IONIC BONDING AND
NOMENCLATURE
Ionic Bonding and Nomenclature
Ionic Bonding
Comparing the Properties of Ionic and Covalent
Compounds
Naming and Writing Formulas for Ions
Naming and Writing Formulas for Ionic Compounds
Metallic Bonding
Naming and Writing Formulas for Acids and Bases
Ionic Bonding
Ionic bonding involves the transfer of
valence electrons.
One atom loses one or more valence
electrons to become a cation (positive ion).
The other atom gains one or more valence
electrons to become an anion (negative ion).
Ionic compounds are electrically neutral.
This means the total number of negative
charges is equal to the total number of
positive charges.
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Ionic Bonding
Ionic bonding usually results from the
bonding of a metal with a nonmetal.
For example, the alkali metals typically
bond with the halogens to form an ionic
compound commonly referred to as a
salt.
The chemical formula for an ionic
compound is referred to as a formula
unit and not a molecule.
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Ionic Bonding
At room temperature, crystals of
ionic compounds exist as regular,
three-dimensional arrangements of
cations and anions held together by
electrostatic attractions.
The arrangements are called
crystal lattices.
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Ionic Bonding
Here is an example of the crystal
lattice for sodium chloride.
(Note: The lines between the ions are not bonds; they are reference lines
showing the relative positions of Na+ and Cl-.)
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Using Lewis Dot Diagrams to Predict
Formulas for Ionic Compounds
Lewis dot diagrams can be used to
illustrate the transfer of valence
electrons that occurs and to predict
the chemical formula for an ionic
compound.
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Example 1. Use Lewis dot diagrams to predict
the formula for the ionic compound formed from
sodium and chlorine.
First draw the Lewis dot diagrams for
sodium and for chlorine.
Next use arrows to illustrate the transfer of
valence electrons.
The resulting chemical formula is NaCl. The
compound formed is called sodium chloride.
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Example 2. Use Lewis dot diagrams to predict
the formula for the ionic compound formed from
calcium and iodine.
First draw the Lewis dot diagrams for
calcium and for iodine.
Next use arrows to illustrate the transfer of
valence electrons.
The resulting chemical formula is CaI2. The
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compound formed is called calcium iodide.
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Example 3. Use Lewis dot diagrams to predict
the formula for the ionic compound formed from
barium and sulfur.
First draw the Lewis dot diagrams for
barium and for sulfur.
Next use arrows to illustrate the transfer of
valence electrons.
The resulting chemical formula is BaS. The
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compound formed is called barium sulfide.
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You Try It
Use Lewis dot diagrams to predict the
formula for the ionic compound formed
from lithium and oxygen.
Chemical Formula
Li2O
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You Try It
Use Lewis dot diagrams to predict the
formula for the ionic compound formed
from aluminum and nitrogen.
Chemical Formula
AlN
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Use Lewis dot diagrams to predict the
formula for the ionic compound formed
from magnesium and nitrogen.
Chemical Formula
Mg3N2
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Comparing the Properties of Ionic and Covalent Compounds
Characteristics of Ionic and Covalent Compounds
Characteristic
Representative
Unit (smallest particle that has all of
Ionic Compound
formula unit
Nonpolar
Covalent
Compound
Polar Covalent
Compound
molecule
the properties)
Bond Formation
transfer of one or more
valence electrons
between atoms
Type of Elements
forming compounds
Metal with a nonmetal
Physical State
Solid
Melting Point
high
Solubility in H2O
soluble
Electrical
Conductivity of
Aqueous Solution
good electrolyte
sharing of electron pairs
between atoms
nonmetals
solid, liquid, or gas
low
insoluble
nonelectrolyte
soluble
poor to
nonelectrolyte (usually
nonelectrolytes)
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Daily Starter (12/3 & 12/4)
The table below represents a student’s experimental
results. Use the information to answer the questions
below.
