The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Tuesday, June 24, 2003 — 9:15 a.m. to 12:15 p.m., only
This is a test of your knowledge of chemistry. Use that knowledge to answer all
questions in this examination. Some questions may require the use of the Reference
Tables for Physical Setting/Chemistry. You are to answer all questions in all parts of
this examination according to the directions provided in the examination booklet.
Your answer sheet for Part A and Part B–1 is the last page of this examination
booklet. Turn to the last page and fold it along the perforations. Then, slowly and
carefully, tear off your answer sheet and fill in the heading.
The answers to the questions in Part B–2 and Part C are to be written in your
separate answer booklet. Be sure to fill in the heading on the front of your answer
booklet.
Record the number of your choice for each Part A and Part B–1 multiple-choice
question on your separate answer sheet. Write your answers to the Part B–2 and
Part C questions in your answer booklet. All work should be written in pen, except for
graphs and drawings, which should be done in pencil. You may use scrap paper to
work out the answers to the questions, but be sure to record all your answers on your
separate answer sheet and in your answer booklet.
When you have completed the examination, you must sign the statement printed
at the end of your separate answer sheet, indicating that you had no unlawful
knowledge of the questions or answers prior to the examination and that you have
neither given nor received assistance in answering any of the questions during the
examination. Your answer sheet and answer booklet cannot be accepted if you fail to
sign this declaration.
Notice. . .
A four-function or scientific calculator and a copy of the Reference Tables for Physical
Setting/Chemistry must be available for your use while taking this examination.
DO NOT OPEN THIS EXAMINATION BOOKLET UNTIL THE SIGNAL IS GIVEN.
1 The atomic number of an atom is always equal
to the number of its
(1) protons, only
(2) neutrons, only
(3) protons plus neutrons
(4) protons plus electrons
2 Which subatomic particle has no charge?
(1) alpha particle (3) neutron
(2) beta particle (4) electron
3When the electrons of an excited atom return to
a lower energy state, the energy emitted can
result in the production of
(1) alpha particles (3) protons
(2) isotopes (4) spectra
4 The atomic mass of an element is calculated
using the
(1) atomic number and the ratios of its naturally
occurring isotopes
(2) atomic number and the half-lives of each of
its isotopes
(3) masses and the ratios of its naturally occur-
ring isotopes
(4) masses and the half-lives of each of its iso-
topes
5 The region that is the most probable location of
an electron in an atom is
(1) the nucleus (3) the excited state
(2) an orbital (4) an ion
6 Which is a property of most nonmetallic solids?
(1) high thermal conductivity
(2) high electrical conductivity
(3) brittleness
(4) malleability
7 Alpha particles are emitted during the radioac-
tive decay of
(1) carbon-14 (3) calcium-37
(2) neon-19 (4) radon-222
8 Which is an empirical formula?
(1) P
2
O
5
(3) C
2
H
4
(2) P
4
O
6
(4) C
3
H
6
9 Which substance can be decomposed by a
chemical change?
(1) Co (3) Cr
(2) CO (4) Cu
10 The percent by mass of calcium in the compound
calcium sulfate (CaSO
4
) is approximately
(1) 15% (3) 34%
(2) 29% (4) 47%
11 What is represented by the dots in a Lewis
electron-dot diagram of an atom of an element
in Period 2 of the Periodic Table?
(1) the number of neutrons in the atom
(2) the number of protons in the atom
(3) the number of valence electrons in the atom
(4) the total number of electrons in the atom
12 Which type of chemical bond is formed
between two atoms of bromine?
(1) metallic (3) ionic
(2) hydrogen (4) covalent
13 Which of these formulas contains the most polar
bond?
(1) H–Br (3) H–F
(2) H–Cl (4) H–I
P.S./Chem.–June ’03 [2]
Part A
Answer all questions in this part.
Directions (1–35): For each statement or question, write on the separate answer sheet the number of the
word or expression that, of those given, best completes the statement or answers the question. Some questions
may require the use of the Reference Tables for Physical Setting/Chemistry.
14 According to Table F, which of these salts is
least soluble in water?
(1) LiCl (3) FeCl
2
(2) RbCl (4) PbCl
2
15 Which of these terms refers to matter that could
be heterogeneous?
(1) element (3) compound
(2) mixture (4) solution
16 In which material are the particles arranged in a
regular geometric pattern?
(1) CO
2
(g) (3) H
2
O()
(2) NaCl(aq) (4) C
12
H
22
O
11
(s)
17 Which change is exothermic?
(1) freezing of water
(2) melting of iron
(3) vaporization of ethanol
(4) sublimation of iodine
18 Which type of change must occur to form a
compound?
(1) chemical (3) nuclear
(2) physical (4) phase
19 Which formula correctly represents the compo-
sition of iron (III) oxide?
