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XIX. Chemistry, High School
486
High School Chemistry TestThe spring 2007 high school MCAS Chemistry test was based on learning standards in the Chemistry content strand of the Massachusetts Science and Technology/Engineering Curriculum Framework (2006). These learning standards appear on pages 69–73 of the Framework.
The Science and Technology/Engineering Curriculum Framework is available on the Department Web site at www.doe.mass.edu/frameworks/current.html.
In Test Item Analysis Reports and on the Subject Area Subscore pages of the MCAS School Reports and District Reports, Chemistry test results are reported under the following four MCAS reporting categories:
■ Atomic Structure and Periodicity
■ Bonding and Reactions
■ Properties of Matter and Thermochemistry
■ Solutions, Equilibrium, and Acid-Base Theory
Test Sessions
The MCAS high school Chemistry test included two separate test sessions, which were administered on consecutive days. Each session included multiple-choice and open-response questions.
Reference Materials and Tools
Each student taking the high school Chemistry test was provided with a Chemistry Formula and Constants Sheet/Periodic Table of the Elements. Copies of both sides of this formula sheet follow the final question in this chapter.
Each student also had sole access to a calculator with at least four functions and a square-root key.
The use of bilingual word-to-word dictionaries was allowed for current and former limited English proficient students only, during both Chemistry test sessions. No other reference tools or materials were allowed.
Cross-Reference Information
The table at the conclusion of this chapter indicates each item’s reporting category and the Framework learning standard it assesses. The correct answers for multiple-choice questions are also displayed in the table.
Idaho Inmate Search
487
DIRECTIONSThis session contains twenty-three multiple-choice questions and three open-response questions. Mark your answers to these questions in the spaces provided in your Student Answer Booklet. You may work out solutions to multiple-choice questions in the test booklet.
ID:206664 208253_methanedot.eps [op A Common
●1 Whichof the followingLewis dotstructures represents the compoundmethane (CH4)?
A.
HH
HC H
B. HH C H H
C.
HH
HCH
D.
HH
HC H
ID:242514 B Common
●2 Whichof the followingmolecules has the same empirical formula asglucose (C6H12O6)?
A. butane (C4H10)
B. ethanoic acid (C2H4O2)
C. propene (C3H6)
D. sucrose (C12H22O11)
ID:242497 C Common
●3 1s22s22p63s23p64s1 is the electronconfiguration forwhich element?
A. aluminum (Al)
B. argon (Ar)
C. potassium (K)
D. sodium (Na)
ID:208297 B Common
●4 What is themassof onemoleof heliumgas?
A. 2 g
B. 4 g
C. 8 g
D. 22g
ChemistrySeSSion 1
Alabama Inmate Search
488
ID:206749 C Common
●5 Whichof the following correctlydescribesmolecules of twodifferentgases if they are at the sametemperature andpressure?
A. Theymust have the samemass.
B. Theymust have the samevelocity.
C. Theymust have the same averagekinetic energy.
D. Theymust have the same averagepotential energy.
Chemistry Session 1
ID:242515 C Common
●6 Aluminum reactswithoxygengas toformaluminumoxide, as shown in thereactionbelow.
4 3 22 2 3Al(s) O (g) Al O (s) →
Howmanygramsof aluminumareneeded to completely reactwith192gof oxygengas?
A. 27.0g
B. 102g
C. 216g
D. 432g
Michigan Inmate Search
489
ID:208229 208229_thoriumdecay.eps, A Common
●8 The equationbelow shows theradioactivedecayof thorium (Th).
Th23290 Ra228
88 � Radiation→
Whichof the followingparticles isreleased in this reaction?
A. alpha ( He)42
B. beta ( e)0–1
C. neutron ( n)10
D. proton ( H)11
ID:226994 3244790_AR1.eps A Common
●7 The table belowgives information about four aqueous solutionsof sodiumnitrate (NaNO3).
BeakerConcentrationof NaNO3 (%)
Temperature (°C)
1
2
3
4
20
20
2
2
0
40
80
100
Inwhichbeakerwill an additional 10gof sodiumnitrate (NaNO3) dissolve atthe slowest rate?
A. 1
B. 2
C. 3
D. 4
Chemistry Session 1
New York Inmate SearchNorth Carolina Inmate Search
490
ID:230487 D Common
●10 A solution that contains less solute thanit canhold at a given temperature is
A. disassociated.
B. saturated.
C. supersaturated.
D. unsaturated.
ID:208291 208291_Voltemp.eps A Common
●9 Assumingpressure is held constant,whichof the followinggraphs showshow thevolumeof an ideal gas changeswith temperature?
