Chemical Bonding
• Why bond anyway?
– Increase Stability
– Decrease Potential Energy… stored energy is
difficult to maintain (batteries expire, food
spoils).
• What is a bond?
– an attractive force between atoms or ions that
binds them together as a unit.
1
Chemical Bonding
• Determining Bond Type
– There are two main bond types ionic and
covalent.
– Ionic bonds can be identified because...
• The first element is a metal (cation)
• The second element is a nonmetal (anion)
• The formula may include a polyatomic ion… look
for formulae that start with a metal and have 3 or
more elements.
– Covalent bonds can be identified because...
• The first element is a nonmetal
• So is the second element; these formulae are
2
Ionic Formulae
• Formula Structure
– Elements present
– Subscripts* (shows how much of each
element)
NaNO3 This is sodium nitrate
*
This
If no subscript is present it means
that there is only one atom of that
element
is
a formula unit of an ionic compound
3
Common Polyatomic Ions
1- charge
2- charge
3- charge
Formula
Name
Formul
a
Name
Formul
a
Name
H2PO4-
Dihydrogen
phosphate
HPO42-
Hydrogen
phosphate
PO33-
Phosphite
C2H3O2-
Acetate
C2O42-
Oxalate
PO43-
Phosphat
e
HSO3-
Hydrogen sulfite
SO32-
Sulfite
BO33-
Borate
HSO4-
Hydrogen sulfate
SO42-
Sulfate
HCO3-
Hydrogen
carbonate
CO32-
Carbonate
NO2-
Nitrite
CrO42-
Chromate
NO3-
Nitrate
Cr2O72-
Dichromate
CN-
Cyanide
SiO32-
Silicate
OH-
Hydroxide
MnO4-
Permanganate
1+ charge
Formul
a
Name4
Ionic Nomenclature
• Naming Rules
– Write the names of both ions, cation first.
– Change the ending of monatomic anions to ide.
• Polyatomic ions have special names that are not to
be altered.
– Stock System: Use Roman numerals to show
the charge of a cation if more than one is
possible.
iron (II)
(II)nitrate
nitrate
• The overall charge must equal zero.
NO3- NO3- → 2- Fe(NO
charge; Fex+)must
therefore have a 2+ charge5
Example:
3 2 becomes
Ionic Nomenclature Practice
• Puzzle pieces – Cations & Anions
– Take the 14 cations and 13 anions provided.
– Come up with as many chemical
combinations as you can (there are 182
possibilities).
– Write the chemical formula and name of each.
• Follow the naming rules and ONLY use one cation
and one anion type at a time.
Example:
Al(NO
AlNO
Al3+ 222+)321+
Aluminum
aluminum nitrite
6
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ FeFeSO
FeF
2
(PO
)
2
Na Fe Fe
Fe(ClO)
4
3FeO
4)22
Fe(NO
FeSO
Fe
FeCl
Fe
FeS
(BO
N
C
Fe
(C
H
O
2
3
3
3
2
2
2
3
322)2 SO 2- Firon
(II)
+
2+ iron
(II)
iron
(II)
3
NH4 Cu iron
iron
(II)
acetate
iron
iron
iron
(II)
(II)
chloride
borate
sulfide
nitride
sulfite
nitrite
iron
(II)
(II)
carbide
oxide
fluoride
2sulfate
hypochlorite
2+
3+ phosphate
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
7
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
Li
LiF
SO
2
2
4
Li
ClO
Na Fe LiLi
C
H
2Li
Li
Li
Li
NO
PO
BO
SO
Cl
O
C
S
N
2
3O
lithium
3
2
2
4
2
3
2433 2
+
2+lithium
SO
F
lithium
3
acetate
phosphate
NH4 Cu lithium
