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Chapter 2
Atoms, Molecules, and Ions
Matter
Matter is anything that has mass and takes up space
2
Atomic Theory of Matter
Atoms are the
fundamental building
blocks of matter
championed by John Dalton
(1803 – 1807)
3
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Atomic Theory of Matter
An element is composed
of atoms
Atoms are the smallest
particle of an element
that still have the
properties of the element
4
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Atomic Theory of Matter
Atoms of an element are
identical in mass and
other properties
Atoms of different
elements have different
properties and different
atomic weights
5
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Atomic Theory of Matter
In a chemical reaction,
the mass of
the products equals
the mass of the reactants
Law of conservation of
mass
6
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Atomic Theory of Matter
Samples of a
pure compound always
contain the same elements
in the same mass
proportion
Law of constant composition
7
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Atomic Theory of Matter
Deduced…
When elements combine,
they do so in the ratio of
small whole numbers
Law of Multiple Proportions
8
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SUBATOMIC PARTICLE DISCOVERY
9
The Electron (Cathode Rays)
• High voltage produced radiation
• Particles are negatively charged
• J. J. Thomson is credited with their discovery (1897)
10
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The Electron
Thomson measured the charge/mass ratio of the
electron to be 1.76  108 coulombs/gram (C/g)
11
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Millikan Oil-Drop Experiment
(Electrons)
• Robert Millikan
(1909)
• Determined charge of
the electron
• 1.60 x 10-19 C
• Calculated mass of
electron
• 9.10 x 10-29 g
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The Atom, circa 1900
“Plum pudding” model put
forward by Thomson
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Discovery of the Nucleus
In 1910 Ernest
Rutherford shot 
particles (positive
charge) at a thin
sheet of gold foil
and observed the
pattern of scatter
of the particles
14
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The Nuclear Atom
Particles deflected at
large angles disproved
Thomson’s model could
not be correct
15
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The Nuclear Atom
Particles deflected at
large angles disproved
Thomson’s model could
not be correct
In 1911, Rutherford
presented his
interpretation
16
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MODERN VIEW OF ATOMIC
STRUCTURE
17
Atom Composition
• Atoms are made of subatomic particles
1. Electron have a negative (-) electrical charge
2. Proton has a positive (+) electrical charge
3. Neutron has no charge
18
Subatomic Particles Arrangement
• Location of subatomic particles
– Protons and neutrons are located in the nucleus
• Nucleus is small, dense and positively charged
• >99.6% of an atom’s mass is found in the nucleus
19
Subatomic Particles Arrangement
• Location of subatomic particles
– Electrons are located in the electron cloud
• Space is mostly empty and negatively charged
• Electrons move rapidly around the nucleus
20
Subatomic Particles Arrangement
• Atoms
– Are neutral
– Contain the same number of protons and
electrons
21
Subatomic Particles in an Atom
• Every element has a set
number of protons
assigned to it
(protons and neutrons)
– All carbon atoms contain
6 protons
– All nitrogen atoms
contain 7 protons
– All oxygen atoms contain
8 protons
The number of protons in a atom is called its atomic
number (Z)
In a neutral atom the atomic number = number of electrons
22
Subatomic Particles in an Atom
• Mass number reports
the number of protons
and neutrons in an
atom
(protons and neutrons)
mass # = # of protons +
.
# of neutrons
23
Subatomic Particles in an Atom
(protons and neutrons)
- number of protons = atomic number (Z)
- number of electrons = atomic number (Z)
- number of neutrons = mass number – atomic number
=A-Z
24
Subatomic Particles in an Atom
Element
- number of protons = atomic number (Z)
- number of electrons = atomic number (Z)
- number of neutrons = mass number – atomic number
=A-Z
25
Subatomic Particles in an Atom
# protons = 9
# electrons = 9
# neutrons = 10
# protons = 79
# electrons = 79
# neutrons = 118
26
Number of neutrons in an atom do not have to
equal number of protons in an atom
27
Subatomic Particles in an Atom
# protons = 6
# electrons = 6
# neutrons = 5
% abundance = trace
# protons = 6
# electrons = 6
# neutrons = 6
% abundance = 98.89%
# protons = 6
# electrons = 6
# neutrons = 7
% abundance = 1.11%
# protons = 6
# electrons = 6
# neutrons = 8
% abundance = trace
• Elements may have
different forms
• The amount of each
naturally occurring form
differ
• Isotope – have equal
number of protons but
a different amount of
neutrons
– Element not in
abundance
28
Atomic Weight
• Atomic mass
# protons = 6
# electrons = 6
# neutrons = 5
% abundance = trace
# protons = 6
# electrons = 6
# neutrons = 6
% abundance = 98.89%
– Mass of one type of isotope
– defined as one twelfth
(1/12) of the mass of an
atom of carbon-12
– 1 amu = 1.66054 × 10–24 g
• Atomic weight (average
atomic mass)
# protons = 6
# electrons = 6
# neutrons = 7
% abundance = 1.11%
# protons = 6
# electrons = 6
# neutrons = 8
% abundance = trace
– Atomic Weight = Ʃ [(isotope
mass) × (fractional natural
abundance)]
– Units amu
29
Atomic Weight
• Atomic mass calculated
for carbon
# protons = 6
# electrons = 6
# neutrons = 5
% abundance = trace
# protons = 6
# electrons = 6
# neutrons = 6
% abundance = 98.89%
1. Multiply each isotope’s
relative mass by the
percent abundance
12
6
C : 12.000 amu * 0.9889 = 11.87 amu
13
6
C : 13.003 amu * 0.0111 = 0.144 amu
2. Sum products from
multiplication to get
average atomic mass
# protons = 6
# electrons = 6
# neutrons = 7
% abundance = 1.11%
# protons = 6
# electrons = 6
# neutrons = 8
% abundance = trace
C: 11.87 amu + 0.144 amu = 12.01 amu
30
PERIODIC TABLE
31
Periodic Table
• A systematic organization of the elements
• Elements are arranged in order of atomic number
32
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Periodic Table
What does this mean?