A. C.
B. D.
Temperature (K)
0.05
0.15
0.25
0.35
0.00
0.10
0.20
0.30
200 250 300 350 400
Vol
ume
of G
as S
ampl
e (L
)
Temperature (K)
0.05
0.15
0.25
0.35
0.00
0.10
0.20
0.30
200 250 300 350 400
Vol
ume
of G
as S
ampl
e (L
)
Temperature (K)
0.05
0.15
0.25
0.35
0.00
0.10
0.20
0.30
200 250 300 350 400
Vol
ume
of G
as S
ampl
e (L
)
Temperature (K)
0.05
0.15
0.25
0.35
0.00
0.10
0.20
0.30
200 250 300 350 400
Vol
ume
of G
as S
ampl
e (L
)
Chemistry Session 1
491
Question 11 is an open-response question.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION.• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 11 in the space provided in your Student Answer Booklet.
ID:206756 Alexma26.eps Common
●11 The temperature of anunknown substancewasmeasured as it cooled.The temperature of the substanceover timewasgraphedand thegraphwasdivided intofivedifferent zones, as shown below. In zoneA, the substancewas a gas.
0
200
250
300
350
400
450
500
10 20 30 40 50
A B C D E
Time (min)
Tem
pera
ture
(K
)
Cooling Curveof an Unknown Substance
Comparewhat happened at theparticle level in three of the four remaining zones: B,C,D, andE.
For each zoneyou choose, discuss all of the following:
• energyof theparticles
• motionof theparticles
• arrangement of theparticles
• state(s) ofmatter present
Chemistry Session 1
492
Mark your answers to multiple-choice questions 12 through 24 in the spaces provided in your Student Answer Booklet. Do not write your answers in this test booklet, but you may work out solutions to multiple-choice questions in the test booklet.
ID:208233 B Common
●12 The atomicnumberof an elementindicateswhichof the following?
A. thenumberof neutrons in the atom
B. thenumberof protons in the atom
C. the sumof theneutrons andprotonsin the atom
D. the sumof theprotons and electronsin the atom
ID:266328 B Common
●13 The table below shows someinformation for four different elements.
Element ClassificationDensity (g/cm³)
barium (Ba) metal 3.6
beryllium (Be) metal 1.8
chromium (Cr) metal 7.2
phosphorus (P) nonmetal 1.8
A cubeof anunknownelement has ashiny, silvery color.The sideof the cubemeasures 2.0 cmand the cubehas amass of 14.56g.
Basedon the information in the table,which elementmakesup the cube?
A. barium
B. beryllium
C. chromium
D. phosphorus
ID:242510 C Common
●14 What is thepercentmass oxygen in acetone (C3H6O)?
A. 1.00%B. 10.3%C. 27.6%D. 62.0%
ID:216961 C Common
●15 Whichof the following isnot true of asampleof gas as it is heated in a rigid,closed container?
A. Thepressureof the molecules increases.
B. The average speedof the molecules increases.
C. The averagedistancebetweenmolecules increases.
D. Thenumberof collisionsbetweenmolecules increases.
Chemistry Session 1
493
ID:230409 3183207_AR1.eps A Common
●16 Thefigurebelow represents a reaction.
S = sulfur atom
oxygen atom=
= hydrogen atom
S + S
What typeof reaction is shown?
A. synthesis
B. decomposition
C. single displacement
D. double displacement
ID:208317 A Common
●18 The equationbelow shows ammoniadissolving inwater.
NH (aq) H O( ) NH (aq) OH (aq)3 2 l 4
Why iswater considered an acidwhenammonia is dissolved in it?
A. Water acts as a proton donor.
B. Water acts as a proton acceptor.
C. Water contains hydrogen atoms.
D. Water has a 2:1 ratio of hydrogen to oxygen.
ID:265419 D Common
●17 Thedensity of a gas is 1.35g/L atstandard temperature andpressure (STP).What is themolarmass of thegas atSTP?
A. 0.0603g/mol
B. 6.02g/mol
C. 22.4g/mol
D. 30.2g/mol
Chemistry Session 1
494
ID:208299 C Common
●19 Howmany atoms are in a 12.0g sampleof lithium?
