Benchmark Test Practice
1a - Students know how to relate the position of
an element in the periodic table to its atomic
number and atomic mass.
Atomic Structure (1a.1)
What is the structure
of an atom?
 An atom has a nucleus containing protons and
neutrons, orbited by electrons.
 Protons are positive, neutrons are neutral, and
electrons are negative.
What is an element’s
mass number?
Mass Number (1a.3)
What is an isotope?
 Mass number is the total weight of the nucleus
(protons + neutrons).
 MOST atoms of an element have the same mass, but
occasionally, one has a different number of neutrons.
 It is called an isotope.
1a
• 4.An element is a collection of a single
kind of ______________.
1a
• ____ 7. How many protons, electrons, and
neutrons, respectively, does O-16 have?
A.8, 8, 8
• B.8, 14, 8
• C.8, 10, 8
• D.8, 18, 8
• E.8, 18, 16
1b - Students know how to use the periodic
table to identify metals, semimetals,
nonmetals, and halogens.
Organization of the Periodic Table
(1b.1)
 Notice the zigzag line running from Boron (#5) to Astatine
(#95)
 Elements to the left are Metals
 Shiny, conduct electricity, maleable (moldable), ductile
(stretchable)
 Elements to the right are Nonmetals.
 Many are gasses, do not conduct electricity, brittle
(breakable)
 Elements touching the line are Semimetals (Metalloids).
 Properties are midway between Metals and Nonmetals.

Semiconductors
Metals
Titanium
Ductile - stretchable
Maleable –
Nonmetals
Sulfur
Oxygen
Semimetals
Silicon
Tellurium
1b
1. Which of the following describes a
chemical property of gold?
• A.Gold is a yellow metal.
• B.Gold is a very dense metal.
• C.Gold is a good conductor of heat and
electricity.
• D.Gold is an inert (nonreactive) metal.
E.Gold is a soft metal.
1b
• ____ 8. The alkali metals have how many
valence electrons?
• A.8
• B.7
• C.2
• D.3
• E.1
1b
• ____ 9. The noble gases contain how
many valence electrons?
• A.0
• B.7
• C.1
• D.8
• E.None of the above
1b
• ____ 10. Which element has the largest
number of electrons in its valence shell?
• A.S
• B.F
• C.Fr
• D.As
• E.K
1c - Students know how to use the periodic
table to identify alkali metals, alkaline earth
metals and transition metals, trends in
ionization energy, electronegativity, and the
relative sizes of ions and atoms.
1c
• ____ 11. When moving down a group
(family) in the periodic table, the number of
valence electrons
• A.remains constant
• B.increases by 2 then 8 then 18 then 32
• C.decreases regularly
• D.changes in an unpredictable manner
• E.doubles with each move
1c
• ____ 12. Which of the following atoms has
the highest ionization energy?
• A.P
• B.Mg
• C.Cl
• D.Na
• E.Si
1c
• ____ 13. Which of the following atoms has
the largest atomic radius?
• A.C
• B.Na
• C.Si
• D.P
• E.Mg
1c
• ____ 21. Nonmetal elements typically
have ______________ electronegativities.
• A.neutral
• B.low
• C.strong
• D.high
• E.None of the above
1c
• ____ 20. Metals typically have
______________ electronegativity values.
A.negative
• B.no
• C.high
• D.low
• E.two of these
1c
• ____ 28. Which of the following elements
has the lowest electronegativity?
• A.S
• B.Na
• C.Ca
• D.Cl
• E.Rb
1c
• ____ 14. Which of the following atoms has
the smallest atomic radius?
• A.N
• B.Bi
• C.Sb
• D.P
• E.As
1c
• ____ 27. The most electronegative
element is
• A.At
• B.He
• C.F
• D.O
• E.Cs
1c
• ____ 16. Of the metals in Group 1, which
has the highest ionization energy?
• A.Na
• B.Li
• C.Cs
• D.K
• E.Rb
1c
• 17.Which has the larger atomic radius, S
or Si?
1d - Students know how to use the periodic
table to determine the number of electrons
available for bonding.
1d
• ____ 15. Metal atoms tend to
______________ electrons and form
______________ ions.
• A.lose; negative
• B.gain; positive
• C.gain; negative
• D.share; neutral
• E.lose; positive
1d
• ____ 30. A phosphorus atom needs to
gain ______________ electrons to
achieve a noble gas configuration.
• A.3
• B.4
• C.6
• D.5
• E.2
1e - Students know the nucleus of the atom is
much smaller than the atom yet contains most
of its mass.
Mass of the Nucleus (1e.1)
• Although the nucleus is tiny, it contains the
vast majority of an atom’s mass.
• Electrons, which weigh almost nothing,
orbit so far away, most of an atom is
empty space.
– In fact, if a proton were the size of your
thumb, the nearest electron would be on the
other side of the 605!!! Where would you find
almost all the mass of
an atom?
Rutherford’s Gold Foil Experiment
1e
• How is the atomic mass calculated?
1e
• T or F When calculating the atomic mass
of an atom, we add the number of
electrons and protons.
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.
2a
• ____ 18. Chemical bonds formed by the
attraction of oppositely charged ions are
called
• A.ionic bonds
• B.coordinate bonds
• C.covalent bonds
• D.magnetic bonds
• E.None of the above
2a
• ____ 19. Atoms with greatly differing
electronegativity values are expected to
form
• A.nonpolar covalent bonds
• B.ionic bonds
• C.no bonds
• D.triple bonds
2a
• ____ 23. Al 2O3
2a
• ____ 24. BF3
2a
• ____ 25. Fe2O3
2a
• ____ 31. Magnesium reacts with sulfur to
form ?
2a
• ____ 32. Al + O2 reacts to form?
2a
• ____ 26. Which of the following
compounds contains an ionic bond?
• A.CCl4
• B.NaCl
• C.HCl(g)
• D.SO2
• E.O2
2b - Students know chemical bonds between
atoms in molecules such as H , CH , NH , H
CCH , N , Cl , and many large biological
molecules are covalent.
2
2
2
2
4
3
2
2a,b
• Use the following choices to classify each
of the following molecules.
• A.ionic
• B.covalent
• ____ 22. N2O
2b,e
• 35.Draw the Lewis electron structure for
the Cl2 molecule.
2e
• True or False:
• __________ 29. The F - and O 2- ions
have the same electron configuration.
2a
• 33.Complete the table by giving the
predicted formulas of the compounds
formed between the elements listed.
2e
• 34.Draw the Lewis electron structure for
the silicon atom.
2e
• 36.Draw the Lewis electron structure for
the HI molecule.
2e
• 37.Draw the Lewis electron structure for
the AsH3 molecule.
2e
• 38.Draw the Lewis structure for SiH4 .
2e
• 39.Draw the Lewis structure for Na2O.
2c – Students know salt crystals, such as NaCl,
are reapeating patterns of positive and negative
ions held together by electrostatic attraction.
• What are the forces that hold positive and
negative ions called?
• Draw what the ionic salt crystal NaCl looks
like.