33
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Periodic Table
• Atomic number (Z)
– Number of protons in the atom
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34
Periodic Table
• Atomic symbol or chemical symbol
– 1 or 2 letter designation of an
element
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35
Periodic Table
• Atomic weight
– Average mass of an atom’s isotope
weighted by its percent abundance
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36
Periodic Table
• The rows are called
periods
• Columns are called
groups
• Elements in the
same group have
similar chemical
properties
37
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Periodic Table: Group Names
These five groups are known by their names
38
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Periodic Table
• Metals are on the
left side of the
periodic table
• Some properties of
metals include
• shiny luster
• conducting heat
and electricity
• solidity (except
mercury)
39
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Periodic Table
• Nonmetals are on
the right side of
the periodic table
(except H)
• Are solid (like
carbon), liquid (like
bromine), or gas
(like neon) at room
temperature
40
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Periodic Table
• Elements on the
steplike line are
metalloids
(except Al)
• Properties are
sometimes like
metals and
sometimes like
nonmetals
41
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MOLECULES AND MOLECULAR
COMPOUNDS
42
Molecules
Aggregation of Atoms
Molecule is a group of two or more atoms
bonded together
43
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Molecules
• Diatomic molecules
contain two atoms
• Some naturally
occurring diatomic
molecules
–
–
–
–
Hydrogen
Nitrogen
Oxygen
Chlorine
44
Molecules
• Molecule that contain
two or more types of
atoms are called
molecular compounds
45
Chemical Formulas
Chemical formula states the relative number
and type of atoms present in a molecule
46
Chemical Formulas
• Molecular formulas
– Type of chemical formula
– Provides the exact number of
atoms of each element in a
compound
• Subscript to the right of the
symbol of an element gives this
information
– Almost always contain only
nonmetals
47
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Chemical Formulas
• Molecular formula
– Gives actual number of atoms present in a compound
• Empirical formula
– Gives smallest whole number ratio of atoms present
in a compound
48
Picturing Molecules
• Structural formulas
– Show the order in which
atoms are attached
– Do NOT depict the threedimensional shape of
molecules
• Perspective drawings
– Show the threedimensional order of the
atoms in a compound
49
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IONS AND IONIC COMPOUNDS
50
Ions
• Electron transfer produces ions
• Ion is a charged atom or molecule
–
–
–
–
Occurs because of loss or gain of an electron
Cation is a positively charged ion
Anion is a negatively charged ion
Ion charge is directly related to the number of
electrons lost or gained
51
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Ions: Predicting Charge
• Ions
– Cations are formed by metals
– Anions are formed by nonmetals
52
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Polyatomic ions
• Polyatomic ions
– Atoms in ion bonded
covalently
– Are not molecules
– Pieces of a compound
53
Ionic Compounds
• Ionic compounds
– Formed from cations and anions
– Generally contain metals and nonmetals
– Use empirical formulas
54
Ionic Compounds: Writing Formulas
• Because compounds are electrically neutral, one
can determine the formula of a compound this
way:
– Charge on the cation becomes the subscript on the
anion
– Charge on the anion becomes the subscript on the
cation
– If these subscripts are not in the lowest whole-number
ratio, divide them by the greatest common factor
55
Way of naming compounds
NOMENCLATURE
56
Compound Classification
• Rules for naming ionic and molecular
compounds differ
1st classify compound as ionic or molecular
57
Compound Classification
• There is no sharp dividing line between
ionic and covalent bond
• For purposes of naming