(1) FeO
3
(3) Fe
3
O
(2) Fe
2
O
3
(4) Fe
3
O
2
20 Given the reaction:
PbCl
2
(aq) + Na
2
CrO
4
(aq) →
PbCrO
4
(s) + 2 NaCl(aq)
What is the total number of moles of NaCl
formed when 2 moles of Na
2
CrO
4
react com-
pletely?
(1) 1 mole (3) 3 moles
(2) 2 moles (4) 4 moles
21 Which hydrocarbon is saturated?
(1) propene (3) butene
(2) ethyne (4) heptane
22 Which statement correctly describes an
endothermic chemical reaction?
(1) The products have higher potential energy
than the reactants, and the ∆H is negative.
(2) The products have higher potential energy
than the reactants, and the ∆H is positive.
(3) The products have lower potential energy
than the reactants, and the ∆H is negative.
(4) The products have lower potential energy
than the reactants, and the ∆H is positive.
23 At standard pressure when NaCl is added to
water, the solution will have a
(1) higher freezing point and a lower boiling
point than water
(2) higher freezing point and a higher boiling
point than water
(3) lower freezing point and a higher boiling
point than water
(4) lower freezing point and a lower boiling
point than water
24 Which element has atoms that can form single,
double, and triple covalent bonds with other
atoms of the same element?
(1) hydrogen (3) fluorine
(2) oxygen (4) carbon
25 Which compound is an isomer of pentane?
(1) butane (3) methyl butane
(2) propane (4) methyl propane
26 In which substance does chlorine have an
oxidation number of +1?
(1) Cl
2
(3) HClO
(2) HCl (4) HClO
2
27 Which statement is true for any electrochemical
cell?
(1) Oxidation occurs at the anode, only.
(2) Reduction occurs at the anode, only.
(3) Oxidation occurs at both the anode and the
cathode.
(4) Reduction occurs at both the anode and the
cathode.
P.S./Chem.–June ’03 [3] [OVER]
28 Given the equation:
2 Al + 3 Cu
2+
→ 2 Al
3+
+ 3 Cu
The reduction half-reaction is
(1) Al → Al
3+
+ 3e
–
(3) Al + 3e
–
→ Al
3+
(2) Cu
2+
+ 2e
–
→ Cu (4) Cu
2+
→ Cu + 2e
–
29 Which 0.1 M solution contains an electrolyte?
(1) C
6
H
12
O
6
(aq) (3) CH
3
OH(aq)
(2) CH
3
COOH(aq) (4) CH
3
OCH
3
(aq)
30 Which equation represents a neutralization
reaction?
(1) Na
2
CO
3
+ CaCl
2
→ 2 NaCl + CaCO
3
(2) Ni(NO
3
)
2
+ H
2
S → NiS + 2 HNO
3
(3) NaCl + AgNO
3
→ AgCl + NaNO
3
(4) H
2
SO
4
+ Mg(OH)
2
→ MgSO
4
+ 2 H
2
O
31 An Arrhenius acid has
(1) only hydroxide ions in solution
(2) only hydrogen ions in solution
(3) hydrogen ions as the only positive ions in
solution
(4) hydrogen ions as the only negative ions in
solution
32 Which type of radioactive emission has a posi-
tive charge and weak penetrating power?
(1) alpha particle (3) gamma ray
(2) beta particle (4) neutron
33 Which substance contains metallic bonds?
(1) Hg()(3) NaCl(s)
(2) H
2
O()(4)C
6
H
12
O
6
(s)
34 What is the name of the process in which the
nucleus of an atom of one element is changed
into the nucleus of an atom of a different ele-
ment?
(1) decomposition (3) substitution
(2) transmutation (4) reduction
Note that question 35 has only three choices.
35 A catalyst is added to a system at equilibrium. If
the temperature remains constant, the activa-
tion energy of the forward reaction
(1) decreases
(2) increases
(3) remains the same
P.S./Chem.–June ’03 [4]
36 The nucleus of an atom of K-42 contains
(1) 19 protons and 23 neutrons
(2) 19 protons and 42 neutrons
(3) 20 protons and 19 neutrons
(4) 23 protons and 19 neutrons
37 What is the total number of electrons in a
Cu
+
ion?
(1) 28 (3) 30
(2) 29 (4) 36
38 Which list of elements is arranged in order of
increasing atomic radii?
(1) Li, Be, B, C (3) Sc, Ti, V, Cr
(2) Sr, Ca, Mg, Be (4) F, Cl, Br, I
39 Which isotope is most commonly used in the
radioactive dating of the remains of organic
materials?
(1)
14
C(3)
32
P
(2)
16
N(4)
37
K
40 According to Reference Table H, what is the
vapor pressure of propanone at 45°C?
(1) 22 kPa (3) 70. kPa
(2) 33 kPa (4) 98 kPa
41 The freezing point of bromine is
(1) 539°C (3) 7°C
(2) –539°C (4) –7°C
42 Hexane (C
6
H
14
) and water do not form a solution.
