Test # _________
Chemistry Common Pretest: Semester I
1. Select the letter that best answers each question or completes each statement. Darken
the appropriate space on the scantron sheet. In each case, there is only one correct
answer. Each question is worth 1 point.
2. Go to the online entry station in the classroom.
 CODE: Get the test code from your teacher and type it into the box.
 STUDENT ID: Enter your 9 digit SIS number and your name should appear
 ONLINE SCANTRON: Begin entering your answers by clicking the appropriate box
for each question. After you receive your score, logout. Turn in your test booklet
and scantron to your teacher.
Do not write on this test booklet!
UNIT 0: ENERGY AND MATTER
Target 1: I can compare and contrast solids, liquids, and gases.
1. Which of the following pictures represents the liquid state of matter?
Container A
Container B
Container C
2. Which state of matter is the densest?
a. Solid
b. Liquid
c. Gas
d. The densities of the three states of matter are the same.
Target 2: I can differentiate between elements, compounds and mixtures and their
properties.
Below is a graph of the chemical make-up of air. Use this chart to answer questions #3 and #4.
Small amounts of Carbon Dioxide (CO2) and Hydrogen (H2)
Argon (Ar) 1%
Oxygen (O2) 21%
Nitrogen (N2) 78%
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3. Looking at the pie chart, what classification of matter best describes carbon dioxide
(CO2)?
a. Element b. Compound c. Homogeneous Mixture
d. Heterogeneous Mixture
4. Looking at the pie chart, what classification of matter best describes the chemical that
makes up the highest percentage of air?
a. Element
b. Compound
c. Homogeneous Mixture
d. Heterogeneous Mixture
Target 3: I can differentiate between physical and chemical properties and changes.
5. Which of the following changes would be considered a chemical change?
a. Bending iron
b. Melting ice
c. Food spoiling
d. Sanding wood
6. Which of the following changes would be considered a physical change?
a. A peach spoils
b. Water boiling
c. A copper bowl tarnishes and changes color
d. A piece of jewelry turns your skin green
UNIT 1: SCIENTIFIC DESIGN
Target 2: I can convert units using dimensional analysis.
7. If a thermos of hot chocolate holds 1.25 L, how many gallons does that equal? (1000 mL
= 1 L; 1L = 1.06 quarts; 4 quarts = 1 gallon)
a. 5.300 gallons
b. 0.3313 gallons
c. 3.313 gallons
d. 3.313 x 105 gallons
Target 3: I can explain density both conceptually and mathematically.
8. Eggnog has a density of 2.5 g/mL. If a carton of eggnog is opened and poured into 5
separate glasses, what is the density of the eggnog in each of the glasses compared to
the density of the eggnog in the carton?
a. ½ the density
b. 64 times the density
c. 4 times the density
d. The same density
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9. Water has a density of 1.0 g/mL. Which of the following objects would sink in water?
Object I:
mass = 50.0 g; volume = 60.8 mL
Object II:
mass = 65.2 g; volume = 42.1 mL
Object III:
mass = 100.0 g; volume = 200.0 mL
a. I
b. II
c. I and III
d. II and III
Target 4: I can make scientific measurements using significant figures.
10. Using the ruler pictured, what is the correct length of Object B?
a. 4.0 cm
b. 4.45 cm
c. 4.500 cm
d. 5 cm
UNIT 2: ATOMIC STRUCTURE
Target 1: I can develop a model of the atom based on scientific claims and evidence. (P)
11. Choose the statement that is true about how the current model of the atom is different
from the Plum Pudding Model shown below.
a. The current model of the atom has electrons that orbit the
nucleus.
b. The current model has negatively charged neutrons that are
found in the nucleus.
c. The current model has two electrons in each orbital.
d. In the current model, protons are able to move back and forth from the ground state
to the excited state to give off light.
Target 2: I can label the parts of an atom and place them correctly within the structure of an
atom.
12. Choose the subatomic particle from the table whose information is correct.
Subatomic Particle
Charge
Location
Electron
-1
Outside the nucleus
Proton
+1
Outside the nucleus
Neutron
0
Outside the nucleus
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a. Electron
b. Proton
c. Neutron
d. All information is correct
13. Which subatomic particles are used to calculate the mass number of an isotope and
why?
a. Neutrons and electrons because they have no mass.
b. Protons and neutrons because they have mass.
c. Neutrons and electrons because they have no charge.
d. Protons and electrons because they have opposite charges.
Target 3: I can identify an element, isotope, and ion based on the number of subatomic
particles.
14. The overall charge on an ion that has 36 protons, 49 neutrons, and 38 electrons is:
a. +2
b. -2
c. +1
d. -1
15. How many neutrons are in an atom with a mass number of 49 and an atomic number of 12?
a. 12
b. 13
c. 25
d. 37
Target 4: I can calculate average atomic mass for an element.
