The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Thursday, August 13, 2009 — 12:30 to 3:30 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 particle has the least mass?
(1)
4
2
He (3)
1
0
n
(2)
1
1
H (4)
0
−1
e
2 What information is necessary to determine the
atomic mass of the element chlorine?
(1) the atomic mass of each artificially produced
isotope of chlorine, only
(2) the relative abundance of each naturally
occurring isotope of chlorine, only
(3) the atomic mass and the relative abundance of
each naturally occurring isotope of chlorine
(4) the atomic mass and the relative abundance
of each naturally occurring and artificially
produced isotope of chlorine
3 In an atom of argon-40, the number of protons
(1) equals the number of electrons
(2) equals the number of neutrons
(3) is less than the number of electrons
(4) is greater than the number of electrons
4 An electron in a sodium atom moves from the
third shell to the fourth shell. This change is a
result of the atom
(1) absorbing energy (3) gaining an electron
(2) releasing energy (4) losing an electron
5 Which statement describes oxygen gas, O
2
(g),
and ozone gas, O
3
(g)?
(1) They have different molecular structures,
only.
(2) They have different properties, only.
(3) They have different molecular structures
and different properties.
(4) They have the same molecular structure and
the same properties.
6 Which statement describes a chemical property
of bromine?
(1) Bromine is soluble in water.
(2) Bromine has a reddish-brown color.
(3) Bromine combines with aluminum to
produce AlBr
3
.
(4) Bromine changes from a liquid to a gas at
332 K and 1 atm.
7 An atom of aluminum in the ground state and an
atom of gallium in the ground state have the
same
(1) mass
(2) electronegativity
(3) total number of protons
(4) total number of valence electrons
8 Which type of matter is composed of two or
more elements that are chemically combined in
a fixed proportion?
(1) solution
(2) compound
(3) homogeneous mixture
(4) heterogeneous mixture
9 Which type of substance can conduct electricity
in the liquid phase but not in the solid phase?
(1) ionic compound
(2) molecular compound
(3) metallic element
(4) nonmetallic element
10 Why is a molecule of CO
2
nonpolar even though
the bonds between the carbon atom and the
oxygen atoms are polar?
(1) The shape of the CO
2
molecule is symmetrical.
(2) The shape of the CO
2
molecule is asymmetrical.
(3) The CO
2
molecule has a deficiency of electrons.
(4) The CO
2
molecule has an excess of electrons.
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.–Aug. ’09 [2]
11 Which formula represents a molecular compound?
(1) HI (3) KCl
(2) KI (4) LiCl
12 Which element has the greatest density at STP?
(1) scandium (3) silicon
(2) selenium (4) sodium
13 Particles are arranged in a crystal structure in a
sample of
(1) H
2
(g) (3) Ar(g)
(2) Br
2
(ᐉ) (4) Ag(s)
14 The relatively high boiling point of water is due
to water having
(1) hydrogen bonding
(2) metallic bonding
(3) nonpolar covalent bonding
(4) strong ionic bonding
15 Matter is classified as a
(1) substance, only
(2) substance or as a mixture of substances
(3) homogenous mixture, only
(4) homogenous mixture or as a heterogeneous
mixture
16 Which substance can not be decomposed by a
chemical change?
(1) ammonia (3) propanol
(2) copper (4) water
17 A beaker contains both alcohol and water.
These liquids can be separated by distillation
because the liquids have different
(1) boiling points (3) particle sizes
(2) densities (4) solubilities
18 Which term is defined as a measure of the
average kinetic energy of the particles in a sample
of matter?
(1) activation energy (3) temperature
(2) potential energy (4) entropy
19 How do the boiling point and freezing point of a
solution of water and calcium chloride at
standard pressure compare to the boiling point
and freezing point of water at standard
pressure?
(1) Both the freezing point and boiling point of
the solution are higher.
(2) Both the freezing point and boiling point of
the solution are lower.
(3) The freezing point of the solution is higher
and the boiling point of the solution is lower.
(4) The freezing point of the solution is lower
and the boiling point of the solution is higher.
