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Section 5.1
Ionic Compounds
Section 5.2
Covalent Compounds
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Ionic Compounds
• Apply ionic charge to writing formulas for ionic
compounds.
• Apply formulas to name ionic compounds.
• Interpret the information in a chemical
formula.
Ionic Compounds
ion: an atom or group of combined atoms that
has a charge because of loss or gain of
electrons
Ionic Compounds
binary compound
hydrate
formula unit
hygroscopic
oxidation number
deliquescent
polyatomic ion
anhydrous
The attraction of oppositely charged
ions holds atoms in ionic compounds
together.
Binary Ionic Compounds
• Ionic compounds are made up of
oppositely charged ions held together
strongly in well-organized units.
Binary Ionic Compounds (cont.)
• A binary compound is a compound that
contains only two elements, such as
sodium chloride (NaCl).
• In naming a binary ionic compound, the
element with the positively charged ion,
usually a metal, is named first with the
negatively charged ion, usually a nonmetal,
named next, modified to end in –ide.
Name the following binary compounds:
• Li2O
• MgS
• Ca3N2
Binary Ionic Compounds (cont.)
• When writing a formula, you add subscripts
to the symbols for the ions until the
algebraic sum of the ions’ charge is zero.
• If more than one ion of a given element is
present in a compound, the subscript
indicates how many ions are present.
Binary Ionic Compounds (cont.)
• The simplest ratio of ions in a compound is
called a formula unit.
Binary Ionic Compounds (cont.)
• Metals tend to lose electrons and become
positively charged while nonmetals tend to
gain electrons and become negatively
charged.
Binary Ionic Compounds (cont.)
• The charge on the ion is known as the
oxidation number of the atom.
Write formulas for the following binary
compounds:
• sodium chloride
• strontium fluoride
• beryllium oxide
Binary Ionic Compounds (cont.)
• In a polyatomic ion, an ion that has two or
more different elements, a group of
elements is covalently bonded together
when the atoms share electrons.
Binary Ionic Compounds (cont.)
• In naming a compound with a polyatomic
ion, the molecule with the positive charge
is named first, followed by the negative ion.
• The ending of the negative polyatomic ion
name does not change.
Binary Ionic Compounds (cont.)
Practice Problems #3-4 page 160
3) a) ammonium and sulfate ions
b) calcium and monohydrogen phosphate ions
c) ammonium and dichromate ions
d) barium and nitrate ions
Practice Problems #3-4 page 160
4) a) sodium phosphate
b) magnesium hydroxide
c) ammonium phosphate
d) potassium dichromate
Compounds of transition elements
• Transition elements can form more than
one type of positive ion and have more
than one oxidation number.
• To distinguish the names of compounds
formed from the different ions of a transition
element, scientists use a Roman numeral to
indicate the oxidation number of a transition
element ion.
Practice Problems #5-6 page 163
5) a) copper(I) and sulfite
b) tin(IV) and fluoride
c) gold(III) and cyanide
d) lead(II) and sulfide
Practice Problems #5-6 page 163
6) a) Pb(NO3)2
b) Mn2O3
c) Ni(C2H3O2)2
d) HgF2
Compounds of transition elements (cont.)
Compounds of transition elements (cont.)
Hydrates
• A compound in which there is a specific
ratio of water to ionic compound is a
hydrate.
• In a hydrate, the water molecules are
chemically bonded to the ionic compound.
Hydrates (cont.)
• A hygroscopic substance is a substance
that absorbs water molecules from the air
to become a hydrate.
• Compounds that form hydrates often are
used as drying agents, also called
desiccants, because they absorb so much
water from the air when they become
hydrated.
Hydrates (cont.)
• Heating hydrates can result in an
anhydrous compound, or a compound in
which all the water has been removed.
• To name hydrates, follow the regular name
for the compound with the word hydrate, to
which a prefix has been added to indicate the
number of water molecules present.
Hydrates (cont.)
Name the hydrates.
MgBr2●6H2O
CaSO4●2H2O
Interpreting Formulas
• A formula summarizes how many atoms of
each element are present.
• If more than one formula unit of a compound
is present, a coefficient is placed before the
formula.
How many formula units are present?
2 NaCl
3 H3PO4
6 CO2
Section Assessment
The simplest ratio of ions in a compound
is called a(n) ___.
A. oxidation unit
B. formula unit
C. binary compound
D. binary ionic compound
Section Assessment
Which compound is a binary compound?
A. Potassium iodide
B. Lithium copper
C. Iron magneside
D. Sulfur hydrogen
Covalent Compounds
• Compare the properties of molecular and ionic
substances.
• Distinguish among allotropes of an element.
• Apply formulas to name molecular
compounds.
Covalent Compounds
anhydrous: a compound in which all of the
water has been removed, usually by heating
Covalent Compounds
distillation
organic compound
molecular element
inorganic compound
allotrope
hydrocarbon
Covalent bonds hold atoms in covalent
compounds together.
Properties of Covalent Compounds
• The properties of most ionic and covalent
compounds are different enough that their
differences can be used to classify and
separate them from one another.
Properties of Covalent Compounds (cont.)
• Distillation is the method of separating
substances in a mixture by the evaporation
of a liquid and subsequent condensation of
its vapor.
• Most covalent compounds are not
electrolytes because they do not easily form
ions.
Molecular Elements
• A molecule that forms when atoms of the
same element bond together is called a
molecular element.
Molecular Elements (cont.)
• Seven nonmetal elements are found
naturally as diatomic elements, or
molecular elements of two identical atoms.
– hydrogen
– chlorine
– nitrogen
– bromine
– oxygen
– iodine
– fluorine
Molecular Elements (cont.)