Compound
Solubility in
Water
Conductivity in
Water
Melting
Point
A
Soluble
Weak Electrolyte
Low
B
Soluble
Strong Electrolyte
High
C
Insoluble
Non Electrolyte
Low
1. Which compound is polar covalent?
A
2. Which compound is nonpolar covalent?
3.
Which compound is ionic? B
C
Predicting Charges for Ions
The periodic table can be used to help predict the charge
on an ion.
Remember:
Cations are formed when an loses one or more valence
electrons. This is typical of metals.
Anions are formed when a metal gains one or more
valence electrons. This is typical of nonmetals.
Symbols of Ions for Cations
The metals in groups 1, 2 and 13
lose electrons when they form ions.
Group 1 forms +1 ions.
Group 2 forms +2 ions
Group 13 forms +3 ions.
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Naming and Writing Symbols for Cations
You Try It. Write the symbol and name for each of the following ions.
Element
Symbol of Ion
Name of Ion
Calcium ion
Sodium
Ca2+
Na+
Aluminum
Al3+
Aluminum ion
Calcium
Sodium ion
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Metals with More than One Common
Oxidation Number
The metals in groups 3-12 are
called transition metals.
They often have more than one
common oxidation number (ionic
charge).
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Metals with More than One Common Oxidation Number
Here are some of the more commonly used transition metals and
their oxidation numbers. Notice that a Roman numeral is used
to indicate the charge on the ion when naming the ions formed.
Fe2+
Cu+
Hg22+
Pb2+
Sn2+
Cr2+
Cr6+
Mn2+
Co2+
Ni2+
Ag+
Zn2+
Cd2+
Iron(II) ion
Fe3+ Iron(III) ion
Copper(I) ion
Cu2+ Copper(II) ion
Mercury(I) ion
Hg2+ Mercury(II) ion
Lead(II) ion
Pb4+ Lead(IV) ion
Tin(II) ion
Sn4+ Tin(IV) ion
Chromium(II) ion
Cr3+ Chromium(III) ion
Chromium(VI) ion
Manganese(II) ion
Mn3+ Manganese(III) ion
Cobalt(II) ion
Co3+ Cobalt(III) ion
Nickel(II) ion
Ni3+
Nickel(III) ion
Silver ion
Note: Silver, Zinc and Cadmium do not have more than
one common oxidation number. Do not use a Roman
Zinc ion
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Cadmium ion numeral when naming them.
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Symbols of Ions for Anions
An anion is an atom or group of atoms with a
negative charge.
An anion has more electrons than a neutral
atom of the element.
Group 17 forms -1 ions.
Group 16 forms -2 ions.
Group 15 forms -3 ions.
The names of monatomic anions end in ide.
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Naming and Writing Formulas for Anions
You Try It. Write the symbol and name for each of the following ions.
Element
Symbol of Ion
Name of Ion
Chloride ion
Nitrogen
ClN3-
Oxygen
O2-
Oxide ion
Chlorine
Nitride ion
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You Try It
Complete the following table.
Symbol of
Ion
Name of Ion
Number of Electrons Lost
or Gained
S2-
Sulfide ion
Cu+
Copper(I) ion
2 e- gained
1 e- lost
2 e- lost
3 e- lost
3 e- lost
1 e- lost
3 e- gained
Ba2+
Al3+
Fe3+
Barium ion
Aluminum ion
Iron(III) ion
Li+
Lithium ion
P3-
Phosphide ion
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Naming and Predicting Formulas for Binary
Ionic Compounds
Binary ionic compounds usually consist of a metal, such as
an alkali metal, bonded to a nonmetal, such as a halogen.
They are electrically neutral. This means that the total
positive charge is equal to the total negative charge.
Empirical formulas are used to represent ionic compounds.
An empirical formula is the simplest ratio in which the
atoms combine to form a compound.
They are named by naming the cation followed by the
anion. ex. LiCl is lithium chloride, FeCl2 is iron(II) chloride
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Examples: Write the formulas for the compounds
formed between the following pairs of ions and then
name the compound.
a.
b.
c.
d.
e.
