Name ___________________________________________ Date ____________ Period ______
BENCHMARK TEST – POWER STANDARDS
1a. Students know how to relate the position of an element in the periodic table to its atomic number and
atomic mass
1. What is the charge of a proton?
A. Positive (+)
B. Negative (-)
C. Neutral (0)
D. Undefined
2. What is the charge of a neutron?
A. Positive (+)
B. Negative (-)
C. Neutral (0)
D. Undefined
3. Where are electrons located in an atom?
A. In the nucleus
B. orbiting the nucleus
C. attached to the protons
D. negative
4. Which particles always have the same quantity in a neutral atom?
A. Protons and neutrons
B. Protons and electrons
C. Electrons and neutrons
D. Electrons and orbitals
5. What does the atomic number tell you about an element?
A. The number of neutrons in the atom
B. The number of protons in the atom
C. The number of protons plus the number of neutrons
D. The mass of the atom
6. How many protons are in an atom of Boron, B?
A. 5
B. 6
C. 10
D. 11
7. Which of the following ordered pairs of elements shows an increase in atomic number, but a
decrease in average atomic mass?
A. Ag to Pd
B. Co to Ni
C. Ge to Sn
D. Cr to Mo
8. Why is the atomic mass of an element on the periodic table a decimal?
A. It is an average of the number of neutrons in the atoms of an element.
B. It is an average of the masses of the naturally occurring isotopes.
C. It is an average of the atomic numbers of the naturally occurring isotopes.
D. None of the above.
9. Which element has the greatest atomic number?
A. Ni - Nickle
B. Cd - Cadmium
C. Hg – Mercury
D. Fr – Francium
1b. Students know how to use the periodic table to identify metals, semimetals, nonmetals, and halogens
For #10-12 classify each element as a
10. K
11. Cl
12. H
A) metal B) nonmetal C) Metalloid
1c. Students know how to use the periodic table to identify alkali metals, alkaline earth metals, transition
metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms
13. Name the family that is in group 18 or 8A on the periodic table.
A. Halogen
B. Alkali Metals
C. Noble Gases
D. Transition Metals
Use the letters on the periodic table to label 14-17:
14. Alkali metals
15. Halogens
16. Alkaline earth metals
17. Transition metals
E
B
D
C
A
Use the following for 18-24:
A. Increases
B. Decreases
C. Stays the same
In general, as you go from LEFT to RIGHT across the periodic table…
18. atomic radius
19. electronegativity
20. ionization energy
In general, as you go from TOP to BOTTOM down the periodic table…
21. electronegativity
22. the number of valence electrons
23. ionization energy
24. atomic radius
25. What is ionization energy?
A. The ability of an atom to attract bonded electrons to itself
B. A measure of the size of an atom
C. The energy required to remove an electron from a neutral atom
D. The energy released when an atom loses or gains electrons
26. Which of the following elements has the highest ionization energy?
A. Cl
B. Al
C. Fe
D. Ba
27.
The chart above shows the relationship
between the first ionization energy and the increase
in atomic number. The letter on the chart for the
alkali family of elements is
A. W
B. X
C. Y
D. Z
28. Put the following in order of increasing (smallest to largest) atomic size: O, S, Po, Te
A. O, Po, S, Te
B. Po, Te, S, O
C. O, S, Te, Po
D. O, S, Po, Te
29. Which of the following is an alkali metal with the largest atomic radius?
A. Na
B. Ba
C. Mg
D. Cs
30. What is electronegativity?
A. A measure of the ability of an atom to attract bonded electrons towards itself
B. A partial negative charge
C. A polar molecule
D. The energy required to remove one electron from a neutral atom.
31. Which of the following elements is most electronegative?
A. Potassium (K)
B. Calcium (Ca)
C. Chlorine (Cl)
D. Aluminum (Al)
1d. Students know how to use the periodic table to determine the number of electrons available for bonding.
32. How many valence electrons are in a neutral atom of Chlorine?
A. 17
B. 7
C. 10
D. 35
33. Which of the following atoms has six valence electrons?
A. Magnesium (Mg)
B. silicon (Si)
C. sulfur (S)
D. argon (Ar)
1e. Students know the nucleus of the atom is much smaller than the atom yet contains most of the mass.