Which statement explains this phenomenon?
(1) Hexane is polar and water is nonpolar.
(2) Hexane is ionic and water is polar.
(3) Hexane is nonpolar and water is polar.
(4) Hexane is nonpolar and water is ionic.
43 The potential energy diagram below represents
a reaction.
Which arrow represents the activation energy of
the forward reaction?
(1) A (3) C
(2) B (4) D
44 Given the formulas of four organic compounds:
Which pair below contains an alcohol and an
acid?
(1) a and b (3) b and d
(2) a and c (4) c and d
Potential Energy
B
C
A
Reaction Coordinate
D
Part B–1
Answer all questions in this part.
Directions (36–50): For each statement or question, write on the separate answer sheet the number of the
word or expression that, of those given, best completes the statement or answers the question. Some questions
may require the use of the Reference Tables for Physical Setting/Chemistry.
P.S./Chem.–June ’03 [5] [OVER]
( a )
( b )
H
H
HH
C C
H
H
C
O
H
H
HH
C C
H
OH
C
O
( c )
H
H
HOH
C C
H
H
( d )
H
C
H
H
H
H
C C
O
H
H
C
H
P.S./Chem.–June ’03 [6]
46 A diagram of a chemical cell and an equation are
shown below.
When the switch is closed, electrons will flow
from
(1) the Pb(s) to the Cu(s)
(2) the Cu(s) to the Pb(s)
(3) the Pb
2+
(aq) to the Pb(s)
(4) the Cu
2+
(aq) to the Cu(s)
47 Which ion has the same electron configuration
as an atom of He?
(1) H
–
(3) Na
+
(2) O
2–
(4) Ca
2+
48 A student was given four unknown solutions.
Each solution was checked for conductivity and
tested with phenolphthalein. The results are
shown in the data table below.
Based on the data table, which unknown solu-
tion could be 0.1 M NaOH?
(1) A (3) C
(2) B (4) D
49 In the reaction
239
93
Np →
239
94
Pu + X, what does X
represent?
(1) a neutron (3) an alpha particle
(2) a proton (4) a beta particle
Note that question 50 has only three choices.
50 As carbon dioxide sublimes, its entropy
(1) decreases
(2) increases
(3) remains the same
Salt
bridge
Pb(s) Cu(s)
Switch
1.0 M
Pb
2+
(aq)
1.0 M
Cu
2+
(aq)
Voltmeter
Pb(s) + Cu
2 +
(aq)
V
Pb
2 +
(aq) + Cu(s)
45 Which type of reaction is represented by the equation below?
Note:
n and n are very large numbers equal to about 2000.
(1) esterification (3) saponification
(2) fermentation (4) polymerization
H
H
CC
H
H
n
H
H
C
n
H
H
C
Solution Conductivity
Color with
Phenolphthalein
A
Good Colorless
B
Poor Colorless
C
Good Pink
D
Poor Pink
P.S./Chem.–June ’03 [7] [OVER]
Part B–2
Answer all questions in this part.
Directions (51–63): Record your answers in the spaces provided in your answer booklet. Some questions
may require the use of the Reference Tables for Physical Setting/Chemistry.
Base your answers to questions 51 and 52 on the electron configuration table shown below.
51 What is the total number of valence electrons in an atom of electron configuration X? [
1]
52 Which electron configuration represents the excited state of a calcium atom? [
1]
Base your answers to questions 53 and 54 on the information below.
Given: Samples of Na, Ar, As, Rb
53 Which two of the given elements have the most similar chemical properties? [
1
]
54 Explain your answer in terms of the Periodic Table of the Elements. [
1]
Base your answers to questions 55 and 56 on the information below.
Diethyl ether is widely used as a solvent.
55 In the space provided in your answer booklet, draw the structural formula for diethyl
ether. [
1]
56 In the space provided in your answer booklet, draw the structural formula for an
alcohol that is an isomer of diethyl ether. [
1]
Element
Electron
Configuration
X
2–8–8–2
Y
2–8–7–3
Z
2–8–8
P.S./Chem.–June ’03 [8]
Base your answers to questions 57 and 58 on the information below.
Two chemistry students each combine a different metal with
hydrochloric acid. Student A uses zinc, and hydrogen gas is readily pro-
duced. Student B uses copper, and no hydrogen gas is produced.
57 State one chemical reason for the different results of students A and B. [
1]
58 Using Reference Table J, identify another metal that will react with hydrochloric acid
to yield hydrogen gas. [
1]
59 Given the reaction between two different elements in the gaseous state:
Box A below represents a mixture of the two reactants before the reaction occurs.
