e /j l / inceton f...!J. Review .....-
Cracking the
Chemistry Subject Test 2013-2014 Edition Theodore Silver, M.D. and the Staff of The Princeton Review Princeton Review.com
Random House. Inc. New York
Contents Part I:
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Orientation
2
3
Part II: Subject Review
4
Introduction .. ......................................................................
3
What Are the SAT Subject Tests?.............................................
4
What Is The Princeton Review? ... ............................................
6
Point 1: Learn Chemistry the Way the Subject Test Tests It.............
7
Point 2: Approach the Test Strategically.....................................
9
What About Practice and Practice Tests? . ..................................
9
Should I Buy Practice Material from ETS?.... ...............................
9
Test Strategies . ...................................................................
11
Cracking the SAT Chemistry Test..............................................
12
Strategy #1 : Study the Right Stuff in the Right Way......................
15
Strategy #2: D o the Easy Ones First..........................................
15
Strategy #3: Take a Guess! .....................................................
16
Strategy #4: Making Associations (Type A . B. and C Questions).......
16
Strategy #5: Rephrase the Question (Type A and C Questions)........
17
Strategy #6: Avoiding the Temptation Trap .................................
22
Strategy #7: Divide and Conquer..............................................
23
Strategy #8: Process of Elimination . .........................................
25
Some Basic Stuff..................................................................
27
Mass.................................................................................
28
Volume ..............................................................................
28
Density..............................................................................
29
Pressure.............................................................................
30
Energy...............................................................................
31
Temperature and Specific Heat................................................
31
How the SAT Chemistry Subject Test Will Test You on All This........
33
Summary............................................................................
37
Atoms: The Building Blocks of Matter........................................
41
Atoms and Elements . ............................................................
42
The Periodic Table ................................................................
43
Summary............................................................................
48
5
Chemical Reactions and Stoichiometry ..................................'....
49
The World of Molecules.........................................................
50
The Mole............................................................................
52
Chemical Reactions-How Molecules Are Formed. Broken Down.
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and Reformed
6
7
8
9
I
55
Stoichiometry ......................................................................
57
Thermodynamics..................................................................
58
Summary............................................................................
64
Electron Configurations and Radioactivity...................................
67
Orbitals ............................... ,..............................................
68
Electron Configurations..........................................................
70
Radioactivity and Half-Lives....................................................
75
Summary.............................................................................
80
The Periodic Table and Bonding................................................
81
The Periodic Table ................................................................
82
Some Important Periodic Trends...............................................
86
Chemical Bonding.................................................................
90
. Molecular Shapes.................................................................
95
Summary......................................................... ...... :...........
1 00
Phases: Gases, Liquids. and Solids............................................
1 03
Gases ................................................................................
1 04
Intermolecular Forces ............................................................
110
Phase Changes . ...................................................................
112
Energy and Phase Changes .....................................................
117
Summary ..... :......................................................................
1 20
Solutions............................................................................
1 23
Measuring Concentrations......................................................
1 24
Boiling Point Elevation and Freezing Point Depression....................
126
Precipitation Reactions ......... .................................................
1 27
Summary............................................................................
130
Kinetics and Equilibrium ........ .................................................
1 33
Kinetics..............................................................................
134
Chemical Equilibrium .............................................................
1 37
Summary............................................................................
1 47
.
10
vi
............................................................... 路
Contents
Acids and Bases...................................................................
149
T he Autoionization of Hp.......................................................
150
Acids and Bases...................................................................
152
Acid-Base Titrations..............................................................
1 63
Summary............................................................................
1 70
Redox and Electrochemistry ....................................................
1 73
Oxidation and Reduction ........................................................
1 74
Redox Reactions...................................................................
1 76
Electrochemistry ..................................................................
1 78
Summary...................................."..... :..................................
1 83
Organic Chemistry and Environmental Chemistry ......... :...............
1 85
Organic Chemistry ................................................................
1 86
Environmental Chemistry........................................................
1 93
Summary............................................................................
1 95
Laboratory ..........................................................................
1 97
Safety Rules........................................................................
1 98
Accuracy ............................................................................
1 98
Significant Figures ................................................................
1 98
Lab Procedures . ...................................................................
200
Laboratory Equipment ...........................................................
202
You're Ready! . .....................................................................
207
Summary............................................................................
