Chemistry-Ions(2)_150824_01

© Art Traynor 2011
Chemistry
Inorganic Binary Ionic Compounds ( Type II – Polyatomic ) Section 2.8 (Pg. 62)
 Type II IBIC’s are composed of Transition and Post-Transition Metals
Atomic Combinations
Nomenclature Conventions
Compounds in this Equivalency Class share the following characteristics
 The ionic electron cardinality must be specified
Current convention is to use roman numeralsn
Deprecated convention assigned an “ – ous ” suffix to
a lesser electron cardinality ion and an “ – ic ” suffix
to the ion with the greater charge
n
Inorganic Binary Ionic Compounds
( IBIC )
 Unlike Type I IBIC’s , Type II’s are Non-Singular as they can form more
than one variation of ion ( same element , differential electron cardinality )
 Type II IBIC’s only form Cations

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
F-Block
Section 2.8 (Pg. 65)
Atomic Combinations
[Hg2 ]
2+
Inorganic Binary Ionic Compounds ( Type II – Polyatomic )
 Mercury ( I ) ( Mercurous )
Hg
Molecular
Constituent
Element
Group
( Elemental )
G12
Valence
Electron
Configuration
[Xe] 4f145d106s2
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
2 x 2 = 4
=
Σ MCVE’s
q
2
Hg–Hg
Single Bond
( Trial )
Lewis Structure
Molecular Ion
V.E.’s
( MIVE’s )
=
①
Molecular
Ion Bonds = 1
( MIB’s )
〈 2 〉
Hg80
12
6

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
F-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
1 x 2 = 2
=· – MIVE’s
– 2 =
Molecular
Unbound VE’ s
( MUVE’s )
0
= Lewis Structure
( Confirmed )
Octet Divergent MC’s
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s
[Hg2 ]
2+
Hg–Hg①
Molecular
Ion Bonds = 1
( MIB’s )
Hg–Hg
The Bonds fully
subscribe all
available
Molecular VE’s
Formal Charge
Cross-Check
This molecule can only
have a single bond as
there are only 2VE’s
available
Hg80
12
6

© Art Traynor 2011
Chemistry
Atomic Combinations
[Hg2 ]
2+
Hg–Hg
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
Formal Charge Calculation
1
Free Element
VE’s
( FEVE’s )
2
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
1

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
H
N
Molecular
Constituent
Element
Group
( Elemental )
2
G1
G15 (5)
Valence
Electron
Configuration
1s1
[He] 2s22p3
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
1 x 4 = 4
=
5 x 1 = 5
Σ MCVE’s
q
8
H–N–H
––
H
H
Single Bond
( Trial )
Lewis Structure
Molecular Ion
V.E.’s
( MIVE’s )
=
①
②
③
④
Molecular
Ion Bonds = 4
( MIB’s )
[NH4 ]
+
 Ammonium
1
〈 1 〉
H1
①
15
N7

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 8 =
Molecular
Unbound VE’ s
( MUVE’s )
0
= Lewis Structure
( Confirmed )
[NH4 ]
+
 Ammonium
H–N–H
––
H
H
2
①
151
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 0
The Bonds fully
subscribe all
available
Molecular VE’s
Formal Charge
Cross-Check
This molecule can only
have a single bond as
there are only 2VE’s
available
H1
N7

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
[NH4 ]
+
 Ammonium
H–N–H
––
H
H
H–N–H
––
H
H
0
1
2
8
1
· 4 5 4=+ – = 1

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
N
O
Molecular
Constituent
Element
Group
( Elemental )
2
G16 (6)
Valence
Electron
Configuration
[He] 2s22p4
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
5 x 1 = 5
=
6 x 2 = 12
Σ MCVE’s
q
18
( Trial )
Lewis Structure(s)
Molecular Ion
V.E.’s
( MIVE’s )
=
Molecular
Ion Bonds = 3
( MIB’s )
[NO2 ]
–
 Nitrite
= 1
[He] 2s22p3G15 (5) N
O
①
②
③
O
Inspection reveals that a
structure composed of only
single bonds will not work
N
O
①
②
③
O
15
N7 O8
16

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
3 x 2 = 6
=· – MIVE’s
– 18 =
Molecular
Unbound VE’ s
( MUVE’s )
12
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
1 x 6 = 6
1 x 4 = 4
Σ ODMC’s 12
Lewis Structure
( Confirmed )
[NO2 ]
–
 Nitrite
N
O
①
②
③
O
N
O
①
②
③
O
Molecular
Ion Bonds = 3
( MIB’s )
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
N1 x 2 = 2
N
O O
N
O O
●●●●
●●
●●
●●
●●
2
15
N7 O8
16

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
2
1
2
1
2
Shared Pair
Electrons
( SPE’s )
6
1·
5
Free Element
VE’s
( FEVE’s )
5
Formal Charge
VE’s
( FCVE’s )
5
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
6
1
2
2
1
· 7 6 7=+ – = – 1
[NO2 ]
–
 Nitrite
N
O O
N
O O
●●
●●
4
1
2
4
1
· 6 6 6=+ – = 0
N
O O
●●
●●
●●

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
N
O
Molecular
Constituent
Element
Group
( Elemental )
2
G16 (6)
Valence
Electron
Configuration
[He] 2s22p4
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
5 x 1 = 5
=
6 x 3 = 18
Σ MCVE’s
q
24
( Trial )
Lewis Structure(s)
Molecular Ion
V.E.’s
( MIVE’s )
=
Molecular
Ion Bonds = 4
( MIB’s )
[NO3 ]
–
 Nitrate
= 1
[He] 2s22p3G15 (5)
N
O
①
②
③
O
structure composed of only
single bonds will not work
N
O
①
②
③
O
O
–
④
O
–
N
O
①
② ③
O
O
––
④
④
15
N7 O8
16

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
16
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
2 x 6 = 12
1 x 4 = 4
Σ ODMC’s 16
Lewis Structure
( Confirmed )
Molecular
Ion Bonds = 4
( MIB’s )
N
O O
N
O O
O
–
O
–
N
O O
O
––
N
O
①
②
③
O
N
O
①
②
③
O
O
–
④
O
–N
O
①
② ③
O
O
––
④
④
[NO3 ]
–
 Nitrate
2
●● ●●
●●
●●
●●
●●
●●
●●
●●
●●
15
N7 O8
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
16◌◌
◌◌
◌◌
◌◌

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
8
1·
4
Free Element
VE’s
( FEVE’s )
5
Formal Charge
VE’s
( FCVE’s )
4
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
1
4
1
2
4
1
· 6 6 6=+ – = 0
[NO3 ]
–
 Nitrate
N
O O
O
–
N
O O
O
––
●●
●●
●●
N
O O
O
––
6
1
2
2
1· 7 6 7=+ – = – 1

