CHEMISTRY — RELEASED ITEMS
1 Which isotope has the greatest number of protons?
A Pa-238
B U-240
C Np-238
D Pu-239
2 A neutral atom of a certain element has the electron configuration
1s22s22p63s23p4. How many valence electrons does the atom have?
D
A 4
D
6
11
16
SE
EA
3 What color of light does a hydrogen atom emit when an electron transitions from
the n=6 energy level to the n=2 energy level?
EL
A orange
B yellow
R
C blue
D violet
1 Go to the next page.
CHEMISTRY — RELEASED ITEMS
4 The equation below represents the radioactive decay of a gold isotope.
174 170
79 Au → 77 Ir + ?
Which choice correctly completes this equation?
A alpha particle
B beta particle
C photon
D neutron
D
5
SE
A neutral atom has a ground state electron configuration of 1s22s22p63s2.
The neutral atom becomes an ion during a chemical reaction. Which is the
most likely charge of the ion?
A 2+
EA
B 1+
C 2–
D 6–
EL
6 How many electrons are in the outermost energy level of a neutral carbon atom?
R
A 2
B 4
C 6
D 8
2 Go to the next page.
CHEMISTRY — RELEASED ITEMS
7 The compound sodium chloride is placed in water and separates into ions. What
are the correct names for these ions?
A The chloride and sodium ions are cations.
B The chloride and sodium ions are anions.
C The sodium ion is the anion, and the chloride ion is the cation.
D The sodium ion is the cation, and the chloride ion is the anion.
8 Which element will form covalent bonds with chlorine?
D
A carbon
D
aluminum
magnesium
potassium
SE
EA
9 Which type of bonding or intermolecular forces is/are weakest?
EL
A London dispersion forces
B hydrogen bonding
C dipole-dipole forces
R
D covalent bonding
3 Go to the next page.
CHEMISTRY — RELEASED ITEMS
10 What is the chemical formula for chromium(III) oxide?
A CrO
B CrO2
C Cr2O3
D Cr3O2
11 Test results on two white crystalline solids are shown in the table below:
D
Solid X Solid Y
Melting Point
Solubility in Water
(grams per 100.0
grams of water)
SE801°C
35.7
186°C
3.2
EA
Electrical
Conductivity good conductor nonconductor
(molten state)
EL
Based on the information in the table, what can be concluded?
A Both solids contain only ionic bonds.
B Both solids contain only covalent bonds.
R
C Solid X contains only covalent bonds, and Solid Y contains only ionic bonds.
D Solid X contains only ionic bonds, and Solid Y contains only covalent bonds.
4 Go to the next page.
CHEMISTRY — RELEASED ITEMS
12 What is the name of the compound with the chemical formula CoF3?
A fluorocobalt
B cobalt trifluoride
C cobalt(III) fluoride
D fluorine(III) cobalt
13 Which statement best compares how bond strengths affect the physical properties
of iron and lead?
D
A Iron has a higher melting point because the bonds in iron are stronger.
D
SE
Iron has a higher melting point because the bonds in iron are weaker.
Lead has a higher density because the bonds in lead are stronger.
Lead has a higher density because the bonds in lead are weaker.
EA
14 How is copper (Cu) classified based on its location on the periodic table?
EL
A a nonmetal
B an alkaline earth metal
C a transition metal
R
D an alkali metal
5 Go to the next page.
CHEMISTRY — RELEASED ITEMS
15 The table below shows the electron configurations of three elements.
Electron
Element
Configuration
Element 1 1s22s22p2
Element 2 1s22s22p5
Element 3 1s22s22p4
What is the order of the elements from smallest to largest atomic radius?
A Element 1, Element 2, Element 3
D
B Element 1, Element 3, Element 2
D
SE
Element 2, Element 1, Element 3
Element 2, Element 3, Element 1
EA
16 Which three elements are arranged according to increasing electronegativity
values?
A N, C, B
EL
B N, P, As
C N, O, F
R
D F, O, N
17 Which group of elements is arranged in order of increasing atomic radii?
A O, S, Se, Te
B Fe, Ni, Ag, Au
C Rb, K, Na, Li
D Y, Zr, Nb, Mo
6 Go to the next page.
CHEMISTRY — RELEASED ITEMS
18 Which statement describes equilibrium between liquid water and water vapor?
A The rate of vaporization equals the rate of condensation.
B The rate of vaporization is greater than the rate of condensation.
C The rate of vaporization equals the rate of sublimation.
D The rate of vaporization is greater than the rate of sublimation.