210
Part Ill: Drill Answers and Explanations .. .........................................
211
15
Practice SAT Chemistry Subject Test 1 ......................................
235
16
Practice SAT Chemistry Subject Test 1: Answers and Explanations...
257
17
Practice SAT Chemistry Subject Test 2 ......................................
273
18
Practice SAT Chemistry Subject Test 2 : Answers and Explanations ..
295
19
Practice SAT Chemistry Subject Test 3 '. .....................................
307
20
Practice SAT Chemistry Subject Test 3: Answers and Explanations ..
327
Formula Cheat Sheet .............................................................
343
Index .................................................................................
349
About the Author..................................................................
353
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12
13
14
Part IV: T he Princeton Review Practice SAT Chemistry Subject Test and Answers and Explanations
Contents
I
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Chapter 1 Introduction The SAT Subject Tests are one-hour exams that assess a student's knowledge of a particular academic subject. Not all colleges require the subject tests, and some subject tests are more appropriate for certain students than for others. The format and content of a given test falls within certain guidelines, and you should prepare accordingly. In this chapter we will answer some basic questions about the SAT Chemistry Subject Test and how you should prepare for it .
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WHAT ARE THE SAT SUBJECT TESTS? The SAT Subject Tests are a series of tests administered by the Educational Test ing Service (ETS). Unlike the regular SAT, the SAT Subject Tests are designed to measure knowledge in very specific areas. Many colleges require that you take one or more of these tests in order to qualify for admission; but even at colleges that do not require that you take them, administrators view student performances on the tests as an important factor that contributes to the decision to grant or with hold admission. Additionally, at some schools, a high score on one or more of the tests might enable you to "place out" of certain required college courses. For example, if you do well on the SAT Chemistry Subject Test, you might be exempt from fulfilling the science requirement at one or more of the schools to which you're applying!
Which SAT Subject Tests Should I Take?
The colleges that do require you to take the SAT Subject Tests will expect you to take two or three of them. In order to find out which tests are required by the col leges to which you're applying, you can ask your guidance counselor, call the ad missions office of the colleges, or check in college guidebooks. Alternately, you can visit the College Board website at sat.collegeboard.org and use their college search engine to look up the colleges you're interested in; each school on this search en gine has a profile in which this information is provided. Once you find out which, if any, tests are required, part of your decision making is done. The next step is to find out which of the tests will show your particular strengths. After all, the SAT Subject Tests are given in a variety of subjects: Litera ture, U.S. History, World History, Biology, Chemistry, Physics, French, German, Spanish, Modern Hebrew, Italian, Latin, Japanese, Korean, Ch inese, and English Language Proficiency. You should take the tests on which you think you'd score the highest. If you're fluent in Chinese, take the SAT Chinese Test. If, however, you're most comfortable in the world of moles, atoms, and titrations, take the SAT Chemistry Test.
When Are the Tests Offered, and H ow Do I Register for Them? The SAT Subject Tests are usually administered in October, November, December, January, May, and June at test centers around the country. Since not all of the tests are offered at each administration, be sure to check the dates and details on the College Board website carefully. You'll want to take the test on a date that's as close as possible to the end of your coursework in the subject. For example, if your chemistry course ends December 21, take the January test. If it ends in May, take the test in May or June-whichever date falls the soonest after your cours� has ended.
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Cracking the SAT Chemistry S u bject Test
CRACKI N G THE SAT CHEMISTRY TEST
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The SAT Chemistry Subject Test is made up of 85 multiple-choice questions, and you have one hour to answer them. You're not allowed to use a calculator on this test, but you won't need one. The test is divided into three sections: Parts A, B, and C, and each section is made up of a different type of question. Let's take a closer look at these parts.
Part A: Classification Questions The first 20 to 25 questions you'll see on the exam fall under the category of what ETS calls classification questions. In this type of question, you'll see a list of five words or phrases lettered A through E, followed by three to five questions. But sometimes the questions aren't really questions; they're phrases. Your job is to match the phrase in the "question" with a word or phrase that appears in the list A through E. Forget about chemistry for a minute, and see how it works. Directions: Each set of lettered choices below refers to the numbered
statements or questions immediately following it. Select the one lettered choice that best fits each statement or answers each question and then fill in the corresponding oval on the answer sheet. A choice may be used once, more than once, or not at all in each set. Questions 1-4 refer to the following.
