The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Thursday, January 24, 2008 — 1:15 to 4:15 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 you to use while taking this examination.
The use of any communications device is strictly prohibited when taking this
examination. If you use any communications device, no matter how briefly, your
examination will be invalidated and no score will be calculated for you.
DO NOT OPEN THIS EXAMINATION BOOKLET UNTIL THE SIGNAL IS GIVEN.
PS/CHEMISTRY
PS/CHEMISTRY
1 Which quantity identifies an element?
(1) atomic number
(2) mass number
(3) total number of neutrons in an atom of the
element
(4) total number of valence electrons in an atom
of the element
2 Which atom in the ground state has a partially
filled second electron shell?
(1) hydrogen atom (3) potassium atom
(2) lithium atom (4) sodium atom
3 What is the total charge of the nucleus of a
nitrogen atom?
(1) +5 (3) +7
(2) +2 (4) +14
4 Which value of an element is calculated using
both the mass and the relative abundance of
each of the naturally occurring isotopes of this
element?
(1) atomic number (3) half-life
(2) atomic mass (4) molar volume
5 The mass of 12 protons is approximately equal to
(1) 1 atomic mass unit
(2) 12 atomic mass units
(3) the mass of 1 electron
(4) the mass of 12 electrons
6 Sodium atoms, potassium atoms, and cesium
atoms have the same
(1) atomic radius
(2) first ionization energy
(3) total number of protons
(4) oxidation state
7 Which statement describes a chemical property
of hydrogen gas?
(1) Hydrogen gas burns in air.
(2) Hydrogen gas is colorless.
(3) Hydrogen gas has a density of 0.000 09 g/cm
3
at STP.
(4) Hydrogen gas has a boiling point of 20. K at
standard pressure.
8 Which element has the greatest density at STP?
(1) calcium (3) chlorine
(2) carbon (4) copper
9 Which equation shows conservation of atoms?
(1) H
2
+ O
2
→ H
2
O
(2) H
2
+ O
2
→ 2H
2
O
(3) 2H
2
+ O
2
→ 2H
2
O
(4) 2H
2
+ 2O
2
→ 2H
2
O
10 Which term indicates how strongly an atom
attracts the electrons in a chemical bond?
(1) alkalinity
(2) atomic mass
(3) electronegativity
(4) activation energy
11 A solid substance is an excellent conductor of
electricity. The chemical bonds in this sub-
stance are most likely
(1) ionic, because the valence electrons are
shared between atoms
(2) ionic, because the valence electrons are
mobile
(3) metallic, because the valence electrons are
stationary
(4) metallic, because the valence electrons are
mobile
Part A
Answer all questions in this part.
Directions (1–30): 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.–Jan. ’08 [2]
12 Magnesium nitrate contains chemical bonds
that are
(1) covalent, only
(2) ionic, only
(3) both covalent and ionic
(4) neither covalent nor ionic
13 Which substance can be broken down by a
chemical change?
(1) antimony (3) hexane
(2) carbon (4) sulfur
14 Which barium salt is insoluble in water?
(1) BaCO
3
(3) Ba(ClO
4
)
2
(2) BaCl
2
(4) Ba(NO
3
)
2
15 Which unit can be used to express solution
concentration?
(1) J/mol (3) mol/L
(2) L/mol (4) mol/s
16 Under which conditions of temperature and
pressure is a gas most soluble in water?
(1) high temperature and low pressure
(2) high temperature and high pressure
(3) low temperature and low pressure
(4) low temperature and high pressure
17 Given the equation representing a system at
equilibrium:
At which temperature does this equilibrium
exist at 101.3 kilopascals?
(1) 0 K (3) 32 K
(2) 0°C (4) 273°C
18 In a redox reaction, the total number of
electrons lost is
(1) less than the total number of electrons
gained
(2) greater than the total number of electrons
gained
(3) equal to the total number of electrons
gained
(4) equal to the total number of protons gained
19 Which formula represents an alkene?
(1) C
2
H
6
(3) C
4
H
10
(2) C
3
H
6
(4) C
5
H
12
20 Which term refers to the difference between
the potential energy of the products and the
potential energy of the reactants for any chemi-
cal change?
(1) heat of deposition (3) heat of reaction
(2) heat of fusion (4) heat of vaporization
21 Which energy conversion occurs in a voltaic
cell?