16. What is the average atomic mass of an element given that one isotope has a mass of
14.00 amu and an abundance of 25% and its other isotope has a mass of 12.00 amu and
a percent abundance of 75%?
a. 13.00 amu
b. 12.50 amu
c. 26.00 amu
d. 13.50 amu
UNIT 3: NUCLEAR CHEMISTRY
Target 2: I can write a balanced nuclear equation supporting the law of conservation of mass.
17. Complete the following nuclear reaction:
+ __________
a.
0
1
e
b.
4
2
1
c. 1 H
He
d.
1
0
n
18. Polonium-210 decays by beta emission. Which isotope does it become?
a. polonium-211
b. astatine-210
c. lead-206
d. polonium-206
19. Identify the missing product from the following reaction and classify the type of decay?
+ __________
0
0
1
a. 1 e , beta decay
b. 1 e , positron emission
c. , beta decay d. 0 n , neutron emission
Target 5: I can find the age of an object or substance using half-life: conceptually,
mathematically, and graphically.
20. What percentage of a radioactive isotope sample remains after three half-
lives?
a. 50%
b. 25.0%
c. 12.5%
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d. 6.25%
21. The half-life of radon-222 is 7.6 days. If the measured amount of radon is 1.25 g currently, how
much was originally present 38 days ago?
a. 0.039 g
b. 5 g
c. 40 g
d. 80 g
22. Using the decay series shown, identify the order of decay Actinium-228 goes through to become
Radon 220.
a. beta—alpha—alpha
b. alpha—alpha—alpha
c.
alpha—beta—beta
d. beta—beta—beta
UNIT 4: ELECTROMAGNETIC RADIATION AND MODERN ATOMIC THEORY
Target 2: I can identify the mathematical relationship between wavelength, frequency and energy.
Wave A
Wave B
23. Which of the following is true for Wave A compared to Wave B?
a. Wave A has a lower frequency than Wave B.
b. Wave A has a higher energy than Wave B.
c. Wave A has a shorter wavelength than Wave B.
d. Wave A would represent blue light while Wave B would represent red light.
Target 3: I can apply the Bohr Model to show how electrons move between states in atoms.
24. The Bohr model pictured shows an electron:
a. absorbing energy to move to a higher energy level
b. releasing energy to move to a lower energy level
c. absorbing energy to move to a lower energy level
d. releasing energy to move to a higher energy level
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25. Diagrams A – D represent the possible electron transitions for hydrogen. The colors emitted
from these transitions include green, red, violet, and blue. Which of the below diagrams
represent the electron transition that will result in the color red?
Target 4: I can relate models of the s, p, d, and f orbitals to the periodic table.
26. Based on the periodic table picture, which letters make up the d-block?
a. D only
b. B, I , and C
c. B and E
d. I, C, F, A, H and G
27. Letter “G” in the periodic table picture has
an ending electron configuration of what?
a. 4p6
b. 4d4
c.
4
5
6p
d. 6p
Target 5: I can use the periodic table to write electron configurations for elements.
28. Which of the following Noble Gas notations is written correctly for the element
strontium (Sr) with an atomic number of 38?
a. 1s22s22p63s23p64s23d104p65s2
b. 5s2
c. [Kr]5s2
d. [Sr]5s2
29. Which element’s electron configuration is written incorrectly?
a. Sulfur (S): 1s22s22p63s24p4
b. Sodium (Na) 1s22s22p63s1
c. Calcium (Ca): 1s22s22p63s23p64s2
d. Fluorine (F): 1s22s22p5
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UNIT 5: THE PERIODIC TABLE
Target 1: I can identify specific families and regions on the periodic table.
30. Which letter in the periodic table picture would be an alkaline earth metal?
a. Letter B
b. Letter C
c. Letter E
d. Letter G
31. Using the periodic table picture, which of
the following letters would you predict
would both be insulators?
a. Letter B and Letter E
b. Letter D and Letter C
c. Letter C and Letter G
Target 3: I can use the periodic trends to predict the properties (atomic radius, electronegativity,
ionization energy, and reactivity) of an element.
32. Which family is the least reactive?
a. Alkali Metals
b. Alkaline Earth Metals
c. Halogens
d. Noble Gases
33. Choose the element below with the smallest atomic radius.
a. Sodium (Na)
b. Magnesium (Mg) c. Potassium (K)
d.Calcium (Ca)
34. Choose the element below with the lowest electronegativity.
a. Chlorine (Cl)
b. Fluorine (F)
c. Germanium (Ge)
d. Oxygen (O)
Target 4: I can determine the number of valence electrons for an element based on the outermost electron patterns.
35. What is the number of valence electrons for the halogens?
a. 2
b. 7
c. 18
d. The period number
36. How many valence electrons does an atom of phosphorus (P) have?
a. 5
b. 15
c. 31
d. 3
Target 5: I can predict an element’s oxidation number (charge) based on the outermost electron patterns.
37. In order to be stable like the Noble Gases, phosphorus (P) will do what to become an
ion?
a. Lose 5 electrons b. Gain 3 electrons c. Lose 3 electrons
d.It is already stable
38. How does a nonmetal form an ion?
a. It loses electrons.
b. It gains electrons. c. It loses protons.
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D. It gains protons.