20 Under which conditions of temperature and
pressure does a sample of neon behave most like
an ideal gas?
(1) 100 K and 0.25 atm
(2) 100 K and 25 atm
(3) 400 K and 0.25 atm
(4) 400 K and 25 atm
21 According to the kinetic molecular theory,
which statement describes the particles in a
sample of an ideal gas?
(1) The force of attraction between the gas
particles is strong.
(2) The motion of the gas particles is random
and straight-line.
(3) The collisions between the gas particles
cannot result in a transfer of energy between
the particles.
(4) The separation between the gas particles is
smaller than the size of the gas particles
themselves.
22 The activation energy of a chemical reaction can
be decreased by the addition of
(1) a catalyst (3) electrical energy
(2) an indicator (4) thermal energy
23 A straight-chain hydrocarbon that has only one
double bond in each molecule has the general
formula
(1) C
n
H
2n−6
(3) C
n
H
2n
(2) C
n
H
2n−2
(4) C
n
H
2n+2
P.S./Chem.–Aug. ’09 [3] [OVER]
24 Why can an increase in temperature lead to more
effective collisions between reactant particles
and an increase in the rate of a chemical reaction?
(1) The activation energy of the reaction
increases.
(2) The activation energy of the reaction
decreases.
(3) The number of molecules with sufficient
energy to react increases.
(4) The number of molecules with sufficient
energy to react decreases.
25 Which reaction results in the production of
soap?
(1) esterification (3) polymerization
(2) fermentation (4) saponification
26 Which substance is always a product when an
Arrhenius acid in an aqueous solution reacts
with an Arrhenius base in an aqueous solution?
(1) HBr (3) KBr
(2) H
2
O (4) KOH
27 Which substance is an electrolyte?
(1) CCl
4
(3) HCl
(2) C
2
H
6
(4) H
2
O
28 One acid-base theory defines a base as an
(1) H
+
donor (3) H donor
(2) H
+
acceptor (4) H acceptor
29 A change in the nucleus of an atom that converts
the atom from one element to another element
is called
(1) combustion (3) polymerization
(2) neutralization (4) transmutation
30 Which particle is emitted from a hydrogen-3
nucleus when it undergoes radioactive decay?
(1) α (3) β
+
(2) β
−
(4) γ
P.S./Chem.–Aug. ’09 [4]
31 Which electron configuration represents an
excited state for a potassium atom?
(1) 2-8-7-1 (3) 2-8-8-1
(2) 2-8-7-2 (4) 2-8-8-2
32 A sample of an element is malleable and can
conduct electricity. This element could be
(1) H (3) S
(2) He (4) Sn
33 Which general trend is demonstrated by the
Group 17 elements as they are considered in
order from top to bottom on the Periodic Table?
(1) a decrease in atomic radius
(2) a decrease in electronegativity
(3) an increase in first ionization energy
(4) an increase in nonmetallic behavior
34 Which element is a liquid at 758 K and standard
pressure?
(1) gold (3) platinum
(2) silver (4) thallium
35 Which equation represents a decomposition
reaction?
(1) CaCO
3
(s) → CaO(s) + CO
2
(g)
(2) Cu(s) + 2AgNO
3
(aq) → 2Ag(s) + Cu(NO
3
)
2
(aq)
(3) 2H
2
(g) + O
2
(g) → 2H
2
O(ᐉ)
(4) KOH(aq) + HCl(aq)
→ KCl(aq) + H
2
O(ᐉ)
36 A compound has the empirical formula CH
2
O
and a gram-formula mass of 60. grams per mole.
What is the molecular formula of this compound?
(1) CH
2
O (3) C
3
H
8
O
(2) C
2
H
4
O
2
(4) C
4
H
8
O
4
37 Which formula represents strontium phosphate?
(1) SrPO
4
(3) Sr
2
(PO
4
)
3
(2) Sr
3
PO
8
(4) Sr
3
(PO
4
)
2
38 Which Lewis electron-dot diagram represents
calcium oxide?
39 Which statement describes the transfer of heat
energy that occurs when an ice cube is added to
an insulated container with 100 milliliters of
water at 25°C?