(1) chemical energy to electrical energy
(2) chemical energy to nuclear energy
(3) electrical energy to chemical energy
(4) nuclear energy to electrical energy
22 Which metal is more active than Ni and less
active than Zn?
(1) Cu (3) Mg
(2) Cr (4) Pb
23 As water is added to a 0.10 M NaCl aqueous
solution, the conductivity of the resulting
solution
(1) decreases because the concentration of ions
decreases
(2) decreases, but the concentration of ions
remains the same
(3) increases because the concentration of ions
decreases
(4) increases, but the concentration of ions
remains the same
24 Which substance is an Arrhenius acid?
(1) Ba(OH)
2
(3) H
3
PO
4
(2) CH
3
COOCH
3
(4) NaCl
25 Which compound releases hydroxide ions in an
aqueous solution?
(1) CH
3
COOH (3) HCl
(2) CH
3
OH (4) KOH
HO(s) HO()
22
ᐉ
P.S./Chem.–Jan. ’08 [3] [OVER]
26 Which reaction converts an atom of one
element to an atom of another element?
(1) combustion (3) saponification
(2) polymerization (4) transmutation
27 Which nuclear emission has the greatest mass?
(1) alpha particle (3) gamma ray
(2) beta particle (4) positron
28 Which two radioisotopes have the same decay
mode?
(1)
37
Ca and
53
Fe (3)
37
K and
42
K
(2)
220
Fr and
60
Co (4)
99
Tc and
19
Ne
29 Which list of nuclear emissions is arranged in
order from the least penetrating power to the
greatest penetrating power?
(1) alpha particle, beta particle, gamma ray
(2) alpha particle, gamma ray, beta particle
(3) gamma ray, beta particle, alpha particle
(4) beta particle, alpha particle, gamma ray
30 One benefit of nuclear fission reactions is
(1) nuclear reactor meltdowns
(2) storage of waste materials
(3) biological exposure
(4) production of energy
P.S./Chem.–Jan. ’08 [4]
31 Which list of elements consists of metalloids,
only?
(1) B, Al, Ga (3) O, S, Se
(2) C, N, P (4) Si, Ge, As
32 Which two notations represent different
isotopes of the same element?
(1)
6
4
Be and
9
4
Be (3)
14
7
N and
14
6
C
(2)
7
3
Li and
7
3
Li (4)
32
15
P and
32
16
S
33 Which general trend is found in Period 2 on the
Periodic Table as the elements are considered in
order of increasing atomic number?
(1) decreasing atomic mass
(2) decreasing electronegativity
(3) increasing atomic radius
(4) increasing first ionization energy
34 What is the gram-formula mass of Ca
3
(PO
4
)
2
?
(1) 248 g/mol (3) 279 g/mol
(2) 263 g/mol (4) 310. g/mol
35 What is the total number of pairs of electrons
shared between the carbon atom and the oxygen
atom in a molecule of methanal?
(1) 1 (3) 3
(2) 2 (4) 4
36 When sodium and fluorine combine to produce
the compound NaF, the ions formed have the
same electron configuration as atoms of
(1) argon, only
(2) neon, only
(3) both argon and neon
(4) neither argon nor neon
37 In which compound is the ratio of metal ions to
nonmetal ions 1 to 2?
(1) calcium bromide (3) calcium phosphide
(2) calcium oxide (4) calcium sulfide
38 What is the concentration of O
2
(g), in parts per
million, in a solution that contains 0.008 gram of
O
2
(g) dissolved in 1000. grams of H
2
O(ᐉ)?
(1) 0.8 ppm (3) 80 ppm
(2) 8 ppm (4) 800 ppm
39 The table below shows data for the temperature,
pressure, and volume of four gas samples.
Data for Four Gas Samples
Which two gas samples have the same total
number of molecules?
(1) A and B (3) B and C
(2) A and C (4) B and D
40 At which temperature is the vapor pressure of
ethanol equal to the vapor pressure of
propanone at 35°C?
(1) 35°C (3) 82°C
(2) 60.°C (4) 95°C
Gas
Sample
Temperature
(K)
Pressure
(atm)
Volume
(mL)
A 100. 2 400.
B 200. 2 200.
C 100. 2 400.
D 200. 4 200.
Part B–1
Answer all questions in this part.
Directions (31–50): 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.–Jan. ’08 [5] [OVER]
41 A rigid cylinder with a movable piston contains
a 2.0-liter sample of neon gas at STP. What is
the volume of this sample when its temperature
is increased to 30.°C while its pressure is
decreased to 90. kilopascals?