– Compounds consisting of metal and nonmetals
are ionic
– Compounds consisting of only nonmetals are
molecular
– Exception:
• Polyatomic ion of nonmetals replace the metal ion
in an ionic compound
• Metalloid elements are considered nonmetals
58
Compound Classification
• Fixed-charge
metal
– Only forms one
type of positive
ion
• Variable-charge
metal
– Forms more than
one type of
positive ion
Ionic Charge
+1
Ionic Charge
+2
Ionic Charge
+3
Li+
Be2+
Al3+
Na+
Mg2+
Ga3+
K+
Ca2+
Rb+
Sr2+
Cs+
Ba2+
Ag+
Zn2+
Cd2+
59
Compound Classification
• Fixed-charge
metal
– Only forms one
type of positive
ion
• Variable-charge
metal
– Forms more than
one type of
positive ion
60
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NOMENCLATURE FOR IONIC
COMPOUNDS
61
Ions Nomenclature
• Ionic compounds are based on the name of
the ions they are composed
• Rules for cations
1. Fix-charged metal ions take full name of
element plus the word ion
-
Na+
Ca2+
Al3+
sodium ion
calcium ion
aluminum ion
62
Ions Nomenclature
• Rules for cations
2. Variable-charge metal ions
•
Take full name of element followed by a Roman
numeral (in parentheses) that represent the
charge magnitude plus the word ion
- Fe2+
- Fe3+
- Cu2+
iron (II) ion
iron (III) ion
copper (II) ion
63
Ions Nomenclature
• Rules for cations
2. Variable-charge metal
ions (Older naming
system)
• Use suffix –ic for the ion
of higher charge
• Use suffix –ous for the ion
of lower charge
3. Cations formed from
nonmetal atoms end in
–ium
- NH4+ ammonium ion
- H3O+ hydronium ion
64
Ions Nomenclature
• Rules for anions
names
1. Nonmetal ions
take the stem
of the name of
the element
followed by the
suffix –ide and
the word ion
65
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Naming Polyatomic Ions
Polyatomic ions must be memorized
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Patterns in Oxygen Containing Anions
Nomenclature
• The most common oxyanion of an element ends in -ate:
– ClO3− is chlorate
• Oxyanion that has one fewer oxygen then the most common oxyanion
ends in -ite:
– ClO2− is chlorite
• Prefix hypo- indicates one O atom fewer than the oxyanion ending in ite:
– ClO− is hypochlorite
• Prefix per- indicates on more O atom than the oxyanion ending in -ate:
– ClO4− is perchlorate
67
Patterns in Oxygen Containing Anions
Nomenclature
• Central atoms on the second row have a bond up to
three oxygens
• Central atoms on the third row have a bond up to
four oxygens
• Charges increase as you go from right to left
68
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Ionic Compounds Nomenclature
• Naming fixed-charge ionic compounds
– Full name of metallic element is given first
– Nonmetal element name follows with the stem of
the name attached with the suffix –ide
– Name of compound contains sufficient information
to determine chemical formula
NaF
MgF2
Na2O
Be3N2
sodium
fluoride
magnesium
fluoride
sodium
oxide
beryllium
nitride
69
Binary Ionic Compounds
Nomenclature
• Naming variable-charge binary ionic compounds
– Full name of metallic element with a Roman numeral
appended is given first
– Nonmetal element name follows with the stem of
the name attached with the suffix –ide
CuO
Cu2O
Mn2S3
AuCl3
copper
(II) oxide
copper (I)
oxide
manganese (III)
sulfide
gold (III)
chloride
70
Polyatomic Ionic Compounds
Nomenclature
• Name of polyatomic ionic compounds are
derived in a similar way as binary ionic
compounds
– If polyatomic ion positive, name is substituted
for metal
– If polyatomic ion negative, name is substituted
for the nonmetal minus the word ion
– If both polyatomic ions, substitute names of
polyatomic ions
71
Polyatomic Ionic Compounds
Nomenclature
• Name of polyatomic ionic compounds are
derived in a similar way as binary ionic
compounds
Na3PO4
Fe(NO3)3
NH4CN
sodium
phosphate
iron (III)
nitrate
ammonium
cyanide
72
ACID NOMENCLATURE
73
Acid Nomenclature
• Acid
– Hydrogen containing molecular compound that
yields hydrogen ions (H+)
• Naming Acids – naming system applies if acid is
dissolved in water
– If anion does not contain oxygen and ends in
-ide
• Prefix hydro• Suffix –ic
• Add acid
HCl: hydrochloric acid
HCN: hydrocyanic acid
74
Acid Nomenclature
• If anion does contain oxygen