A. 1 74 1023. 3 atoms
B. 6 02 1023. 3 atoms
C. 1 04 1024. 3 atoms
D. 7 24 1024. 3 atoms
Chemistry Session 1
ID:230371 3183204_AR1.eps A Common
●20 The table belowcontains data for watersamples from four sources.
Analysis of Water Samples
Source of Water
Sample Volume (mL)
pH
Rain
Creek
Pool
Faucet
5
20
10
20
5.7
7.9
7.4
6.8
Nancy analyzedwater samples fromseveral sources: rainfall, a nearby creek,a swimmingpool, andherkitchen faucet.She recordedherdata in the table.
Whichsamplewasmostacidic?
A. rain
B. creek
C. pool
D. faucet
495
Chemistry Session 1
ID:208310 208310_equation.eps A Common
●21 An equation for an equilibrium reactionis shown below.
SO2(g) � NO2(g) � SO3(g) � NO(g) � 41.7 kJ
Whichof the following changes inreaction conditionswillnot shift theequilibriumof the system?
A. an increase in thepressure
B. an increase in the temperature
C. a decrease in theSO3 concentration
D. a decrease in theNO2 concentration
ID:242505 D Common
●22 The threemain typesof nuclearradiation are alpha, beta, andgamma.Whichof the following lists these typesof radiation fromhighest penetratingpower to lowest penetratingpower?
A. alpha, gamma, beta
B. beta, alpha, gamma
C. beta, gamma, alpha
D. gamma, beta, alpha
ID:206655 C Common
●23 Water cools from2°C to2°C.Duringthis time,what happens to themotionofthemolecules?
A. Themotionof themolecules stops.
B. Themotionof themoleculesincreases.
C. Themotionof themoleculesdecreases.
D. Themotionof themolecules remains the same.
ID:208247 A Common
●24 Whichof the following elements hascharacteristics of somemetals and alsoof somenonmetals?
A. antimony (51Sb)
B. calcium (20Ca)
C. sulfur (16S)
D. zinc (30Zn)
496
Questions 25 and 26 are open-response questions.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF EACH QUESTION.• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 25 in the space provided in your Student Answer Booklet.
ID:266331 Alexma27.eps Common
●25 An earlymodel of the atom, shownbelow, incorrectly described the structure of the atom as an areaof positive chargeswith small, negatively chargedparticles inside.
The Plum PuddingModel of an Atom
Positively charged
Negativelycharged particles
Compare a currently acceptedmodel of the atomwith this plumpuddingmodel. Includeinformation about (1) the typesof particles, (2) their charges, and (3) their locations for eachmodel.
Chemistry Session 1
497
Write your answer to question 26 in the space provided in your Student Answer Booklet.
ID:208280 208280_scoring1.eps, 2082 Common
●26 Magnesiumoxide,MgO(s), is an ionic compound.Water,H2O(l ), is a covalent compound.
a. Explainhowatoms are held together in both ionic and covalent compounds.
Thebondingof atoms in a compoundusuallymakes themmore stable than atoms that exist by themselves.
b. Chooseoneof thegiven compounds,MgO(s) orH2O(l ), and explain in detail how itsatomsbond to forma stable compound.Youmayuse a diagram inyour response.
Chemistry Session 1
498
DIRECTIONSThis session contains seventeen multiple-choice questions and two open-response questions. Mark your answers to these questions in the spaces provided in your Student Answer Booklet. You may work out solutions to multiple-choice questions in the test booklet.
ID:206654 D Common
●27 Whichof the following explainswhysaltwater is considered amixture?
A. It is composedof one element.
B. It is composedof one compound.
C. It is composedof twoor more substances andhas newchemical properties.
D. It is composedof twoormoresubstances that retain their own chemical properties.
ID:251822 A Common
●28 The tablebelowcontainsa listofproperties foranunidentifiedelement,X.
Physical Characteristics
Verysoftwithsilvery-whitelusterwhencut
ReactivityIgnitesinairandreactsviolentlywithcoldH2O
Some Common Compounds
XCl,X2SO4,X3PO4,XOH,X2O
Melting Point (°C)
39.1
Boiling Point (°C)
688
Basedon theproperties in the table,towhichof the followinggroups fromtheperiodic table does elementXmost likely belong?
