Chapter 5 - Ionic Bonding
4-1
Bonds
• Chemical bond - forces of attraction that hold
atoms together.
• The molecule is more stable than the separate
ions/ atoms.
• Bond energy - the energy required to break (or
form) a chemical bond.
• Energy is released when the bond is formed.
• Ionic bonds - bond formed by the attraction
between oppositely charged particles (anion
and cation)
• The transfer of one or more electrons from one
atom to another
4-2
Ionic Compounds
• Ionic compounds - a chemical
compound that has an equal amount of
positive and negative charges so the
compound is electrically neutral. Formed
by ionic bonds.
• Salt - an inorganic compound containing
cations other than H+ and anions other
than OH- and O2-.
4-3
Properties of Salts
• All salts are made of ions and are held together by
ionic bonds.
• Salts form a crystal lattice - an ordered packing 3dimensional arrangement of atoms or ions in a crystal
• Crystalline versus amorphous- crystalline solids have
a fixed arrangement of atoms while amorphous solids
like talcum powder have haphazard/ random
arrangement.
4-4
Properties of Salts
• Salts do not melt or boil easily because
of the strong attraction between ions
• Salts are hard and brittle
• Salts conduct electricity when melted or
dissolved to form an aqueous solution
(in water- aq.)
4-5
Energy and Ionic Bonding
• Removing an electron from an atom requires
an input of energy- Ionization energy
• Adding an electron to an atom releases
energy- Electron Affinity
• Lattice energy - the energy released when
the crystal lattice of an ionic solid is formed
4-6
Nomenclature
3-
PO4
phosphate ion
HC2H3O2
Acetic Acid
C2H3O2acetate ion
4-7
Forms of Chemical Bonds
Most bonds are
somewhere in
between ionic
and covalent.
• There are 3 forms of bonding
between atoms:
• Ionic—complete transfer of 1
or more electrons from one
atom to another (one loses,
the other gains)
• Covalent—some valence
electrons shared between
atoms
• Metallic – holds atoms of a
metal together. Electrons
form a common pool called
sea of electrons.
4-8
Common Names
• A lot of chemicals have common
names as well as the proper
IUPAC name.
• Chemicals that should always be
named by common name and
never named by the IUPAC
method are:
• H2O water, not dihydrogen
monoxide
• NH3 ammonia, not nitrogen
trihydride
4-9
COMPOUNDS
FORMED
FROM IONS
CATION +
ANION --->
COMPOUND
Na+ + Cl- -->
NaCl
A neutral compound
requires
equal number of +
and - charges.
4-10
Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
Cd+2
4-11
0
Properties of Ionic Compounds
Forming NaCl from Na and Cl2
• A metal atom can
transfer an electron
to a nonmetal.
• The resulting cation
and anion are
attracted to each
other by
electrostatic
forces.
4-12
IONIC COMPOUNDS
NH4
+
Cl
ammonium chloride, NH4Cl
4-13
Some Ionic Compounds
Ca2+ + 2 F- ---> CaF2
Mg2+ + N-3 ---->
Mg3N2
magnesium nitride
Sn4+ + O2- ---->
SnO2
Tin (IV) oxide
4-14
calcium fluoride
Formulas of Ionic Compounds
Formulas of ionic compounds are determined
from the charges on the ions
atoms
ions

Na  +


F : 

sodium + fluorine
Na+
–
: F :  NaF

sodium fluoride
Charge balance:
1+
4-15
1-
formula
= 0
Monatomic Ions
4-16
Writing a Formula
Write the formula for the ionic compound that
will form between Ba2+ and Cl.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the
Ba2+
negative ion
Cl
Cl
3. Write the number of ions needed as
BaCl2
subscripts
4-17
• Writing BINARY FORMULAS
• 1.
CANCEL CHARGES TO GET A TOTAL CHARGE
OF ZERO.
• 2.
CROSS- MULTIPLY TILL YOU GET THE LOWEST
COMMON MULTIPLE.
• 3.
WHAT YOU MULTIPLIED WITH IS YOUR
SUBSCRIPT.
• 4.
DO NOT WRITE CHARGES ON YOUR FINAL
FORMULA.
• 5.
METAL IS WRITTEN FIRST AND THEN NONMETAL.
• SIMPLEST FORMULA IS WRITTEN
4-18
Learning Check
Write the correct formula for the
compounds containing the following ions:
1. Na+, S2a) NaS
b) Na2S
c) NaS2
2. Al3+, Cla) AlCl3
b) AlCl
c) Al3Cl
3. Mg2+, N3a) MgN
b) Mg2N3
c) Mg3N2
4-19
Solution
1. Na+, S2b) Na2S
2. Al3+, Cla) AlCl3
3. Mg2+, N3c) Mg3N2
4-20
Naming Compounds
Binary Ionic Compounds:
• 1. Cation first, then anion
• 2. Monatomic cation = name of the
element
• Ca2+ = calcium ion
• 3. Monatomic anion = root + -ide
• Cl = chloride
• CaCl2 = calcium chloride
4-21
Naming Binary Ionic Compounds