The product of this reaction is a gas. In Box B provided in your answer booklet, draw
the system after the reaction has gone to completion, based on the Law of
Conservation of Matter. [
2]
60 As a neutral sulfur atom gains two electrons, what happens to the radius of the atom? [
1]
61 After a neutral sulfur atom gains two electrons, what is the resulting charge of the ion? [
1]
62 a In the space provided in your answer booklet, calculate the heat released when
25.0 grams of water freezes at 0°C. Show all work. [
1]
b Record your answer with an appropriate unit. [
1]
63 State one difference between voltaic cells and electrolytic cells. Include information
about both types of cells in your answer. [
1]
Box A
System Before Reaction
+ +
P.S./Chem.–June ’03 [9] [OVER]
Part C
Answer all questions in this part.
Directions (64–79): Record your answers in the spaces provided in your answer booklet. Some questions
may require the use of the Reference Tables for Physical Setting/Chemistry.
Base your answers to questions 64 and 65 on the diagram below, which shows a piston confining a gas in a
cylinder.
64 Using the set of axes provided in your answer booklet, sketch the general relationship
between the pressure and the volume of an ideal gas at constant temperature. [
1]
65 The gas volume in the cylinder is 6.2 milliliters and its pressure is 1.4 atmospheres. The
piston is then pushed in until the gas volume is 3.1 milliliters while the temperature
remains constant.
a In the space provided in your answer booklet, calculate the pressure, in atmospheres,
after the change in volume. Show all work. [
1]
b Record your answer. [
1]
66 A student recorded the following buret readings during a titration of a base with an acid:
a In the space provided in your answer booklet, calculate the molarity of the KOH.
Show all work. [
1]
b Record your answer to the correct number of significant figures. [
1]
67 John Dalton was an English scientist who proposed that atoms were hard, indivisible
spheres. In the modern model, the atom has a different internal structure.
a Identify one experiment that led scientists to develop the modern model of the atom. [1]
b Describe this experiment. [
1]
c State one conclusion about the internal structure of the atom, based on this experi-
ment. [
1]
Standard 0.100 M HCl Unknown KOH
Initial reading
9.08 mL 0.55 mL
Final reading
19.09 mL 5.56 mL
Base your answers to questions 68 through 73 on the information below and on your knowledge of chemistry.
Nuclear Waste Storage Plan for Yucca Mountain
In 1978, the U.S. Department of Energy began a study of Yucca Mountain which is
located 90 miles from Las Vegas, Nevada. The study was to determine if Yucca Mountain
would be suitable for a long-term burial site for high-level radioactive waste. A three-
dimensional (3-D) computer scale model of the site was used to simulate the Yucca
Mountain area. The computer model study for Yucca Mountain included such variables as:
the possibility of earthquakes, predicted water flow through the mountain, increased rain-
fall due to climate changes, radioactive leakage from the waste containers, and increased
temperatures from the buried waste within the containers.
The containers that will be used to store the radioactive waste are designed to last 10,000
years. Within the 10,000-year time period, cesium and strontium, the most powerful
radioactive emitters, would have decayed. Other isotopes found in the waste would decay
more slowly, but are not powerful radioactive emitters.
In 1998, scientists discovered that the compressed volcanic ash making up Yucca Mountain
was full of cracks. Because of the arid climate, scientists assumed that rainwater would move
through the cracks at a slow rate. However, when radioactive chlorine-36 was found in rock
samples at levels halfway through the mountain, it was clear that rainwater had moved
quickly down through Yucca Mountain. It was only 50 years earlier when this chlorine-36
isotope had contaminated rainwater during atmospheric testing of the atom bomb.
Some opponents of the Yucca Mountain plan believe that the uncertainties related to the
many variables of the computer model result in limited reliability of its predictions.
However, advocates of the plan believe it is safer to replace the numerous existing radio-
active burial sites around the United States with the one site at Yucca Mountain. Other
opponents of the plan believe that transporting the radioactive waste to Yucca Mountain
from the existing 131 burial sites creates too much danger to the United States. In 2002,
after years of political debate, a final legislative vote approved the development of Yucca
Mountain to replace the existing 131 burial sites.
68 State one uncertainty in the computer model that limits the reliability of this
computer model. [
1]
69 Scientists assume that a manufacturing defect would cause at least one of the waste
containers stored in the Yucca Mountain repository to leak within the first 1,000 years.
State one possible effect such a leak could have on the environment near Yucca
Mountain. [
1]
70 State one risk associated with leaving radioactive waste in the 131 sites around the
country where it is presently stored. [
1]
71 If a sample of cesium-137 is stored in a waste container in Yucca Mountain, how much
time must elapse until only of the original sample remains unchanged? [
1]
72 The information states “Within the 10,000-year time period, cesium and strontium, the
most powerful radioactive emitters, would have decayed.” Use information from
Reference Table N to support this statement. [
1]
73 Why is water flow a crucial factor in deciding whether Yucca Mountain is a suitable
burial site? [
1]
1
32
P.S./Chem.–June ’03 [10]
P.S./Chem.–June ’03 [11]
Base your answers to questions 74 through 76 on the information below.