lithium
lithium
lithium
lithium
lithium
chloride
carbide
borate
sulfide
sulfite
nitrite
oxide
nitride
fluoride
sulfate
hypochlorite
22+
3+
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
8
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
Cu
Cu
Cu
PO
C
O
Na Fe
Cu
CuF
SO
CuClO
Cu
CuCl
BO
323SO
4
2S 4
2433
Cu
2
Cu
CuNO
Cu
C
H
N
O
2
+
2+
SO
F
2
3
3
2
2
copper
copper
(I)
(I)carbide
(I)
oxide
copper
(I)
3
copper
copper
copper
(I)
(I)
borate
(I)
NH4 Cu copper
copper
(I)
sulfite
copper
copper
copper
(I)
(I)
(I)
nitrite
nitride
2fluoride
sulfate
2+
3+ phosphate
hypochlorite
chloride
sulfide
SO4
acetate
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
9
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ MgSO
2
MgF
Mg
Mg
Mg(ClO)
Mg
(BO
(PO
Cl
N
)
Na Fe Mg(C
2
4
H
O
)
Mg(NO
Mg
Mg
MgS
3 2SO
32C
233
4)22222
232
MgO
+
2+ magnesium
SO
F
magnesium
magnesium
3
magnesium
NH4 Cu magnesium
oxide
fluoride
sulfate
2phosphate
chloride
nitride
borate
acetate
2+
3+ hypochlorite
carbide
sulfide
nitrite
sulfite
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
10
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ Al(C
2
Al
AlF
(SO
H
O
)
)
Na Fe Al
2
2
3
3
4
2
3
3
Al(NO
Al(ClO)
AlPO
Al
Al
AlN
(SO
C
O2333334))33
2Al
Al
BO
S
2
422Cl
+
2+aluminum
SO
F
aluminum
aluminum
3
aluminum
aluminum
oxide
NH4 Cu aluminum
aluminum
2acetate
fluoride
sulfate
2+
3+ hypochlorite
phosphate
carbide
chloride
nitride
nitrite
sulfite
SO4
sulfide
borate
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
11
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
Na Fe
Na
NaNO
NaClO
Na
NaCl
PO
O
C
2Na
Na
Na
BO
SO
S3O
3SO
2
4
NaC
Na
NaF
H
N
2
3
2
2
4324 2
+
2+sodium
SO
F
2
3
3
sodium
sodium
sodium
sodium
carbide
chloride
oxide
nitrite
NH4 Cu sodium
sodium
sodium
sodium
sulfate
borate
sulfide
sulfite
sodium
fluoride
acetate
nitride
22+
3+ hypochlorite
phosphate
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
12
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
Fe(ClO)
Na Fe Fe(NO
Fe
FeF
(SO
)
FePO
FeBO
Fe
Cl
22(SO
3O
Fe
FeN
O
C
3
434))333)
Fe
Fe(C
H
2
4
3
2
+
2+iron
SO
F
2
3
2
3
2
3
3
iron
(III)
iron
iron
(III)
(III)
3
iron
iron
(III)
(III)
(III)
borate
NH4 Cu iron
iron
iron
iron
(III)
(III)
(III)
carbide
nitride
nitrite
oxide
iron
(III)
iron
(111)
(III)
sulfite
sulfide
2fluoride
sulfate
2+
3+ hypochlorite
phosphate
chloride
SO4
acetate
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
13
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
(NH
(NH
NH
NH
)
NO
ClO
)
F
SO
Cl
C
Na Fe (NH
(NH
PO
N
444))444
23)))SO
4
23
44
2(NH
(NH
(NH
BO
S
4
2
32O
NH
C
H
O
4
4
4
3
2
3
+
2+ ammonium
SO
F
4
2
3
2
ammonium
ammonium
3
ammonium
NH4 Cu ammonium
ammonium
oxide
ammonium
2carbide
fluoride
chloride
sulfate
nitrite
2+
3+ hypochlorite
phosphate
nitride
sulfite
SO4
borate
sulfide
acetate
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
14
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
CuSO
CuF
Cu(ClO)
Na Fe Cu
2
4
CuCl
(PO
2Cu
Cu(NO