19 A phase diagram is shown below.
D
2.0
SE
Pressure (atm)
EA
X
1.0
EL
R
0 10 30 50 70 90 110
Temperature (°C)
Which choice describes the state of the substance at X?
A A boiling liquid is in equilibrium with its vapor.
B A subliming solid is in equilibrium with its vapor.
C A freezing liquid is in equilibrium with its solid.
D A melting solid is in equilibrium with its liquid.
7 Go to the next page.
CHEMISTRY — RELEASED ITEMS
20 A sample of metal has a mass of 5.2 g and absorbs 20.0 J of energy as it is heated
from 30.0°C to 40.0°C. What is the identity of the metal?
A iron
B gold
C copper
D magnesium
21 A 2.0-liter closed container holds 1.0 mole of an ideal gas at a certain temperature
D
and pressure. Which closed container will hold 3.0 moles of this ideal gas at the
same temperature and pressure?
B
a 3.0-liter container
a 6.0-liter container
SE
C a 9.0-liter container
EA
D a 12.0-liter container
EL
R
8 Go to the next page.
CHEMISTRY — RELEASED ITEMS
22 A phase diagram is shown below.
D
Pressure (kPa)
101.3
SE
EA
EL
0 100 374
R
Temperature (°C)
What is the condition of the sample at point X?
A The sample is in a gaseous state.
B The sample is in a liquid state.
C The sample is at its critical point.
D The sample is at its triple point.
9 Go to the next page.
CHEMISTRY — RELEASED ITEMS
23 What is the approximate temperature of 1.4 moles of a gas with a pressure of
3.25 atmospheres in a 4.738-liter container?
A 180 K
B 170 K
C 150 K
D 130 K
D
SE
EA
EL
R
10 Go to the next page.
CHEMISTRY — RELEASED ITEMS
24 A potential energy diagram of a chemical reaction is shown below.
Potential Energy
of a Chemical Reaction
10
8
Potential Energy (J)
D
U
6
S
4 SE T
EA
R
EL
0 5 10 15 20
Reaction Coordinate
R
Which choice would be changed by the addition of a catalyst to the reaction?
A R
B S
C T
D U
11 Go to the next page.
CHEMISTRY — RELEASED ITEMS
25 A student conducts the following demonstration:
• A 15-g sample of NaHCO3 is placed in a test tube.
• The bottom of the test tube is heated with an open flame.
• Condensation forms on the inside walls of the test tube.
• A burning splint is extinguished when placed at the mouth of the test
tube.
What can the student conclude after conducting this demonstration?
A The burning splint was extinguished because of a lack of CO2 in the
test tube.
D
B The burning splint was extinguished because of a lack of H2O vapor.
D SE
Decomposition produced CO2 and H2O.
Combustion produced O2 and H2O.
EA
26 A chemical equation is shown below.
CaSO4 + AlBr3 → CaBr2 + Al2(SO4)3
EL
What will be the coefficient of CaBr2 when the equation is balanced using the
smallest possible whole-number coefficients?
A 2
R
B 3
C 4
D 5
12 Go to the next page.
CHEMISTRY — RELEASED ITEMS
27 The equation below represents a chemical reaction.
Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g)
A 5.00-g sample of zinc is added to hydrochloric acid. The amount of hydrochloric
acid is sufficient to allow the zinc to react completely. What mass of hydrogen gas
does this reaction produce?
A 0.0308 g
B 0.0771 g
C 0.121 g
D
D 0.154 g
28 SE
What is the molecular formula of a compound with the empirical formula CH2O and
a molecular mass of 60 g/mol?
A CH2O
EA
B C2H4O2
C C2H4O4
EL
D C2H2O2
R
13 Go to the next page.
CHEMISTRY — RELEASED ITEMS
29 A student experimented with magnesium ribbon and hydrochloric acid.
• The student placed a piece of solid magnesium ribbon in a test tube
containing hydrochloric acid solution.
• The student observed that vigorous bubbling occurred.
• The student collected some of the gas generated by the bubbles in a
test tube.
• The student tested the gas produced with a burning wood splint, which
ignited quickly with a popping sound.
What can the student conclude about the experiment?
D
A A chemical reaction occurred because new atoms were created.
B A chemical reaction occurred because a new substance was formed.
D
SE
The popping sound provided evidence that the acid changed physical states.
The popping sound provided evidence that the magnesium atoms were
destroyed.
EA
30 How many O2 particles are in 2.50 moles of O2 at Standard Temperature and
Pressure (STP)?