– If anion ends in –ate
• Suffix –ic
• Add acid
HNO3: nitric acid
HClO4: perchloric acid
– If anion ends in –ite
• Suffix –ous
• Add acid
HNO2: nitrous acid
HClO: hypochlorous acid
75
Acid Nomenclature
• Series of oxyacid nomenclature
76
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BINARY MOLECULAR COMPOUND
NOMENCLATURE
77
Binary Molecular Compound
Nomenclature
• Binary molecular compound only has two
nonmetallic elements present
• List nonmetals in a chemical formula by
increasing nonmetallic behavior
– Element with highest atomic number is listed first if in
same group
• Name compound in the order listed in chemical
formula
78
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Binary Molecular Compound
Nomenclature
• Naming binary molecular
compounds
– Full name of first nonmetal is
given first
– Second nonmetal name follows
with the stem of the name
attached with the suffix –ide
– Numerical prefixes giving
numbers of atoms present follow
both nonmetals
N2O5
Dinitrogen
Pentoxide
dinitrogen
pentoxide
PF3
S4N4
phosphorus tetrasulfur
trifluoride
phosphorus tetranitride
tetrasulfur
trifluoride
tetranitride
79
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NOMENCLATURE SIMPLE ORGANIC
COMPOUNDS
80
Nomenclature of Organic Compounds
• Organic chemistry
– Study of carbon
– Own system of nomenclature
• Alkanes contain only hydrogen and carbon
• Stem of name refers to number of carbons
Nomenclature of Organic Compounds
• Alcohol
– Replace a hydrogen with –OH
– Suffix becomes –ol
– Determine type of compound by studying the suffix
83
EXAMPLE ATOMIC NUMBER, ATOMIC SYMBOL, AND
ELEMENT NAME
List the atomic symbol and atomic number for each element.
(a)
(b)
(c)
(d)
silicon
potassium
gold
antimony
SOLUTION
As you become familiar with the periodic table, you will be able
to quickly locate elements on it. At first you may find it easier
to locate them in the alphabetical listing on the inside back
cover of this book, but you should become familiar with their
positions in the periodic table.
84
EXAMPLE CLASSIFYING ELEMENTS AS METALS, NONMETALS, OR
METALLOIDS
Classify each element as a metal, nonmetal, or metalloid.
(a) Ba
(b) I
(c) O
(d) Te
SOLUTION
(a) Barium is on the left side of the periodic table; it is a metal.
(b) Iodine is on the right side of the periodic table; it is a nonmetal.
(c) Oxygen is on the right side of the periodic table; it is a nonmetal.
(d) Tellurium is in the middle-right section of the periodic table, along the line
that divides the metals from the nonmetals; it is a metalloid.
85
EXAMPLE GROUPS AND FAMILIES OF ELEMENTS
To which group or family of elements does each element belong?
(a) Mg (b) N
(c) K
(d) Br
SOLUTION
(a)
(b)
(c)
(d)
Mg is in Group 2A; it is an alkaline earth metal.
N is in Group 5A.
K is in Group 1A; it is an alkali metal.
Br is in Group 7A; it is a halogen.
86
EXAMPLE ATOMIC NUMBERS, MASS NUMBERS, AND ISOTOPE SYMBOLS
What are the atomic number (Z), mass number (A), and symbols of the carbon
isotope that has 7 neutrons?
SOLUTION
You can determine that the atomic number (Z) of carbon is 6 (from the periodic
table). This means that carbon atoms have 6 protons. The mass number (A) for
the isotope with 7 neutrons is the sum of the number of protons and the number
of neutrons.
A = 6 + 7 = 13
So, Z = 6, A = 13, and the symbols for the isotope are C-13 and
87
EXAMPLE NUMBERS OF PROTONS AND NEUTRONS FROM
ISOTOPE SYMBOLS
How many protons and neutrons are in the chromium
isotope
SOLUTION
#p+ = Z = 24
The number of protons is equal to Z (lower left number).
The number of neutrons is equal to A (upper left number)
– Z (lower left number).
#n = A – Z
= 52 – 24
= 28
SKILLBUILDER | Numbers of Protons and Neutrons from Isotope
Symbols
How many protons and neutrons are in the potassium isotope
Answer:
19 protons, 20 neutrons
88
EXAMPLE WRITING CHEMICAL FORMULAS
Write a chemical formula for each compound.
(a) the compound containing two aluminum atoms to every three oxygen
atoms
(b) the compound containing three oxygen atoms to every sulfur atom
(c) the compound containing four chlorine atoms to every carbon atom
Aluminum is the metal, so list it first.