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O
S
Molecular
Constituent
Element
Group
( Elemental )
2
Valence
Electron
Configuration
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
6 x 3 = 18
=
6 x 1 = 6
Σ MCVE’s
q
26
( Trial )
Lewis Structure(s)
Molecular Ion
V.E.’s
( MIVE’s )
=
[SO3 ]
2 –
 Sulfite
= 2
O8
16
G16 (6) [He] 2s22p4
G16 (6) [Ne] 3s23p4
3S16
O–S–O
–
O
① ②
③
Molecular
Ion Bonds = 3
( MIB’s )

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
3 x 2 = 6
=· – MIVE’s
– 26 =
Molecular
Unbound VE’ s
( MUVE’s )
20
= Lewis Structure
( Postulated )
2O8
16
3S16
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
3 x 6 = 18
1 x 2 = 2
Σ ODMC’s 20
O–S–O
–
O
① ②
③
Molecular
Ion Bonds = 3
( MIB’s )
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
[SO3 ]
2 –
 Sulfite
Because our central atom is
a Third Period ( and greater )
element we need to consider
the Formal Charge to more
precisely determine the
molecular structure

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
– 1
2
1
2
6
1
· 5 6 5=+ – = 1
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
[SO3 ]
2 –
 Sulfite
Third Period ( and greater )
elements can violate the
Octet Rule by allocating
additional electrons to their
empty 3d orbitals.

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
2
1
2
8
1
· 6 6 6=+ – = 0
O–S–O
O
●●
●●
●●
●●
●●
●●
●●
O–S–O
O
●●
●●
●●
●●
●●
●●
●●
[SO3 ]
2 –
 Sulfite
empty 3d orbitals.
––––
6
1
2
2
1· 7 7 6=+ – = 1O–S–O
O
●●
●●
●●
●●
●●
●●
●●
––

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 26 =
Molecular
Unbound VE’ s
( MUVE’s )
18
= Resonant Lewis Structure(s)
( Confirmed )
2O8
16
3S16
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O2 x 6 = 12
Σ ODMC’s 18
Molecular
Ion Bonds = 4
( MIB’s )
[SO3 ]
2 –
 Sulfite
O S–O
O
●●
●●
●●
●●
O–S–O
O
●●
●●
●●
●●
●●
●●
●●
––
–
–– O–S O
O
●●
●●
●●
●●
––
–
●●
●●
●●
●●
●●
●●
O–S–O
O
––
O1 x 4 = 4
S1 x 2 = 2

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O
S
Molecular
Constituent
Element
Group
( Elemental )
2
Valence
Electron
Configuration
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
6 x 4 = 24
=
6 x 1 = 6
Σ MCVE’s
q
32
( Trial )
Lewis Structure(s)
Molecular Ion
V.E.’s
( MIVE’s )
=
[SO4 ]
2 –
 Sulfate
= 2
O8
16
G16 (6) [He] 2s22p4
G16 (6) [Ne] 3s23p4
3S16
O–S–O
–
O
①
②
③
Molecular
Ion Bonds = 4
( MIB’s )
–
O
④

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
24
= Lewis Structure
( Postulated )
2O8
16
3S16
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 24
Molecular
Ion Bonds = 4
( MIB’s )
molecular structure
[SO4 ]
2 –
 Sulfate
O–S–O
–
O
①
②
③
–
O
④
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
O4 x 6 = 24
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
–
O
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
– 1
0
1
2
8
1
· 4 6 4=+ – = 2
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
empty 3d orbitals.
[SO4 ]
2 –
 Sulfate
–
O
●●
●●
●●
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
–
O
●●
●●
●●
The – 1 Formal Charge Value for a Single Oxygen
Bond May be improved by an equivalent structure
featuring one or more Double Oxygen Bonds...
The +2 Formal Charge Value for all
Single Sulfur Bonds May be improved
by an equivalent structure featuring one
or more Double Sulfur Bonds...

© Art Traynor 2011
Chemistry
Atomic Combinations
Formal Charge Comparison Table – Trial Lewis Structures
O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●All Single Bonds One Double Bond
All Else Single Bonds
Trial
Lewis
Structures
Sulfur
Fc ( S ) =S 2
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
Two Double Bonds
O–S–O–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
[SO4 ]
2 –
 Sulfate●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
10
1· 5 6 5=+ – = 1
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
empty 3d orbitals.
[SO4 ]
2 –
 Sulfate
O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
O
––
O
––
The 0 FC value for one double-bond Oxygen MC
represents an improvement over the – 1 FC
obtained for an equivalent single-bond Oxygen MC.
The 1 FC value for a one Sulfur double-bond
suggests further improvement can be
obtained by the introduction of a second
Sulfur double-bond

© Art Traynor 2011
Chemistry
Atomic Combinations
O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Trial
Lewis
Structures
Sulfur
Fc ( S ) =S 2
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
Two Double Bonds
O–S–O–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
[SO4 ]
2 –
 Sulfate●●
●●
=S 2
=O – 1
=O 0

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
12
1· 6 6 6=+ – = 0
O–S–O
O
●●
●●
●●
●●
●●
●●
empty 3d orbitals.
[SO4 ]
2 –
 Sulfate
O–S–O
O
●●
●●
●●
●●
●●
●●
O
––
O
––
At 0 FC, the optimized bond configuration
structure for Oxygen in the Ionic Molecule
has been determined.
The introduction of a second Sulfur double-bond
further improves the Molecular Ionic FC…any
further introduction of Sulfur double bonds
degrades the FC (e.g. – 1 for 3, and – 2
for 4 double Sulfur bonds )
––––

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s =· – MIVE’s
Molecular
Unbound VE’ s
( MUVE’s )
= Resonant Lewis Structure(s)
( Confirmed )
2O8
16
3S16
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 24
Molecular
Ion Bonds = 6
( MIB’s )
①
② ③
④
O4 x 6 = 24
4 x 2 = 8 – 32 = 24
[SO4 ]
2 –
 Sulfate
O–S–O
O
●●
●●
●●
●●
●●
●●
––
O
––
O S O
O
●●
●●
●●
●●
●●
●●
O
––
––––
O–S–O
O
––
O
––
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
⑤⑥

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
S16
O8
H
O
S
Molecular
Constituent
Element
Group
( Elemental )
3
2
16
G1
G16 (6)
G16 (6)
Valence
Electron
Configuration
1s1
[He] 2s22p4
[Ne] 3s23p4
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
1 x 1 = 1
=
6 x 4 = 24
6 x 1 = 6
Σ MCVE’s
q = 1
32
Sub-Group
( Molecular )
H–O
[ OH ]
–
Hydroxide
H–O–S–O
––
O
O
Single Bond
( Trial )
Lewis Skeleton
Molecular Ion
V.E.’s
( MIVE’s )
=
① ②
③
④
⑤
Molecular
Ion Bonds = 5
( MIB’s )
[HSO ]
–
 Hydrogen Sulfate ( Bisulfate )
4
1 H1
①

