Fundamentals Of General Organic And Biological Chemistry 7th Edition By John E. McMurry – Test Bank
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Fundamentals of General, Organic, and Biological Chemistry,
7e (McMurry)
Chapter 3 Ionic Compounds
1) A positively charged particle formed by loss of one or more
electrons from an atom is called a(an)
1. A)
anion.
2. B)
cation.
3. C)
isotope.
4. D)
nucleus.
5. E)
proton.
Answer: B
Diff: 1
Section: 3.1
2) A small negatively charged particle formed when an atom gains
one or more electrons is called a(an)
1. A)
anion.
2. B)
cation.
3. C)
isotope.
4. D)
nucleus.
5. E)
proton.
Answer: A
Diff: 1
Section: 3.1
3) When an atom donates an electron, that electron
1. A) is
lost for all time.
2. B) is
acquired by another atom which becomes an anion.
3. C) is
acquired by another atom which becomes a cation.
4. D)
neutralizes a proton to form a neutron.
5. E)
pairs with another electron to form a covalent bond.
Answer: B
Diff: 2
Section: 3.1
4) Main group elements that are metals usually ________ one or
more electrons to form ________, which have a ________ charge.
1. A)
lose; anions; negative
2. B)
lose; cations; negative
3. C)
lose; cations; positive
4. D)
gain; cations; positive
5. E)
gain; anions; negative
Answer: C
Diff: 2
Section: 3.1
5) Main group elements that are non-metals usually ________ one
or more electrons to form ________, which have a ________ charge.
1. A)
lose; anions; negative
2. B)
lose; cations; negative
3. C)
lose; cations; positive
4. D)
gain; cations; positive
5. E)
gain; anions; negative
Answer: E
Diff: 2
Section: 3.1
6) One characteristic of a cation is that
1. A) it
has more protons than electrons.
2. B) it
has equal numbers of protons and electrons.
3. C) it
has more electrons than protons.
4. D)
the number of neutrons is related to the number of electrons.
5. E)
the relationship between protons and electrons varies with the cation in
question.
Answer: A
Diff: 3
Section: 3.1
7) The property that describes the ease with which an atom gives
up an electron to form a positive ion is
1. A)
atomic number.
2. B)
electron affinity.
3. C)
electronegativity.
4. D)
ionization energy.
5. E)
none of the above
Answer: D
Diff: 1
Section: 3.2
8) The property defined as the energy released on adding an
electron to an isolated gas phase atom is
1. A)
atomic number.
2. B)
electron affinity.
3. C)
electronegativity.
4. D)
ionization energy.
5. E)
none of the above
Answer: B
Diff: 1
Section: 3.2
9) Which of the following has the largest ionization
energy?
1. A) Ne
2. B) Br
3. C) P
4. D) Al
5. E) Ca
Answer: A
Diff: 2
Section: 3.2
10) The property defined as the energy required to remove one
electron from an atom in the gaseous state is
1. A)
atomic number.
2. B)
electron affinity.
3. C)
ionization energy.
4. D)
electronegativity.
5. E)
none of the above
Answer: C
Diff: 2
Section: 3.2
11) An element belonging to the halogen family would be expected
to have a ________ ionization energy and a ________ electron affinity.
1. A)
large; large
2. B)
large; small
3. C)
small; small
4. D)
small; large
5. E)
none of the above
Answer: A
Diff: 3
Section: 3.2
12) An element belonging to the alkaline earth family would be
expected to have a ________ ionization energy and a ________ electron affinity.
1. A)
large; large
2. B)
large; small
3. C)
small; small
4. D)
small; large
5. E)
none of the above
Answer: C
Diff: 3
Section: 3.2
13) The term which best describes the crystalline substance that
results when a large number of metal atoms transfers electrons to a large
number of non-metal atoms is
1. A)
covalent compound.
2. B)
molecule.
3. C)
ionic solid.
4. D)
cation.
5. E)
anion.
Answer: C
Diff: 2
Section: 3.3
14) The statement that best describes the formation of an
ionic compound is:
1. A)
Electrons are transferred from a metal to a non-metal, and the resulting
charged particles form a crystalline network.
2. B)
Electrons are transferred from a non-metal to a metal, and the resulting
charged particles form a crystalline network.
3. C)
Electrons are shared between two atoms and discrete molecules are formed.
4. D)
Electrons move freely among a network of nuclei in fixed positions.
5. E) Each
atom achieves an octet using electrons provided from an external electrical
supply.