K+, ClMg2+, S2Na+, N3Al3+, S2Sn4+, O2-
KCl
MgS
Na3N
Al2S3
SnO2
potassium chloride
magnesium sulfide
sodium nitride
aluminum sulfide
tin(IV) oxide
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You Try It
Write the formulas for the following binary ionic
compounds. Hint: First determine the symbols for the ions
involved. Always write the cation first. The first one has
been done for you as an example.
a. Sodium bromide
Na+,
Br-
b. Magnesium sulfide
Mg2+,
c. Copper(I) chloride
Cu+,
d. Calcium bromide
Ca2+,
e. Strontium fluoride
Sr2+,
S2-
Cl-
NaBr
MgS
CuCl
Br-
CaBr2
F-
SrF2
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You Try It
Write the formulas for the following binary ionic
compounds. Hint: First determine the symbols for the ions
involved. Always write the cation first. The first one has
been done for you as an example.
O2-
Na2O
f. Sodium oxide
Na+,
g. Lead(II) bromide
Pb2+,
Br-
PbBr2
h. Zinc sulfide
Zn2+,
S2-
ZnS
i. Aluminum oxide
Al3+,
O2-
Al2O3
j. Chromium(VI) nitride
Cr6+,
N3-
CrN2
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Roman Numerals
So far, you have been given examples where
the Roman numeral has been indicated either
by the name of the compound or by the symbol
of the cation.
But how do you determine the charge of the
Roman numeral if it is not given to you?
To determine the charge of the Roman
numeral you have to first identify the ions
making up the compound.
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Roman Numerals
Examples.
Ions
Fe3+, O2Cu+, S2-
Co2+, ISn4+, O2Fe2+, S2Cu+, N3-
Chemical
Formula
Fe2O3
Cu2S
CoI2
SnO2
FeS
Cu3N
Name of Compound
Iron(III) oxide
Copper(I) sulfide
Cobalt(II) iodide
Tin(IV) oxide
Iron(II) sulfide
Copper(I) nitride
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You Try It
Write formulas for the following compounds. Remember to
determine the ions involved first.
Name of Compound
Ions
Formula of
Compound
Lithium oxide
Li+, O2Sn4+, S2Ba2+, N3Na+, F-
Li2O
SnS2
Ba3N2
NaF
Tin(IV) sulfide
Barium nitride
Sodium fluoride
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You Try It
Name the following compounds.
a.
CaS
Calcium sulfide
b.
FeN
Iron(III) nitride
c.
K2O
Potassium oxide
d.
PbO
Lead(II) oxide
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Naming and Writing Formulas for Ternary Ionic Compounds
Ternary ionic compounds contain more than two elements. They usually
contain one or more polyatomic ions.
POLYATOMIC IONS
Name of Ion
Symbol
Name of Ion
Symbol
Acetate
C2H3O2-, CH3COO-
Hyroxide
OH-
Ammonium
NH4+
Hypochlorite
ClO-
Carbonate
CO32-
Nitrate
NO3-
Chlorate
ClO3-
Nitrite
NO2-
Chlorite
ClO2-
Perchlorate
ClO4-
Chromate
CrO42-
Permanganate
MnO4-
Cyanide
CN-
Phosphate
PO43-
Dichromate
Cr2O72-
Sulfate
SO42-
Hydrogen Carbonate
HCO3-
Sulfite
SO32-
Note: You are expected to be able to use this list to help you determine the
names/symbols of polyatomic ions not given in the list.
Predict the symbol for each of the following polyatomic ions.
Bromate ion
Phosphite ion
BrO3PO33-
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Writing the Formulas and Naming Ternary Ionic
Compounds
Writing the formulas and naming ternary
ionic compounds is just like writing the
formula and naming binary ionic
compounds.
To write the formula, you write the symbol
and charge of the ions involved and then
balance the charges.
To name the compound, you name the ions.