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
[HSO ]
–
S16
O8
4
MIB’s Single Bond
Electrons
3
2
16
MIB-VE’s
5 x 2 = 10
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
22
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
3 x 6 = 18
1 x 4 = 4
Σ ODMC’s 22
Lewis Structure
( Postulated )
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
1 H1
①
Because our central atom is a
molecular structure
H–O–S–O
––
O
O
① ②
③
④
⑤
Molecular
Ion Bonds = 5
( MIB’s )
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
Molecular
Ion Bonds = 5
( MIB’s )

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
8
1
· 4 6 4=+ – = 2
[HSO ]
–
4
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
–1
4
1
2
4
1
· 6 6 6=+ – = 0
[HSO ]
–
4
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
[HSO ]
–
4
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
All Single Bonds One Double Bond
Trial
Lewis
Structures
Hydrogen
Fc ( H ) =H 0
Sulfur
Fc ( S ) =S 2
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
Two Double Bonds
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
[HSO ]
–
S16
O8
4
MIB’s Single Bond
Electrons
3
2
16
MIB-VE’s
6 x 2 = 12
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
20
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
2 x 6 = 12
2 x 4 = 8
Σ ODMC’s 20
Lewis Structure
( Postulated )
1 H1
①
molecular structure
H–O–S–O
–
O
O
① ②
③ ④
⑤
Molecular
Ion Bonds = 6
( MIB’s )
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
Molecular
Ion Bonds = 6
( MIB’s )
––
⑥

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
10
1
· 5 6 5=+ – = 1
[HSO ]
–
4
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
–1
4
1
2
4
1
· 6 6 6=+ – = 0
[HSO ]
–
4
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O

© Art Traynor 2011
Chemistry
Atomic Combinations
[HSO ]
–
4
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
Trial
Lewis
Structures
Hydrogen
Fc ( H ) =H 0
Sulfur
Fc ( S ) =S 2
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
=H 0
=S 1
=O 0
Two Double Bonds
H–O–S–O
O
●●
●●
●●
●●
●●
––
O
––
=O – 1

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
[HSO ]
–
S16
O8
4
MIB’s Single Bond
Electrons
3
2
16
MIB-VE’s
7 x 2 = 14
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
18
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
1 x 6 = 6
3 x 4 = 12
Σ ODMC’s 18
Lewis Structure
( Postulated )
1 H1
①
molecular structure
H–O–S–O
O
O
① ②
③ ④
⑤
Molecular
Ion Bonds = 7
( MIB’s )
◌◌
◌◌
◌◌
◌◌
◌◌ Molecular
Ion Bonds = 6
( MIB’s )
––
⑥⑦
–– H–O–S–O
O
●●
●●
●●
●●
●●
––
O
––

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
12
1
· 6 6 6=+ – = 0
[HSO ]
–
4
H–O–S–O
O
●●
●●
●●
●●
●●
––
O
––
H–O–S–O
O
●●
●●
●●
●●
●●
––
O
––

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
–1
4
1
2
4
1
· 6 6 6=+ – = 0
[HSO ]
–
4
H–O–S–O
O
●●
●●
●●
●●
●●
––
O
––
H–O–S–O
O
●●
●●
●●
●●
●●
––
O
––

© Art Traynor 2011
Chemistry
Atomic Combinations
[HSO ]
–
4
H–O–S–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H– O–S–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
Trial
Lewis
Structures
Hydrogen
Fc ( H ) =H 0
Sulfur
Fc ( S ) =S 2
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
=H 0
=S 1
=O 0
Two Double Bonds
H–O–S–O
O
●●
●●
●●
●●
●●
––
O
––
=H 0
=S 0
=O 0
=O – 1 =O – 1

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
H
O
Molecular
Constituent
Element
Group
( Elemental )
2
G1
G16 (6)
Valence
Electron
Configuration
1s1
[He] 2s22p4
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
1 x 1 = 1
=
6 x 1 = 6
Σ MCVE’s
q
8
Single Bond
( Trial )
Lewis Structure
Molecular Ion
V.E.’s
( MIVE’s )
=
O–H①
Molecular
Ion Bonds = 1
( MIB’s )
[OH ]
–
 Hydroxide
1 H1
①
= 1
O8
16

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
1 x 2 = 2
=· – MIVE’s
– 8 =
Molecular
Unbound VE’ s
( MUVE’s )
6
=
2O8
16
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O1 x 6 = 6
Σ ODMC’s 6
Molecular
Ion Bonds = 4
( MIB’s )
O–H①
Lewis Structure
( Postulated )
Second Period central
element must follow Octet
Rule ( as no additional 3d
orbitals are available ).
1 H1
①
O–H①
◌◌
◌◌
◌◌
[OH ]
–
 Hydroxide
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
6
1
2
2
1
· 7 6 7=+ – = – 1
O–H
●●
●●
●●
The 0 Formal Charge Value for a Single Hydrogen
Bond indicates that a single bond configuration is
the most reflective of the actual bond in this ion
The – 1 Formal Charge Value for the
single Oxygen bond may indicate that a
more favorable configuration can be
attained by the formation of a double
bond ( but the S1 orbital for H is full )
[OH ]
–
 Hydroxide Second Period central
O–H
●●
●●
●●

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
C
N
Molecular
Constituent
Element
Group
( Elemental )
2
G16 (5)
Valence
Electron
Configuration
[He] 2s22p3
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
4 x 1 = 4
=
5 x 1 = 5
Σ MCVE’s
q
10
( Trial )
Lewis Structure(s)
Molecular Ion
V.E.’s
( MIVE’s )
=
Molecular
Ion Bonds
[CN]
–
 Cyanide
= 1
[He] 2s22p2G15 (4)
15
N7
14
C6
C–N
①
C N–– –––
② ③
C N
3 ( MIB’s )2 ( MIB’s )1 ( MIB )

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
3 x 2 = 6
=· – MIVE’s
– 10 =
Molecular
Unbound VE’ s
( MUVE’s )
4
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
C1 x 2 = 2
Σ ODMC’s 4
Lewis Structure
( Postulated )
[CN]
–
 Cyanide
2
15
N7
14
C6Molecular
Ion Bonds
C–N
①
C N–– –––
② ③
C N
3 ( MIB’s )2 ( MIB’s )1 ( MIB )
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
–––
③
C N
●●
●●
No! No! Yes!
Molecular
Ion Bonds = 3
( MIB’s )
N1 x 2 = 2

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
2
1
2
1
2
Shared Pair
Electrons
( SPE’s )
6
1·
5
Free Element
VE’s
( FEVE’s )
4
Formal Charge
VE’s
( FCVE’s )
5
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
– 1
2
1
2
6
1
· 5 5 5=+ – = 0
[CN]
–
 Cyanide
–––
③
C N
●●
●●
–––
③
C N
●●
●●