Examples:
NaCl
sodium chloride
ZnI2
zinc iodide
Al2O3
aluminum oxide
4-22
Learning Check
Complete the names of the following binary
compounds:
Na3N
sodium
________________
KBr
potassium ________________
Al2O3
aluminum ________________
MgS
_________________________
4-23
Name the ionic compounds
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
BaCl2
NaF
Ag2O
CuBr
CuBr2
FeO
Fe2O3
MgS
Al2O3
CaI2
11. K2S
12. CrCl2
13. CrCl3
14. CaO
15. Ba3P2
16. Hg2I2
17. Na2O
18. BeS
19. MnO
20. Mn2O3
4-24
Transition Metals
Elements that can have more than one possible
charge MUST have a Roman Numeral to
indicate the charge on the individual ion.
1+ or 2+
Cu+, Cu2+
copper(I) ion
copper (II) ion
2+ or 3+
Fe2+, Fe3+
iron(II) ion
iron(III) ion
4-25
Names of Variable Ions
These elements REQUIRE Roman Numerals
because they can have more than one possible
charge:
anything except Group 1A, 2A, Ag, Zn, Cd, and Al
(You should already know the charges on these!)
Or another way to say it is: Transition metals and the metals in groups 4A and
5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl3
CuCl
SnF4
PbCl2
Fe2S3
(Fe3+)
(Cu+ )
(Sn4+)
(Pb2+)
(Fe3+)
4-26
iron (III) chloride
copper (I) chloride
tin (IV) fluoride
lead (II) chloride
iron (III) sulfide
Examples of Older Names of Cations
formed from Transition Metals
(you do not have to memorize these)
4-27
Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2
iron (_____) bromide
CuCl
copper (_____) chloride
SnO2
___(_____ ) ______________
Fe2O3
________________________
Hg2S
________________________
4-28
Polyatomic
Ions
-
NO3
nitrate ion
NO2nitrite ion
4-29
Polyatomic Ions
You can make additional polyatomic
ions by adding a H+ to the ion!
CO3 -2 is carbonate
HCO3– is hydrogen carbonate
H2PO4– is dihydrogen phosphate
HSO4– is hydrogen sulfate
4-30
Ternary Ionic Nomenclature
Writing Formulas
• Write each ion, cation first. Don’t show
charges in the final formula.
• Overall charge must equal zero.
• If charges cancel, just write symbols.
• If not, use subscripts to balance charges.
• Use parentheses to show more than one
of a particular polyatomic ion.
• Use Roman numerals indicate the ion’s
charge when needed (stock system)
4-31
Ternary Ionic Nomenclature
Sodium Sulfate
Na+ and SO4 -2
Na2SO4
Iron (III) hydroxide
Fe+3 and OHFe(OH)3
Ammonium carbonate
NH4+ and CO3 –2
(NH4)2CO3
4-32
Learning Check
1. aluminum nitrate
a) AlNO3
b) Al(NO)3
c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3
b) Cu(NO3)2
c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH
b) Fe3OH
c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2
4-33
c) Sn4(OH)
Naming Ternary Compounds
 Contains at least 3 elements
 There MUST be at least one polyatomic ion
(it helps to circle the ions)
 Examples:
NaNO3
Sodium nitrate
K2SO4
Potassium sulfate
Al(HCO3)3
Aluminum bicarbonate
or
Aluminum hydrogen carbonate
4-34
Learning Check
Match each set with the correct name:
1.
Na2CO3
a) magnesium sulfite
MgSO3
b) magnesium sulfate
MgSO4
c) sodium carbonate
2.
Ca(HCO3)2
CaCO3
a) calcium carbonate
b) calcium phosphate
Ca3(PO4)2
c) calcium bicarbonate
4-35
Mixed Practice!
Name the following:
1. Na2O
2. CaCO3
3. PbS2
4. Sn3N2
5. Cu3PO4
6. HgF2
4-36
Mixed Up… The Other Way
Write the formula:
1. Copper (II) chlorate
2. Calcium nitride
3. Aluminum carbonate
4. Potassium bromide
5. Barium fluoride
6. Cesium hydroxide
4-37
Naming Molecular
(Covalent) Compounds
CO2 Carbon dioxide
CH4 methane
BCl3
boron trichloride
4-38
All are
formed from
two or more
nonmetals.
Ionic
compounds
generally
involve a metal
and nonmetal
(NaCl)
IONIC BONDING
1. COMPOUNDS
FORMED BY
TRANSFER OF
ELECTRONS
2. FORMED BETWEEN
METALS AND
NONMETALS
3.IONS ARE FORMED
4. NO CONCEPT OF
SINGLE, DOUBLE OR
TRIPLE BOND
5. COMPOUNDS
CONDUCT
ELECTRICITY IN
WATER SOLUTION
6. COMPOUNDS HAVE
HIGHER BOILING
AND MELTING
POINTS DUE TO
NETWORK
4-39
COVALENT BONDING
COMPOUNDS
FORMED BY SHARING
ELECTRONS
FORMED BETWEEN
NONMETALS
NOT FORMED
MOLECULES CAN BE
FORMED BY SHARING
ONE ELECTRON PAIR
(SINGLE BOND), OR
DOUBLE OR TRIPLE
BOND.
COMPOUNDS DO NOT
CONDUCT
ELECTRICITY
LOWER MELTING
AND BOILING POINTS
DUE TO SEPARATE
MOLECULES
Molecular (Covalent) Nomenclature
for two nonmetals
• Prefix System (binary compounds)
1. Less electronegative atom
comes first.
2. Add prefixes to indicate # of atoms. Omit monoprefix on the FIRST element. Mono- is
OPTIONAL on the SECOND element .
3. Change the ending of the
second element to -ide.
4-40
Molecular Nomenclature Prefixes
PREFIX
monoditritetrapentahexaheptaoctanonadeca-
4-41
NUMBER
1
2
3
4
5
6
7
8
9
10
Molecular Nomenclature: Examples
• CCl4
• carbon tetrachloride
• N 2O
• dinitrogen monoxide
• SF6
• sulfur hexafluoride
4-42
More Molecular Examples
• arsenic trichloride
• AsCl3
• dinitrogen pentoxide
• N2O5
• tetraphosphorus decoxide
• P4O10
4-43
Learning Check
Fill in the blanks to complete the following
names of covalent compounds.
CO
carbon ______oxide
CO2
carbon _______________
PCl3
phosphorus _______chloride
CCl4
carbon ________chloride
N2O
_____nitrogen _____oxide
4-44
Learning Check
1.
P2O5
a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2.
Cl2O7
a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3.
Cl2
a) chlorine
b) dichlorine
c) dichloride
4-45
Overall strategy for naming chemical
compounds.
4-46
A flow chart for naming binary compounds.
4-47
Mixed Review
Name the following compounds:
1.
CaO
a) calcium oxide
c) calcium (II) oxide
2.
3.
SnCl4
a) tin tetrachloride
c) tin(IV) chloride
b) calcium(I) oxide
b) tin(II) chloride
N2O3
a) nitrogen oxide
c) nitrogen trioxide
4-48
b) dinitrogen trioxide
Solution
Name the following compounds:
1.
CaO
a) calcium oxide
2.
SnCl4
c) tin(IV) chloride
3.
N2O3
b) Dinitrogen trioxide
4-49
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
Dinitrogen monoxide
Potassium sulfide
Copper (II) nitrate
Dichlorine heptoxide
Chromium (III) sulfate
Iron (III) sulfite
Calcium oxide
Barium carbonate
Iodine monochloride
4-50
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
BaI2
P4S3
Ca(OH)2
FeCO3
Na2Cr2O7
I2O5
Cu(ClO4)2
CS2
B2Cl4
4-51
Acid Nomenclature
• Acids
• Compounds that form H+ in water.
• Formulas usually begin with ‘H’.
• In order to be an acid instead of a gas, binary
acids must be aqueous (dissolved in water)
• Ternary acids are ALL aqueous
• Examples:
• HCl (aq) – hydrochloric acid
• HNO3 – nitric acid
• H2SO4 – sulfuric 4-52
acid
Acid Nomenclature
Anion
Ending
Binary 
Acid Name
-ide
hydro-(stem)-ic acid
-ate
(stem)-ic acid
-ite
(stem)-ous acid
Ternary
An easy way to remember which goes with which…
“In the cafeteria, you ATE something ICky”
4-53
Acid Nomenclature Flowchart
ACIDS
start with 'H'
2 elements
3 elements
hydro- prefix
-ic ending
no hydro- prefix
-ate ending
becomes
-ic ending
4-54
-ite ending
becomes
-ous ending
Acid Nomenclature
• HBr (aq)
• 2 elements, -ide