(1) Both the ice cube and the water lose heat
energy.
(2) Both the ice cube and the water gain heat
energy.
(3) The ice cube gains heat energy and the
water loses heat energy.
(4) The ice cube loses heat energy and the
water gains heat energy.
40 What is the mass of NH
4
Cl that must dissolve in
200. grams of water at 50.°C to make a saturated
solution?
(1) 26 g (3) 84 g
(2) 42 g (4) 104 g
( 1 ) ( 3 )
O
Ca
O
Ca
( 2 ) ( 4 )
O
Ca
2–
2+
O
Ca
2–
2+
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.–Aug. ’09 [5] [OVER]
41 Given the bright-line spectra of three elements and the spectrum of a mixture formed from at least two of
these elements:
Which elements are present in this mixture?
(1) E and D, only
(2) E and G, only
(3) D and G, only
(4) D, E, and G
42 Given the balanced particle-diagram equation:
Which statement describes the type of change and the chemical properties of the
product and reactants?
(1) The equation represents a physical change, with the product and reactants having
different chemical properties.
(2) The equation represents a physical change, with the product and reactants having
identical chemical properties.
(3) The equation represents a chemical change, with the product and reactants having
different chemical properties.
(4) The equation represents a chemical change, with the product and reactants having
identical chemical properties.
Key
= an atom of an element
= an atom of a different element
+
Bright-Line Spectra
Mixture
Element D
Element E
Element G
750 nm 360 nm
P.S./Chem.–Aug. ’09 [6]
43 Which quantity of heat is equal to 200. joules?
(1) 20.0 kJ (3) 0.200 kJ
(2) 2.00 kJ (4) 0.0200 kJ
44 Which graph represents the relationship between
pressure and volume for a sample of an ideal gas
at constant temperature?
45 The entropy of a sample of H
2
O increases as the
sample changes from a
(1) gas to a liquid (3) liquid to a gas
(2) gas to a solid (4) liquid to a solid
46 Ethanol and dimethyl ether have different
chemical and physical properties because they
have different
(1) functional groups
(2) molecular masses
(3) numbers of covalent bonds
(4) percent compositions by mass
47 Which formula represents an unsaturated
hydrocarbon?
48 What is the oxidation state of nitrogen in the
compound NH
4
Br?
(1) –1 (3) –3
(2) +2 (4) +4
49 A student completes a titration by adding
12.0 milliliters of NaOH(aq) of unknown
concentration to 16.0 milliliters of 0.15 M HCl(aq).
What is the molar concentration of the NaOH(aq)?
(1) 0.11 M (3) 1.1 M
(2) 0.20 M (4) 5.0 M
50 What is the half-life of a radioisotope if 25.0 grams
of an original 200.-gram sample of the isotope
remains unchanged after 11.46 days?
(1) 2.87 d (3) 11.46 d
(2) 3.82 d (4) 34.38 d
( 2 )
HH
H
HC
H
H
C
( 3 )
H
H
HC
O
CH
( 1 )
HC
HH
CH
( 4 )
OH
HC
H
H
H
H
C
( 1 )
Volume
( 3 )
Volume
( 2 )
Volume
( 4 )
Volume
Pressure
Pressure
Pressure
Pressure
P.S./Chem.–Aug. ’09 [7] [OVER]
P.S./Chem.–Aug. ’09 [8]
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.
51 Identify the element in Period 3 of the Periodic Table that reacts with oxygen to form
an ionic compound represented by the formula X
2
O. [1]
52 Given the balanced equation representing a reaction:
2C
2
H
6
+7O
2
→ 4CO
2
+6H
2
O
Determine the total number of moles of oxygen that react completely with 8.0 moles
of C
2
H
6
. [1]
53 On the potential energy diagram in your answer booklet, draw an arrow to represent the
activation energy of the forward reaction. [
1]
54 Describe the electrons in an atom of carbon in the ground state. Your response must
include:
• the charge of an electron [
1]
• the location of electrons based on the wave-mechanical model [
1]
• the total number of electrons in a carbon atom [
1]
55 Determine the mass of 5.20 moles of C
6
H
12
(gram-formula mass = 84.2 grams/mole). [1]
Base your answers to questions 56 through 58 on the information below.