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O
P
Molecular
Constituent
Element
Group
( Elemental )
2
G15 (5)
Valence
Electron
Configuration
[He] 2s22p3
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
6 x 4 = 24
=
5 x 1 = 5
Σ MCVE’s
q
32
( Trial )
Lewis Structure(s)
Molecular Ion
V.E.’s
( MIVE’s )
=
[PO4 ]
3 –
 Phosphate
= 3
[He] 2s22p4G16 (6)
O8
16
3P15
15
O–P–O
–
O
①
②
③
Molecular
Ion Bonds = 4
( MIB’s )
–
O
④

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
24
= Lewis Structure
( Postulated )
2O8
16
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 24
Molecular
Ion Bonds = 4
( MIB’s )
molecular structure
O–P–O
–
O
①
②
③
–
O
④
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
O4 x 6 = 24
O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
–
O
●●
●●
●●
[PO4 ]
3 –
 Phosphate
3P15
15

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
– 1
0
1
2
8
1
· 4 5 4=+ – = 1
O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
empty 3d orbitals.
–
O
●●
●●
●●
O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
–
O
●●
●●
●●
The +1 Formal Charge Value for all
Single Phosphorous Bonds May be
improved by an equivalent structure
featuring one or more Double
Phosphorous Bonds...
[PO4 ]
3 –
 Phosphate

© Art Traynor 2011
Chemistry
Atomic Combinations
O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Trial
Lewis
Structures
Phosphorus
Fc ( P ) =P 1
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
Two Double Bonds
O–P–O–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O●●
●●
[PO4 ]
3 –
 Phosphate

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
5 x 2 = 10
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
22
= Lewis Structure
( Postulated )
2O8
16
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 22
O3 x 6 = 18
[PO4 ]
3 –
 Phosphate
3P15
15
O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
O
––
Molecular
Ion Bonds = 5
( MIB’s )
①
② ③
④
O–S–O
O
––
O
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
⑤
–◌◌
◌◌
◌◌
O1 x 4 = 4

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
empty 3d orbitals.
––
O
The 0 FC value for one double-bond Oxygen MC
represents an improvement over the – 1 FC
obtained for an equivalent single-bond Oxygen MC.
[PO4 ]
3 –
 Phosphate
6
1
2
2
1· 7 6 7=+ – = – 1
O–P–O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
–––
O

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
1
2
Shared Pair
Electrons
( SPE’s )
Free Element
VE’s
( FEVE’s )
Formal Charge
VE’s
( FCVE’s )
FCVE’s
=+ – =
Formal
Charge
( FC )
0
1
2
10
1
· 5 5 5=+ – = 0
empty 3d orbitals.
O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
O
––
The 0 FC value for a one Phosphorous
double-bond represents a further
improvement over the + 1 FC obtained for
an equivalent single-bond Phosphorous MC.
[PO4 ]
3 –
 Phosphate

© Art Traynor 2011
Chemistry
Atomic Combinations
O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Trial
Lewis
Structures
Phosphorus
Fc ( P ) =P 1
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
Two Double Bonds
O–P–O–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O●●
●●
=P 0
=O – 1
=O 0
[PO4 ]
3 –
 Phosphate
Inspection suggests that
no further improvement
can be made in the FC of
the molecular ensemble
by introduction of any
additional compound
bonds
Added Compound Bonds
Will Turn FC Negative

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O8
H
O
P
Molecular
Constituent
Element
Group
( Elemental )
3
2
16
G1
G16 (6)
G15 (5)
Valence
Electron
Configuration
1s1
[He] 2s22p4
[Ne] 3s23p3
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
1 x 1 = 1
=
6 x 4 = 24
5 x 1 = 5
Σ MCVE’s
q = 2
32
Sub-Group
( Molecular )
H–O
[ OH ]
–
Hydroxide
H–O–P–O
––
O
O
Molecular Ion
V.E.’s
( MIVE’s )
=
① ②
③
④
⑤
Molecular
Ion Bonds = 5
( MIB’s )
1 H1
①
[HPO4 ]
2 –
 Hydrogen Phosphate
3P15
15
Single Bond
( Trial )
Lewis Skeleton

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O8
MIB’s Single Bond
Electrons
3
2
16
MIB-VE’s
5 x 2 = 10
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
22
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
3 x 6 = 18
1 x 4 = 4
Σ ODMC’s 22
Lewis Structure
( Postulated )
H–O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
1 H1
①
molecular structure
H–O–P–O
––
O
O
① ②
③
④
⑤
Molecular
Ion Bonds = 5
( MIB’s )
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
[HPO4 ]
2 –
P15
15

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
8
1
· 4 5 4=+ – = 1
H–O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H–O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
[HPO4 ]
2 –

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
–1
4
1
2
4
1
· 6 6 6=+ – = 0
H–O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H–O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
[HPO4 ]
2 –

© Art Traynor 2011
Chemistry
Atomic Combinations
H–O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Trial
Lewis
Structures
Hydrogen
Fc ( H ) =H 0
Phosphorous
Fc ( S ) =P 1
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
Two Double Bonds
H– O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
[HPO4 ]
2 –

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
S16
O8
MIB’s Single Bond
Electrons
3
2
16
MIB-VE’s
6 x 2 = 12
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
20
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
2 x 6 = 12
2 x 4 = 8
Σ ODMC’s 20
Lewis Structure
( Postulated )
1 H1
①
molecular structure
H–O–P–O
–
O
O
① ②
③ ④
⑤
Molecular
Ion Bonds = 6
( MIB’s )
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
H– O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
Molecular
Ion Bonds = 6
( MIB’s )
––
⑥
[HPO4 ]
2 –

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
10
1
· 5 5 5=+ – = 0
H– O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
H– O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
[HPO4 ]
2 –

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
–1
4
1
2
4
1
· 6 6 6=+ – = 0
H– O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
H– O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
[HPO4 ]
2 –

© Art Traynor 2011
Chemistry
Atomic Combinations
H–O–P–O
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Trial
Lewis
Structures
Hydrogen
Fc ( H ) =H 0
Phosphorous
Fc ( S ) =P 1
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
Two Double Bonds
H– O–P–O
–
O
●●
●●
●●
●●
●●
●●
●●
●●
––
O
=H 0
=P 0
=O – 1
=O 0
additional compound
bonds
[HPO4 ]
2 –

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O8
H
O
P
Molecular
Constituent
Element
Group
( Elemental )
3
2
16
G1
G16 (6)
G15 (5)
Valence
Electron
Configuration
1s1
[He] 2s22p4
[Ne] 3s23p3
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
1 x 2 = 2
=
6 x 4 = 24
5 x 1 = 5
Σ MCVE’s
q = 1
32
Sub-Group
( Molecular )
H–O
[ OH ]
–
Hydroxide
H–O–P–O–H
––
O
O
Molecular Ion
V.E.’s
( MIVE’s )
=
① ②
③
④ ⑤
Molecular
Ion Bonds = 6
( MIB’s )
1 H1
①
[H2 PO4 ]
–
 Dihydrogen Phosphate
3P15
15
Single Bond
( Trial )
Lewis Skeleton
⑥