SOLUTION
(a) Al2O3
Sulfur is below oxygen on the periodic table and it
occurs before oxygen in Table 5.1, so list it first.
(b) SO3
Carbon is to the left of chlorine on the periodic table
and it occurs before chlorine in Table 5.1, so list it
first.
(c) CCl4
89
EXAMPLE WRITING CHEMICAL FORMULAS
Continued
SKILLBUILDER | Writing Chemical Formulas
Write a chemical formula for each compound.
(a) the compound containing two silver atoms to every sulfur atom
(b) the compound containing two nitrogen atoms to every oxygen atom
(c) the compound containing two oxygen atoms to every titanium atom
Answers:
(a) Ag2S
(b) N2O
(c) TiO2
90
EXAMPLE CLASSIFYING SUBSTANCES AS ATOMIC ELEMENTS, MOLECULAR
ELEMENTS, MOLECULAR COMPOUNDS, OR IONIC COMPOUNDS
Classify each substance as an atomic element, molecular element, molecular
compound, or ionic compound.
(a) krypton
(b) CoCl2
(c) nitrogen
(d) SO2
(e) KNO3
SOLUTION
(a) Krypton is an element that is not diatomic; therefore, it is an atomic element.
(b) CoCl2 is a compound composed of a metal (left side of periodic table) and
nonmetal (right side of the periodic table); therefore, it is an ionic compound.
(c) Nitrogen is an element that is listed as diatomic in Table 5.2; therefore, it is a
molecular element.
(d) SO2 is a compound composed of two nonmetals; therefore, it is a molecular
compound.
(e) KNO3 is a compound composed of a metal and two nonmetals; therefore, it is
an ionic compound.
91
EXAMPLE NAMING IONIC COMPOUNDS CONTAINING A METAL THAT FORMS
ONLY ONE TYPE OF CATION
Name the compound MgF2.
SOLUTION
The cation is magnesium. The anion is fluorine, which becomes fluoride. Its
correct name is magnesium fluoride.
SKILLBUILDER | Naming Ionic Compounds Containing a Metal
That Forms Only One Type of Ion
Name the compound KBr.
Answer: potassium bromide
SKILLBUILDER PLUS Name the compound Zn3 N2.
Answer: zinc nitride
92
EXAMPLE Naming Ionic Compounds Containing a Metal That Forms More Than
One Type of Cation
Name the compound PbCl4.
SOLUTION
The name for PbCl4 consists of the name of the cation, lead, followed by the
charge of the cation in parentheses (IV), followed by the base name of the
anion, chlor-, with the ending -ide. The full name is lead(IV) chloride. We
know the charge on Pb is 4+ because the charge on Cl is 1–. Since there are 4
Cl– anions, the Pb cation must be Pb4+.
PbCl4 lead(IV) chloride
SKILLBUILDER | Naming Ionic Compounds Containing a Metal
That Forms More Than One Type of Cation
Name the compound PbO.
Answer: lead(II) oxide
93
EXAMPLE NAMING IONIC COMPOUNDS CONTAINING A POLYATOMIC ION
Name the compound K2CrO4.
SOLUTION
The name for K2CrO4 consists of the name of the cation, potassium, followed by
the name of the polyatomic
ion, chromate.
K2CrO4 potassium chromate
SKILLBUILDER | NAMING IONIC COMPOUNDS CONTAINING A
POLYATOMIC ION
Name the compound Mn(NO3)2.
Answer: manganese(II) nitrate
94
EXAMPLE NAMING MOLECULAR COMPOUNDS
Name each compound.
(a) CCl4
(b) BCl3
(c) SF6
SOLUTION
(a)The name of the compound is the name of the first element, carbon, followed by
the base name of the second element, chlor, prefixed by tetra- to indicate four, and
the suffix -ide.
CCl4 carbon tetrachloride
(b)
The name of the compound is the name of the first element, boron, followed
by the base name of the second element, chlor, prefixed by tri- to indicate three,
and the suffix -ide.
BCl3 boron trichloride
(c) The name of the compound is the name of the first element, sulfur, followed by the
base name of the second element, fluor, prefixed by hexa- to indicate six, and the
suffix -ide. The entire name is sulfur hexafluoride.
SF6 sulfur hexafluoride
95
EXAMPLE Naming Binary Acids
Give the name of H2S(aq).
The base name of S is sulfur, so the
name is hydrosulfuric acid.
SOLUTION
H2S (aq) hydrosulfuric acid
SKILLBUILDER | Naming Binary Acids
Name HF(aq).
Answer: hydrofluoric acid
96
EXAMPLE Naming Oxyacids
Name HC2H3O2(aq).
The oxyanion is acetate, which ends in
-ate; therefore, the name of the acid is
acetic acid.