A student wishes to investigate how the reaction rate changes with a change in concen-
tration of HCl(aq).
Given the reaction: Zn(s) + HCl(aq) → H
2
(g) + ZnCl
2
(aq)
74 Identify the independent variable in this investigation. [1]
75 Identify one other variable that might affect the rate and should be held constant
during this investigation. [
1]
76 Describe the effect of increasing the concentration of HCl(aq) on the reaction rate and
justify your response in terms of collision theory. [
1]
Base your answers to questions 77 through 79 on the information below.
A truck carrying concentrated nitric acid overturns and spills its contents. The acid drains
into a nearby pond. The pH of the pond water was 8.0 before the spill. After the spill, the
pond water is 1,000 times more acidic.
77 Name an ion in the pond water that has increased in concentration due to this spill. [
1]
78 What is the new pH of the pond water after the spill? [
1]
79 What color would bromthymol blue be at this new pH? [
1]
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Tuesday, June 24, 2003 — 9:15 a.m. to 12:15 p.m., only
ANSWER SHEET
Student . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Sex: ■■ Male ■■ Female Grade . . . . . . . . . . .
Teacher . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . School . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
Record your answers to Part A and Part B–1 on this answer sheet.
Write your answers to Part B–2 and Part C in your answer booklet.
The declaration below should be signed when you have completed the examination.
I do hereby affirm, at the close of this examination, that I had no unlawful knowledge of the questions or answers prior to
the examination and that I have neither given nor received assistance in answering any of the questions during the examination.
Signature
Tear Here
Tear Here
Part A
1 . . . . . . . . . . . . 13 . . . . . . . . . . . . 25 . . . . . . . . . . .
2 . . . . . . . . . . . . 14 . . . . . . . . . . . . 26 . . . . . . . . . . .
3 . . . . . . . . . . . . 15 . . . . . . . . . . . . 27 . . . . . . . . . . .
4 . . . . . . . . . . . . 16 . . . . . . . . . . . . 28 . . . . . . . . . . .
5 . . . . . . . . . . . . 17 . . . . . . . . . . . . 29 . . . . . . . . . . .
6 . . . . . . . . . . . . 18 . . . . . . . . . . . . 30 . . . . . . . . . . .
7 . . . . . . . . . . . . 19 . . . . . . . . . . . . 31 . . . . . . . . . . .
8 . . . . . . . . . . . . 20 . . . . . . . . . . . . 32 . . . . . . . . . . .
9 . . . . . . . . . . . . 21 . . . . . . . . . . . . 33 . . . . . . . . . . .
10 . . . . . . . . . . . . 22 . . . . . . . . . . . . 34 . . . . . . . . . . .
11 . . . . . . . . . . . . 23 . . . . . . . . . . . . 35 . . . . . . . . . . .
12 . . . . . . . . . . . . 24 . . . . . . . . . . . .
Part B–1
36 . . . . . . . . . . . . 44 . . . . . . . . . . . .
37 . . . . . . . . . . . . 45 . . . . . . . . . . . .
38 . . . . . . . . . . . . 46 . . . . . . . . . . . .
39 . . . . . . . . . . . . 47 . . . . . . . . . . . .
40 . . . . . . . . . . . . 48 . . . . . . . . . . . .
41 . . . . . . . . . . . . 49 . . . . . . . . . . . .
42 . . . . . . . . . . . . 50 . . . . . . . . . . . .
43 . . . . . . . . . . . .
Part A Score
Part B–1 Score
Tear Here
Tear Here
Maximum Student’s
Part Score Score
A35
B–1 15
B–2 15
C20
Total Written Test Score
(Maximum Raw Score: 85)
Final Score
(from conversion chart)
Raters’ Initials:
Rater 1 . . . . . . . . . . Rater 2 . . . . . . . . . . .
[a] [OVER]
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Tuesday, June 24, 2003 — 9:15 a.m. to 12:15 p.m., only
ANSWER BOOKLET
Student . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Sex: ■■ Female
Teacher . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
School . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Grade . . . . . . . . .
Answer all questions in Part B–2 and Part C. Record your answers
in this booklet.
■■ Male
51
52
53 and
54
55
Part B–2
51
52
53
54
55
For Raters
Only
56
57
58
59
60
61
[b]
56
57
58
59
60
61
For Raters
Only
Box A
System Before Reaction
Box B
System After Reaction Has
Gone to Completion
[c]
[OVER]
62a
b
63
62 a
b
63
64
65a
b
Part C
64
65 a
b
atm
Total Score
for Part B–2
For Raters
Only
[d]
66 a
b
M
67 a
b
c
68
69
70
68
69
70
For Raters
Only
66a
b
67a
b
c
[e]
71
72
73
74
75
76
77
78
79
For Raters
Only
Total Score
for Part C
71
72
73
74
75
76
77
78
79
Part B–1
36 . . . . . . . . . . . . 44 . . . . . . . . . . . .