(1) 2.5 L (3) 1.6 L
(2) 2.0 L (4) 0.22 L
42 Which compound is a saturated hydrocarbon?
(1) CH
2
CH
2
(3) CH
3
CHO
(2) CH
3
CH
3
(4) CH
3
CH
2
OH
43 A molecule of a compound contains a total of
10 hydrogen atoms and has the general formula
C
n
H
2n+2
. Which prefix is used in the name of
this compound?
(1) but- (3) oct-
(2) dec- (4) pent-
44 Reduction occurs at the cathode in
(1) electrolytic cells, only
(2) voltaic cells, only
(3) both electrolytic cells and voltaic cells
(4) neither electrolytic cells nor voltaic cells
45 What are the products of a reaction between
KOH(aq) and HCl(aq)?
(1) H
2
and KClO (3) KH and HClO
(2) H
2
O and KCl (4) KOH and HCl
46 Which volume of 0.10 M NaOH(aq) exactly
neutralizes 15.0 milliliters of 0.20 M HNO
3
(aq)?
(1) 1.5 mL (3) 3.0 mL
(2) 7.5 mL (4) 30. mL
47 Which indicator, when added to a solution,
changes color from yellow to blue as the pH of
the solution is changed from 5.5 to 8.0?
(1) bromcresol green (3) litmus
(2) bromthymol blue (4) methyl orange
48 The pH of an aqueous solution changes from
4 to 3 when the hydrogen ion concentration in
the solution is
(1) decreased by a factor of
(2) decreased by a factor of 10
(3) increased by a factor of
(4) increased by a factor of 10
49 Which fraction of an original 20.00-gram
sample of nitrogen-16 remains unchanged after
36.0 seconds?
(1) (3)
(2) (4)
50 Which radioactive isotope is used in treating
cancer?
(1) carbon-14 (3) lead-206
(2) cobalt-60 (4) uranium-238
1
32
1
8
1
16
1
5
4
3
3
4
P.S./Chem.–Jan. ’08 [6]
Part B–2
Answer all questions in this part.
Directions (51–65): 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.
P.S./Chem.–Jan. ’08 [7] [OVER]
51 Describe one chemical property of Group 1 metals that results from the atoms of each
metal having only one valence electron.
[1]
52 Given the balanced equation representing a reaction:
N
2
(g) + O
2
(g) + 182.6 kJ → 2NO(g)
On the labeled axes in your answer booklet, draw a potential energy diagram for this
reaction.
[1]
53 Write one electron configuration for an atom of silicon in an excited state. [1]
54 Write the empirical formula for the compound C
8
H
18
. [1]
Base your answers to questions 55 through 57 on the information below.
55 Identify one piece of information shown in the electron-shell diagrams that is not shown
in the Lewis electron-dot diagrams.
[1]
56 Determine the mass number of the magnesium atom represented by the electron-shell
diagram.
[1]
57 Explain why Lewis electron-dot diagrams are generally more suitable than
electron-shell diagrams for illustrating chemical bonding.
[1]
= electron
Key
Element
Lewis Electron-Dot
Diagram
magnesium
aluminum
Al
Mg
Atomic Diagrams of Magnesium and Aluminum
Electron-Shell
Diagram
12 p
11 n
13 p
14 n
P.S./Chem.–Jan. ’08 [8]
Base your answers to questions 58 through 60 on the information below.
A 100.0-gram sample of NaCl(s) has an initial temperature of 0°C. A chemist measures
the temperature of the sample as it is heated. Heat is not added at a constant rate. The
heating curve for the sample is shown below.
58 Determine the temperature range over which the entire NaCl sample is a liquid.
[1]
59 Identify one line segment on the curve where the average kinetic energy of the
particles of the NaCl sample is changing.
[1]
60 Identify one line segment on the curve where the NaCl sample is in a single phase and
capable of conducting electricity.
[1]
Base your answers to questions 61 through 63 on the information below.
A beaker contains 100.0 milliliters of a dilute aqueous solution of ethanoic acid at
equilibrium. The equation below represents this system.
61 Compare the rate of the forward reaction to the rate of the reverse reaction for this
system.