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O8
MIB’s Single Bond
Electrons
3
2
16
MIB-VE’s
6 x 2 = 12
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
20
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
2 x 6 = 12
2 x 4 = 8
Σ ODMC’s 20
Lewis Structure
( Postulated )
H–O–P–O–H
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
1 H1
①
molecular structure
H–O–P–O–H
––
O
O
① ②
③
④ ⑤
Molecular
Ion Bonds = 6
( MIB’s )
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
P15
15
[H2 PO4 ]
–
⑥

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
8
1
· 4 5 4=+ – = 1
H–O–P–O–H
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H–O–P–O–H
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
[H2 PO4 ]
–

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
–1
4
1
2
4
1
· 6 6 6=+ – = 0
H–O–P–O–H
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
H–O–P–O–H
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
[H2 PO4 ]
–

© Art Traynor 2011
Chemistry
Atomic Combinations
H–O–P–O–H
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Trial
Lewis
Structures
Hydrogen
Fc ( H ) =H 0
Phosphorous
Fc ( S ) =P 1
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
Two Double Bonds
H– O–P–O–H
–O
●●
●●
●●
●●
●●
●●
●●
––
O
[H2 PO4 ]
–

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
10
1
· 5 5 5=+ – = 0
H– O–P–O–H
–
O
●●
●●
●●
●●
●●
●●
●●
––
O
H– O–P–O–H
–
O
●●
●●
●●
●●
●●
●●
●●
––
O
[H2 PO4 ]
–

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1
· 7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
–1
4
1
2
4
1
· 6 6 6=+ – = 0
H– O–P–O–H
–
O
●●
●●
●●
●●
●●
●●
●●
––
O
H– O–P–O–H
–
O
●●
●●
●●
●●
●●
●●
●●
––
O
[H2 PO4 ]
–

© Art Traynor 2011
Chemistry
Atomic Combinations
H–O–P–O–H
––
O
O
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Trial
Lewis
Structures
Hydrogen
Fc ( H ) =H 0
Phosphorous
Fc ( S ) =P 1
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
Two Double Bonds
H– O–P–O–H
–O
●●
●●
●●
●●
●●
●●
●●
––
O
[H2 PO4 ]
–
=H 0
=P 0
=O – 1
=O 0
additional compound
bonds

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
[SCN]
–
 Thiocyanate
C
N
S
Molecular
Constituent
Element
Group
( Elemental )
3
2
16
Valence
Electron
Configuration
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
4 x 1 = 4
=
5 x 1 = 5
6 x 1 = 6
Σ MCVE’s
q = 1
16
Sub-Group
( Molecular )
C–N
[ CN ]
–
Cyanide
Molecular Ion
V.E.’s
( MIVE’s )
=
3
15
Single Bond
( Trial )
Lewis Skeleton
N7
14
C6
S16
[He] 2s22p2G15 (4)
G16 (5) [He] 2s22p3
G16 (6) [Ne] 3s23p4
S–C–N① ②
Molecular
Ion Bonds = 2
( MIB’s )

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
2 x 2 = 4
=· – MIVE’s
– 16 =
Molecular
Unbound VE’ s
( MUVE’s )
12
= Lewis Structure
( Postulated )
OD7
OD6
OD5
OD4
OD3
OD2
OD1
N
C
1 x 6 = 6
0 x 4 = 0
Σ ODMC’s 12
S–C–N① ②
Molecular
Ion Bonds = 2
( MIB’s )
S–C–N
●●
●●
●●
●●
●●
●●
●●
Because one of our MC
atoms is a Third Period ( and
greater ) element we need to
consider the Formal Charge
to more precisely determine
the molecular structure
[SCN]
–
 Thiocyanate
●●
S1 x 6 = 6
Lewis Structure featuring
only single bonds is not
descriptive as at least one of
the MC’s will be Octet
deficient by four electrons
3
2
16
3
15
N7
14
C6
S16
◌◌ ◌◌
◌◌
◌◌
◌◌
◌◌
◌◌
◌◌

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
3 x 2 = 6
=· – MIVE’s
– 16 =
Molecular
Unbound VE’ s
( MUVE’s )
10
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
S1 x 4 = 4
Σ ODMC’s 10
Molecular
Ion Bonds = 3
( MIB’s )
S C–N––
N1 x 6 = 6
C0 x 2 = 0
Lewis Structure
( Postulated )
[SCN]
–
 Thiocyanate
Molecular
Ion Bonds = 3
( MIB’s )
3
2
16
3
15
N7
14
C6
S16
S C–N––
Lewis Structure featuring a
single Compound bond is not
deficient by four electrons
◌◌ ◌◌
◌◌
◌◌
●●
●●
●●
●●
①
②
③

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 16 =
Molecular
Unbound VE’ s
( MUVE’s )
8
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
S1 x 4 = 4
Σ ODMC’s 8
S C N––
N1 x 4 = 4
Lewis Structure
( Postulated )
[SCN]
–
 Thiocyanate
Molecular
Ion Bonds = 4
( MIB’s )
3
2
16
3
15
N7
14
C6
S16
––
S C N–– ––①
②
③
④

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
8
1
· 4 4 4=+ – = 0
4
1
2
4
1· 6 5 6=+ – = –1
[SCN]
–
 Thiocyanate
S C N–– ––
S C N–– ––
S C N–– ––

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
Two Double Bonds
[SCN]
–
 Thiocyanate
S–C–N
●●
●●
●●
●●
●●
●●
●●
●●
S C–N––
●●
●●
●●
●●
S C N–– ––
Carbon
Fc ( C ) =C 0
Nitrogen
Fc ( N ) =N – 1
Sulfur
Fc ( S ) =S 0
Invalid Configuration
- at least one of the
MC’s will be Octet
deficient by 4
electrons
deficient by 2
electrons
One Triple Bond

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 16 =
Molecular
Unbound VE’ s
( MUVE’s )
8
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 8
Lewis Structures
( Postulated )
[SCN]
–
 Thiocyanate
3
2
16
3
15
N7
14
C6
S16
–––S – C N
–––S – C N
●●
① ②③
④
◌◌
◌◌
◌◌
◌◌
S1 x 6 = 6
N1 x 2 = 2
–––S C – N
●●
●●
●●
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
– 1
0
1
2
8
1
· 4 4 4=+ – = 0
2
1
2
6
1· 5 5 5=+ – = 0
[SCN]
–
 Thiocyanate
–––S – C N
●●
●●
●●
●●
–––S – C N
●●
●●
●●
●●
–––S – C N
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
Two Double Bonds
[SCN]
–
 Thiocyanate
S–C–N
●●
●●
●●
●●
●●
●●
●●
●●
S C–N––
●●
●●
●●
●●
S C N–– ––
Carbon
Fc ( C ) =C 0
Nitrogen
Fc ( N ) =N – 1
Sulfur
Fc ( S ) =S 0
deficient by 4
electrons
deficient by 2
electrons
One Triple Bond
–––S – C N
●●
●●
●●
●●
=C 0
=N 0
=S – 1