37 . . . . . . . . . . . . 45 . . . . . . . . . . . .
38 . . . . . . . . . . . . 46 . . . . . . . . . . . .
39 . . . . . . . . . . . . 47 . . . . . . . . . . . .
40 . . . . . . . . . . . . 48 . . . . . . . . . . . .
41 . . . . . . . . . . . . 49 . . . . . . . . . . . .
42 . . . . . . . . . . . . 50 . . . . . . . . . . . .
43 . . . . . . . . . . . .
Part B–1 Score
Part A
1 . . . . . . . . . . . . 13 . . . . . . . . . . . . 25 . . . . . . . . . . .
2 . . . . . . . . . . . . 14 . . . . . . . . . . . . 26 . . . . . . . . . . .
3 . . . . . . . . . . . . 15 . . . . . . . . . . . . 27 . . . . . . . . . . .
4 . . . . . . . . . . . . 16 . . . . . . . . . . . . 28 . . . . . . . . . . .
5 . . . . . . . . . . . . 17 . . . . . . . . . . . . 29 . . . . . . . . . . .
6 . . . . . . . . . . . . 18 . . . . . . . . . . . . 30 . . . . . . . . . . .
7 . . . . . . . . . . . . 19 . . . . . . . . . . . . 31 . . . . . . . . . . .
8 . . . . . . . . . . . . 20 . . . . . . . . . . . . 32 . . . . . . . . . . .
9 . . . . . . . . . . . . 21 . . . . . . . . . . . . 33 . . . . . . . . . . .
10 . . . . . . . . . . . . 22 . . . . . . . . . . . . 34 . . . . . . . . . . .
11 . . . . . . . . . . . . 23 . . . . . . . . . . . . 35 . . . . . . . . . . .
12 . . . . . . . . . . . . 24 . . . . . . . . . . . .
Part A Score
1
3
4
3
2
3
4
1
2
2
3
4
1
1
4
1
3
4
3
2
3
4
1
1
3
4
2
3
4
2
4
1
1
2
4
4
2
3
4
3
3
1
2
2
4
3
1
1
2
1
FOR TEACHERS ONLY
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING/CHEMISTRY
Tuesday, June 24, 2003 — 9:15 a.m. to 12:15 p.m., only
SCORING KEY AND RATING GUIDE
PS–CH
Directions to the Teacher:
Refer to the directions on page 3 before rating student papers.
Part A and Part B–1
Allow 1 credit for each correct response.
[1] [OVER]
Part B–1
Directions to the Teacher
Follow the procedures below for scoring student answer papers for the Physical
Setting/Chemistry examination. Additional information about scoring is provided in the
publication Information Booklet for Administering and Scoring Regents Examinations in the
Sciences.
Use only red ink or red pencil in rating Regents papers. Do not correct the student’s
work by making insertions or changes of any kind.
On the detachable answer sheet for Part A and Part B–1, indicate by means of a check-
mark each incorrect or omitted answer. In the box provided at the end of each part, record
the number of questions the student answered correctly for that part.
At least two science teachers must participate in the scoring of each student’s responses
to the Part B–2 and Part C open-ended questions. Each of these teachers should be respon-
sible for scoring a selected number of the open-ended questions on each answer paper. No
one teacher is to score all the open-ended questions on a student’s answer paper.
Students’ responses must be scored strictly according to the Scoring Key and Rating
Guide. For open-ended questions, credit may be allowed for responses other than those
given in the rating guide if the response is a scientifically accurate answer to the question
and demonstrates adequate knowledge as indicated by the examples in the rating guide.
Complete sentences are not required. Phrases, diagrams, and symbols may be used. In the
student’s answer booklet, record the number of credits earned for each answer in the box
printed to the right of the answer lines or spaces for that question.
Fractional credit is not allowed. Only whole-number credit may be given to a response.
Units need not be given when the wording of the questions allows such omissions.
Raters should enter the scores earned for Part A, Part B–1, Part B–2, and Part C on the
appropriate lines in the box printed on the answer booklet and then should add these four
scores and enter the total in the box labeled “Total Written Test Score.” Then, the student’s
raw score should be converted to a scaled score by using the conversion chart printed at the
end of this Scoring Key and Rating Guide. The student’s scaled score should be entered in
the labeled box on the student’s answer booklet. The scaled score is the student’s final
examination score.
All student answer papers that receive a scaled score of 60 through 64 must be scored
a second time. For the second scoring, a different committee of teachers may score the stu-
dent’s paper or the original committee may score the paper, except that no teacher may
score the same open-ended questions that he/she scored in the first rating of the paper. The
school principal is responsible for assuring that the student’s final examination score is based
on a fair, accurate, and reliable scoring of the student’s answer paper.