[1]
62 Describe what happens to the concentration of H
+
(aq) when 10 drops of concentrated
HC
2
H
3
O
2
(aq) are added to this system. [1]
63 In the space in your answer booklet, draw a structural formula for ethanoic acid. [1]
HC H O (aq) H (aq) + C H O (aq)
32
+
232
–
2
1465
0
A
DE
Time
Heating Curve for Sodium Chloride
BC
801
Temperature (°C)
P.S./Chem.–Jan. ’08 [9] [OVER]
Base your answers to questions 64 and 65 on the information below.
A solution is made by completely dissolving 90. grams of KNO
3
(s) in 100. grams of
water in a beaker. The temperature of this solution is 65°C.
64 Describe the effect on the solubility of KNO
3
(s) in this solution when the pressure on
the solution increases.
[1]
65 Determine the total mass of KNO
3
(s) that settles to the bottom of the beaker when the
original solution is cooled to 15°C.
[1]
P.S./Chem.–Jan. ’08 [10]
Part C
Answer all questions in this part.
Directions (66–83): 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 66 through 68 on the information below.
The compound 1,2-ethanediol can be mixed with water. This mixture is added to
automobile radiators as an engine coolant. The cooling system of a small van contains
6690 grams of 1,2-ethanediol. Some properties of water and 1,2-ethanediol are given in the
table below.
Properties of Water and 1,2-ethanediol
66 Identify the class of organic compounds to which 1,2-ethanediol belongs. [1]
67 State, in terms of molecular polarity, why 1,2-ethanediol is soluble in water. [1]
68 In the space in your answer booklet, calculate the total number of moles of 1, 2-ethanediol
in the small van’s cooling system. Your response must include both a correct
numerical setup and the calculated result.
[2]
Base your answers to questions 69 through 71 on the information below.
“Hand Blasters” is a toy that consists of a set of two ceramic balls, each coated with a
mixture of sulfur and potassium chlorate, KClO
3
. When the two balls are struck together,
a loud popping noise is produced as sulfur and potassium chlorate react with each other.
69 Balance the equation in your answer booklet for the “Hand Blaster” reaction, using the
smallest whole-number coefficients.
[1]
70 Identify one source of the activation energy for this reaction. [1]
71 Determine the oxidation number of chlorine in the reactant that contains chlorine. [1]
P.S./Chem.–Jan. ’08 [11] [OVER]
Property
Water
(H
2
O)
1,2-ethanediol
(CH
2
OHCH
2
OH)
gram-formula mass (g/mol) 18.0 62.0
boiling point at standard pressure (°C) 100.0 197.2
Base your answers to questions 72 through 74 on the information below.
A laboratory worker filled a bottle with a hydrochloric acid solution. Another bottle was
filled with methanol, while a third bottle was filled with a sodium hydroxide solution.
However, the worker neglected to label each bottle. After a few days, the worker could not
remember which liquid was in each bottle.
The worker needed to identify the liquid in each bottle. The bottles were labeled A, B,
and C. Using materials found in the lab (indicators, conductivity apparatus, and pieces of
Mg metal), the worker tested samples of liquid from each bottle. The test results are shown
in the table below.
Table of Tests and Results
72 Using the test results, state how the worker differentiated the bottle that contained
methanol from the other two bottles.
[1]
73 The worker concluded that bottle C contained hydrochloric acid. Identify one test and
state the corresponding test result that supports this conclusion.
[1]
74 Explain, in terms of pH, why the methyl orange indicator test results were the same for
each of the three liquids.
[1]
P.S./Chem.–Jan. ’08 [12]
Test
Test Results
Bottle A Bottle B Bottle C
methyl orange indicator yellow yellow yellow
bromthymol blue indicator blue green yellow
electrical conductivity conductor nonconductor conductor
reactivity with Mg metal no reaction no reaction reaction
Base your answers to questions 75 and 76 on the information below.
A student performed an experiment to determine the total amount of energy stored in
a peanut. The accepted value for the energy content of a peanut is 30.2 kilojoules per gram.
The student measured 100.0 grams of water into a metal can and placed the can on a
ring stand, as shown in the diagram below. The peanut was attached to a wire suspended
under the can. The initial temperature of the water was recorded as 22.0°C. The peanut
was ignited and allowed to burn. When the peanut finished burning, the final water
temperature was recorded as 57.0°C. The student’s experimental value for the energy
content of this peanut was 25.9 kilojoules per gram.
75 In the space in your answer booklet, calculate the total amount of heat absorbed by the
water. Your response must include both a correct numerical setup and the calculated
result.