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
C
O
Molecular
Constituent
Element
Group
( Elemental )
2
G16 (6)
Valence
Electron
Configuration
[He] 2s22p4
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
4 x 1 = 4
=
6 x 3 = 18
Σ MCVE’s
q
24
Molecular Ion
V.E.’s
( MIVE’s )
=
= 2
[He] 2s22p2G14 (4)
O8
16
[CO3 ]
2 –
 Carbonate
14
C6
Molecular
Ion Bonds = 3
( MIB’s )
C
O
①
②
③
O
O
–
Single Bond
( Trial )
Lewis Skeleton

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
3 x 2 = 6
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
18
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
C
3 x 6 = 18
1 x 2 = 2
Σ ODMC’s 20
Molecular
Ion Bonds = 3
( MIB’s )
2O8
16
[CO3 ]
2 –
 Carbonate
Molecular
Ion Bonds = 3
( MIB’s )
C
O
①
②
③
O
O
–
Single Bond
( Trial )
Lewis Skeleton
C
O
①
②
③
O
O
–◌◌
◌◌
◌◌◌◌
◌ ◌
◌◌
◌◌
◌◌
◌◌
Period Two elements
must follow the Octet Rule
◌◌
●●
●●
●●
●●
Lewis Structure featuring all
single bonds is not
deficient by two electrons
14
C6

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
12 x 2 = 24
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
0
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 0
Molecular
Ion Bonds = 12
( MIB’s )
2O8
16
[CO3 ]
2 –
 Carbonate
Molecular
Ion Bonds = 12
( MIB’s )
C
O ①
②
③
O
O
Double Bond
( Trial )
Lewis Skeleton
Period Two elements
double bonds is not
descriptive as Carbon (P2
Element) is incapable of
accommodating more than
eight electrons
––
⑥
④
⑤
C
O ①
②
③
O
O
––
⑥
④
⑤
14
C6

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
16
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
2 x 6 = 12
1 x 4 = 4
Σ ODMC’s 16
Molecular
Ion Bonds = 4
( MIB’s )
2O8
16
[CO3 ]
2 –
 Carbonate
Molecular
Ion Bonds = 4
( MIB’s )
Period Two elements
Lewis Structure featuring at
least one double bond and all
else single bonds is
descriptive as all Period Two
MC’s satisfy the Octet rule
C
O
①
② ③
O
O
––
④
C
O
①
② ③
O
O
––
④
Lewis Structure
( Postulated )
14
C6

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
8
1·
4
Free Element
VE’s
( FEVE’s )
4
Formal Charge
VE’s
( FCVE’s )
4
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
4
1
2
4
1
· 6 6 6=+ – = 0
6
1
2
2
1· 7 6 7=+ – = – 1
[CO3 ]
2 –
 Carbonate
C
O O
O
––
C
O O
O
––
C
O O
O
––

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
16
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
O
2 x 6 = 12
1 x 4 = 4
Σ ODMC’s 16
Molecular
Ion Bonds = 4
( MIB’s )
2O8
16
[CO3 ]
2 –
 Carbonate
Molecular Ion Bonds = 4 ( MIB’s )
The singular double bond can
exist as between any of the
Oxygen MC’s such that three
equivalent resonant Lewis
Structures are descriptive of
the Carbonate Ion
C
O
①
② ③
O
O
––
④
Resonant Lewis Structures
( Confirmed )
C
O ①
②
③
O
O
–
④
C
O
①
② ③
O
O
––
④
C
O
①
②
③
O
O
–
④
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
14
C6

© Art Traynor 2011
Chemistry
Atomic Combinations
All Single Bonds All Double Bonds
Trial
Lewis
Structures
One Double Bonds
Carbon
Fc ( C ) =C 0
– at least one of the
deficient by 2
electrons
– Carbon ( P2
Element) cannot
accommodate Octet
surplus electrons
[CO3 ]
2 –
 Carbonate
C
O
①
②
③
O
O
–
●●
●●
●●
●●
C
O ①
②
③
O
O
––
⑥
④
⑤
C
O
①
② ③
O
O
––
④
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O8
H
C
O
Molecular
Constituent
Element
Group
( Elemental )
2
16
G1
G14 (4)
G16 (6)
Valence
Electron
Configuration
1s1
[He] 2s22p2
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
1 x 1 = 1
=
4 x 1 = 4
Σ MCVE’s
q = 1
24
Sub-Group
( Molecular )
O–H
[ OH ]
–
Hydroxide
Molecular Ion
V.E.’s
( MIVE’s )
=
Molecular Ion Bonds = 4
( MIB’s )
1 H1
①
[HCO3 ]
–
 Hydrogen Carbonate ( Bicarbonate )
Single Bond
( Trial )
Lewis Skeleton
[He] 2s22p4 6 x 3 = 18
C
O
①
②
③
O
O
–
H④
14
C6

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
16
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O
C
2 x 6 = 12
1 x 2 = 2
Σ ODMC’s 18
Molecular
Ion Bonds = 4
( MIB’s )
2O8
16
Molecular
Ion Bonds = 4
( MIB’s )
C
O
①
②
③
O
O
–
All Single Bond
( Trial )
Lewis Skeleton
Period Two elements
●●
●●
●●
●●
14
C6
[HCO3 ]
–
H④
single bonds is not
deficient by two electrons
O1 x 4 = 4
C
O
①
②
③
O
O
–◌◌
◌◌
◌◌
◌◌
H④
1 H1
①

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
7 x 2 = 14
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
10
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 10
Molecular
Ion Bonds = 7
( MIB’s )
2O8
16
Molecular
Ion Bonds = 7
( MIB’s )
All Central Atom
Double Bonds
( Trial ) Lewis Skeleton
Period Two elements
14
C6
[HCO3 ]
–
H
central atom double bonds is
not descriptive as Carbon
(P2 Element) is incapable of
accommodating more than
eight electrons
C
O ①
②
③
O
O
––
⑥
④
⑤
HC
O ①
②
③
O
O
––
⑥
④
⑤
⑦
⑦
1 H1
①
◌ ◌
◌◌
◌ ◌
●●
●●
●●
O2 x 4 = 8
O1 x 2 = 2

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
5 x 2 = 10
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
14
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 14
Molecular
Ion Bonds = 5
( MIB’s )
2O8
16
Molecular
Ion Bonds = 5
( MIB’s )
All Central Atom
Double Bonds
( Postulated ) Lewis Structure
Period Two elements
14
C6
[HCO3 ]
–
H
least one double bond and all
else single bonds is
descriptive as all Period Two
MC’s satisfy the Octet rule
C
O
①
② ③
O
O
––
④ ⑤
1 H1
①
O2 x 4 = 8
O1 x 6 = 6
HC
O
①
② ③
O
O
––
④ ⑤