A. 1 (1A)
B. 2 (2A)
C. 14 (4A)
D. 16 (6A)
ChemistrySeSSion 2
499
ID:208225 Wolcar006_Alpha_deflect.e B Common
●29 ErnestRutherfordperformed an experiment inwhichhe shot alphaparticles through a thinlayer of gold foil.Hepredicted that the alphaparticleswould travel straight through thegoldatoms, as shownbelow.
Path of alpha particles
Gold atom
However,Rutherfordobserved that althoughmost of the alphaparticles passed straight throughthe foil, a fewalphaparticlesweredeflected, as shownbelow.
Path of alpha particles
Gold atom
Whichof the following statements about the atomdidRutherford’s experiment support?
A. An atomcontains protons, neutrons, and electrons.
B. An atom’snucleus is small andhas a positive charge.
C. Electrons followapredictable path around thenucleus.
D. Different isotopesof an element havedifferentmasses.
Chemistry Session 2
500
ID:206665 B Common
●30 Whichof the following chemicalequations is balanced correctly?
A. C H O CO H O6 6 2 2 22 3 →B. CS Cl CCl S Cl2 2 4 2 23 →C. B O C B C CO2 3 42 →D. Cl NaI NaCl I2 22 →
ID:242566 C Common
●31 Under certain conditions, solidmagnesium (Mg) and solid sulfur (S)can combine and formmagnesiumsulfide (MgS).Theoxidation-reductionreaction is shownbelow.
Mg(s) S(s) MgS(s) →
Whichof the following is theoxidationnumber forMg inMgS in this reaction?
A. 1
B. 1
C. 2
D. 2
Chemistry Session 2
501
ID:229560 Common
●32 The equationbelow represents the reactionofwater andoxygen to producehydrogenperoxide(H2O2).The equation shows the reaction to be at equilibrium.
2H O(g) O (g) heat 2H O (g)2 2 2 2+ +
Describe twoways to shift the equilibrium to the right in order to increase the amount ofH2O2produced.Explainyour reasoning.
Chemistry Session 2
Question 32 is an open-response question.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION.• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 32 in the space provided in your Student Answer Booklet.
502
Mark your answers to multiple-choice questions 33 through 38 in the spaces provided in your Student Answer Booklet. Do not write your answers in this test booklet, but you may work out solutions to multiple-choice questions in the test booklet.
ID:230545 3075934_AR1.eps C Common
●35 Thetablebelowshowssomecharacteristicsof four substances at 1 atmpressure.
Bromine
Chlorine
Ethanol
Mercury
red-brown
green-yellow
colorless
silver-white
–7
–101
–117
–39
59
–34
78
357
Substance ColorMelting
Point(°C)
Boiling Point (°C)
Whichof the following substances isa liquid at temperatures ranging from50°C to0°C?
A. bromine
B. chlorine
C. ethanol
D. mercury
ID:216955 D Common
●33 Whichof the following is the formulafor ammoniumhydroxide?
A. Al2O3
B. AmO2
C. NH3OH
D. NH4OH
ID:242553 A Common
●34 A student adds68.4gof sucrose(C12H22O11) to 750mLof 20°Cwater.She stirs the solutionuntil all of thesucrose crystals dissolve.She thentransfers the solution to a volumetricflask andfills it to the1.00Lmark with20°Cwater.
What is themolarity of the sucrosesolution the student prepared?
A. 0.20M
B. 0.70M
C. 1.0M
D. 6.8M
Chemistry Session 2
503
ID:229512 3152384_AR1.eps, 3152384_ C Common
●36 In the followingdiagrams, the spheresrepresent particles.Different shadingsrepresent different particles.
Whichof the following contains onlyonepure substance?
A.
B.
C.
D.
ID:266337 B Common
●37 Nuclear fusionoccurs in the core of astarwhendeuteriumand tritium react.The equationbelow represents thisfusion reaction.
12
13
24
01H H He+ → + n
Whichof the followingbest explainswhy a large amount of energy isreleased in this reaction?
A. Thehydrogen converts the light into energy.
B. Someof the reactantmass isconverted into energy.
C. All of thehydrogen isotopes undergo radioactivedecay.
D. The temperature of theproducts islower than that of the reactants.
ID:208268 C Common
●38 Anunknownmetal,X, combineswithnitrogen to form the compoundXN.MetalX also combineswithoxygen to produce the compoundX2O3.
MetalX ismost likelywhichof thefollowing elements?
A. 3Li
B. 12Mg
C. 31Ga
D. 50Sn
Chemistry Session 2
504
Question 39 is an open-response question.