hydrobromic acid

carbonic acid

sulfurous acid
• H2CO3
• 3 elements, -ate
• H2SO3
• 3 elements, -ite
4-55
Acid Nomenclature
• hydrofluoric acid
 H+ F-
• 2 elements
 HF (aq)
• sulfuric acid
 H+ SO42-  H2SO4
• 3 elements, -ic
• nitrous acid
• 3 elements, -ous
4-56
 H+ NO2-
 HNO2
Name ‘Em!
• HI (aq)
• HCl
• H2SO3
• HNO3
• HIO4
4-57
Write the Formula!
• Hydrobromic acid
• Nitrous acid
• Carbonic acid
• Phosphoric acid
• Hydrotelluric acid
4-58
Nomenclature Summary Flowchart
Now it’s Study Time
DONE
4-60
Rainbow Matrix Game
• Link on Chemistry Geek.com on
Chemistry I page
• http://chemistrygeek.com/rainbow
Use [ ] to represent subscripts since you
can’t enter subscripts into the computer
So H2O would be H[2]O
And Al2(SO4)3 would be Al[2](SO[4])[3]
Additional Polyatomic Ions (you do not have
to memorize these, but they are in the
game!)
Borate = BO3 -3 ; Silicate = SiO4 -4 ;
Manganate = MnO4 -2 (permanganate is -1)
4-61