• Molecules of a single element that differ in
crystalline or molecular structure are called
allotropes.
• The properties of allotropes are usually
different even though they contain the same
element.
Molecular Elements (cont.)
• Phosphorous has three common allotropes
formed from P4 molecules that are joined in
different ways.
– Each allotrope of phosphorous has a
unique structure and set of properties.
Molecular Elements (cont.)
• Carbon occurs as several important
allotropes with different properties.
– Diamonds are crystals in which the atoms
of carbon are held rigidly in place in a
three-dimensional network.
– In graphite, carbon atoms are held together
closely in flat layers that can slide over
each other.
Molecular Elements (cont.)
• Allotropes of oxygen
– Ozone consists of three atoms of oxygen,
occurs naturally, and is harmful to living
things.
Formulas and Names of
Covalent Compounds
• Substances are either organic or
inorganic.
• Compounds that contain carbon, with a few
exceptions, are classified as organic
compounds.
Formulas and Names of
Covalent Compounds (cont.)
• Compounds that do not contain carbon are
called inorganic compounds.
• If inorganic compounds contain only two
nonmetal elements, they are bonded
covalently and are referred to as molecular
binary compounds.
Formulas and Names of
Covalent Compounds (cont.)
• Naming the compound
– Name of the first nonmetal farthest left on
the periodic table is listed first, followed by
name of second nonmetal with its ending
changed to –ide.
– Add a prefix to the name of each element
to indicate how many atoms of each
element are present.
Formulas and Names of
Covalent Compounds (cont.)
Practice Problems page 179
13) Name the following covalent compounds.
a) S2Cl2
b) CS2
c) SO3
d) P4O10
14) Write the formula for the following compounds.
a) carbon tetrachloride
b) iodine heptafluoride
c) dinitrogen monoxide
d) sulfur dioxide
Formulas and Names of
Covalent Compounds (cont.)
• Some scientists use the more common
names for certain compounds, such as
water, ammonia, and sulfuric acid.
Formulas and Names of
Covalent Compounds (cont.)
Naming Acids
Binary Acids
• The first word has the prefix hydro- followed by the root
of the element plus the suffix –ic.
• The second word is always acid.
Oxyacids
• An oxyacid is an acid that contains both a hydrogen
atom and an ion containing oxygen.
• Identify the oxygen-containing ion present.
• The first word is the root of the ion plus the suffix
-ic if the anion ends in -ate
or -ous if the oxyanion ends in -ite.
• The second word is always acid.
Formulas and Names of
Covalent Compounds (cont.)
• The name of even the most complex
organic compound is based on the name of
a hydrocarbon, an organic compound that
contains only the elements hydrogen and
carbon.
• Compounds containing the noble gases
helium, neon, and argon have never been
found.
Formulas and Names of
Covalent Compounds (cont.)
Section Assessment
Which of the following is not a
hydrocarbon?
A. hexane
B. nonane
C. heptane
D. lexane
Section Assessment
What is the correct formula for dinitrogen
trioxide?
A. N2O3
B. N2O2
C. N3O2
D. N2O
Chemistry Online
Study Guide
Chapter Assessment
Standardized Test Practice
Image Bank
Concepts in Motion
Key Concepts
•
The position of an element in the periodic table indicates what
charge its ions will have.
•
Binary ionic compounds are named by first naming the metal
element and then the nonmetal element, with its ending changed
to –ide. Subscripts are used in formulas to indicate how many
atoms of each element are present in the compound.
•
Polyatomic ions can combine with ions of opposite charge to form
ionic compounds which are named by writing the name of the
positive ion first and then the name of the negative ion.
•
Most transition elements can form two or more positively charged
ions. The oxidation number of the transition element is indicated
by a Roman numeral in parentheses.
•
Hydrates are ionic compounds bonded to
water molecules.
Key Concepts
•
Covalent compounds generally have low melting points, low
water solubility, and little or no ability to act as electrolytes.
•
Seven elements occur naturally as diatomic molecules. They are
hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and
iodine.
•
Some elements exist in different structural forms called allotropes.
•
Binary covalent compounds are named by writing the two
elements in the order they are found in the formula, changing the
ending of the second element to –ide, and adding Greek prefixes
to the element names to indicate how many atoms of each are
present.
Which compound is not a polyatomic ion?
A. sulfate
B. potassium chloride
C. ammonium
D. hydrogen carbonate
What kind of substance absorbs water
molecules from the air to become a
hydrate?
A. oxidation compound
B. anhydrous compound
C. desiccant
D. hygroscopic substance
A formula summarizes how many ___ are
present.
A. electrons
B. atoms
C. elements
D. compounds
To create an anhydrous compound, what
must be added to the hydrates?
A. water
B. air
C. heat
D. light
What is the method of separating
substances in a mixture by the
evaporation of a liquid and subsequent
condensation of its vapor?
A. distillation
B. hydration
C. oxidation
D. molecular division
How many nonmetal elements are found
naturally as molecular elements of two
identical atoms?
A. six
B. seven
C. eight
D. twelve
Which of the following is not a diatomic
element?
A. nitrogen
B. bromine
C. chlorine
D. sulfur
Which is an allotrope of oxygen?
A. graphite
B. diamond
C. fullerene
D. ozone
Which is the most versatile element in
forming allotropes?
A. phosphorous
B. carbon
C. oxygen
What is the chemical name for water?
A. dihydroxide oxygen
B. dioxide monohydride
C. dihydrogen monoxide
D. dioxygen hydroxide
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Table 5.5
Naming Prefixes
Table 5.7
Names of Common Acids
and Bases
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