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Naming and Writing Formulas for Ternary Ionic
Compounds
Examples:
a.
K+, NO3-
b.
Ba2+, PO43- Ba3(PO4)2
KNO3
Potassium nitrate
Barium phosphate
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You Try It
1. Write the formulas for the following ternary
ionic compounds, given the ions involved
then name the compounds.
a.
Ca2+, SO42- CaSO4
b.
K+, PO43-
K3PO4
Potassium Phosphate
c.
NH4+, N3-
(NH4)3N
Ammonium nitride
d.
Fe3+, SO42- Fe2(SO4)3 Iron(III) sulfate
Calcium Sulfate
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You Try It
2. Write the formulas for the following
ternary ionic compounds given their
names.
Lithium hypochlorite Li+, ClO-
LiClO
Sodium sulfite
Na+, SO32-
Na2SO3
Calcium acetate
Ca2+, C2H3O2- Ca(C2H3O2)2
Barium phosphate Ba2+, PO43Copper(II) nitrite Cu2+, NO2-
Ba3(PO4)2
Cu(NO2)2
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You Try It
3. Name the following compounds.
a. Ca(NO3)2
Calcium nitrate
b. K2SO4
Potassium sulfate
c. PbSO3
Lead(II) sulfite
d. NaC2H3O2
Sodium Acetate
e. (NH4)2S
Ammonium sulfide
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Daily Starter (12/5 & 12/6)
1. Name the following compounds.
a. LiCl Lithium chloride
b. MgS Magnesium sulfide
c. Cu2O Copper(I) oxide
d. BaCO3 Barium carbonate
e. Fe(NO3)3 Iron(III) nitrate
Daily Starter (12/5 & 12/6)
2.
Write the chemical formula for each of the
following compounds.
a.
Sodium nitride
Na3N
b.
Lithium phosphate
Li3PO4
c.
Tin(IV) carbonate
Sn(CO3)2
d.
Calcium sulfide
CaS
e.
Lead(II) nitrate
Pb(NO3)2
Metallic Bonding
Metals have some characteristics that
distinguish them from nonmetals.
Name some properties of metals.
Good conductors of heat and
electricity
Ductile: Capable of being drawn into
fine wires
Malleable: Capable of being shaped
(hammered) without breaking
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Metallic Bonding and Sea of Electrons
Metals have these properties because
metal atoms form a special type of
bond with each other called a metallic
bond.
In metallic bonding, metal atoms don’t
lose their valence electrons. The
metal atoms release their valence
electrons into a “sea of electrons”
shared by all of the metal atoms.
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Metallic Bonding and Sea of Electrons
The electrons are said to be delocalized
because they are not held in one “locality”
as part of a specific ion or covalent bond.
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Metallic Bonding and Sea of Electrons
Metallic bonding between different
metals results in the formation of
solutions, also called alloys.
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Explaining Metallic Properties - Hardness
The hardness of a metal is determined
by the number of delocalized valence
electrons.
The alkali metals are very soft metals
which can be easily cut by a knife.
This is due to the fact that the alkali
metals only have one valence electron
per atom.
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Explaining Metallic Properties - Luster
The delocalized valence electrons
interact readily with light, creating
the luster of metals.
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Explaining Metallic Properties
Malleability and Ductility
The delocalized valence electrons of a
metal are spread more or less
uniformly throughout the metal.
When a piece of metal is subjected to
pressure, the positive cores of the
atoms slide past each other but are
still held together by the delocalized
sea of electrons.
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Why aren’t ionic compounds malleable?
If an ionic compound is struck with
a hammer, the blow tends to push
ions of like charge together. they
repel, and the crystal shatters.
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Explaining Metallic Properties
Conductivity of Metals
Because the valence electrons of
all metal atoms are not attached to
any one metal atom, they can
move easily through the metal
when an external force, such as
that provided by a battery, is
applied.
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Why aren’t molecular or ionic compounds
good conductors?