A 1.0-gram strip of zinc is reacted with hydrochloric acid in a test tube. The unbalanced
equation below represents the reaction.
Zn(s) + HCl(aq)
→ H
2
(g) + ZnCl
2
(aq)
56 Balance the equation in your answer booklet for the reaction of zinc and hydrochloric
acid, using the smallest whole-number coefficients. [
1]
57 Explain, using information from Reference Table F, why the symbol (aq) is used to
describe the product ZnCl
2
. [1]
58 Explain, in terms of collision theory, why using 1.0 gram of powdered zinc, instead of
the 1.0-gram strip of zinc, would have increased the rate of the reaction. [
1]
Base your answers to questions 59 through 63 on the information below.
Bond energy is the amount of energy required to break a chemical bond. The table
below gives a formula and the carbon-nitrogen bond energy for selected nitrogen compounds.
59 Describe, in terms of electrons, the type of bonding between the carbon atom and the
nitrogen atom in a molecule of methanamine. [
1]
60 Identify the noble gas that has atoms in the ground state with the same electron
configuration as the nitrogen in a molecule of isocyanic acid. [
1]
61 State the relationship between the number of electrons in a carbon-nitrogen bond and
carbon-nitrogen bond energy. [
1]
62 Explain, in terms of charge distribution, why a molecule of hydrogen cyanide is polar. [
1]
63 A 3.2-gram sample of air contains 0.000 74 gram of hydrogen cyanide. Determine the
concentration, in parts per million, of the hydrogen cyanide in this sample. [
1]
Selected Nitrogen Compounds
Compound Formula
Carbon-Nitrogen
Bond Energy
(kJ/mol)
hydrogen cyanide 890.
isocyanic acid 615
H
H
HC
N
O
HC
N
methanamine
293
H
C
H
H
N
P.S./Chem.–Aug. ’09 [9] [OVER]
P.S./Chem.–Aug. ’09 [10]
64 Based on data collected during a laboratory investigation, a student determined an
experimental value of 322 joules per gram for the heat of fusion of H
2
O. Calculate the
student’s percent error. Your response must include a correct numerical setup and the
calculated result. [
2]
Base your answers to questions 65 through 67 on the information below.
A student used blue litmus paper and phenolphthalein paper as indicators to test the
pH of distilled water and five aqueous household solutions. Then the student used a pH
meter to measure the pH of the distilled water and each solution. The results of the
student’s work are recorded in the table below.
Testing Results
65 Identify the liquid tested that has the lowest hydronium ion concentration. [
1]
66 Explain, in terms of the pH range for color change on Reference Table M, why litmus
is not appropriate to differentiate the acidity levels of tomato juice and vinegar. [
1]
67 Based on the measured pH values, identify the liquid tested that is 10 times more acidic
than vinegar. [
1]
Liquid Tested
Color of
Blue Litmus
Paper
Color of
Phenolphthalein
Paper
Measured pH
Value Using a
pH Meter
2% milk blue colorless 6.4
distilled water blue colorless 7.0
household ammonia blue pink 11.5
lemon juice red colorless 2.3
tomato juice red colorless 4.3
vinegar red colorless 3.3
Part C
Answer all questions in this part.
Directions (64–81): 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 68 through 72 on the information below.
Biodiesel is an alternative fuel for vehicles that use petroleum diesel. Biodiesel is
produced by reacting vegetable oil with CH
3
OH. Methyl palmitate, C
15
H
31
COOCH
3
, a
compound found in biodiesel, is made from soybean oil. One reaction of methyl palmitate
with oxygen is represented by the balanced equation below.
2C
15
H
31
COOCH
3
+ 49O
2
→ 34CO
2
+ 34H
2
O + energy
68 Write an IUPAC name for the compound that reacts with vegetable oil to produce
biodiesel. [
1]
69 Explain, in terms of both atoms and molecular structure, why there is no isomer of
CH
3
OH. [1]
70 Identify the class of organic compounds to which methyl palmitate belongs. [
1]
71 Identify the type of organic reaction represented by the balanced equation. [
1]
72 State evidence from the balanced equation that indicates the reaction is exothermic. [
1]
Base your answers to questions 73 through 76 on the information below.