(A) (B) (C) (D) (E)
Red light Swimming pool Piano Fire engine Ocean liner
1. Musical instrument that involves keyboard outside and strings inside 2. Motor vehicle designed to assist in effort to extinguish flames 3. Sea vessel that carries passengers across large bodies of water 4.
Water-filled pit designed for recreational or athletic activities
The answers, of course, are C, D, E, and B. Now let's move on to see what the questions in Part B look like.
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Cracking the SAT Chemistry S u bject Test
Part B: Relationshi p Ana lysis Questions
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The questions that make up Part B of the exam won't ask you to decide among . choices A, B, C, D, or E. Relationship analysis questions consist of two statements with the word BECAUSE in between them. You're supposed to figure out if the statements are true or false. If both are true, you're also expected to figure out whether the word BECAUSE belongs there. Once again, forget about chemistry for a second so we can show you how the questions work. The questions in part B of the exam are numbered in a peculiar manner. This section begins with the number 101, though there are only 85 questions in the whole test!
CE? On your answer sheet
for Part 8, you' l l see
ova l s m a rked T and F for
true a n d false, but the
"because" circle i s m arked
CE, which stands for
Cause I Effect. You're looking to see if I and II
have a cause-and-effect
Directions: Each question below consists of two statements, I in the
relationship.
left-hand column and II in the right-hand column. For each question, determine whether statement I is true or false and whether statement II is true or false and fill in the corresponding T or F ovals on your answer sheet. Fill in oval CE only if statement II is a correct explanation of statement I.
101.
102.
I
If one takes a shower, one gets wet
If one walks rapidly, one will be in motion 103. A boat will sink if it fills with water 104. President Lincoln died of natural causes 105. Omaha, Nebraska, is the capital of the United States
BECAUSE
BECAUSE BECAUSE BECAUSE BECAUSE
II
the shower head releases water that falls on the individual taking the shower. automobiles burn gasoline. it is impossible for a boat to develop a leak. Lincoln was president during the Civil War. Omaha is the largest city in the entire world.
Question 101 Both statements are true, and the "because"
belongs there. You get wet in a shower because the shower pours water on you.
Question 102 Both statements are true. If you walk, you move,
and automobiles do burn gasoline. But the "because'! doesn't belong there. A walker doesn't move because automobiles burn gasoline. The statements have nothing to do with one another.
Test Strategies
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PRESSURE When test writers say "pressure," they are usually talking about (1) the force that a sample of gas in a closed container exerts on the container walls, or (2) a solid or liquid standing in an environment and the force that a gas is exerting on the walls of the environment and everything in it-including the surface of the solid or liquid. (2)
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(1 )
30
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! • So, what units do we use to express pressure? A few. There are torr, millimeters of mercury (mmHg), and atmospheres (atm): 1 torr and 1 mmHg are equal, and 760 torr (or 760 mmHg) 1 atm. =
What instruments are used to measure pressure? The barometer and the manometer. Both the barometer and manometer involve the use of the liquid metal mercury (Hg) to determine atmo spheric pressure.
Cracking the SAT Chemistry Subject Test
ENERGY
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You will have to know a few things about energy for the SAT Chemistry Subject Test. First, remember that energy exists in different forms, but is always defined as the ability to do work or transfer heat. Energy can exist as heat, light, kinet ic energy, OI chemical bond energy. When we say kinetic energy, we're talking about the energy that an object possesses by virtue of the fact that it is moving. A moving bus, train, or car has kinetic energy. When we deal with chemistry, we're usually thinking about molecules that move; moving molecules have kinetic energy. The faster molecules move, the higher their kinetic energy. What units are used to describe energy? •
calories (cal) joules (J) or kilojoules (1 kJ equals 1,000 J)
•
One calorie (1 cal) is equal to slightly more than 4 J. What instrument is used to measure energy? •
a calorimeter
Keep the following things in mind when considering energy: •
•
•
•
Kinetic energy is the energy contained in the movement of molecules. The greater the kinetic energy, the faster the move ment and the higher the temperature of the molecules. Chemical bonds contain energy. Breaking bonds requires energy; forming bonds releases energy. Heat is the transfer of kinetic energy from one thing to an other. A calorimeter measures energy.