Answer: A
Diff: 2
Section: 3.3
15) Which one of the compounds below is most likely to be ionic?
1. A)
SrBr2
2. B)
NO2
3. C)
CBr4
4. D)
H2O
Answer: A
Diff: 2
Section: 3.3
16) Which of the following pairs will form ionic bonds with one
another?
1. A) N,
C
2. B)
Na, Ca
3. C)
Cs, Br
4. D) S,
Cl
Answer: C
Diff: 2
Section: 3.3
17) All of the following are properties typical of ionic
compounds except
1. A)
exist as crystalline solids at room temperature.
2. B)
conduct electrical current if dissolved in water.
3. C)
form distinct molecules by interaction of specific particles.
4. D)
have very high melting points and boiling points.
5. E)
shatter when crystals are struck.
Answer: C
Diff: 2
Section: 3.4
18) Which of the following electron configurations is most
stable?
1. A)
1s2 2s2
2. B)
1s2 2s2 2p2
3. C)
1s2 2s2 2p3
4. D)
1s2 2s2 2p4
5. E)
1s2 2s2 2p6
Answer: E
Diff: 2
Section: 3.5
19) What is the most likely charge on an ion formed by an
element with a valence electron configuration of ns2np4?
1. A) 2-
2. B) 1-
3. C) 2+
4. D) 4+
5. E) 6+
Answer: A
Diff: 2
Section: 3.5
20) What is the most likely charge on an ion formed by an
element with a valence electron configuration of ns1?
1. A) 7-
2. B) 1-
3. C) 0
4. D) 1+
5. E) 7+
Answer: D
Diff: 2
Section: 3.5
21) What is the most likely charge on an ion formed by an
element with a valence electron configuration of ns2np5?
1. A) 5-
2. B) 1-
3. C) 1+
4. D) 2+
5. E) 5+
Answer: B
Diff: 2
Section: 3.5
22) What is the most likely charge on an ion formed by an
element with a valence electron configuration of ns2np1?
1. A) 3-
2. B) 1-
3. C) 1+
4. D) 3+
5. E) 5+
Answer: D
Diff: 2
Section: 3.5
23) What is the valence shell electron configuration of the ion
formed from an atom of the halogen family?
1. A)
ns2
2. B)
ns2 np2
3. C)
ns2 np4
4. D)
ns2 np6
5. E)
ns2 np8
Answer: D
Diff: 3
Section: 3.5
24) Which of the following ions does not have the
same electron configuration as the noble gas neon?
1. A)
O-2
2. B) F-
3. C)
Al+3
4. D)
S-2
5. E)
Mg+2
Answer: D
Diff: 2
Section: 3.5
25) An atom with 3 valence electrons will most likely
1. A)
lose three electrons.
2. B)
gain three electrons.
3. C)
gain five electrons.
4. D)
gain one electron.
5. E)
lose one electron.
Answer: A
Diff: 3
Section: 3.5
26) How are noble gases related to the octet rule?
Answer: Noble gases, except helium, illustrate the
stability of elements with a full outer shell (an octet). These elements are
unreactive because their valence shell is filled. Helium is also grouped with
these elements because it is unreactive due to its filled 1s shell.
Diff: 1
Section: 3.5
27) Briefly explain how the octet rule determines the charge,
both sign and magnitude, of an ion.
Answer: The octet rule states that main group elements
will do chemistry in order to have eight electrons in their outer shell. If an
atom has one or two electrons past an octet, it will lose the appropriate
number to have a full outer shell, resulting in a positively charged ion. If an
atom is one or two electrons away from having an octet, it will gain the
appropriate number, resulting in a negatively charged ion.
Diff: 2
Section: 3.5
28) Predict the charge that would be found on a carbide ion and
on a nitride ion. Explain why these ions are seldom found in compounds.
Answer: The names of both ions end in “ide,” suggesting
that they have gained electrons to form anions. In order to achieve an octet,
carbon would have to gain four electrons, forming C4-. Likewise for nitride,
the ion would be N3-. Both of these ions are less common because it is extremely
difficult to add additional electrons to an ion that already has a -2 charge.
Diff: 3
Section: 3.5
29) Which element will form an ion with the greatest positive
charge?
1. A) Al
2. B) Na
3. C) Mg
4. D) Sr
5. E) P
Answer: A
Diff: 3
Section: 3.6
30) In order to form an octet, an atom of selenium will
1. A)
lose 6 electrons.