SOLUTION
HC2H3O2(aq) acetic acid
SKILLBUILDER | Naming Oxyacids
Name HNO2(aq)
Answer: nitrous acid
97
Conceptual Checkpoint
An atom composed of which of these particles would have a mass of
approximately 12 amu and be charge-neutral?
(a) 6 protons and 6 electrons
(b) 3 protons, 3 neutrons, and 6 electrons
(c) 6 protons, 6 neutrons, and 6 electrons
(d) 12 neutrons and 12 electrons
Answer:
(c) The mass in amu is approximately equal to the number of
protons plus the number of neutrons. In order to be chargeneutral, the number of protons must equal the number of
electrons.
98
Conceptual Checkpoint
Which statement is NEVER true?
(a) An element can be both a transition element and a metal.
(b) An element can be both a transition element and a metalloid.
(c) An element can be both a metalloid and a halogen.
(d) An element can be both a main-group element and a halogen.
Answer:
(b) An element can be both a transition element and a metalloid.
99
Conceptual Checkpoint
Carbon has two naturally occurring isotopes:
and
Using circles to
represent protons and squares to represent neutrons, draw the nucleus of each
isotope.
100
Conceptual Checkpoint
If an atom with a mass number of 27 has 14 neutrons, it is an isotope of which
element?
(a) silicon
(b) aluminum
(c) cobalt
(d) niobium
Answer:
(b) This atom must have (27 − 14) = 13 protons; the element with an
atomic number of 13 is Al.
101
What is the charge on the electron, the proton, and the
neutron, respectively?
A.
B.
C.
D.
E.
–1,+1,+1
–1,+1,–1
–1, 0,+1
–1,+1, 0
+1,+1, 0
102
What is the charge on the electron, the proton, and the
neutron, respectively?
A.
B.
C.
D.
E.
–1,+1,+1
–1,+1,–1
–1, 0,+1
–1,+1, 0
+1,+1, 0
103
Which of the following subatomic particles has the
least mass?
A.
B.
C.
D.
E.
Electron
Neutron
Proton
Two of the above
All of the above
104
Which of the following subatomic particles has the
least mass?
A.
B.
C.
D.
E.
Electron
Neutron
Proton
Two of the above
All of the above
105
What subatomic particle(s) is/are found in the nucleus?
A.
B.
C.
D.
E.
Electron
Neutron
Proton
Two of the above
All of the above
106
What subatomic particle(s) is/are found in the nucleus?
A.
B.
C.
D.
E.
Electron
Neutron
Proton
Two of the above
All of the above
107
Which element has the chemical symbol “Pb”?
A.
B.
C.
D.
E.
Mercury
Polonium
Platinum
Tungsten
Lead
108
Which element has the chemical symbol “Pb”?
A.
B.
C.
D.
E.
Mercury
Polonium
Platinum
Tungsten
Lead
109
What is the chemical symbol for potassium?
A.
B.
C.
D.
E.
Po
P
Pt
Pb
K
110
What is the chemical symbol for potassium?
A.
B.
C.
D.
E.
Po
P
Pt
Pb
K
111
How many protons are in one silver atom?
A.
B.
C.
D.
E.
47
60
94
108
154
112
How many protons are in one silver atom?
A.
B.
C.
D.
E.
47
60
94
108
154
113
Which of the following elements is a metalloid?
A.
B.
C.
D.
E.
Aluminum
Silicon
Tin
Phosphorus
Iodine
114
Which of the following elements is a metalloid?
A.
B.
C.
D.
E.
Aluminum
Silicon
Tin
Phosphorus
Iodine
115
Which of the following elements is a metalloid?
A.
B.
C.
D.
E.
Arsenic
Bismuth
Carbon
Iodine
Gallium
116
Which of the following elements is a metalloid?
A.
B.
C.
D.
E.
Arsenic
Bismuth
Carbon
Iodine
Gallium
117
Strontium is in which of the following groups?
A.
B.
C.
D.
E.
Halogens
Noble gases
Alkaline earth metals
Alkali metals
Transition metals
118
Strontium is in which of the following groups?
A.
B.
C.
D.
E.
Halogens
Noble gases
Alkaline earth metals
Alkali metals
Transition metals
119
Chlorine is in which of the following groups?
A.
B.
C.
D.
E.
Halogens
Noble gases
Alkaline earth metals
Alkali metals
Transition metals
120
Chlorine is in which of the following groups?
A.
B.
C.
D.
E.
Halogens
Noble gases
Alkaline earth metals
Alkali metals
Transition metals
121
The sum of neutrons and protons in a given nucleus is
referred to as the
A.
B.
C.
D.
E.
proton number.
mass number.
atomic number.
isotope number.
neutron number.