34. Which statement best describes the density of an atom’s nucleus?
A. The nucleus occupies most of the atom’s volume but contains little of its mass.
B. The nucleus occupies very little of the atom’s volume and contains little of its mass.
C. The nucleus occupies most of the atom’s volume and contains most of its mass.
D. The nucleus occupies very little of the atom’s volume but contains most of its mass.
35. If a tiny particle is shot into the middle of an atom, it hits something in the center and
bounces back. If the particle is shot into the edges of the atom, it goes through. This
discovery led to a model of the atom with
A. electrons
B. a neutral charge
C. a nucleus
D. electron orbital shells
36. Use the table below to answer the question:
Results of Firing Alpha Particles at Gold Foil
Observations
Alpha Particles went straight through gold foil
Alpha particles went through gold foil but were
deflected at large angles
Alpha particles bounced off gold foil
Proportion
> 98%
= 2%
=0.01 %
What information do the experimental results above reveal about the nucleus of the gold
atom?
A.
B.
C.
D.
The nucleus contains less than half the mass of the atom.
The nucleus is small and is the densest part of the atom.
The nucleus contains small positive and negative particles.
The nucleus is large and occupies most of the atom’s space.
2a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds
or by exchanging electrons to form ionic bonds
37. Why don’t noble gases lose or gain electrons?
A. They are unstable
B. They have 10 electrons in their outer shell
C. They have a full valence shell
D. None of the above
38. Iodine would have chemical properties most like:
A. manganese (Mn)
B. tellurium (Te)
C. Chlorine (Cl)
D. Xenon (Xe)
39. Fluorine gains one electron and becomes a Fluorine ion with a negative charge. Why
doesn’t it become a Neon atom?
A. The neutrons did not change, and the neutrons determine the identity of an atom.
B. The number of protons did not change, and the protons determine the identity of an
atom.
C. Electrons cannot be lost or gained.
D. None of the above
40. Which of the following is a monatomic gas?
A. Chlorine
B. Fluorine
C. Helium
D. Nitrogen
41. Which of the following is a diatomic gas?
A. Argon
B. Chlorine
C. Boron
D. Helium
42. What is an ion?
A. a neutral atom
B. an atom that has gained or lost neutrons and therefore has an overall charge
C. atoms of the same element that have different numbers of neutrons
D. an atom that has gained or lost electrons and therefore has an overall charge
43. Which of the following is a cation?
A) K+
B) BrC) H2
D) Li
For # 44-46: A. ionic bond B. covalent bond
C. metallic bond
44. involves sharing electrons
45. bendable solids
46. conducts electricity when dissolved in water
47. What type of bond will form between two atoms with very different electronegativities?
A. Ionic
B. Polar covalent
C. Nonpolar covalent
D. Metallic
2e. Students know how to draw Lewis dot structures
48. Which of the following is the correct dot symbol for Phosphorus
A)
B)
C)
D)
49. Which of the following elements has the same dot symbol as silicon?
A. germanium (Ge)
B. aluminum (Al)
C. arsenic (As)
D. gallium (Ga)
50. Which of the following is the correct Lewis Dot Structure for NH3?
A)
B)
A.
C)
A.
D)
A.
H N H
H
H N H
H
H N H
H
H N H
H
3a. Students know how to describe chemical reactions by writing balanced equations
(For 51-53) When zinc is added to hydrochloric acid, the following reaction occurs:
Zn(s) +
HCl(aq) 
ZnCl2(aq) +
H2(g)
51. In the equation above the reactants are
A. ZnCl2 and H2
B. ZnCl2
C. Zn and HCl
D. on the right
52. The abbreviation (aq) means
A. gas
B. dissolved in water
C. aquafina
D. liquid
53. The total mass of the reactants before the chemical reactants is 50g. What will the mass of the
products be?
A. 50g
B. Slightly less than 50g.
C. More than 50g
D. None of the above
54. The correct balanced equation for
A. 2N2 + H2  2NH3
B. N2 + H2  2NH3
C. N2 + 3H2  2NH3
D. 2N2 + 2H2  2NH3
55.
N2 + H2  NH3
C3H8 +
O2 
CO2 + ? H2O
This chemical equation represents the combustion of propane. When correctly balanced, the
coefficient for water is
A. 2
B. 4
C. 8
D. 16
56. Which of the following is a balanced equation for the combustion of ethanol (CH3CH2OH)?
A. CH3CH2OH + 3O2  CO2 + 2H2O
B. CH3CH2OH + 3O2  2CO2 + 3H2O
C. CH3CH2OH + O2  2CO2 + 3H2O
D. CH3CH2OH + 2O2  3CO2 + 2H2O
57. Which of the following is NOT part of the Law of Conservation of Matter?
A. Matter cannot be created or destroyed.
B. Atoms cannot come in and out of existence.
C. Mass can increase during a chemical reaction.
D. Mass does not change during a chemical reaction.