2. B)
gain 6 electrons.
3. C)
lose 2 electrons.
4. D)
gain 2 electrons.
Answer: D
Diff: 2
Section: 3.6
31) The charge on a sulfide ion is ________.
1. A) 3+
2. B) 2+
3. C) 0
4. D) 2-
5. E) 3-
Answer: D
Diff: 1
Section: 3.6
32) Which of the following elements is most likely to form an
ion with a +2 charge?
1. A) Mg
2. B) Si
3. C) S
4. D) K
5. E) Br
Answer: A
Diff: 1
Section: 3.6
33) Which pair of elements is most likely to form an ionic
compound if allowed to react together?
1. A) Al
and Si
2. B) Fe
and Ca
3. C) C
and F
4. D) K
and Br
5. E) H
and N
Answer: D
Diff: 2
Section: 3.6
34) What fourth period element is represented by the dot
structure shown?
X:
1. A) K
2. B) Ca
3. C) V
4. D) As
5. E) Ti
Answer: B
Diff: 2
Section: 3.6
35) What fourth period element is represented by the dot
structure shown?
1. A) K
2. B) Ca
3. C) Mn
4. D) Br
5. E) Co
Answer: D
Diff: 2
Section: 3.6
36) Which of the following elements is most likely to form an
ion with a -2 charge?
1. A) Mg
2. B) Si
3. C) S
4. D) K
5. E) Ti
Answer: C
Diff: 1
Section: 3.6
37) Which of the following elements is most likely to form an
ion with a -1 charge?
1. A) Mg
2. B) Si
3. C) S
4. D) Cl
5. E) Sc
Answer: D
Diff: 1
Section: 3.6
38) The name of Cl- is
1. A)
chlorine ion.
2. B)
chloride ion.
3. C)
chlorate ion.
4. D)
chlorite ion.
5. E)
diatomic chlorine.
Answer: B
Diff: 1
Section: 3.7
39) The name of S2- is
1. A)
sulfur.
2. B)
sulfate ion.
3. C)
sulfite ion.
4. D)
sulfide ion.
5. E)
sulfurous ion.
Answer: D
Diff: 1
Section: 3.7
40) The name of Cu2+ is ________ ion or ________ ion.
1. A)
copper; cupric
2. B)
copper(i); cupric
3. C)
copper(II); cupric
4. D)
copper(I); cuprous
5. E)
copper(II); cuprous
Answer: C
Diff: 2
Section: 3.7
41) The correct Roman numeral for the chromium ion in the
compound CrCl3 is
1. A) I
2. B) II
3. C) III
4. D) IV
Answer: C
Diff: 2
Section: 3.7
42) The name of Sn2+ is ________ ion or ________ ion.
1. A)
tin; stannous
2. B)
tin(IV); stannic
3. C)
tin(II); stannic
4. D)
tin(IV); stannous
5. E)
tin(II); stannous
Answer: E
Diff: 2
Section: 3.7
43) Which of the following formulas in incorrect for a
cobalt(III) compound?
1. A)
CoCO3
2. B)
CoCl3
3. C)
Co2O3
4. D)
CoPO4
Answer: A
Diff: 2
Section: 3.7
44) What is the formula of the ammonium ion?
1. A)
Am-
2. B)
Am+
3. C)
NH4+
4. D)
NH4+
5. E)
N4H+
Answer: C
Diff: 1
Section: 3.8
45) What is the formula of the carbonate ion?
1. A)
CO2 3-
2. B)
CO3 2-
3. C)
C2O4 2-
4. D)
C2O4 -1
5. E)
C2H3O2 -1
Answer: B
Diff: 1
Section: 3.8
46) What is the formula of the nitrate ion?
1. A)
NO32-
2. B) NO
3-
3. C)
NO2-1
4. D)
NO3 -1
5. E)
none of the above
Answer: D
Diff: 1
Section: 3.8
47) What is the formula of the sulfite ion?
1. A)
SO3 2-
2. B)
SO4 2-
3. C)
HSO4 2-
4. D) S
2-
5. E)
none of the above
Answer: A
Diff: 1
Section: 3.8
48) The formula PO4 3- means that this ion is composed of
1. A)
one atom of phosphorus, one atom of oxygen, and three extra electrons.
2. B)
four atoms of phosphorus, four atoms or oxygen, and three extra electrons.
3. C)
one atom of phosphorus,four atoms of oxygen, and three electrons have been
lost.