122
The sum of neutrons and protons in a given nucleus is
referred to as the
A.
B.
C.
D.
E.
proton number.
mass number.
atomic number.
isotope number.
neutron number.
123
How many electrons are in the bromide ion?
A.
B.
C.
D.
E.
35
36
46
70
80
124
How many electrons are in the bromide ion?
A.
B.
C.
D.
E.
35
36
46
70
80
125
How many electrons, protons, and neutrons respectively
are in the iron(III) ion, 56Fe3+?
A.
B.
C.
D.
E.
23, 26, 30
26, 26, 30
26, 26, 56
26, 26, 26
29, 26, 30
126
How many electrons, protons, and neutrons respectively
are in the iron(III) ion, 56Fe3+?
A.
B.
C.
D.
E.
23, 26, 30
26, 26, 30
26, 26, 56
26, 26, 26
29, 26, 30
127
What is the symbol for an ion having 12 protons and
10 electrons?
A.
B.
C.
D.
E.
Si2+
Si
Mg2+
Ne
Ne2–
128
What is the symbol for an ion having 12 protons and
10 electrons?
A.
B.
C.
D.
E.
Si2+
Si
Mg2+
Ne
Ne2–
129
What is the symbol for an ion having 15 protons and
18 electrons?
A.
B.
C.
D.
E.
Ph3–
Ar
P3+
Cl–
P3–
130
What is the symbol for an ion having 15 protons and
18 electrons?
A.
B.
C.
D.
E.
Ph3–
Ar
P3+
Cl–
P3–
131
How many electrons are in the scandium ion, Sc3+?
A.
B.
C.
D.
E.
45
42
48
24
18
132
How many electrons are in the scandium ion, Sc3+?
A.
B.
C.
D.
E.
45
42
48
24
18
133
Which atom has the same number of protons as 59Ni?
A.
B.
C.
D.
E.
59Fe
58Ni
59Co
141Pr
102Rh
134
Which atom has the same number of protons as 59Ni?
A.
B.
C.
D.
E.
59Fe
58Ni
59Co
141Pr
102Rh
135
The nucleus of a fluorine-19 atom contains
A.
B.
C.
D.
E.
19 protons and
19 electrons.
19 protons and
0 electrons.
9 protons and
10 electrons.
19 protons and
19 neutrons.
9 protons and
10 neutrons.
136
The nucleus of a fluorine-19 atom contains
A.
B.
C.
D.
E.
19 protons and
19 electrons.
19 protons and
0 electrons.
9 protons and
10 electrons.
19 protons and
19 neutrons.
9 protons and
10 neutrons.
137
Which of the following species has 10 electrons and
14 neutrons?
A.
B.
C.
D.
E.
27Al3+
27Al
14N3–
24Mg2+
20Ne
138
Which of the following species has 10 electrons and
14 neutrons?
A.
B.
C.
D.
E.
27Al3+
27Al
14N3–
24Mg2+
20Ne
139
Isotopes have
A.
B.
C.
D.
E.
the same number of protons, but different numbers
of neutrons.
the same number of protons and neutrons.
the same chemical symbol.
the same number of electrons and neutrons.
Two of the above
140
Isotopes have
A.
B.
C.
D.
E.
the same number of protons, but different numbers
of neutrons.
the same number of protons and neutrons.
the same chemical symbol.
the same number of electrons and neutrons.
Two of the above
141
Which of the following is characteristic of metals?
A.
B.
C.
D.
E.
Solid at room temperature
Malleable
Ductile
Located toward the left side of the periodic table
All of the above
142
Which of the following is characteristic of metals?
A.
B.
C.
D.
E.
Solid at room temperature
Malleable
Ductile
Located toward the left side of the periodic table
All of the above
143
Which of the following is NOT a part of Dalton’s
atomic theory?
A.
B.
C.
D.
E.
Each element is composed of small indestructible particles called “atoms.”
Atoms of a given element are identical to each other.
Matter is neither created nor destroyed.
Atoms combine in simple, whole-number ratios to form compounds.
All of the above are part of the atomic theory.
144
Which of the following is NOT a part of Dalton’s
atomic theory?
A.
B.
C.
D.
E.
Each element is composed of small indestructible particles called “atoms.”
Atoms of a given element are identical to each other.
Matter is neither created nor destroyed.
Atoms combine in simple, whole-number ratios to form compounds.
All of the above are part of the atomic theory.
145
The nucleus of an atom
contains
a.
b.
c.
d.
protons and neutrons.
protons and electrons.
electrons and neutrons.
protons, neutrons, and electrons.
146
The nucleus of an atom
contains
a.
b.
c.
d.
protons and neutrons.
protons and electrons.
electrons and neutrons.
protons, neutrons, and electrons.