• BE SURE TO ANSWER AND LABEL ALL PARTS OF THE QUESTION.• Show all your work (diagrams, tables, or computations) in your Student Answer Booklet.• If you do the work in your head, explain in writing how you did the work.
Write your answer to question 39 in the space provided in your Student Answer Booklet.
ID:254468 Common
●39 Propane (C3H8) burns in oxygen to produce carbondioxide andwater.
a. Write a balanced chemical equation for this reaction.
b. If 11.0gof propanegas is burned completely, 33.0gof carbondioxide and18.0gofwater are produced.Determine themassof oxygen consumed.Showyour calculations andincludeunits in your answer.
Chemistry Session 2
505
ID:266338 A Common
●41 When stirred in 30°Cwater, 5 g ofpowderedpotassiumbromide,KBr,dissolves faster than5gof largecrystals of potassiumbromide.Whichof the followingbest explainswhy thepowderedKBrdissolves faster?
A. Powdered potassiumbromide exposesmore surface area towatermolecules than large crystals ofpotassiumbromide.
B. Potassium ions andbromide ionsin thepowder are smaller thanpotassium ions andbromide ionsin the large crystals.
C. Fewerpotassium ions andbromideionshavebeen separated from eachother in thepowder thanin the crystals.
D. Powdered potassiumbromide isless dense than large crystals ofpotassiumbromide.
ID:206658 B Common
●40 A1.00kg sampleofwater (H2O)contains 0.11kgof hydrogen (H) and0.89kgof oxygen (O).According to thelawof constant composition, howmuchhydrogen andoxygenwould a 1.5 kgsampleofwater contain?
A. 0.11kgHand0.89kgO
B. 0.17kgHand1.34kgO
C. 0.22kgHand1.78kgO
D. 1.34kgHand0.17kgO
Chemistry Session 2
Mark your answers to multiple-choice questions 40 through 45 in the spaces provided in your Student Answer Booklet. Do not write your answers in this test booklet, but you may work out solutions to multiple-choice questions in the test booklet.
506
ID:208244 D Common
●42 Whichof the following is an example of a physical change?
A. Iron exposed to air produces rust.
B. Hydrogen combinedwithoxygenformswater.
C. Sulfur combinedwithoxygenproduces sulfur dioxide.
D. Liquidnitrogen exposed to airbecomesnitrogengas.
ID:216950 B Common
●43 Whichof the following trends in theperiodic table shouldbe expected as theatomicnumberof thehalogens increasesfromfluorine (F) to iodine (I)?
A. Atomic radius decreases.
B. Electronegativity decreases.
C. Atomicmassdecreases.
D. Electronnumberdecreases.
ID:208276 A Common
●44 Whichof the following statementsdescribes the elements in family16 of theperiodic table?
A. Theyhave six valence electrons.
B. Theyareallgasesatroomtemperature.
C. They exist commonly as cations in nature.
D. They combine easilywith elementsin family17.
ID:208251 C Common
●45 What is thevolumeof onemoleof hydrogengas (H2) at standardtemperature andpressure (STP)?
A. 1.0L
B. 2.0L
C. 22.4L
D. 44.8L
Chemistry Session 2
507
Common Polyatomic Ions
Ion Ionic Formula
Ammonium NH4
Carbonate CO32-
Hydroxide OH-
Nitrate NO3-
Phosphate PO43-
Sulfate SO42-
Combined Gas Law: P V
T
P V
T1 1
1
2 2
2
5
Ideal Gas Law: PV nRT5
Absolute Temperature Conversion: K 5 °C 273
Moles of Solute: M V M V1 1 2 25
Definition of pH: pH5log[H3O]5log[H]
Molar Volume of Ideal Gas at STP: 22.4L/mol
Ideal Gas Constant: R 5 0.0821L• atm/mol• K 58.31L• kPa/mol• K
Avogadro’s Number: 6.0231023particles/mol
STP: 1atm(101.3kPa),273K(0°C)
Nuclear Symbols
Name Symbol
Alpha particle or 24 He
Beta particle bor−10e
Gamma ray
Neutron 01n
Massachusetts Comprehensive Assessment System Chemistry Formula and Constants Sheet
508
6.94
1 Li 3Li
thiu
m
1.00
794 H 1
Hyd
roge
n
9.01
218
Be 4
Ber
ylliu
m
2A 23A 13
4A 145A 15
6A 167A 17
3B 34B 4
5B 56B 6
7B 7
8B
89
101B 11
2B 12
22.9
8977
Na
11S
odiu
m
24.3
05 Mg
12M
agne
sium
39.0
983 K 19
Pot
assi
um
40.0
8 Ca
20C
alci
um85
.467
8
Rb
37R
ubid
ium
87.6
2 Sr
38S
tron
tium
132.