In a laboratory investigation, a student constructs a voltaic cell with iron and copper
electrodes. Another student constructs a voltaic cell with zinc and iron electrodes. Testing
the cells during operation enables the students to write the balanced ionic equations below.
Cell with iron and copper electrodes: Cu
2+
(aq) + Fe(s) → Cu(s) + Fe
2+
(aq)
Cell with zinc and iron electrodes: Fe
2+
(aq) + Zn(s) → Fe(s) + Zn
2+
(aq)
73 State evidence from the balanced equation for the cell with iron and copper electrodes
that indicates the reaction in the cell is an oxidation-reduction reaction. [
1]
74 Identify the particles transferred between Fe
2+
and Zn during the reaction in the cell
with zinc and iron electrodes. [
1]
75 Write a balanced half-reaction equation for the reduction that takes place in the cell
with zinc and iron electrodes. [
1]
76 State the relative activity of the three metals used in these two voltaic cells. [
1]
P.S./Chem.–Aug. ’09 [11] [OVER]
P.S./Chem.–Aug. ’09 [12]
Base your answers to questions 77 through 79 on the information below.
A method used by ancient Egyptians to obtain copper metal from copper(I) sulfide ore
was heating the ore in the presence of air. Later, copper was mixed with tin to produce a
useful alloy called bronze.
77 Calculate the density of a 129.5-gram sample of bronze that has a volume of 14.8 cubic
centimeters. Your response must include a correct numerical setup and the calculated
result. [
2]
78 Convert the melting point of the metal obtained from copper(I) sulfide ore to degrees
Celsius. [
1]
79 A 133.8-gram sample of bronze was 10.3% tin by mass. Determine the total mass of tin
in the sample. [
1]
Base your answers to questions 80 and 81 on the information below.
Scientists are investigating the production of energy using hydrogen-2 nuclei
(deuterons) and hydrogen-3 nuclei (tritons). The balanced equation below represents one
nuclear reaction between two deuterons.
2
1
H +
2
1
H →
3
2
He +
1
0
n + 5.23 × 10
−13
J
80 State, in terms of subatomic particles, how a deuteron differs from a triton. [
1]
81 Identify the type of nuclear reaction represented by the equation. [
1]
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING
CHEMISTRY
Thursday, August 13, 2009 — 12:30 to 3:30 p.m., only
ANSWER SHEET
Student . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Sex: I Male I 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
Tear Here
Tear Here
PS/CHEMISTRY
PS/CHEMISTRY
51 __________________________________
52 mol
53
Reaction Coordinate
Potential Energy
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, August 13, 2009 — 12:30 to 3:30 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
51
53
52
54
55 g
56 ________ Zn(s)
+ ________ HCl(aq) → ________ H
2
(g) + ________ ZnCl
2
(aq)
57
58
[2]
For Raters
Only
54
55
56
57
58
[3] [OVER]
59
60 __________________________________
61
62
63 ppm
For Raters
Only
60
61
62
59
63
Total Score
for Part B–2
[4]
For Raters
Only
64
%
65
66
67
Part C
67
64
66
65
[5] [OVER]
68
69
70
71
72
73
74
75
76
For Raters
Only
69
68
70
71
72
73
74
75
76
For Raters
Only
77
g/cm
3
78 °C
79 g
80
81
[6]
81
Total Score
for Part C
79
80
77
78
PS/CHEMISTRY
PS/CHEMISTRY
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 . . . . . . . . . . .
4
3
1
1
3
3
4
2
1
1
2
4
2
4
1
2
4
4
3
4
1
3
3
4
3
1
1
3
2
2
1
2
4
1
2
2
1
3
4
3
2
1
3
3
4
2
3
2
4
2
FOR TEACHERS ONLY
The University of the State of New York
REGENTS HIGH SCHOOL EXAMINATION
PHYSICAL SETTING/CHEMISTRY
Thursday, August 13, 2009 — 12:30 to 3:30 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.