147
Two atoms with the same
atomic number but different
mass numbers are called
a.
b.
c.
d.
mutants.
isomers.
isotopes.
symbiots.
148
Two atoms with the same
atomic number but different
mass numbers are called
a.
b.
c.
d.
mutants.
isomers.
isotopes.
symbiots.
149
Select the incorrect statement
about the mass and volume of
an atom.
a. The mass is determined mostly by the
protons and neutrons.
b. The volume is mostly empty space.
c. The mass is concentrated in the nucleus.
d. The volume is determined by the
arrangement of the protons.
150
Select the incorrect statement
about the mass and volume of
an atom.
a. The mass is determined mostly by the
protons and neutrons.
b. The volume is mostly empty space.
c. The mass is concentrated in the nucleus.
d. The volume is determined by the
arrangement of the protons.
151
Metals and nonmetals react to
form ________ compounds.
a.
b.
c.
d.
molecular
mixed
empirical
ionic
152
Metals and nonmetals react to
form ________ compounds.
a.
b.
c.
d.
molecular
mixed
empirical
ionic
153
Positive ions are called
a.
b.
c.
d.
positrons.
anions.
cations.
nucleons.
154
Positive ions are called
a.
b.
c.
d.
positrons.
anions.
cations.
nucleons.
155
The elements located in Group
VIIA (Group 17) on the periodic
table are called
a.
b.
c.
d.
alkali metals.
noble gases.
chalcogens.
halogens.
156
The elements located in Group
VIIA (Group 17) on the periodic
table are called
a.
b.
c.
d.
alkali metals.
noble gases.
chalcogens.
halogens.
157
Which name is incorrectly
paired with the formula?
a.
b.
c.
d.
hydroxide ion; OH–
barium(II) chloride; BaCl2
ammonia; NH3
sulfur dioxide; SO2
158
Which name is incorrectly
paired with the formula?
a.
b.
c.
d.
hydroxide ion; OH–
barium(II) chloride; BaCl2
ammonia; NH3
sulfur dioxide; SO2
159
Acids produce _____ ions.
a.
b.
c.
d.
OH–1
OH+1
H+1
H–1
160
Acids produce _____ ions.
a.
b.
c.
d.
OH–1
OH+1
H+1
H–1
161
NaOCl is named
a.
b.
c.
d.
sodium chlorate.
sodium chlorite.
sodium perchlorate.
sodium hypochlorite.
162
NaOCl is named
a.
b.
c.
d.
sodium chlorate.
sodium chlorite.
sodium perchlorate.
sodium hypochlorite.
163
LiNO3 is named
a.
b.
c.
d.
lithium nitrate.
lanthanum nitrate.
lanthanum nitrite.
lithium nitrite.
164
LiNO3 is named
a.
b.
c.
d.
lithium nitrate.
lanthanum nitrate.
lanthanum nitrite.
lithium nitrite.
165
The formula for aluminum
carbonate is
a.
b.
c.
d.
Al2(CO3)3.
AlCO3.
Al2C3.
Al3(CO3)2.
166
The formula for aluminum
carbonate is
a.
b.
c.
d.
Al2(CO3)3.
AlCO3.
Al2C3.
Al3(CO3)2.
167
Fe2O3 is named
a.
b.
c.
d.
diiron trioxide.
iron(III) oxide.
ferrous oxide.
ironic oxide.
168
Fe2O3 is named
a.
b.
c.
d.
diiron trioxide.
iron(III) oxide.
ferrous oxide.
ironic oxide.
169
Which acid is not an oxyacid?
a.
b.
c.
d.
hydrochloric acid
nitric acid
sulfurous acid
acetic acid
170
Which acid is not an oxyacid?
a.
b.
c.
d.
hydrochloric acid
nitric acid
sulfurous acid
acetic acid
171
HIO4 is named
a.
b.
c.
d.
iodic acid.
iodous acid.
periodic acid.
hydrogen iodate.
172
HIO4 is named
a.
b.
c.
d.
iodic acid.
iodous acid.
periodic acid.
hydrogen iodate.
173
Cl2O7 is named
a.
b.
c.
d.
chlorine(VII) oxide.
dichlorine hexaoxide.
dichlorine heptaoxide.
bichlorine heptaoxide.
174
Cl2O7 is named
a.
b.
c.
d.
chlorine(VII) oxide.
dichlorine hexaoxide.
dichlorine heptaoxide.
bichlorine heptaoxide.
175
C3H8 is named
a.
b.
c.
d.
ethane.
propane.
propanol.
pentane.
176
C3H8 is named
a.
b.
c.
d.
ethane.
propane.
propanol.
pentane.
177