905
Cs
55C
esiu
m
137.
33 Ba
56B
ariu
m(2
23) Fr 87
Fran
cium
226.
025
Ra
88R
adiu
m
44.9
559
Sc
21S
cand
ium
47.8
8 Ti
22T
itani
um88
.905
9 Y 39Y
ttriu
m
91.2
24 Zr
40Z
ircon
ium
138.
906
La 57La
ntha
num
178.
49 Hf
72H
afni
um22
7.02
8
Ac
89A
ctin
ium
(261
) Rf*
104
Rut
herf
ordi
um
50.9
415 V 23
Van
adiu
m
51.9
96 Cr
24C
hrom
ium
92.9
064
Nb
41N
iobi
um
95.9
4 Mo
42M
olyb
denu
m18
0.94
8
Ta 73Ta
ntal
um
183.
85 W 74Tu
ngst
en(2
62) Db
105
Dub
nium
(263
) Sg
106
Sea
borg
ium
54.9
380
Mn
25M
anga
nese
55.8
47 Fe 26 Iron
(98)
Tc
43Te
chne
tium
101.
07 Ru
44R
uthe
nium
186.
207
Re
75R
heni
um
190.
2 Os
76O
smiu
m(2
62) Bh
107
Boh
rium
(265
) Hs
108
Has
sium
58.9
332
Co
27C
obal
t
58.6
9 Ni
28N
icke
l10
2.90
6
Rh
45R
hodi
um
106.
42 Pd
46P
alla
dium
192.
22 Ir 77Ir
idiu
m
195.
08 Pt
78P
latin
um(2
66?) M
t10
9M
eitn
eriu
m
(269
?)
63.5
46 Cu
29C
oppe
r
65.3
9 Zn
30 Zin
c10
7.86
8
Ag
47S
ilver
112.
41 Cd
48C
adm
ium
196.
967
Au
79 Gol
d
200.
59 Hg
80M
ercu
ry
10.8
1 B 5B
oron
12.0
111 C 6
Car
bon
26.9
8154
Al
13A
lum
inum
28.0
855
Si
14S
ilico
n69
.72 Ga
31G
alliu
m
72.5
9 Ge
32G
erm
aniu
m11
4.82 In 49
Indi
um
118.
71 Sn
50 Tin
204.
383
Tl
81T
halli
um
207.
2 Pb
82 Lead
14.0
067 N 7
Nitr
ogen
15.9
994 O 8
Oxy
gen
30.9
7376 P 15
Pho
spho
rus
32.0
6 S 16S
ulfu
r74
.921
6
As
33A
rsen
ic
78.9
6 Se
34S
elen
ium
121.
75 Sb
51A
ntim
ony
127.
60 Te 52Te
lluriu
m20
8.98
0
Bi
83B
ism
uth
(209
) Po
84P
olon
ium
18.9
9840
3
F 9F
luor
ine
20.1
79 Ne
10N
eon
35.4
53 Cl
17C
hlor
ine
39.9
48 Ar
18A
rgon
79.9
04 Br
35B
rom
ine
83.8
0 Kr
36K
rypt
on12
6.90
5 I 53Io
dine
131.
29 Xe
54X
enon
(210
) At
85A
stat
ine
(222
) Rn
86R
adon
Gro
up (
Fam
ily)
1A 14.
0026
0
He 2
Hel
ium
8A 18
1
111
112
113
114
115
116
117
118
110
140.
12 Ce
58C
eriu
m
140.
908
Pr
59P
rase
odym
ium
232.
038
Th
90T
horiu
m
231.
036
Pa
91P
rota
ctin
ium
144.
24 Nd
60N
eody
miu
m
(145
) Pm 61
Pro
met
hium
238.
029 U 92
Ura
nium
237.
048
Np
93N
eptu
nium
150.
36 Sm 62
Sam
ariu
m
151.
96 Eu
63E
urop
ium
(244
) Pu
94P
luto
nium
(243
) Am 95
Am
eric
ium
157.