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
0
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
1
Free Element
VE’s
( FEVE’s )
1
Formal Charge
VE’s
( FCVE’s )
1
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
8
1
· 4 4 4=+ – = 0
[HCO3 ]
–
HC
O
①
② ③
O
O
––
④ ⑤
HC
O
①
② ③
O
O
––
④ ⑤

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
6
1
2
2
1
· 7 6 7=+ – = – 1
[HCO3 ]
–
HC
O
①
② ③
O
O
––
④ ⑤
HC
O
①
② ③
O
O
––
④ ⑤

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bonds
Carbon
Fc ( C ) =C 0
– at least one of the
deficient by 2
electrons
– Carbon ( P2
Element) cannot
accommodate Octet
surplus electrons
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
[HCO3 ]
–
C
O
①
②
③
O
O
–
●●
●●
●●
●●
H④ HC
O ①
②
③
O
O
––
⑥
④
⑤ ⑦
●●
●●
●●
HC
O
①
② ③
O
O
––
④ ⑤

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
5 x 2 = 10
=· – MIVE’s
– 24 =
Molecular
Unbound VE’ s
( MUVE’s )
14
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
Σ ODMC’s 14
Molecular
Ion Bonds = 5
( MIB’s )
2O8
16
14
C6
[HCO3 ]
–
HC
O
①
② ③
O
O
––
④ ⑤
1 H1
①
O2 x 4 = 8
O1 x 6 = 6
HC
O
①
② ③
O
O
––
④ ⑤
( Confirmed )
HC
O ①
②
③
O
O
–
④ ⑤
●●
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O
Cl
Molecular
Constituent
Element
Group
( Elemental )
2
G17 (7)
Valence
Electron
Configuration
[He] 3s23p5
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
6 x 1 = 6
=
7 x 1 = 7
Σ MCVE’s
q
14
Molecular Ion
V.E.’s
( MIVE’s )
=
[ClO]
–
 Hypochlorite
= 1
[He] 2s22p4G16 (6) Cl–O
Single Bond
( Trial )
Lewis Skeleton
①
Molecular
Ion Bonds = 1
( MIB’s )
Cl17
17
3
O8
16

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
1 x 2 = 2
=· – MIVE’s
– 14 =
Molecular
Unbound VE’ s
( MUVE’s )
12
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O1 x 6 = 6
Σ ODMC’s 12
Molecular
Ion Bonds = 1
( MIB )
Lewis Structure
( Postulated )
Even though Cl is a P3 Element
(and capable of accommodating
surplus Octet electrons) Oxygen
is its only bond and is a P2
obliged to follow the Octet Rule
Cl–O①
◌◌
◌◌
◌◌
[ClO]
–
 Hypochlorite
2
Cl17
17
3
O8
16
Cl–O
●●
●●
●●
●●
●●
●●
Molecular
Ion Bonds = 1
( MIB )
Cl1 x 5 = 5
e1 x 1 = 1
–
◌◌
◌◌
◌◌
①

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
7
Free Element
VE’s
( FEVE’s )
7
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
6
1
2
2
1
· 7 6 7=+ – = – 1
[ClO]
–
 Hypochlorite
Cl–O
●●
●●
●●
●●
●●
●●
①
Cl–O
●●
●●
●●
●●
●●
●●
①

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O
Cl
Molecular
Constituent
Element
Group
( Elemental )
2
G17 (7)
Valence
Electron
Configuration
[He] 3s23p5
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
6 x 2 = 12
=
7 x 1 = 7
Σ MCVE’s
q
20
Molecular Ion
V.E.’s
( MIVE’s )
=
= 1
[He] 2s22p4G16 (6)
Single Bond
( Trial )
Lewis Skeleton
Molecular
Ion Bonds = 2
( MIB’s )
Cl17
17
3
O8
16
Cl
O
① ②
O
[ClO2 ]
–
 Chlorite

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
2 x 2 = 4
=· – MIVE’s
– 20 =
Molecular
Unbound VE’ s
( MUVE’s )
16
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O2 x 6 = 12
Σ ODMC’s 16
Molecular
Ion Bonds = 2
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Cl1 x 4 = 4
[ClO2 ]
–
 Chlorite
Molecular
Ion Bonds = 2
( MIB’s )
Cl
O
① ②
O
Cl
O
① ②
O

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
7
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
1
6
1
2
2
1
· 7 6 7=+ – = – 1
Cl
O
① ②
O
Cl
O
① ②
O
[ClO2 ]
–
 Chlorite

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
[ClO2 ]
–
 Chlorite
Cl
O
① ②
O
Cl
O
②
O①
③
④
=Cl 1
=O – 1

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 20 =
Molecular
Unbound VE’ s
( MUVE’s )
12
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O2 x 4 = 8
Σ ODMC’s 12
Molecular
Ion Bonds = 4
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
O2 x 2 = 4
[ClO2 ]
–
 Chlorite
Molecular
Ion Bonds = 4
( MIB’s )
Cl
O
②
O①
③
④
Even though Cl is a P3 Element
(and capable of accommodating
surplus Octet electrons) Oxygen
is its only bonds and is a P2
obliged to follow the Octet Rule
Cl
O
②
O①
③
④
double bonds is not
descriptive as the P2 MC’s
must satisfy the Octet rule

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
[ClO2 ]
–
 Chlorite
Cl
O
① ②
O
Cl
O
②
O①
③
④
Cl
O
②
O
①
③
●●
●●
=Cl 1
=O – 1
– Oxygen ( P2
Element) cannot
accommodate Octet
surplus electrons

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
3 x 2 = 6
=· – MIVE’s
– 20 =
Molecular
Unbound VE’ s
( MUVE’s )
14
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O2 x 4 = 8
Σ ODMC’s 12
Molecular
Ion Bonds = 3
( MIB’s )
2
Cl17
17
3
O8
16
O2 x 2 = 4
[ClO2 ]
–
 Chlorite
Cl
O
②
O①
③
Cl
O
②
O①
③
④
least one double bond, all
else single bonds, is
descriptive and provides the
lowest Formal Charge Value
for the Ion
Cl
O
②
O
①
③
( Confirmed )
●●
●●
●●
●●
◌◌
◌◌
Even though Cl is
bonded exclusively
to P2 elements in the
Chlorite Ion, so long
as the Oxygen
bonds conform to the
Octet Rule, Cl may
take on Octet
surplus electrons

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
6
1·
7
Free Element
VE’s
( FEVE’s )
7
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
6
1
2
2
1
· 7
6 7
=+
– = – 1
[ClO2 ]
–
 Chlorite
Cl
O
②
O
①
③
●●
●●
Cl
O
②
O
①
③
●●
●●
Cl
O
②
O
①
③
●●
●●
4
1
2
4
1
· 6 6 6=+ – = 0
The –1 FC value for the single-bond Oxygen
reflects MIT Professor Donald Sadoway’s
(3.091SC - Introduction to Solid State
Chemistry ) observation that double bonds
are energetically preferable to single bonds.