Cu
Cu
CuO
(BO
N
C
33CuS
2O
43)))2222)
CuSO
Cu(C
H
3
2
2
+
2+ copper
SO
F
(II)
2
3
2
2
3
3
copper
(II)
NH4 Cu copper
copper
copper
(II)(II)
(II)
(II)
oxide
copper
(II)
copper
2fluoride
sulfate
2+
3+ hypochlorite
phosphate
chloride
SO4
carbide
borate
sulfide
nitride
nitrite
acetate
sulfite
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
15
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
SnF
2
SnSO
2
Sn
Sn(ClO)
(PO
)
Na Fe Sn(C
4
SnO
3(BO
4)2)2
H
O
Sn
Sn(NO
SnSO
Sn
SnCl
Sn
SnS
N
C
)
2
3
22 2 SO 2- Ftin
(II)
3
3
2
2
2
3
+
2+ tin tin
(II)
tinacetate
(II)
3
(II)
oxide
NH4 Cu tin
tin
(II)
tin
tin(II)
(II)
(II)
chloride
borate
sulfide
nitride
carbide
nitrite
sulfite
fluoride
2sulfate
phosphate
2+
3+ hypochlorite
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
16
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
NiF
Ni
NiPO
NiCl
NiN
(SO
)
Na Fe Ni(C
H
O
)
3
Ni
Ni(ClO)
Ni(NO
NiBO
Ni
Ni
(SO
O
C
2
44)2333
33
22 24S
33
2
3323
+
2+nickel
SO
F
nickel
(III)
nickel
(III)
3
nickel
nickel
nickel
(III)(III)
(III)
(III)
(III)
oxide
NH4 Cu nickel
2fluoride
phosphate
chloride
nitride
sulfate
acetate
2+
3+ hypochlorite
sulfide
carbide
borate
sulfite
nitrite
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
17
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
Na Fe
Ag
AgClO
22SO
4
AgC
Ag
Ag
AgNO
Ag
AgCl
Ag
AgF
BO
SO
PO
H
O
N
C
S3O
+
2+ silver
SO
F
3
2
3
2
2
3
4
2
2
3
4
2
3
silver
sulfate
NH4 Cu silver
silver
silver
silver
silver
phosphate
chloride
acetate
carbide
borate
fluoride
sulfide
nitride
sulfite
nitrite
oxide
2+
3+ hypochlorite SO 24
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
18
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
SrF
Na Fe Sr(C
SrSO
2
Sr
Sr(ClO)
Sr(NO
SrSO
SrCl
Sr
(BO
(PO
N
C322O
)222)2
2SrS
H
33SrO
32
2343)2
2
+
2+ strontium
SO
F
strontium
3
strontium
strontium
NH4 Cu strontium
strontium
oxide
2fluoride
sulfate
2+
3+ hypochlorite
phosphate
chloride
carbide
borate
nitride
sulfite
nitrite
SO4
acetate
sulfide
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
19
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ Mo(C
2
)6
Mo(PO
Mo(SO
Mo(BO
Mo(ClO)
Mo
MoCl
MoO
MoN
MoS
Mo(SO
MoF
2H
36O
4
4C
3
263
4
6
2))3262
3
6
Na Fe Mo(NO
molybdenum (VI) SO 2- F+
2+
3
NH4 Cu hypochlorite
acetate
phosphate
chloride
carbide
fluoride
sulfate
sulfide
borate
nitride
sulfite
nitrite
oxide
22+
3+
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
20
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
MoO
Na Fe
3
2FeO
Cu
Ag
Ni
Al
Li
SnO
CuO
SrO
O
O
O
(NH
Fe
Na
MgO
O
)
O
O
2
2
2
3
+
2+
SO
F
2
4
2
2
3
(VI)
3
NH4 Cu molybdenum
copper
nickel
aluminum
strontium
lithium
tin
silver
(II)
(III)
(I)
(II)
oxide
oxide
oxide
oxide
iron
(II)
oxide
ammonium
iron
sodium
magnesium
(III)
oxide
oxide
oxide
2oxide
2+
3+
SO4
oxide
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
21
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
Mo
C
Na Fe
(NH
Ni
Na
Cu
Sr44244C
)C
C
C
6
2Fe
Mg
Cu
Ag
Al
Li
C
C
2