25 Gd
64G
adol
iniu
m
158.
925
Tb
65Te
rbiu
m(2
47) Cm 96
Cur
ium
(247
) Bk
97B
erke
lium
162.
50 Dy
66D
yspr
osiu
m
164.
930
Ho
67H
olm
ium
(251
) Cf
98C
alifo
rniu
m
(252
) Es
99E
inst
eini
um
167.
26 Er
68E
rbiu
m
168.
934
Tm 69
Thu
lium
(257
) Fm
100
Fer
miu
m
(258
) Md
101
Men
dele
vium
173.
04 Yb
70Y
tterb
ium
(259
) No
102
Nob
eliu
m
174.
967
Lu 71Lu
tetiu
m(2
60) Lr 10
3La
wre
nciu
m
7654321
Period
Lant
hani
de S
erie
s
Act
inid
e S
erie
s
Mas
s nu
mbe
rs in
par
enth
eses
are
thos
e of
the
mos
t sta
ble
or m
ost c
omm
on is
otop
e.
Mas
sach
use
tts
Com
pre
hen
sive
Ass
essm
ent
Sys
tem
509
High School Chemistry Spring 2007 Released Items:
Reporting Categories, Standards, and Correct Answers
Item No. Page No. Reporting Category StandardCorrect Answer
(MC)*
1 487 Bonding and Reactions 4.2 A
2 487 Bonding and Reactions 5.4 B
3 487 Atomic Structure and Periodicity 2.4 C
4 487 Bonding and Reactions 5.3 B
5 488 Properties of Matter and Thermochemistry 6.3 C
6 488 Bonding and Reactions 5.5 C
7 489 Solutions, Equilibrium, and Acid-Base Theory 7.3 A
8 489 Atomic Structure and Periodicity 2.6 A
9 490 Properties of Matter and Thermochemistry 6.1 A
10 490 Solutions, Equilibrium, and Acid-Base Theory 7.1 D
11 491 Properties of Matter and Thermochemistry 1.3
12 492 Atomic Structure and Periodicity 3.1 B
13 492 Properties of Matter and Thermochemistry 1.1 B
14 492 Bonding and Reactions 5.4 C
15 492 Properties of Matter and Thermochemistry 6.3 C
16 493 Bonding and Reactions 5.2 A
17 493 Properties of Matter and Thermochemistry 6.2 D
18 493 Solutions, Equilibrium, and Acid-Base Theory 8.1 A
19 494 Bonding and Reactions 5.3 C
20 494 Solutions, Equilibrium, and Acid-Base Theory 8.2 A
21 495 Solutions, Equilibrium, and Acid-Base Theory 7.6 A
22 495 Atomic Structure and Periodicity 2.5 D
23 495 Properties of Matter and Thermochemistry 1.3 C
24 495 Atomic Structure and Periodicity 3.2 A
25 496 Atomic Structure and Periodicity 2.1
26 497 Bonding and Reactions 4.1
27 498 Properties of Matter and Thermochemistry 1.2 D
28 498 Atomic Structure and Periodicity 3.1 A
29 499 Atomic Structure and Periodicity 2.2 B
30 500 Bonding and Reactions 5.1 B
31 500 Bonding and Reactions 8.4 C
32 501 Solutions, Equilibrium, and Acid-Base Theory 7.6
33 502 Bonding and Reactions 4.6 D
34 502 Solutions, Equilibrium, and Acid-Base Theory 7.2 A
35 502 Properties of Matter and Thermochemistry 1.3 C
36 503 Properties of Matter and Thermochemistry 1.2 C
37 503 Atomic Structure and Periodicity 2.7 B
38 503 Bonding and Reactions 4.1 C
39 504 Bonding and Reactions 5.1
40 505 Atomic Structure and Periodicity 2.3 B
41 505 Solutions, Equilibrium, and Acid-Base Theory 7.3 A
42 506 Properties of Matter and Thermochemistry 1.1 D
510
Item No. Page No. Reporting Category StandardCorrect Answer
(MC)*
43 506 Atomic Structure and Periodicity 3.4 B
44 506 Atomic Structure and Periodicity 3.1 A
45 506 Properties of Matter and Thermochemistry 6.2 C
*Answersareprovidedhereformultiple-choiceitemsonly.Sampleresponsesandscoringguidelinesforopen-responseitems,whichareindicatedbyshadedcells,willbepostedtotheDepartment’sWebsitelaterthisyear.