EL
A 4.15 × 1022 particles
B 2.41 × 1023 particles
R
C 5.02 × 1023 particles
D 1.51 × 1024 particles
14 Go to the next page.
CHEMISTRY — RELEASED ITEMS
31 Why does an increase in temperature usually increase the rate of a chemical
reaction?
A because the activation energy of the reaction increases
B because the surface area of reacting particles increases
C because the proper orientation of reacting particles improves
D because the number of effective collisions between reacting particles
increases
D
32 The chemical equation below represents a reaction at equilibrium in a closed flask.
A
SE
Which action will cause the reaction to shift to the left?
heating the flask with a hot plate
EA
B placing the flask in an ice bath
C removing H2O from the flask
D adding CO to the flask
EL
R
15 Go to the next page.
CHEMISTRY — RELEASED ITEMS
33 In a hypothetical reaction, reactants X and Y are combined in an evacuated vessel
and allowed to come to equilibrium with product Z at a temperature of 200K.
X (g) + Y (g) → Z (g)
After equilibrium is established, the temperature is slowly raised, and additional
values of Keq are determined as shown in this data table:
Temperature Keq
200K 3 × 10-2
300K 1 × 10-2
D
400K 4 × 10-3
500K 5 × 10-4
A 200K
SE
Which temperature has the greatest concentration of product Z?
EA
B 300K
C 400K
D 500K
EL
R
16 Go to the next page.
CHEMISTRY — RELEASED ITEMS
34 An equilibrium is established between substances W, X, Y, and Z.
W+X Y+Z
How would the conditions of equilibrium be affected by decreasing the
concentration of substance W?
A Substances X and Y would react to replace substance W, and the position of
equilibrium would shift to the right.
B Substances Y and Z would react to replace substance W, and the position of
equilibrium would shift to the left.
C This would increase pressure, causing only substance Y to replace substance
D
W and shifting the equilibrium to the right.
SE
This would decrease temperature, causing only substance Z to replace
substance W and shifting the equilibrium to the left.
EA
35 A solution has a pOH of 12. Which best describes the solution?
A It has a pH of 2 and is a base.
B It has a pH of 12 and is a base.
EL
C It has a pH of 2 and is an acid.
D It has a pH of 12 and is an acid.
R
36 A student describes a liquid as feeling slippery. The student places red litmus
paper into the liquid, and the paper turns blue. What can the student conclude
from these observations?
A The substance is likely a nonmetal.
B The substance is likely a metal.
C The substance is likely a base.
D The substance is likely an acid.
17 Go to the next page.
CHEMISTRY — RELEASED ITEMS
37 An acid-base titration is represented by the chemical equation below.
CsOH (aq) + HBr (aq) → CsBr (aq) + H2O (l)
In the titration, 15.0 mL of CsOH solution is neutralized by 38.2 mL
of 0.250 M HBr solution. What is the molarity of the CsOH solution?
A 0.0982 M
B 0.637 M
C 1.36 M
D 10.2 M
D
38
in water?
A
SE
What type of solution is formed when solid sodium hydroxide (NaOH) is dissolved
an electrolytic solution, because NaOH will dissociate into ions
EA
B an electrolytic solution, because NaOH will not dissociate into ions
C a nonelectrolytic solution, because NaOH will dissociate into ions
D a nonelectrolytic solution, because NaOH will not dissociate into ions
EL
R
18 Go to the next page.
CHEMISTRY — RELEASED ITEMS
40 Which statement explains what happens when potassium chloride (KCl) dissolves
in water?
A Water molecules surround the potassium chloride but do not exert forces of
attraction strong enough to break any bonds.
B Water molecules exert forces of attraction that break the potassium chloride
apart into potassium ions and chloride ions.
C Water molecules exert forces of attraction that break the potassium chloride
apart into neutral atoms of potassium and neutral atoms of chlorine.
D Water molecules exert forces of attraction that break the potassium chloride
apart into potassium atoms and diatomic chlorine gas.
D
SE
EA
EL
R
20 Go to the next page.
CHEMISTRY — RELEASED ITEMS
This is the end of Chemistry Released Items.
Directions:
1. Look back over your answers for the test questions.
2. Make sure all your answers are entered on the answer sheet. Only what is
entered on your answer sheet will be scored.
3. Put all of your papers inside your test book and close the test book.
D
4. Place your calculator on top of the test book.
finished. SE
5. Stay quietly in your seat until your teacher tells you that testing is
6. Remember, teachers are not allowed to discuss items from the test with
EA
you, and you are not allowed to discuss with others any of the test
questions or information contained within the test.
EL
R
21
