Chapter 13
Chemical Bonding
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Chapter 13
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1. How many electrons are in the second energy level
of the atom shown?
A 2
B 7
C 8
D 9
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Chapter 13
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1. How many electrons are in the second energy level
of the atom shown?
A 2
B 7
C 8
D 9
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Chapter 13
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2. Which of the following statements about helium
atoms is true?
A Helium atoms can never have a full set of valence
electrons.
B Helium atoms need only 2 valence electrons to have
a full outermost energy level.
C Helium atoms do not have valence electrons.
D Helium atoms have the same number of valence
electrons as sulfur atoms do.
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2. Which of the following statements about helium
atoms is true?
A Helium atoms can never have a full set of valence
electrons.
B Helium atoms need only 2 valence electrons to have
a full outermost energy level.
C Helium atoms do not have valence electrons.
D Helium atoms have the same number of valence
electrons as sulfur atoms do.
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3. Sodium chloride, or table salt, forms when a chlorine
atom takes an electron from a neighboring sodium
atom. Which of the following describes the force that
holds sodium chloride together?
A an ionic bond
B a hydrogen bond
C a metallic bond
D a covalent bond
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3. Sodium chloride, or table salt, forms when a chlorine
atom takes an electron from a neighboring sodium
atom. Which of the following describes the force that
holds sodium chloride together?
A an ionic bond
B a hydrogen bond
C a metallic bond
D a covalent bond
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4. An aluminum ion has 13 protons, 14 neutrons,
and 10 electrons. What is the charge of an aluminum
ion?
A 10 –
B 3–
C 1+
D 3+
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4. An aluminum ion has 13 protons, 14 neutrons,
and 10 electrons. What is the charge of an aluminum
ion?
A 10 –
B 3–
C 1+
D 3+
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5. What property of copper allows copper wire to bend
without breaking?
A Copper atoms have 29 protons.
B Copper is found in Group 11 on the periodic table.
C Copper atoms do not have a full outermost energy
level.
D Copper atoms form metallic bonds with each other.
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5. What property of copper allows copper wire to bend
without breaking?
A Copper atoms have 29 protons.
B Copper is found in Group 11 on the periodic table.
C Copper atoms do not have a full outermost energy
level.
D Copper atoms form metallic bonds with each other.
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6. According to the electron-dot diagram of oxygen
shown, how many more valence electrons does the
oxygen atom need to fill its outermost energy level?
A 1
B 2
C 6
D 8
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6. According to the electron-dot diagram of oxygen
shown, how many more valence electrons does the
oxygen atom need to fill its outermost energy level?
A 1
B 2
C 6
D 8
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7. The ions that make up an ionic compound are
bonded in a repeating three-dimensional pattern. What
is this pattern called?
A chloride lattice
B covalent bond
C crystal lattice
D crystal pattern
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7. The ions that make up an ionic compound are
bonded in a repeating three-dimensional pattern. What
is this pattern called?
A chloride lattice
B covalent bond
C crystal lattice
D crystal pattern
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8. Which of the following forms when a neutral atom
loses an electron?
A a negative atom
B a neutral ion
C a positive ion
D a negative ion
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8. Which of the following forms when a neutral atom
loses an electron?
A a negative atom
B a neutral ion
C a positive ion
D a negative ion
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9. During a laboratory experiment at Georgia State
University, Juanita observes a model of two bonded
atoms. She is told that the atoms are both nonmetals.
Which of the following is a valid conclusion?
A She is looking at a model of atoms held together by
a covalent bond.
B She is looking at a model of atoms held together by
an ionic bond.
C She is looking at a model of a metalloid.
D She is looking at a model of a crystal lattice.
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9. During a laboratory experiment at Georgia State
University, Juanita observes a model of two bonded
atoms. She is told that the atoms are both nonmetals.
Which of the following is a valid conclusion?
A She is looking at a model of atoms held together by
a covalent bond.
B She is looking at a model of atoms held together by
an ionic bond.
C She is looking at a model of a metalloid.
D She is looking at a model of a crystal lattice.
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10. Which of an atom’s electrons are most likely to
be involved in chemical bonding? Why?
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10. Answer - Full-credit answers should include the
following points:
• The valence electrons are most likely to be involved in
chemical bonding.
• When two atoms are close to each other, the outermost
electrons of one atom are closest to the nucleus of the
other atom.
• The attraction between the outermost electrons in one
atom and the positively-charged nucleus of the other atom
contributes to the bond between the two atoms.
• The outermost electrons are shared, lost, or gained
most easily.
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11. Why do atoms of the noble gases, in Group 18
on the periodic table, usually not form chemical
bonds?
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11. Answer - Full-credit answers should include the
following points:
• The number of electrons in the outermost energy
level of an atom determines whether an atom will form
bonds.
• Atoms of the noble gases (Group 18) do not usually
form chemical bonds because each atom has a full set
of valence electrons.
• When the outermost energy level of an atom is full,
the atom does not usually form bonds.
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