424
2
433C
Sn
C
4
+
2+
SO
F
2
3
sodium
ammonium
nickel
copper
strontium
carbide
(III)
(II) (VI)
NH4 Cu molybdenum
iron
lithium
silver
magnesium
copper
aluminum
(III)
carbide
carbide
carbide
(I)
iron
(II)
tin (II)
carbide
2carbide
2+
3+ carbide
carbide
carbide
SO4
carbide
carbide
Sn Ni carbide
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
22
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
MoCl
SrCl
Al
NH
NiCl
Cl
Cl
2
6
Na Fe
Mg
CuCl
CuCl
Fe
NaCl
Li Cl
Cl
4 3232
2FeCl
SnCl
AgCl
3 (VI)
2
2
molybdenum
strontium
+
2+
SO
F
ammonium
aluminum
nickel
(III)
3
lithium
magnesium
copper
copper
iron
chloride
chloride
(III)
(II)
(I)
NH4 Cu sodium
iron
(II)
chloride
tin
silver
(II)
chloride
chloride
chloride
2chloride
chloride
2+
3+ chloride
chloride
chloride
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
23
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ Fe
2
Mo(PO
Na
Cu
AlPO
PO
)
(PO
)
Sr
Ag
Li
FePO
(PO
PO
PO
)
3
4
4
2
Na Fe Mg
33334(PO
(NH
Sn
CuNiPO
)24222
33)3PO
24444444
molybdenum
copper
aluminum
sodium
(I)
(VI)
+
2+ magnesium
SO
F
lithium
(II)
strontium
iron
silver
(III)
3
copper
nickel
tin
(II)
(III)
(II)
NH4 Cu ammonium
phosphate
phosphate
phosphate
2phosphate
phosphate
2+
3+ phosphate
phosphate
phosphate
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
24
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+
2
MoS
SrS
(NH
Ni
Al
CuS
S
)
S
3
Na Fe Fe
Cu
SnS
MgS
224S
23 )
2FeS
Na
Ag
(SO
S
S
Li
S
2
2
2
3
3
molybdenum
strontium
(VI)
+
2+
SO
F
2
ammonium
copper
nickel
aluminum
(III)
(II)
3
tin
magnesium
(II)
(I)
sulfide
sulfide
NH4 Cu copper
iron
(II)
sulfide
iron
sodium
silver
(III)
sulfide
sulfide
lithium
sulfide
sulfide
sulfide
2sulfide
2+
3+
sulfide
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
25
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Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ Mo(NO )
2
Sr(NO
Ni(NO
CuNO
)
2
6
Na Fe Fe(NO
Mg(NO
Sn(NO
Al(NO
AgNO
Li NO
))))23)3322222
222
2Fe(NO
Cu(NO
NH
NO
22
2
2
NaNO
4
2
molybdenum
(VI)
+
2+ lithium
SO
F
2
copper
nickel
strontium
(III)
(I)
3
magnesium
silver
tin
aluminum
(II)
nitrite
nitrite
NH4 Cu ammonium
iron
(II)
copper
iron
(III)
(II)
nitrite
nitrite
nitrite
sodium
nitrite
nitrite
2nitrite
nitrite
2+
3+
nitrite
nitrite
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
26
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ Mo(SO
2
CuSO
)
Fe
Al
Na
Mg
Cu
SrSO
(SO
)
SO
SO
SO
)
3
3
3
Na Fe (NH
Ni
22(SO
4222 333)3333
2SnSO
33
FeSO
Li
Ag
SO
SO
3
molybdenum
copper
(II)
(VI)
+
2+ ammonium
SO
F
3
2
2
3
magnesium
aluminum
iron
strontium
copper
sodium
(III)
(I)
3
nickel
(III)
NH4 Cu iron
tin
(II)
sulfite
(II)
sulfite
lithium
silver
sulfite
sulfite
2sulfite
sulfite
sulfite
sulfite
2+
3+
sulfite
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
27
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
CuF
SrF
NiF
NH
F
+
3+
MoF
MgF
SnF
FeF
CuF
AlF
3
22
2
6
4
2
FeF
LiF
23
NaF
AgF
Na Fe molybdenum
2
copper
nickel
strontium
(III)