[2]
76 Determine the student’s percent error for the energy content of this peanut. [1]
Base your answers to questions 77 through 79 on the information below.
Some dry chemicals can be used to put out forest fires. One of these chemicals is
NaHCO
3
. When NaHCO
3
(s) is heated, one of the products is CO
2
(g), as shown in the
balanced equation below.
77 In the space in your answer booklet, show a correct numerical setup for calculating the
percent composition by mass of carbon in the product Na
2
CO
3
. [1]
78 Identify the type of chemical reaction represented by this equation. [1]
79 Determine the total number of moles of CO
2
(g) produced when 7.0 moles of
NaHCO
3
(s) is completely reacted. [1]
2NaHCO (s) + heat Na CO (s) + H O(g) + CO
32322
→ ((g)
Metal can
Peanut
H
2
O( )
100.0 g
Thermometer
P.S./Chem.–Jan. ’08 [13] [OVER]
Base your answers to questions 80 and 81 on the information below.
In an investigation, a dripless wax candle is massed and then lighted. As the candle
burns, a small amount of liquid wax forms near the flame. After 10 minutes, the candle’s
flame is extinguished and the candle is allowed to cool. The cooled candle is massed.
80 Identify one physical change that takes place in this investigation.
[1]
81 State one observation that indicates a chemical change has occurred in this
investigation.
[1]
Base your answers to questions 82 and 83 on the information below.
The graph below shows the relationship between boiling point and molar mass at
standard pressure for pentane, hexane, heptane, and nonane.
82 Octane has a molar mass of 114 grams per mole. According to this graph, what is the
boiling point of octane at standard pressure?
[1]
83 State the relationship between molar mass and the strength of intermolecular forces for
the selected alkanes.
[1]
Molar Mass (g/mol)
Boiling Point (°C)
80. 90. 100. 110.
40.
60.
80.
100.
Boiling Point Versus Molar Mass of Some Alkanes
20.
120.
140.
160.
70. 120. 130.
P.S./Chem.–Jan. ’08 [14]
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Thursday, January 24, 2008 — 1:15 to 4:15 p.m., only
ANSWER SHEET
Student . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Sex: II Male II 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 . . . . . . . . . . . . 11 . . . . . . . . . . . . 21 . . . . . . . . . . .
2 . . . . . . . . . . . . 12 . . . . . . . . . . . . 22 . . . . . . . . . . .
3 . . . . . . . . . . . . 13 . . . . . . . . . . . . 23 . . . . . . . . . . .
4 . . . . . . . . . . . . 14 . . . . . . . . . . . . 24 . . . . . . . . . . .
5 . . . . . . . . . . . . 15 . . . . . . . . . . . . 25 . . . . . . . . . . .
6 . . . . . . . . . . . . 16 . . . . . . . . . . . . 26 . . . . . . . . . . .
7 . . . . . . . . . . . . 17 . . . . . . . . . . . . 27 . . . . . . . . . . .
8 . . . . . . . . . . . . 18 . . . . . . . . . . . . 28 . . . . . . . . . . .
9 . . . . . . . . . . . . 19 . . . . . . . . . . . . 29 . . . . . . . . . . .
10 . . . . . . . . . . . . 20 . . . . . . . . . . . . 30 . . . . . . . . . . .
Part B–1
31 . . . . . . . . . . . . 41 . . . . . . . . . . . .
32 . . . . . . . . . . . . 42 . . . . . . . . . . . .
33 . . . . . . . . . . . . 43 . . . . . . . . . . . .
34 . . . . . . . . . . . . 44 . . . . . . . . . . . .
35 . . . . . . . . . . . . 45 . . . . . . . . . . . .
36 . . . . . . . . . . . . 46 . . . . . . . . . . . .
37 . . . . . . . . . . . . 47 . . . . . . . . . . . .
38 . . . . . . . . . . . . 48 . . . . . . . . . . . .
39 . . . . . . . . . . . . 49 . . . . . . . . . . . .
40 . . . . . . . . . . . . 50 . . . . . . . . . . . .
Part A Score
Part B–1 Score
51
52
Maximum Student’s
Part Score Score
A30
B–1 20
B–2 15
C20
Total Written Test Score
(Maximum Raw Score: 85)
Final Score
(from conversion chart)
Raters’ Initials:
Rater 1 . . . . . . . . . . Rater 2 . . . . . . . . . . .