4. D)
one atom of phosphorus, four atoms of oxygen, and three extra electrons.
5. E)
four atoms of phosphorus, four atoms of oxygen, and three electrons have been
lost.
Answer: D
Diff: 2
Section: 3.8
49) The permanganate ion is composed of
1. A)
one atom of magnesium, four atoms of oxygen, and one extra electron.
2. B)
one atom of manganese, four atoms of oxygen, and one extra electron.
3. C)
four atoms of magnesium, four atoms of oxygen, and one extra electron.
4. D)
four atoms of manganese, four atoms of oxygen, and one extra electron.
5. E)
one manganese(II) ion, four oxide ions, and two extra electrons.
Answer: B
Diff: 2
Section: 3.8
50) The HCO3 -1 ion is called ________.
1. A)
hydrogen carbonate
2. B)
hydrogen carbide
3. C)
carbide
4. D)
carbonate
5. E)
carbonite
Answer: A
Diff: 3
Section: 3.8
51) Which is the correct formula for the ionic compound
containing iron(III) ions and oxide ions?
1. A)
FeO
2. B)
FeO2
3. C)
Fe2O2
4. D)
Fe2O3
5. E)
Fe3O2
Answer: D
Diff: 2
Section: 3.9
52) What is the formula for the ionic compound formed between
lithium and bromide?
1. A)
LiB
2. B) LiBr
3. C)
Li2Br
4. D)
LiBr2
5. E)
Li+Br-
Answer: B
Diff: 2
Section: 3.9
53) What is the formula for the ionic compound formed between
calcium and sulfur?
1. A)
CaS
2. B)
CaSi
3. C)
Ca2S
4. D)
CaS2
5. E)
CaSi2
Answer: A
Diff: 2
Section: 3.9
54) What is the formula of a compound formed by the ions
M2+ and X3-?
1. A)
M2X3
2. B)
M3X2
3. C)
MX3
4. D)
M2X
5. E)
none of the above
Answer: B
Diff: 2
Section: 3.9
55) What is the formula of a compound formed by the ions
M+ and X3-?
1. A)
MX3
2. B)
M3X
3. C)
M3X3
4. D)
M2X6
5. E)
none of the above
Answer: B
Diff: 2
Section: 3.9
56) The main group element E reacts with chlorine to form an
ionic compound with the formula ECl2. The element E is a member of what group
in the Periodic Table?
1. A) 1A
2. B) 2A
3. C) 6A
4. D) 7A
5. E)
none of the above
Answer: B
Diff: 3
Section: 3.9
57) If an element G could react with sulfur to form an ionic
compound with formula GS2, the charge on the ion formed by G would be ________.
1. A) 4-
2. B) 2-
3. C) 1+
4. D) 2+
5. E) 4+
Answer: E
Diff: 3
Section: 3.9
58) A formula unit of the ionic compound copper(II) carbonate
consists of ________ copper(II) ions and ________ carbonate ions.
1. A)
one; one
2. B)
one; two
3. C)
two; one
4. D)
two; two
5. E)
some other combination of ions
Answer: A
Diff: 2
Section: 3.9, 3.10
59) A formula unit of ammonium sulfate consists of ________
ammonium ions and ________ sulfate ions.
1. A)
one; two
2. B)
two; one
3. C)
two; three
4. D)
three; two
5. E)
four; four
Answer: B
Diff: 2
Section: 3.9, 3.10
60) The formula Ca(NO3)2 tells us that one formula unit of
this compound is composed of ________ calcium atoms, ________ nitrogen atoms,
and ________ oxygen atoms.
1. A)
one; two; six
2. B)
two; two; six
3. C)
one; two; five
4. D)
one; one; five
5. E)
one; one; six
Answer: A
Diff: 2
Section: 3.9, 3.10
61) The formula for potassium dichromate is ________.
1. A)
KCr2O7
2. B)
K2Cr2O7
3. C)
K2CrO4
4. D)
PCr2 O7
5. E)
PCrO4
Answer: B
Diff: 1
Section: 3.9, 3.10
62) The formula for the compound chromium(II) nitrate is
________.
1. A)
C2NO3
2. B)
Cr2NO3
3. C)
CrNO3
4. D)
Cr(NO3)2
5. E)
CrNO2
Answer: D
Diff: 2
Section: 3.10
63) The formula (NH4)3PO4 indicates that one formula unit
of this compound is composed of
1. A)
three atoms of nitrogen, twelve atoms of hydrogen, one atom of phosphorus, four
atoms of oxygen, and six extra electrons.