TEMPERATURE AND SPECIFIC H EAT What exactly is heat? When you touch something warm, you feel heat, but what is that? Technically, heat is defined as the flow of energy from a body at a higher temperature to one at a lower temperature. If a particular sample of a substance experiences an increase in temperature, then you can say that particular sample has experienced an increase in heat content. So what exactly does temperature measure? Temperature measures the average kinetic energy of molecules in a sample; as the molecules in a sample move more quickly, the temperature of that sample increases.
Some Basic Stuff
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Phase Change Equilibrium Thing or Things? The principle of e q u i l i b rium would also h o l d true if more than one thing i n a system were being revers
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ibly transformed.
The principle of equilibrium does not only apply to chemical reactions but also to any system in which one thing is transforming, reversibly, into another-such as a phase change, for instance. Remember vapor pressure? Suppose water is in a sealed container, at a temperature below water's boiling point; some molecules will still gather enough kinetic energy to escape from the liquid and become gas. Then they will lose their kinetic energy-they will cool down and fall back into the container as water. Other liquid molecules gain enough kinetic energy to escape into the gas phase, and the process continues. Some liquid is converted to gas, and some gas is converted to liquid. The process is in equilibrium.
Le Chatelier's Principle The Effects of Substrate Concentration on Equilibrium Look at this equilibrium. A+B� C+D On the left side of the equilibrium equation, we find A and B. On the right side, we find C and D. A and B act together to produce C and D; meanwhile, C and D act together to produce A and B. If we add more A to the reaction system, the reaction will shift to the right, to produce more C and D at equilibrium.
�A+ B � t c + t n
If we add more B to the reaction, the reaction will shift to the right, to produce more C and D at equilibrium.
� A+ B � t c + t n Adding more A and B, of course, will also increase the production of C and D.
� � 1 40
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Cracking the SAT Chemistry Subject Test
A+B �tt C + tt D
Adding more C or more D to the system has an analogous but opposite effect.
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tt A+ ttB � C + D Think about it this way. When you add more A to the system, you're increasing the amount of reactant available to react and form products. Similarly, if you add more C or D to the system, you're increasing the amount of product available to react and form reactants. The system will adjust by moving to the left to reestab lish equilibrium. When we increase the concentration of one species on the left side of an equation, what happens to the concentration of the other species on the left side of the equa tion? Say we add more A to the system: There will be more collisions between A particles and B particles. Since we did not add any B to the system, the increased collisions among A and B particles, along with the increased production of C and 0, will tend to reduce the concentration of B at equilibrium. After equilibrium has shifted, there will be more A particles than there were before we added any more A. There will be fewer B particles than there were before we began, and there will, of course, be more C and D particles. To give you an idea of what we mean by "driving or shifting equilibrium to the right," consider this example. Suppose for the reaction, 2A(g) + B(g) � C(g), equilibrium concentrations at a particular temperature are [A] = 2 M, [B] = 6 M, and [C] = 8 M. When we �lug these into the equilibrium expression K eq
=
LB ] [2 ]2 [6 ]
=
3
_!_
·
Keq
=
[c] � [ A� J2 [� B]
we get
Now, according to Le Chatelier's principle, if we add more A into the system at equilibrium, equilibrium will shift to the right. So once equilibrium is reestab lished, the concentration of C will be greater than 8 M, and the concentration of B will be less than 6 M. Of course, the concentration of A will also be greater than before. But as long as we maintain the original temperature, K,q will stay the same. So when the new equilibrium concentrations are plugged back into the 1 equilibrium expression, it will still equal - . For instance, the new equilibrium 3 concentrations could be [A] 3 M [B] 4 M, and [C] = 12 M. The equilibrium =
,
=
concentr.ations have changed, but the Keq has not. Kinetics and Equilibrium
I
1 41
Question Type B
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I
II
109.
For any chemical reaction in dynamic equilibrium, increasing the concentration of one product will decrease the concentration of all reactants
BECAUSE
a dynamic equilibrium will shift in a direction that tends to relieve a stress imposed on it.
1 10.
When a reversible chemical reaction reaches equilibrium, concentrations of products and reactants are always equal
BECAUSE
on the right side of any equilibrium expression, the numerator and denominator are always equal.
1 1 1.
Increasing the concentration of a gaseous reactant typically increases the reaction rate
BECAUSE
the reaction rate is increased as the energy per molecular collision increases.