(I)
ammonium
(VI) SO 2- Fmagnesium
copper
aluminum
iron
tin
(II)
(III)
(II)
+
2+sodium
iron
lithium
(II)
fluoride
fluoride
fluoride
3
NH4 Cu silver
fluoride
fluoride
fluoride
fluoride
fluoride
22+
3+
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
28
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2Mo(SO
)
S
NO
Fe
(SO
)
SO
+
3+ (NH
44)))334
MgSO
Al
Cu
CuSO
SnSO
FeSO
Li
SrSO
SO
SO
2(SO
2
Ni
4
2
4
2
2
2
4
4
4
3
Na
Ag
SO
SO
2
4
3
Na Fe molybdenum
22 (III)44(VI)
2iron
ammonium
magnesium
copper
aluminum
strontium
iron
lithium
tin
(II)
(II)
(II)
(I)
nickel
(III)
+
2+sodium
SO
F
sulfate
sulfate
3
sulfate
NH4 Cu silver
sulfate
sulfate
sulfate
sulfate
22+
3+
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
29
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
Mo(ClO)
CuClO
+
3+ Fe(ClO)
2
Ni(ClO)
NH
Fe(ClO)
Sr(ClO)
AgClO
Li 4ClO
ClO3232623
Cu(ClO)
Mg(ClO)
Sn(ClO)
Al(ClO)
NaClO
Na Fe molybdenum
copper
(I) (VI) SO 2- Flithium
nickel
strontium
iron
silver
(III)
(III)
iron
(II)
+
2+ ammonium
magnesium
copper
aluminum
sodium
tin (II)
(II)
3
NH4 Cu hypochlorite
hypochlorite
hypochlorite
hypochlorite
hypochlorite
hypochlorite
hypochlorite SO 22+
3+ hypochlorite
4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
30
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
Mo(BO
Cu
BO
)
+
3+ Cu
2
Mg
Sr
Li
NiBO
(BO
(BO
BO
)
)
3
3
2
(NH
Ag
Al
BO
)
BO
BO
3
3
3
3
3
3
2
2
Na Fe copper
SnNa
FeBO
)33(VI)
4(I)
3 BO
3 borate
3
2Fe
(BO
)
3(BO
3333
2
molybdenum
3
2
3
lithium
magnesium
copper
nickel
strontium
borate
(III)
(II)
+
2+
SO
F
silver
aluminum
borate
borate
3
iron
tin
(II)
(III)
borate
borate
NH4 Cu ammonium
iron
(II)
borate
sodium
borate
borate
borate
borate
borate
2borate
2+
3+
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
31
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
Mg
MoN
NiN
N
+
3+
2
(NH
Cu
Sr
AlN
N
N
)
3
2
22N
Cu
Ag
Sn
Li
N
N
3
3
4
3
2
Na Fe molybdenum
Na
FeN
N22(VI)
333N
2Fe
magnesium
nickel
(III)
3
ammonium
copper
aluminum
strontium
(II)
+
2+
SO
F
lithium
silver
tin (II)
(I)
nitride
nitride
nitride
3
sodium
iron
(III)
nitride
nitride
NH4 Cu copper
ironnitride
(II)
nitride
nitride
nitride
22+
3+
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
32
Go To Next Slide
Ionic Compound Formulae
(Formula Units)
Cation
Anion
2+
2- 4Fe
O
C
+
+
Li Cu
3Cl PO4
2+
3+
Mg Al
2S
NO
+
3+ Sn(C
2
Sr(C
Ni(C
Al(C
Cu
Li
C
C
H
H
H
H
O
O
O
O
)
)
Mo(C
H
O
)
NH
H
O
Na Fe Cu(C
Fe
Fe(C
(C
H
H
O
O
)
Mg(C
H
)
2
2
2
2
2
2
3
3
3
3
3
3
2
2
2
2
2
2
3
2
2
2
22226322
NaC
AgC
4 2222 3333O
2+
2+
SO
F
aluminum
nickel
copper
strontium
copper
lithium
tin
(II)
(III)
(II)
(I)
ammonium
magnesium
iron
ironacetate
(III)
(II) (VI)
3
sodium
silver
acetate
NH4 Cu molybdenum
2acetate
acetate
acetate
acetate
acetate
2+
3+ acetate
SO4
Sn Ni
+
2+
ClO
Ag Sr
3- 36+
BO3 N
Mo
C 2H 3O 2-
33
Go To Next Slide
Ionic Nomenclature
• Getting a formula out of a name
– Write the symbol of both ions, cation first.
– Include known charges of the ions.