2. B) three
atoms of nitrogen, twelve atoms of hydrogen, four atoms of phosphorus, and four
atoms of oxygen.
3. C)
one atom of nitrogen, twelve atoms of hydrogen, one atom of phosphorus, and
four atoms of oxygen.
4. D)
three atoms of nitrogen, seven atoms of hydrogen, one atom of phosphorus, and
four atoms of oxygen.
5. E)
three atoms of nitrogen, twelve atoms of hydrogen, one atom of phosphorus, and
four atoms of oxygen.
Answer: E
Diff: 3
Section: 3.9, 3.10
64) What is the formula for calcium phosphate?
1. A) Ca3(PO4)2
2. B)
Ca2PO4
3. C)
Ca3PO4
4. D)
Ca2(PO3)3
5. E)
Ca4(PO3)3
Answer: A
Diff: 3
Section: 3.10
65) What is the name of Mg3(PO4)2?
1. A)
trimagnesium diphosphate
2. B)
magnesium diphosphate
3. C)
trimagnesium phosphate
4. D)
magnesium phosphate
5. E)
magnesium phosphorus oxide
Answer: D
Diff: 1
Section: 3.10
66) What is the name of AlCl3?
1. A)
aluminum chloride
2. B)
aluminum(III) chloride
3. C)
aluminum carbide
4. D)
aluminum trichloride
5. E)
aluminum tricarbide
Answer: A
Diff: 1
Section: 3.10
67) What is the name of SnCl2?
1. A) ditin
chloride
2. B)
tin dichloride
3. C)
tin(II) chloride
4. D)
tin chloride
5. E)
strontium chloride
Answer: C
Diff: 1
Section: 3.10
68) Iron pyrite (fool’s gold) is iron(II) sulfide. What is
its formula?
1. A)
FeS
2. B)
FeSO3
3. C)
FeSO4
4. D)
Fe2S3
5. E)
Fe2(SO3)3
Answer: A
Diff: 2
Section: 3.10
69) What is the name of K2S?
1. A)
dipotassium sulfide
2. B)
potassium disulfide
3. C)
potassium(II) sulfide
4. D)
potassium sulfide
5. E)
none of the above
Answer: D
Diff: 1
Section: 3.10
70) The name of the compound with formula NaMnO4 is
1. A)
sodium magnesium oxide.
2. B)
sodium magnesium tetraoxide.
3. C)
sodium manganate.
4. D)
sodium permanganate.
5. E)
sodium manganese tetraoxide.
Answer: D
Diff: 1
Section: 3.10
71) The formula for ammonium hydroxide is ________.
1. A)
OHNH4
2. B) NH4NO3
3. C)
NH4O
4. D)
NH4OH
5. E)
Al(OH)3
Answer: D
Diff: 2
Section: 3.10
72) Which of the following formulas represents a compound that
is a base?
1. A)
CaSO4
2. B)
NH4Cl
3. C)
Mg(OH)2
4. D) H2
5. E)
none of the above
Answer: C
Diff: 2
Section: 3.11
73) One definition of an acid is a substance that provides which
ion in water solution?
1. A)
Na+
2. B) H+
3. C)
OH-
4. D)
NH4+
5. E)
none of the above
Answer: B
Diff: 2
Section: 3.11
74) One definition of a base is a substance that provides
which ion in water solution?
1. A)
Na+
2. B) H+
3. C)
OH-
4. D)
H3O+
5. E)
NH4+
Answer: C
Diff: 2
Section: 3.11
75) Which of the following formulas represents a compound that
is an acid?
1. A)
CaSO4
2. B)
NH4Cl
3. C)
Mg(OH)2
4. D)
H2O
5. E)
H3PO4
Answer: E
Diff: 2
Section: 3.11
Match the following.