Kinetics and Equilibrium
I
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Question Type C (1) N/g) + 3H2 (g) ďż˝ 2NH3 (g), Ke (472 C) = 0.105 q (2) Hz (g) + 12 (g) ďż˝ 2Hl(g), Ke (448 C) = 50 q
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53. In comparing the two reactions above, performed at the indicated temperatures, which of the following is true? (A) Reaction 1 is favored in the forward direction, and reaction 2 is favored in the reverse direction. (B) Reaction 1 is favored in the reverse direction, and reaction 2 is favored in the forward direction. (C) Both reactions 1 and 2 are favored in the forward direction. (D) Both reactions 1 and 2 are favored in the reverse direction. (E) Neither reaction favors either the forward or reverse direction.
1 46
56. If the reaction given above is at equilibrium, the result of a sudden increase in the concentration of 02 will result in (A) increased concentration of S02 and decreased concentration of so3 (B) increased concentration of S02 and increased concentration of so3 (C) decreased concentration of so2 and increased concentration of S03 (D) decreased concentration of S02 and decreased concentration of so3 (E) no change in concentration of any product or reactant ,
I
58. Which of the following statements is NOT true regarding the activated complex? (A) It represents the highest energy state achieved during the course of a reaction. (B) It is not consumed during the course of a reaction. (C) It is very unstable. (D) It is formed before reactant bonds are completely broken. (E) It is formed before product bonds are completely formed. Cracking the SAT Chemistry Subject Test
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Question
Answer
Explanation
9
B
Solid KCl (potassium chloride) salt is held together by ionic bonds. The positively charged potassium ions and the negatively charged chloride ions are held together by the electrostatic force between them. Remember: The electrostatic force comes from the attraction between two atoms that differ very significantly in electronegativity and is very strong.
10
c
Fluorine (F) has 7 electrons in its second shell, 1 short of a complete stable octet.
11
B
Aluminum (Al) has 3 electrons in its third shell, 2 in the s subshell, and � in the p subshell.
12
A
13
D
A positively charged sodium ion (Na+) has given up the 1 electron from its third shell, so it has the same electron configuration as a neon atom, which has a completed second shell. D is correct. Titaniu� (Ti) is a transition metal and has 2 electrons in its 3d subshell.
14
c
2 The solution containing Cu + ion will be blue. Most solutions containing salts of transition metals are distinctly colored because the d subshell electrons of transition metals absorb and emit electromagnetic radiation in the visible spectrum.
15
A
HN03 is a strong acid, so it will dissociate completely in solution. That means that a 0.01-molar solution of HN03 will have a hydrogen ion concentration of 0.01molar. pH is -log[H ], and -log(0.01) 2, so the pH of the solution will be 2. =
16
c
Freezing point depression is a colligative property, which means that it depends only on the number of particles in a solution, not on their identities. For every unit of 2 Cu(N03) 2 in a solution, 3 particles are produced: 1 Cu + and 2 N03-. For all of the other choices, each unit in solution produces only 2 particles.
17
B
HC2H 3 02 (acetic acid) is a weak acid, which means that it does not dissociate significantly in solur.ion. That means that most of the particles present in the acetic acid solution will be undissociated HC2 H 3 02 • All of the other solutions listed contain solutes that dissociate completely.
18
E
The specific heat capacity is the amount of energy that must be added to raise the temperature ·of 1 gram of a substance 1°C. If a substance has a large specific heat capacity, it can absorb a large amount of heat while undergoing a small temperature change.
19
c
The value of the Gibbs free energy change (8G) for a reaction indicates the spontaneity of the reaction. If 8G is neg�tive, then the forward reaction is spontaneous. If 8G is positive, then the reaction is not spontaneous. If 8G is zero, then the forward reaction is at equilibrium. Practice SAT Chemistry S u bject Test 2: Answers and Explanations
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Question
Answer
Explanation
20
A
The value of the enthalpy change (b.H) for a reaction indicates whether the reaction is endothermic or exothermic. If b.H is positive, energy is absorbed over the course of the reaction, and the reaction is endothermic. If b.H is negative, energy is released over the course of the reaction, and the reaction is exothermic.
21
B
Electronegativity indicates how strongly an atom will attract the electrons of another atom in a bond. The larger the electronegativity difference between two atoms in a'bond, the more polar the bond will be.