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Thursday, January 24, 2008 — 1:15 to 4:15 p.m., only
ANSWER BOOKLET
Student . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Sex: I Female
Teacher . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
School . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Grade . . . . . . . . .
Answer all questions in Part B–2 and Part C. Record your answers
in this booklet.
I Male
Part B–2
For Raters
Only
52
51
Reaction Coordinate
Potential Energy
53
54
55
56
57
58
59
60
[2]
For Raters
Only
54
55
56
57
58
59
60
53
[3] [OVER]
61
62
63
64
65 g
For Raters
Only
61
62
63
Total Score
for Part B–2
65
64
[4]
For Raters
Only
Part C
66
67
68
mol
69 _____
S(s) + _____ KClO
3
(s) → _____ SO
2
(g) + _____ KCl(s) + energy
70
71
66
68
69
67
70
71
[5] [OVER]
72
73 Test:
Test result:
74
75
J
76
%
For Raters
Only
72
75
73
74
76
77
78
79 mol
80
81
82 °C
83
For Raters
Only
[6]
78
79
80
81
Total Score
for Part C
82
77
83
Part B–1
31 . . . . . . . . . . . . 41 . . . . . . . . . . . .
32 . . . . . . . . . . . . 42 . . . . . . . . . . . .
33 . . . . . . . . . . . . 43 . . . . . . . . . . . .
34 . . . . . . . . . . . . 44 . . . . . . . . . . . .
35 . . . . . . . . . . . . 45 . . . . . . . . . . . .
36 . . . . . . . . . . . . 46 . . . . . . . . . . . .
37 . . . . . . . . . . . . 47 . . . . . . . . . . . .
38 . . . . . . . . . . . . 48 . . . . . . . . . . . .
39 . . . . . . . . . . . . 49 . . . . . . . . . . . .
40 . . . . . . . . . . . . 50 . . . . . . . . . . . .
Part A
1 . . . . . . . . . . . . 11 . . . . . . . . . . . . 21 . . . . . . . . . . .
2 . . . . . . . . . . . . 12 . . . . . . . . . . . . 22 . . . . . . . . . . .
3 . . . . . . . . . . . . 13 . . . . . . . . . . . . 23 . . . . . . . . . . .
4 . . . . . . . . . . . . 14 . . . . . . . . . . . . 24 . . . . . . . . . . .
5 . . . . . . . . . . . . 15 . . . . . . . . . . . . 25 . . . . . . . . . . .
6 . . . . . . . . . . . . 16 . . . . . . . . . . . . 26 . . . . . . . . . . .
7 . . . . . . . . . . . . 17 . . . . . . . . . . . . 27 . . . . . . . . . . .
8 . . . . . . . . . . . . 18 . . . . . . . . . . . . 28 . . . . . . . . . . .
9 . . . . . . . . . . . . 19 . . . . . . . . . . . . 29 . . . . . . . . . . .
10 . . . . . . . . . . . . 20 . . . . . . . . . . . . 30 . . . . . . . . . . .
1
2
3
2
2
4
1
4
3
3
4
1
4
4
2
2
1
2
2
2
1
2
1
3
2
4
2
4
4
2
4
3
3
1
3
4
2
3
2
3
1
2
1
3
4
4
1
1
1
4
FOR TEACHERS ONLY
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING/CHEMISTRY
Thursday, January 24, 2008 — 1:15 to 4:15 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.
Updated information regarding the rating of this examination may be posted on the New York
State Education Department’s web site during the rating period. Check this web site
http://www.emsc.nysed.gov/osa/
and select the link “Examination Scoring Information” for any
recently posted information regarding this examination. This site should be checked before the rating
process for this examination begins and several times throughout the Regents examination period.
Part A and Part B–1
Allow 1 credit for each correct response.
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 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 that will be
posted on the Department’s web site http://www.emsc.nysed.gov/osa/
on Thursday,
January 24, 2008. 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
student’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 for that administration be used to determine the student’s final score.
[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. Acceptable responses include, but are not limited to:
form 1
+
ions
react vigorously with water
easily lose one electron
form ionic bonds with nonmetals
form halides with the general formula MX
52 [1] Allow 1 credit.
Example of a 1-credit response:
53 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
2–7–4–1
2–7–5
2–8–3–1
1–8–5
Note: Do not allow credit for 2–8–4.
Reaction Coordinate
Potential Energy
PHYSICAL SETTING/CHEMISTRY – continued
[5] [OVER]
54 [1] Allow 1 credit for C
4
H
9
.