76) chromium(II) hydroxide
Diff: 1
Section: 3.10
A)
B)
S
NCC
77) calcium sulfate
Diff: 1
Section: 3.10
C)
D)
(NH4)2CO3
CaS
78) aluminum phosphate
Diff: 1
Section: 3.10
E)
F)
NaN
HCl
79) potassium sulfide
Diff: 1
Section: 3.10
G)
H)
Fe(OH
NaCC
80) sodium acetate
Diff: 1
Section: 3.10
I)
J)
AlP
S
81) ammonium acetate
Diff: 1
1. K) Cr
Section: 3.10 L) (C
82) ammonium carbonate
Diff: 1
Section: 3.10
83) aluminum carbonate
Diff: 1
Section: 3.10
84) potassium sulfite
Diff: 1
Section: 3.10
85) hydrogen chloride
Diff: 1
Section: 3.10
86) sodium nitrite
Diff: 1
Section: 3.10
87) iron(II) hydroxide
Diff: 1
Section: 3.10
Answers: 76) K 77) D 78) I
79) A 80) H 81) B
82) C 83) L 84) J 85)
F 86) E 87) G
Fundamentals of General, Organic, and Biological Chemistry,
7e (McMurry)
Chapter 4 Molecular Compounds
1) A chemical bond formed between two identical atoms is a(an)
________ bond.
1. A)
atomic
2. B)
covalent
3. C)
hydrogen
4. D)
ionic
5. E)
molecular
Answer: B
Diff: 1
Section: 4.1
2) A chemical bond formed when two atoms share two pairs of
electrons is a ________ bond; it is best described as ________.
1. A)
double; covalent
2. B)
double; ionic
3. C)
single; covalent
4. D)
single; ionic
5. E) triple;
covalent
Answer: A
Diff: 2
Section: 4.1
3) Which representation of a hydrogen molecule is not correct?
1. A)
H=H
2. B) H2
3. C) H:H
4. D)
HH
5. E)
none of the above
Answer: A
Diff: 1
Section: 4.2
4) Which representation of a methane molecule is not correct? (A
methane molecule is composed of one carbon atom and four hydrogen atoms.)
1. A)
CH4
2. B)
1. C)
1. D)
1. E)
none of the above
Answer: D
Diff: 1
Section: 4.2
5) Which element is most likely to form three covalent bonds?
1. A) C
2. B) Si
3. C) P
4. D) S
5. E) Se
Answer: C
Diff: 1
Section: 4.2
6) In a covalent compound the bond length can be defined as
1. A)
the distance between any two pairs of electrons.
2. B)
the distance between the two largest atoms.
3. C)
the distance between two nuclei when the repulsion is greatest.
4. D)
the distance between two nuclei when the attraction is greatest.
5. E)
the distance between two nuclei when repulsion and attraction are balanced.
Answer: E
Diff: 2
Section: 4.2
7) Which group contains only elements which normally exist as
diatomic molecules?
1. A)
nitrogen; sulfur, bromine
2. B)
helium; neon, argon
3. C)
nitrogen; oxygen, fluorine
4. D)
hydrogen; lithium, sodium
5. E)
oxygen; phosphorus, germanium
Answer: C
Diff: 2
Section: 4.2
8) A chemical bond formed when two atoms share one pair of electrons
is a ________ bond; it is best described as ________.
1. A)
double; covalent
2. B)
double; ionic
3. C)
single; covalent
4. D)
single; ionic
5. E)
triple; covalent
Answer: C
Diff: 2
Section: 4.2
9) For the dot structure shown the most likely elements are X =________
and Y = ________.
1. A)
carbon; hydrogen
2. B)
carbon; fluorine
3. C)
carbon; oxygen
4. D)
hydrogen; carbon
5. E)
fluorine; carbon
Answer: B
Diff: 3
Section: 4.2
10) When two atoms share one or more pairs of electrons, a
covalent bond is formed.
Answer: TRUE
Diff: 1
Section: 4.2
11) When a non-metal atom bonds with another non-metal atom, an
ionic bond is formed.
Answer: FALSE
Diff: 1
Section: 4.2
12) Which point identifies the bond length between the two atoms
of the diatomic molecule whose potential energy is shown on the graph?
Answer: C
Diff: 1
Section: 4.2
13) Which point identifies the maximum repulsion between the two
atoms of the diatomic molecule whose potential energy is shown in the graph?
Answer: A
Diff: 1
Section: 4.2
14) Which element is most likely to be “X” in the diatomic
molecule shown?
1. A)
nitrogen
2. B)
oxygen
3. C)
fluorine
4. D)
hydrogen
5. E)
helium
Answer: B
Diff: 2
Section: 4.3
15) Which group in the Periodic Table is most likely to contain
the element X in the molecule whose dot structure is shown?
1. A) 2A
2. B) 3A
3. C) 4A
4. D) 5A
5. E) 6A
Answer: E
Diff: 2
Section: 4.3
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