Because scaled scores corresponding to raw scores in the conversion chart may change
from one examination to another, it is crucial that for each administration, the conversion
chart provided in the scoring key for that administration be used to determine the student’s
final score. The chart in this scoring key is usable only for this administration of the exami-
nation.
[3] [OVER]
PHYSICAL SETTING/CHEMISTRY – continued
PHYSICAL SETTING/CHEMISTRY – continued
[4]
Part B–2
Allow a total of 15 credits for this part. The student must answer all questions in this part.
51 [1] Allow 1 credit for 2.
52 [1] Allow 1 credit for Y or 2–8–7–3.
53 [1] Allow 1 credit for Na and Rb.
54 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
same number of valence electrons
Group 1
Elements in the same group (family) have similar chemical properties.
Both lose one electron when they react.
55 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
56 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
or
Allow 1 credit for a response consistent with the student’s answer to question 55.
C C CC
OHHHH
HHHH
HH
C C CC
OH
C C C
OH
C
C C OHC
C
C
C C COC
C CH
H
H
H
H
O C
H
H
H
H
H
57 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
Cu is less active than hydrogen gas.
Zn more reactive
Cu is below H
2
on the activity series and Zn is above H
2
.
58 [1] Allow 1 credit for any metal other than Zn, that is above H
2
on Table J. Acceptable responses include,
but are not limited to, these examples:
magnesium or Mg
aluminum or Al
59 [2] Allow 1 credit for correctly drawing four particles and one particle.
and
Allow 1 credit for showing any particles in a gaseous state.
Acceptable responses include, but are not limited to, this example:
60 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
gets bigger
increases
The ion is larger than the atom.
61 [1] Allow 1 credit for –2 or negative.
Box B
System After Reaction Has
Gone to Completion
PHYSICAL SETTING/CHEMISTRY – continued
[5] [OVER]
PHYSICAL SETTING/CHEMISTRY – continued
62 [2] a Allow 1 credit for a correct setup. Writing the formula in the setup is not required. Acceptable
responses include, but are not limited to, these examples:
q = mH
f
= (25.0 g)(334 J/g)
25.0(334)
b Allow 1 credit for 8350 J or 8350 joules.
or
Allow 1 credit for a response consistent with the student’s setup and that has an appropriate unit.
Note: Significant figures do not need to be shown.
63 [1] Allow 1 credit for a correct response. Students must discuss both voltaic and electrolytic cells.
Acceptable responses include, but are not limited to, these examples:
Voltaic cells produce energy; electrolytic cells consume energy.
voltaic changes chemical to electrical, electrolytic opposite
Voltaic cells involve spontaneous redox reactions; electrolytic cells involve nonspontaneous redox
reactions.
voltaic spontaneous/electrolytic not
[6]
Part C
Allow a total of 20 credits for this part. The student must answer all questions in this part.
64 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
65 [2] a Allow 1 credit for a correct setup. Writing the formula in the setup is not required. Units and sig-
nificant figures do not need to be shown. Acceptable responses include, but are not limited to,
these examples:
(6.2 mL)(1.4 atm) = (3.1 mL)(P
2
)
6.2 mL(1.4 atm)
P
2
=
3.1 mL
The volume is halved so pressure must double.
b Allow 1 credit for 2.8.
or
Allow 1 credit for a response consistent with the student’s setup.
Note: Significant figures do not need to be shown.
66 [2] a Allow 1 credit for a correct setup. Writing the formula and/or the unit in the setup is not required.
Acceptable responses include, but are not limited to, these examples:
(0.100 M)(10.01 mL)
M
KOH
=
5.01 mL
M
A
V
A
= M
B
V
B
(0.100 M)(10.01 mL) = (M
B
)(5.01 mL)
b Allow 1 credit for 0.200. The response must contain three significant figures.
or
Allow 1 credit for a response containing two or three significant figures consistent with the
student’s setup.
V
P
P
V
[7] [OVER]
PHYSICAL SETTING/CHEMISTRY – continued
67 [3] a Allow 1 credit for identifying one experiment. Acceptable responses include, but are not limited
to, these examples:
gold foil (Rutherford)
cathode rays (Thomson)
electron bombardment (Moseley)
b Allow 1 credit for a description consistent with the experiment chosen by the student. Acceptable
responses include, but are not limited to, this example:
In the gold-foil experiment, gold foil was bombarded with alpha particles. Some alpha par-
ticles were deflected.
c Allow 1 credit for stating a conclusion drawn from the experiment chosen by the student.
Acceptable responses include, but are not limited to, these examples:
The gold-foil experiment shows that an atom is mostly empty space.
An atom has a small dense core.
An atom has a positively charged center.