55 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
The electron-shell diagram shows the total number of protons and the total number of neutrons
in an atom.
shows number of electrons in each inner shell
shows total number of protons in an atom
shows the number of electron shells
56 [1] Allow 1 credit for 23.
57 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
Lewis electron-dot diagrams only show valence electrons, which are involved in bonding.
shows only electrons involved in bonding
58 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
801°C to 1465°C
59 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
AB
CD
60 [1] Allow 1 credit for CD.
61 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
The rate of the forward reaction equals the rate of the reverse reaction.
PHYSICAL SETTING/CHEMISTRY – continued
[6]
62 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
The H
+
(aq) concentration increases.
[H
3
O
+
] increases.
Concentration increases.
63 [1] Allow 1 credit.
Examples of 1-credit responses:
64 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
The solubility of KNO
3
(s) is not affected by an increase in pressure.
When the pressure on the solution increases, the solubility of KNO
3
remains the same.
65 [1] Allow 1 credit for 62 g ± 2 g.
CC
OH
O
H
HO
O
C
H
H
C
Part C
Allow a total of 20 credits for this part. The student must answer all questions in this part.
PHYSICAL SETTING/CHEMISTRY – continued
[7] [OVER]
66 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
alcohol
67 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
Water and 1,2-ethanediol molecules are both polar.
Both molecules have similar polarity.
68 [2] Allow a maximum of 2 credits, allocated as follows:
• Allow 1 credit for a correct numerical setup. Acceptable responses include, but are not limited to:
• Allow 1 credit for 108 mol or for a response consistent with the student’s numerical setup.
Significant figures do not need to be shown.
Note: Do not allow credit for a numerical setup and calculated result that are not related to the
concept assessed by the question.
69 [1] Allow 1 credit for 3
S(s) + 2 KClO
3
(s) → 3 SO
2
(g) + 2 KCl(s) + energy.
70 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
The activation energy results from striking the balls together.
heat produced as the balls collide
mechanical energy
friction
6690
62
6690
62 0
g
g/mol.
PHYSICAL SETTING/CHEMISTRY – continued
[8]
71 [1] Allow 1 credit for +5.
72 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
Methanol does not conduct an electric current.
Bromthymol blue tests blue in a base and yellow in an acid, so bottle B must be methanol.
Bromthymol blue would be green in methanol because methanol is not an acid or a base.
73 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
Test: bromthymol blue
Test result: yellow
Test: reactivity with Mg
Test result: reaction
74 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
All three solutions have a pH greater than 4.4.
Methyl orange changes to yellow at a pH of 4.4, which is still in the acid range.
A solution with a pH greater than 4.4 could be acidic, basic, or neutral.
75 [2] Allow a maximum of 2 credits, allocated as follows:
• Allow 1 credit for a correct numerical setup. Acceptable responses include, but are not limited to:
q = mCΔT = (100.0 g)(4.18 J/g•°C)(57.0°C − 22.0°C)
(100)(4.18)(35)
• Allow 1 credit for 14 600 J or for a response consistent with the student’s numerical setup.
Significant figures do not need to be shown.
Note: Do not allow credit for a numerical setup and calculated result that are not related to the
concept assessed by the question.
76 [1] Allow 1 credit for −14% or 14%. Significant figures do not need to be shown.
PHYSICAL SETTING/CHEMISTRY – continued
77 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
78 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
decomposition
endothermic
79 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
3.5 mol
3
80 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
melting
vaporization
solidification
81 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
The burning candle releases heat and light.
A cobalt chloride test indicates water is produced.
A limewater test indicates carbon dioxide gas is produced.
1
2
mol
7
2
mol
12
106
100
gmol
gmol
/
/
×
12
22312 316
100
() ()×++×
×
[9] [OVER]
PHYSICAL SETTING/CHEMISTRY – concluded
82 [1] Allow 1 credit for 124°C ± 2°C.
83 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
As molar mass increases, there are stronger intermolecular forces.
The forces are greater between heavier molecules.
[10]
[11] [OVER]
The Chart for Determining the Final Examination Score for the January 2008
Regents Examination in Physical Setting/Chemistry will be posted on the
Department’s web site http://www.emsc.nysed.gov/osa/
on Thursday,
January 24, 2008. Conversion charts provided for previous administrations
of the Regents Examination in Physical Setting/Chemistry must NOT be
used to determine students’ final scores for this administration.