Part A 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 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,
August 13, 2009. 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:
Na
sodium
element 11
52 [
1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are
not limited to:
28 mol
53 [
1] Allow 1 credit.
Example of a 1-credit response:
54 [
3] Allow a maximum of 3 credits, allocated as follows:
• Allow 1 credit for stating that an electron has a negative charge.
• Allow 1 credit for stating that electrons are located in orbitals or regions of most probable location.
• Allow 1 credit for stating that a carbon atom has six electrons.
Reaction Coordinate
Potential Energy
55 [1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are
not limited to:
438 g
437.8 g
56 [
1] Allow 1 credit for _____ Zn(s) + __2__ HCl(aq) → _____ H
2
(g) + _____ ZnCl
2
(aq).
Allow credit even if the coefficient “1” is written in front of Zn(s), H
2
(g), and/or ZnCl
2
(aq).
57 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
The product ZnCl
2
is soluble in water.
58 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
The greater surface area in powdered zinc would have resulted in more frequent collisions
between the zinc atoms and the hydrogen ions in the HCl(aq).
59 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
The structural formula for methanamine shows electrons being shared, so the bond is covalent.
Electrons are shared in the bond.
covalent bonding due to shared electrons
60 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
Ne
neon
element 10
PHYSICAL SETTING/CHEMISTRY – continued
[5] [OVER]
PHYSICAL SETTING/CHEMISTRY – continued
[6]
61 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
As the number of shared electrons in a carbon-nitrogen bond increases, the bond energy
increases.
Less energy is required to break a single carbon-nitrogen bond than to break a triple
carbon-nitrogen bond.
62 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
The molecule has an asymmetrical charge distribution.
The molecule has an unequal distribution of charge.
63 [
1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are
not limited to:
230 ppm
2.31 × 10
2
ppm
PHYSICAL SETTING/CHEMISTRY – continued
[7] [OVER]
Part C
Allow a total of 20 credits for this part. The student must answer all questions in this part.
64 [
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 a correct response or for a response consistent with the student’s numerical setup.
Significant figures do not need to be shown. Acceptable responses include, but are not limited to:
–3.6%
4%
Note: Do not allow credit for a numerical setup and calculated result that are not related to the
concept assessed by the question.
65 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
household ammonia
NH
3
(aq)
66 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
Because litmus changes color in a pH range of 5.5 to 8.2, litmus cannot be used to differentiate
between a pH of 3.3 and 4.3.
Litmus is red for all pH values below 5.5.
67 [
1] Allow 1 credit for lemon juice.
12
334
100×
322 334
334
100
J/g J/g
J/g
−
×
PHYSICAL SETTING/CHEMISTRY – continued
[8]
68 [1] Allow 1 credit for methanol or methyl alcohol.
69 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
With only one carbon atom bonded to one oxygen atom, there can be no rings or chains with
branches in the molecular structure.
There are too few atoms to create a different molecular structure.
70 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
ester
esters
71 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
combustion
72 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
The balanced equation shows energy as a product of the reaction.
Energy is on the right side of the arrow.
73 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
The oxidation number of Cu
2+
changes to 0.
Iron’s oxidation state changes from zero to +2.
Oxidation numbers change during the reaction because electrons are transferred.
74 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
electrons
e
−
75 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
Fe
2+
+2e
−
→ Fe
PHYSICAL SETTING/CHEMISTRY – concluded
76 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
Zinc is more reactive than iron, and iron is more reactive than copper.
The order of decreasing activity is Zn, Fe, Cu.
Copper is least active and zinc is most active.
77 [
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 8.75 g/cm
3
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.
78 [
1] Allow 1 credit for 1084°C.
79 [
1] Allow 1 credit. Significant figures do not need to be shown. Acceptable responses include, but are
not limited to:
13.8 g
80 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
A deuteron has one neutron and a triton has two neutrons.
A deuteron has one fewer neutron than a triton.
81 [
1] Allow 1 credit. Acceptable responses include, but are not limited to:
fusion
thermonuclear fusion
129 5
14 8
.