68 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
corrosion rates of the waste containers
the area’s vulnerability to earthquakes
climate changes that increase rainfall
69 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
pollution of fresh water in the area
adverse effects on humans, fish, and wildlife
Radioactivity would get into the food chain.
Groundwater would become contaminated.
70 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
The other sites may be in more populated areas so more people would be at risk.
Leaving radioactive waste in sites spread around the country would expose more regions to
contamination.
terrorism
71 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
any response from 150 to 152
5 half-lives
[8]
PHYSICAL SETTING/CHEMISTRY – continued
72 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
The half-life of cesium-137 is short, and the sample would almost be entirely decayed after
10,000 years.
The half-life of strontium-90 is short, and the sample would almost be entirely decayed after
10,000 years.
73 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
because water may transport the radioactive materials
cause containers to corrode
74 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
concentration of HCl
HCl(aq)
HCl
[HCl]
75 [1] Allow 1 credit for a correct response. Acceptable responses include, but are not limited to, these
examples:
temperature
surface area of Zn
amount of Zn
Zn
concentration of Zn
[Zn]
76 [1] Allow 1 credit for a response with a correct justification. Acceptable responses include, but are not
limited to, these examples:
rate ↑, more collisions
The rate will increase because the higher concentration of HCl will lead to a greater number of
collisions.
[9] [OVER]
PHYSICAL SETTING/CHEMISTRY – continued
PHYSICAL SETTING/CHEMISTRY – concluded
[10]
77 [1] Allow 1 credit for H
+
or hydrogen or H
3
O
+
or hydronium or NO
3
–
or nitrate.
78 [1] Allow 1 credit for 5. Significant figures do not need to be shown.
79 [1] Allow 1 credit for yellow.
or
Allow 1 credit for a response consistent with the student’s answer to question 78.
Regents Examination in Physical Setting/Chemistry
June 2003
Chart for Converting Total Test Raw Scores to
Final Examination Scores (Scaled Scores)
To determine the student’s final examination score, find the student’s total test raw score
in the column labeled “Raw Score” and then locate the scaled score that corresponds to that
raw score. The scaled score is the student’s final examination score. Enter this score in the
space labeled “Final Score” on the student’s answer sheet.
Raw Scaled Raw Scaled Raw Scaled Raw Scaled
Score Score Score Score Score Score Score Score
85 100 63 74 41 57 19 35
84 98 62 73 40 56 18 33
83 97 61 72 39 55 17 32
82 95 60 72 38 55 16 30
81 94 59 71 37 54 15 29
80 93 58 70 36 53 14 27
79 91 57 69 35 52 13 26
78 90 56 68 34 51 12 24
77 89 55 68 33 50 11 22
76 87 54 67 32 49 10 21
75 86 53 66 31 48 9 19
74 85 52 66 30 47 8 17
73 84 51 65 29 46 7 15
72 83 50 64 28 45 6 13
71 82 49 63 27 44 5 11
70 81 48 62 26 43 4 9
69 80 47 62 25 42 3 7
68 79 46 61 24 41 2 5
67 78 45 60 23 40 1 2
66 77 44 59 22 38 0 0
65 76 43 59 21 37
64 75 42 58 20 36
[12]
Map to Core Curriculum
June 2003 Physical Setting/ Chemistry
Question Numbers
Key Ideas Part A Part B Part C
Standard 1
Math Key Idea 1 66b,74,75
Math Key Idea 2
Math Key Idea 3
Sci. Inq. Key Idea 1 54,60,61 67
Sci. Inq. Key Idea 2
Sci. Inq. Key Idea 3 56 71,72
Eng. Des. Key Idea 1
Standard 2
Key Idea 1 40,41
Key Idea 2 68
Standard 6
Key Idea 1
Key Idea 2
Key Idea 3 77
Key Idea 4
Key Idea 5
Standard 7
Key Idea 1 69,70,73
Key Idea 2
Standard 4 Process Skills
Key Idea 3 36,37,38,41,42,
44,45,46,48,50,
51,52,53,55,57,
58,59,63
64,65,66a,76,78,
79
Key Idea 4
39,43,49,62
71,72
Key Idea 5
47
Standard 4
Key Idea 3 1,2,3,4,5,6,8,9,
10,14,15,16,18,
19,20,21,23,24,
25,26,27,28,29,
30
,
31
,
32
,
35
36,37,38,42,44,
45,46,48,50,51,
52,53,54,55,56,
57,58,59,63
64,65,66,67,74,
75,76,77,78,79
Key Idea 4 7,17,22 39,43,49,62 69,70,71,72,73
Key Idea 5 11,12,13,33,34 40,41,47,60,61
Reference Tables
2002 Edition 2,7,10,13,14,
19,24,26,32
36,37,40,41,44,
47,48,49,52,53,
54,55,56,57,58,
62
64,65,66,71,72,79
