?
122.
What is a pressure of 0.520 atm equal to in mm of Hg?
Kinetics and Equilibrium
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Energy that is available to do work is called ____.
____ is defined as the number of atoms, ions, or molecules that react in a given time to form products.
What is the name of the minimum energy that colliding particles must have in order to react?
What is the arrangement of atoms at the peak of an energy barrier?
At equilibrium, what is the rate of production of reactants compared with the rate of production of
products?
What is the equilibrium constant expression for the following reaction: C(s) + O2(g) ↔ CO2(g)
Which of the following is true about the combustion of carbon: a) the reaction is spontaneous, or
b) entropy decreases?
The rate of a chemical reaction normally ____ as reactant concentration increases.
Why does a higher concentration make a reaction faster?
The amount of disorder in a system is measured by its ____.
Entropy measures ____
What happens to a reaction at equilibrium when more reactant is added to the system?
Which reaction results in the greatest increase in entropy:
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A → B, or b) A → 2B
If a reaction has an equilibrium constant (Keq) just greater than 1, how do we interpret that information?
A catalyst works by ____.
If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction?
What is the effect of adding more water to the following equilibrium reaction: CO2 + H2O ↔ H2CO3
In an endothermic reaction at equilibrium, what is the effect of raising the temperature?
The energy that is available to do work in a reaction is called ____.
What is the numerical value (+ or -) of Gibbs free-energy change for a spontaneous reaction?
At what stage of a reaction do atoms have the highest energy?
Which of the following systems has the highest entropy:a) 10 mL of water at 50 oC, or
b) 10 mL of
water at 100 oC?
What happens to a catalyst in a reaction?
Is the melting of ice at a temperature above 0 oC:
endothermic, or b) exothermic?
Consider the reaction:
N2(g) + 3H2(g) ↔ 2NH3(g)
What is the effect of decreasing the volume on the contained gases?
Spontaneous reactions always ____ free energy.
Why does a higher temperature cause a reaction to go faster?
What 2 factors determine whether or not a reaction is spontaneous?
If a reaction is reversible, what are the relative amounts of reactant and product at the end of the
reaction?
What physical state of nitrogen has the highest entropy?
What is another name for the catalysts in your body?
In an equilibrium reaction with a Keq of 1 x 108, the ____ are favored.
Which of the following explains why melting of ice is spontaneous at room temperature and pressure:
a) it is accompanied by an increase in entropy, or b) it is accompanied by an increase in energy?
The Keq of a reaction is 4 x 10-7. At equilibrium, the ____ are favored.
Which change would shift the following reaction to the right:
4HCl(g) + O2(g) ↔ 2Cl2(g) + 2H2O(g) a) decrease of pressure, or
b) increase of pressure?
In which of these systems is the entropy decreasing:
a) salt dissolving in water, or
b) a liquid cooling?
Acids and Bases
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An indicator is what type of compound?
In a titration, when the number of moles of hydrogen ions equals the number of moles of hydroxide ions,
what is said to have happened?
Which base is strong, but never concentrated? a) sodium hydroxide, or b) magnesium hydroxide
When an acid reacts with a base, what compounds are produced?
Which type of solution is one with a pH of 8?
With solutions of strong acids and strong bases, the word strong refers to ____.
What is the charge on the hydronium ion?
Which of the following represents a Bronsted-Lowry conjugate acid-base pair: a) SO32- and SO2, or
b) NH41+ and NH3?
Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base? a) water, or b)
hydrochloric acid
What type of acid (monoprotic, diprotic, etc.) is sulfuric acid?
Know the properties of a base.
Know the properties of an acid.
What is an acid according to Arrhenius?
In the reaction of aluminum bromide with sodium bromide, which compound is the Lewis acid?
Which of these is an Arrhenius base: a) LiOH, or b) CH3COOH?
What is pH?
In a neutral solution, the [H1+] is ____.
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The acid dissociation constant (Ka) for an acid dissolved in water is equal to the ____ x ____.
A 0.12 M solution of an acid that ionizes only slightly in solution would be termed ____.
In the reaction:
CO32- + H2O ↔ HCO31- + OH1-, the carbonate ion (CO32-) is acting as a(n) ____.
What is transferred between a conjugate acid-base pair?
What are the acids in the following: CN1- + H2O ↔ HCN + OH1-?
A Lewis acid is a substance that can ____.
If the hydrogen ion concentration of a solution is 1 x 10-10 M, is the solution acidic, alkaline, or neutral?
The process of adding a known amount of solution of known concentration to determine the
concentration of another solution is called ____.
If the hydroxide-ion concentration is 1 x 10-12 M, what is the pH of the solution? (Use significant
figures guideline.)
What is the hydrogen-ion concentration if the pH is 3.7?
If the hydrogen-ion concentration is 1 x 10-13 M, what is the pOH of the solution?
A 0.500 M solution of a weak acid, HX, is only partially ionized. The [H1+] was found to be 4.02 x 10-3
M. Find the dissociation constant (Ka) for this acid.
What is the pH if the hydrogen-ion concentration is 6.8 x 10-7 M?
What is the pH of a solution with a concentration of 0.01 M HCl?
If the hydroxide-ion concentration is 1 x 10-10 M, what is the pH of the solution?
If [OH1-] = 1 x 10-4 M, what is the pH of the solution?
If the hydrogen ion concentration is 1 x 10-7 M, what is the pH of the solution?
What is the pH when the hydrogen ion concentration is 7.0 x 10-3 M?
Solutions
*** Use the Ch.16 test review to study for this section. This material should be relatively fresh as you took the
exam very recently.