Regents Examination in Physical Setting/Chemistry
January 2008
Chart for Converting Total Test Raw Scores to
Final Examination Scores (Scaled Scores)
Submitting Teacher Evaluations of the Test to the Department
Suggestions and feedback from teachers provide an important contribution to the test
development process. The Department provides an online evaluation form for State
assessments. It contains spaces for teachers to respond to several specific questions and to
make suggestions. Instructions for completing the evaluation form are as follows:
1. Go to www.emsc.nysed.gov/osa/exameval
.
2. Select the test title.
3. Complete the required demographic fields.
4. Complete each evaluation question and provide comments in the space provided.
5. Click the SUBMIT button at the bottom of the page to submit the completed form.
[12]
Map to Core Curriculum
January 2008 Physical Setting/Chemistry
Question Numbers
Key Ideas Part A Part B Part C
Standard 1
Math Key Idea 1 38, 41, 46 68, 75, 76, 77, 82
Math Key Idea 2
Math Key Idea 3
34, 43, 49, 54, 56,
58, 65
68, 69, 71, 79
Sci. Inquiry Key Idea 1 55, 57, 61, 64 70, 72, 80, 81
Sci. Inquiry Key Idea 2
Sci. Inquiry Key Idea 3
35, 37, 39, 40, 47,
53, 65
66, 69, 71, 72, 73
Eng. Design Key Idea 1
Standard 2
Key Idea 1
Key Idea 2
Standard 6
Key Idea 1
Key Idea 2
41
Key Idea 3
48
Key Idea 4
62
Key Idea 5
64, 65 82, 83
Standard 7
Key Idea 1
Key Idea 2
Standard 4 Process Skills
Key Idea 3
31, 32, 33, 34, 38,
41, 42, 44, 45, 46,
47, 51, 53, 54, 55,
56, 61, 62, 63, 65
66, 67, 68, 69, 73,
74, 77, 78, 79, 80,
81
Key Idea 4
49, 50, 52, 58, 59,
60
70, 75
Key Idea 5
36, 57 83
Standard 4
Key Idea 3
1, 2, 3, 4, 5, 6, 7,
8, 9, 13, 14, 15,
16, 17, 18, 19, 21,
22, 23, 24, 25, 27,
29
31, 32, 33, 34, 37,
38, 39, 41, 42, 43,
44, 45, 46, 47, 48,
51, 53, 54, 55, 56,
61, 62, 63, 64, 65
66, 67, 68, 69, 71,
72, 73, 74, 77, 78,
79, 80, 81, 82
Key Idea 4 20, 28, 30
40, 49, 50, 52, 58,
59
70, 75, 76
Key Idea 5 10, 11, 12, 26 35, 36, 57, 60 83
Reference Tables
2002 Edition
2, 3, 6, 8, 14, 15,
19, 22, 25, 27, 28
34, 35, 36, 37, 38,
40, 41, 42, 43, 46,
47, 49, 50, 51, 53,
63, 64, 65
66, 71, 74, 75, 76,
77
Regents Examination in Physical Setting/Chemistry
January 2008
Chart for Converting Total Test Raw Scores to
Final Examination Scores (Scaled Scores)
Raw
Score
Scaled
Score
Raw
Score
Scaled
Score
Raw
Score
Scaled
Score
Raw
Score
Scaled
Score
85 100 63 74 41 60 19 39
84 98 62 74 40 59 18 37
83 96 61 73 39 58 17 36
82 95 60 72 38 57 16 34
81 93 59 71 37 57 15 33
80 92 58 71 36 56 14 31
79 90 57 70 35 55 13 30
78 89 56 69 34 54 12 28
77 88 55 69 33 54 11 26
76 86 54 68 32 53 10 24
75 85 53 67 31 52 9 22
74 84 52 67 30 51 8 20
73 83 51 66 29 50 7 18
72 82 50 66 28 49 6 16
71 81 49 65 27 48 5 13
70 80 48 64 26 47 4 11
69 79 47 64 25 46 3 8
68 78 46 63 24 45 2 6
67 77 45 62 23 44 1 3
66 77 44 62 22 43 0 0
65 76 43 61 21 41
64 75 42 60 20 40
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.
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 student’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 change from one
examination to another, it is crucial that for each administration, the conversion chart provided for that
administration be used to determine the student’s final score. The chart above is usable only for this
administration of the Physical Setting/Chemistry Examination.