• Roman numerals in the Stock system tell the
charge of cations with multiple oxidation states.
• Polyatomic ions don’t have more than one
oxidation state.
– Paying no attention to the signs of the
charges crisscross them as subscripts for the
opposite ions.
• Use parentheses if there is more than one of a
polyatomic ion type.
Fe22+NO
Fe(NO
NO
NO) 11-
Example: iron (II) nitrate becomes
3 233
23
34
Chemical Formulae
• Ionic versus Molecular/Covalent
– Ionic compounds typically feature a metal
(cation) and a nonmetal (anion).
– Molecular compounds are composed of
nonmetals exclusively.
– Both must be electrically neutral in charge.
– Nomenclature (naming) has similarities… the
differences occur because of the law of multiple
proportions.
• The same elements can make multiple, different
35
compounds... Roman numerals or prefixes are used.
Molecular Formulae
• Formula Structure
– Elements present
– Subscripts* (shows how much of each
element)
CO2
This is carbon dioxide
*
If no subscript is present it means
that there is only one atom of that
element
This is a molecule of a molecular compound
36
Molecular Nomenclature
Naming Rules
– Write the names of both elements.
• You will only learn covalent naming for binary
compounds
– Change the ending of the second element to ide.
– Add prefixes to each element to indicate the
subscripted number of atoms present.
• If the first element only has one
atom then
no prefix
carbon
dioxide
oxide
oxygen
is added.
Example: CO2 becomes
37
Molecular Nomenclature
•
Prefixes
- Greek prefixes used…
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
monodi–
tritetrapentahexaheptaoctanonadeca-
- The final “o” or “a” of the prefix is usually dropped
when preceding an element beginning with a vowel.
38
Binary/Ternary Acid
Nomenclature
• Binary Acids are acids made of two
components.
– Hydrogen and,
– A single nonmetal (F, S, Cl, Se, Br, and I)
• Ternary Acids are acids made of two
components.
– Hydrogen and,
– A polyatomic ion
• Acids act as molecular and ionic compounds.
39
• When dissolved in water, acids ionize or, in
Binary Acid Formulae
• Formula Structure
– Elements present (always starts with
hydrogen)
– Subscripts* (shows how much of each
element)
This is hydrochloric acid.
HCl
*
If no subscript is present it means
that there is only one atom of that
element
This is a molecule of a molecular compound
40
Binary Acid Nomenclature
• Naming those featuring a single
nonmetal…
– Write “hydro” immediately followed by the
second element, the nonmetal.
– Change the ending of the second element to ic.
• Had this been a normal molecular formulae the
ending would have been –ide…
• It maybe helpful to think “Change –ide to –ic.”
hydrochlorineacid
hydrochloric
– Write the word “acid”
Example: HCl becomes
41
Ternary Acid Formulae
• Formula Structure
– Elements present (always starts with
hydrogen)
– Subscripts* (shows how much of each
element)
This is nitrous acid.
HNO2
*
If no subscript is present it means
that there is only one atom of that
element
This is a molecule of a molecular compound
42
Binary Acid Nomenclature
• Naming those featuring a polyatomic ion…
– Write the name of the polyatomic ion.
– Change the ending of the polyatomic ion…
• -ate turns to -ic.
• -ite turns to –ous.
“Change –ate to –ic.”
“Change –ite to –ous.”
– Write the word “acid”
nitrous acid
nitrite
Example: HNO2 becomes
43
Binary Acid Formulae
Cl- NO3SO42- FH
H
HCl
HF
PO
S
H
HClO
HNO
HBr
HI
PO
BO
SO
3
2
332
34
344
S2hydrofluoric
hydrochloric
phosphoric
H hydrosulfuric
hydrobromic
chloric
phosphoric
hydroiodic
boric
nitric
sulfuric
acid
acid
3BO
+
3
acid
acid
acid
acid
acid
acid
PO43- IClO3- BrHPO4244
Practice
• Go practice… over and over and over
–
crsciences.com/hw/075_nomenclature__simple_naming_wp.htm
–
crsciences.com/hw/076_nomenclature__names_to_formulas_wp.h
tm
– crsciences.com/hw/077_nomenclature__stock_naming_wp.htm
45