In molecular compounds, the valence
electrons are localized in electron pair
bonds between neutral atoms.
In ionic compounds, the electrons are
bound to individual ions that are held in
place in crystal structures.
Since the electrons are not free to move
throughout the solid, ionic and molecular
compounds are not good conductors ofBack to
heat and electricity.
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Naming Bases
Bases are compounds that produce
hydroxide ions (OH-) in water.
Bases are named by naming the
metallic ion and adding the word
hydroxide.
Example: LiOH
Lithium hydroxide
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You Try It
Write names for the following
bases.
a.
b.
c.
d.
NaOH
KOH
Mg(OH)2
CuOH
Sodium hydroxide
Potassium hydroxide
Magnesium hydroxide
Copper(I) hydroxide
An exception is NH3.
This is ammonia.
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Writing Formulas for Bases
Balance the charges as you would
other ionic compounds.
Example: Strontium hydroxide
Sr2+, OHSr(OH)2
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You Try It
Write the formulas for the following
bases.
a. Tin(II) hydroxide
b. Lithium hydroxide
c. Barium hydroxide
d. Tin(IV) hydroxide
Sn2+, OHLi+, OHBa2+, OHSn4+, OH-
Sn(OH)2
LiOH
Ba(OH)2
Sn(OH)4
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Naming Binary Acids (H + Nonmetal)
Acids are compounds that produce
hydrogen ions (H+) in water.
Binary acids contain hydrogen and a
nonmetal – they do not contain
oxygen.
Binary acids are named by using the
prefix hydro, then the root followed by
the ic suffix.
Example: HBr
hydrobromic acid
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You Try It
Write names for the following
binary acids.
a. HCl
b. HI
c. H2S
Hydrochloric acid
Hydroiodic acid
Hydrosulfuric acid
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Writing Formulas for Binary Acids
Balance the charges just as you did
for ionic compounds.
Example: Hydrophosphoric acid
H+, P3H3P
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You Try It
Write the formulas for the following
binary acids.
a. Hydrofluoric acid H+, Fb. Hydroselenic acid H+, Se2-
HF
H2Se
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Naming Oxyacids (H + Polyatomic Ion)
Oxyacids contain polyatomic ions.
The name indicates the number of
oxygen atoms in each molecule
and the nonmetallic element
present.
Suffixes and prefixes are used to
indicate the number of oxygen
atoms present.
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Naming Oxyacids
In order to name oxyacids, it is important to known the
name of the polyatomic ion from which the acid is
formed.
Note: Not all forms of a polyatomic ion are given
on your state formula chart.
Note: The common polyatomic ions for bromine
and iodine, follow the same pattern as chlorine.
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Example – Naming the Acids of Chlorine
Ion
Name of Ion
Formula of
Acid
ClO3-
chlorate
HClO3
chloric acid
ClO2-
chlorite
HClO2
chlorous acid
ClO-
hypochlorite
HClO2
hypochlorous acid
ClO4-
perchlorate
HClO4
perchloric acid
chloride
HCl
Cl-
Name of Acid
hydrochloric acid
(This is a binary acid)
Examples to be Worked Together
a. HNO3 nitric acid (-ate ion)
b. H3PO3 phosphorous acid (-ite
ion)
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You Try It
Name the following acids.
a. H2SO3 sulfurous acid
b. HNO2
nitrous acid
c. H3PO4 phosphoric acid
d. HIO2
Iodous acid
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Writing Formulas for Oxyacids
1. Identify the polyatomic ion
2. Balance the charges just as you did
for ionic compounds.
Example: Carbonic Acid
-ic comes from ate
Carbonate is CO32H+, CO32- H2CO3
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You Try It
Write the formulas for the following
acids.
a. Bromous acid
b. Periodic acid
c. Carbonous acid
d. Acetic Acid
H+, BrO2H+, IO4H+, CO22H+, C2H3O2-
HBrO2
HIO4
H2CO2
HC2H3O2
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