.
d
m
V
==
129 5
14 8
.
.
g
cm
3
[9] [OVER]
[10]
The Chart for Determining the Final Examination Score for the August 2009
Regents Examination in Physical Setting/Chemistry will be posted on the
Department’s web site http://www.emsc.nysed.gov/osa/
on Thursday,
August 13, 2009. 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
August 2009
Chart for Converting Total Test Raw Scores to
Final Examination Scores (Scaled Scores)
Online Submission of 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.
[11]
Map to Core Curriculum
August 2009 Physical Setting/Chemistry
Question Numbers
Key Ideas Part A Part B Part C
Standard 1
Math Key Idea 1
40, 43 64, 69, 77
Math Key Idea 2
40, 44, 61
Math Key Idea 3
36, 37, 48, 49, 52,
63
64, 77, 78, 79
Sci. Inquiry Key Idea 1
58, 59 69, 74, 76
Sci. Inquiry Key Idea 2
Sci. Inquiry Key Idea 3
31, 32, 33, 34, 37,
42, 46, 48, 51, 57,
62
65, 66, 67, 68, 70,
71, 72, 73, 77
Eng. Design Key Idea 1
Standard 2
Key Idea 1 34 78
Key Idea 2 63
Standard 6
Key Idea 1
39
Key Idea 2
38, 42 64
Key Idea 3
65, 67
Key Idea 4
Key Idea 5
Standard 7
Key Idea 1
Key Idea 2
Standard 4 Process Skills
Key Idea 3
31, 32, 33, 35, 36,
40, 41, 45, 46, 47,
48, 49, 51, 52, 54,
55, 56, 58, 63
65, 66, 67, 70, 71,
75, 76, 80
Key Idea 4
50, 53 72, 81
Key Idea 5
38, 59, 60
Standard 4
Key Idea 3
1, 2, 3, 4, 6, 7, 8,
12, 13, 15, 16, 17,
19, 20, 21, 22, 23,
24, 25, 26, 27, 28
31, 32, 33, 34, 35,
36, 37, 40, 41, 42,
44, 45, 46, 47, 48,
49, 51, 52, 54, 55,
56, 57, 58, 63
65, 66, 67, 68, 69,
70, 71, 73, 74, 75,
76, 77, 78, 79, 80
Key Idea 4
18, 30 39, 43, 50, 53 64, 72, 81
Key Idea 5
5, 9, 10, 11, 14, 29 38, 59, 60, 61, 62
Reference Tables
2002 Edition
1, 2, 3, 7, 11, 12,
23, 30
31, 32, 33, 34, 36,
37, 38, 40, 43, 44,
46, 47, 48, 49, 50,
51, 55, 57, 59, 60,
63
64, 65, 66, 68, 70,
75, 77, 78
Regents Examination in Physical Setting/Chemistry
August 2009
Chart for Converting Total Test Raw Scores to
Final Examination Scores (Scale Scores)
Raw
Score
Scale
Score
Raw
Score
Scale
Score
Raw
Score
Scale
Score
Raw
Score
Scale
Score
85
100
63
74
41
58
19
38
84
98
62
73
40
58
18
37
83
97
61
72
39
57
17
36
82
95
60
71
38
56
16
35
81
93
59
71
37
55
15
33
80
92
58
70
36
55
14
32
79
90
57
69
35
54
13
30
78
89
56
68
34
53
12
28
77
88
55
68
33
52
11
27
76
87
54
67
32
52
10
25
75
85
53
66
31
51
9
23
74
84
52
66
30
50
8
21
73
83
51
65
29
49
7
19
72
82
50
64
28
48
6
17
71
81
49
64
27
47
5
14
70
80
48
63
26
46
4
12
69
79
47
62
25
45
3
9
68
78
46
62
24
44
2
6
67
77
45
61
23
43
1
3
66
76
44
60
22
42
0
0
65
75
43
60
21
41
64
74
42
59
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 scale score that corresponds to that raw score. The
scale 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 scale score of 60 through 64 must be scored a
second time to ensure the accuracy of the score. 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 scale 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.