22
A
Ionization energy is the energy required to remove an electron from an atom or ion. The larger the ionization energy, the more difficult it is to remove the electron. The atomic number, which determines the identity of an element, is equal to the number of protons in the atom's nucleus. The mass number is equal to the sum of the protons and neutrons in an atom's nucleus. Atoms with the same atomic numher and different mass numbers are isotopes.
路
23
0
PART B Question
1 01
F, T
1 02
T, T, CE
1 03
T, T, CE
' 1 04
298
I
Answer
T, T
Explanation
Divide and conquer. The first statement is false. Neither the electrons nor the ions in an ionic solid are free to move about, so an ionic solid will not conduct electricity. The second statement is true. An ionic solid is composed of positive and negative ions joined in a lattice structure by electrostatic forces. The first statement is false and the second statement is true. Divide and conquer. Both statements are true. Since the oxygen atoms are identical to each other, they will have equal attraction for the bonding electrons. The second statement is a correct explanation for the first statement, so we fill in the CE oval. Divide and conquer. Both statements are true. Ice has stronger intermolecular forces and more stability than water, so when water freezes, energy is released. The second statement is a correct explanation of the first statement, so fill in the CE oval. Divide and conquer. The first statement is true . For an aqueous solution at 25掳C, pH + pOH = 14. The second statement is also true. The definition of a buffer is a solution whose pH is not easily changed by the addition ofan acid or base. Now, ask yourself if the word "because" relates the two statements. The second statement does not explain the first statement, so do not fill in the CE oval.
Cracking the SAT Chemistry Subject Test
CHEMISTRY SUBJECT TEST 3- Continued PLEASE GO TO THE SPECIAL SECTION LABELED CHEMIST�Y AT THE LOWER RIGHT HAND CORNER OF THE ANSWER SHEET YOU ARE WORKING ON AND ANSWER QUESTIONS 101-1 16 ACCORDING TO THE FOLLOWING DIRECTIONS. Part B Directions: Each question below consists of two statements, I in the left-hand column and II in the right-hand
column. For each question, determine whether statement I is true or false lmd whether statement II is true or false,
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and fill in the corresponding T or F ovals on your answer sheet. Fill in oval CE only if statement II is a correct explanation of statement I.
EXAMPLES:
n
I
EX 1. H2 S04 is a strong acid
BECAUSE
H2 S(\ contains sulfu&
EX 2. An atom of oxygen is electrically neutral
BECAUSE
an oxygen atom contains an equal number of protons and electrons.
SAMPLE ANSWERS EX 1
EX 2
I
II
CE
• 0• 00 • 0 • 0-
II
I
101.
Transition metal compounds are often colored
BECAUSE
they frequently possess partially filled d orbitals.
102.
Chemical reactions slow down with lower temperature
BECAUSE
the energy barrier for the formation of products decreases with decreasing temperature.
103.
Exothermic reactions absorb heat
BECAUSE
breaking covalent bonds always requires energy.
104.
The solubility of gases in liquids does not depend upon pressure
BECAUSE
the vapor pressure of a substance is independent of external pressure.
105.
MgO has a high melting point
BECAUSE
highly charged ions result in strong ionic forces and high latti�e energies.
106.
The ground state electron configuration orbitals of elemental Cu is [Ar] 4s13d1 0
BECAUSE
completely half-filled and filled d bestow special electronic stabilization.
107.
Isotopes of a particular element have nearly identicat chemical behavior
BECAUSE
they have identical electron configurations.
108.
In an electrochemical cell, the electrode that is the site of reduction is called the anode
BECAUSE
oxidation always occurs at the cathode.
G O ON TO THE N EXT PAGE
Practice SAT Chemistry S u bject Test 3
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CHEMISTRY SUBJECT TEST 3- Continued Questions 61-64 refer to the following data at standard conditions.
Dull gray solid with white oxide coating
Dissolved with bubbles of clear gas
Dissolved with bubbles of clear gas
Unknown metal #2
Solid; lustrous, smooth silver-gray surface
No reaction
Dissolved with bubbles of orange gas
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Unknown metal #1
6 1 . Unknown metal #1 could be (A) (B) (C) (D) (E)
mercury copper zinc iron silver
62. Unknown metal #2 could be (A) (B) (C) (D) (E)
carbon copper zinc sodium silver
63. The addition of dilute HCl to unknown metal #1 produced a transparent gas. What is the likely identity of this gas? (A) (B) (C) (D) (E)
Cďż˝ H2 02 co2 N02
64. The addition of dilute HN03 to unknown metal #2 produced an orange gas. What is the likely identity of this gas? (A) (B) (C) (D) (E)
Cl2 H2 02 co2 N02
65. Which of the following solutions is the product of the neutralization reaction between 10 ml 0.2 M KOH and 10 ml 0.2 M HI ? (A) (B) (C) (D) (E)
0. 1 M Kl3 0. 1 M KI 0.2 M KI 0.4 M KI 0.4 M HOH
66. Which of the following is true regarding an Ne atom with a mass number of 20 and an 02- ion with a mass number of 16 ? (A) They contain the same number of protons. (B) They contain the same number of neutrons. (C) They contain the same number of protons plus neutrons. (D) They are isoelectronic. (E) They are isomers. 67. Which of the following statements is NOT correct regarding chemical catalysts? (A) They are not consumed during the chemical reaction. (B) They cannot make nonspontaneous reactions occur. (C) They do not have to be the same phase as the reactant molecules. (D) They shift equilibrated reactions to the product's side. (E) Enzymes are biological catalysts. GO ON TO THE N EXT PAGE
Practice SAT Chemistry S u bject Test 3
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HOW TO SCORE TH E PRINCETON REVIEW PRACTICE SAT CHEMISTRY SUBJECT TEST b
When you take the real exam, the proctors will collect your test booklet and bubble sheet and send your answer sheet to New Jersey, where a computer looks at the pattern of filled-in ovals on your answer sheet and gives you a score. We couldn't include even a small computer with this book, so we are providing this more primitive way of scoring your exam.
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Determining Your Score STEP l
Using the answer key on the next page, determine how many questions you got right and how many you got wrong on the test. Remember: Questions that you do not answer don't count as either right or wrong answers.
STEP 2
List the number of right answers here.
(A)
STEP 3
List the number of wrong answers here. Now divide that number by 4. (Use a calculator if you're feeling particularly lazy.)
(B)
__ T
STEP 4
Subtract the number of wrong answers divided by 4 from the number of correct answers. Round this score to the nearest whole number. This is your raw score.
(A)
--
STEP 5
To determine your real score, take the number from Step 4 above, and look it up in the left column of the Score Conversion Table on page 325; the correspond足 ing score on the right is your score on the exam.
4 = (C)
_____
- (C)
Practice SAT Chemistry S u bject Test 3
I
323
ANSWERS TO THE PRINCETON REVtEW PRACTICE SAT CHEMISTRY SUBJECT TEST 3 Question Number
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1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 1 1. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45 .
324
I
Correct Answer E A B B c
A E
D B
D c
B A B c
D
E
D
A B c
E
D
B B A c
c
D
A A E
D
A
D B E
D D
B E B A
D E
Cracking the SAT Chemistry S u bject Test
Right
Wrong
Question Number
Correct Answer
46. 47. 48. 49. 50 . ... 51. 52. 53. 54. 55. 56. 57. 58. 59. 60. 61. 62. 63.
A
64 . .
65. 66. 67 . 68. 69.
101. 1 02. 103. 1 04. 105 . 1 06. 107 . 108. 1 09. 1 1 0. 1 1 1. 1 1 2. 1 13. 1 14. 1 15. 1 1 6.
Right
B
c
c
A E
D
A
D
B E A
D
E A c
E B E B
D D
A c
T, T, T, F F, T F, T T, T, T, T, T, T, F, F T, T, T, F F, T T, T F, F T, T, T, F T, T
CE
CE CE CE CE
CE
Wrong
THE PRI N CETON REVIEW PRACTICE SAT CHEMISTRY SUBJECT TEST SCORE CONVERSION TABLE
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Raw Score Scaled 45 44 43 42 41
620 620 610 610 600
40 39 38 37 36
590 590 580 580 570
35 34 33 32 31
560 560 550 550 540
30 29 28 27 26
530 530 520 520 520
25 24 23 22 21
5 10 510 500 500 490
20 19 18 17 16
480 480 470 470 460
15 14 13 12 11
450 450 440 440 430
10 9 8 7 6
420 420 410 410 400
Score
Practice SAT Chemistry S u bject Test 3
I
325