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl ) =Cl 0
Oxygen
Fc ( O )6LPE
=O – 1
Oxygen
Fc ( O )4LPE
=O 0
[ClO2 ]
–
 Chlorite
Cl
O
① ②
O
Cl
O
②
O①
③
④
Cl
O
②
O
①
③
●●
●●
=Cl 1
=O – 1
– Oxygen ( P2
Element) cannot
accommodate Octet
surplus electrons

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O
Cl
Molecular
Constituent
Element
Group
( Elemental )
2
G17 (7)
Valence
Electron
Configuration
[He] 3s23p5
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
6 x 3 = 18
=
7 x 1 = 7
Σ MCVE’s
q
26
Molecular Ion
V.E.’s
( MIVE’s )
=
= 1
[He] 2s22p4G16 (6)
Single Bond
( Trial )
Lewis Skeleton
Molecular
Ion Bonds = 3
( MIB’s )
Cl17
17
3
O8
16
Cl
O
①
②
O
[ClO3 ]
–
 Chlorate
O
③

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
3 x 2 = 6
=· – MIVE’s
– 26 =
Molecular
Unbound VE’ s
( MUVE’s )
20
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O3 x 6 = 18
Σ ODMC’s 20
Molecular
Ion Bonds = 3
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Cl1 x 2 = 2
[ClO3 ]
–
 Chlorate
Molecular
Ion Bonds = 3
( MIB’s )
Cl
O
①
②
OO
③
●●
●●
●●
●●
Cl
O
①
②
OO
③
◌ ◌
◌◌
◌◌
◌ ◌

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
2
1
2
1
2
Shared Pair
Electrons
( SPE’s )
6
1·
5
Free Element
VE’s
( FEVE’s )
7
Formal Charge
VE’s
( FCVE’s )
5
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
2
6
1
2
2
1
· 7 6 7=+ – = – 1
Cl
O
①
②
OO
③
●●
●●
●●
●●
Cl
O
①
②
OO
③
●●
●●
●●
●●
A FC of 2 – in an otherwise valid Lewis
Structure – augurs very poorly for the posited
structure! Alternative bonding schemes will
likely result in more acceptably minimized FC’s
Similarly, a companion species FC of –1 where
FC values for a “central” species are equally
dismal, strongly indicates that an improved
structure can be realized by the introduction
of compound bonding structures…
[ClO3 ]
–
 Chlorate

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
=Cl 2
=O – 1
Cl
O
①
②
OO
③
●●
●●
●●
●●
[ClO3 ]
–
 Chlorate
Cl
O ①
②
OO
③
●●
⑥
④
⑤
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
6 x 2 = 12
=· – MIVE’s
– 26 =
Molecular
Unbound VE’ s
( MUVE’s )
14
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O3 x 4 = 12
Σ ODMC’s 14
Molecular
Ion Bonds = 6
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Cl1 x 2 = 2
[ClO3 ]
–
 Chlorate
Molecular
Ion Bonds = 6
( MIB’s )
Cl
O ①
②
OO
③
●●
⑥
④
⑤
●●
●●
●●
●●
Cl
O ①
②
OO
③
◌ ◌
⑥
④
⑤
◌ ◌
◌◌
◌ ◌
◌◌

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
2
1
2
1
2
Shared Pair
Electrons
( SPE’s )
12
1·
8
Free Element
VE’s
( FEVE’s )
7
Formal Charge
VE’s
( FCVE’s )
8
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
– 1
2
1
2
4
1
· 4 6 4=+ – = 2
[ClO3 ]
–
 Chlorate
Cl
O ①
②
OO
③
●●
⑥
④
⑤
●●
●●
●●
●●
Cl
O ①
②
OO
③
●●
⑥
④
⑤
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
=Cl 2
=O – 1
Cl
O
①
②
OO
③
●●
●●
●●
●●
[ClO3 ]
–
 Chlorate
Cl
O ①
②
OO
③
●●
⑥
④
⑤
●●
●●
●●
●●
=Cl – 1
=O 2

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 26 =
Molecular
Unbound VE’ s
( MUVE’s )
18
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O1 x 4 = 4
Σ ODMC’s 18
Molecular
Ion Bonds = 4
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Cl1 x 2 = 2
[ClO3 ]
–
 Chlorate
Molecular
Ion Bonds = 4
( MIB’s )
Cl
O
①
②
OO
③
●●
④
Cl
O
①
②
OO
③
◌ ◌
④
O2 x 6 = 12

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
2
1
2
1
2
Shared Pair
Electrons
( SPE’s )
8
1·
6
Free Element
VE’s
( FEVE’s )
7
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
1
2
1
2
6
1
· 5 6 5=+ – = 1
[ClO3 ]
–
 Chlorate
Cl
O
①
②
OO
③
●●
④
Cl
O
①
②
OO
③
●●
④
Cl
O
①
②
OO
③
●●
④
4
1
2
4
1
· 6 6 6=+ – = 0

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
=Cl 2
=O – 1
Cl
O
①
②
OO
③
●●
●●
●●
●●
[ClO3 ]
–
 Chlorate
Cl
O ①
②
OO
③
●●
⑥
④
⑤
●●
●●
●●
●●
=Cl – 1
=O 2
Cl
O
①
②
OO
③
●●
④
=Cl 1
=O 1
=O 0
Cl
O
①
②
OO
③
●●
④
⑤
●●
●●
●●
●●
Two Double Bonds
●●
●●
●●

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
5 x 2 = 10
=· – MIVE’s
– 26 =
Molecular
Unbound VE’ s
( MUVE’s )
16
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O2 x 4 = 8
Σ ODMC’s 16
Molecular
Ion Bonds = 5
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Cl1 x 2 = 2
[ClO3 ]
–
 Chlorate
Molecular
Ion Bonds = 5
( MIB’s )
O1 x 6 = 6
Cl
O
①
②
OO
③
●●
④
⑤
●●
●●
●●
●●
●●
●●
●●
Cl
O
①
②
OO
③
◌ ◌
④
⑤
◌ ◌
◌◌
◌ ◌
◌◌
◌ ◌
◌◌
◌◌

© Art Traynor 2011
Chemistry
Zumdahl
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
2
1
2
1
2
Shared Pair
Electrons
( SPE’s )
10
1·
7
Free Element
VE’s
( FEVE’s )
7
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
6
1
2
2
1
· 7 6 7=+ – = – 1
[ClO3 ]
–
 Chlorate
4
1
2
4
1
· 6 6 6=+ – = 0
Cl
O
①
②
OO
③
●●
④
⑤
●●
●●
●●
●●
●●
●●
●●
Cl
O
①
②
OO
③
●●
④
⑤
●●
●●
●●
●●
●●
●●
●●
Cl
O
①
②
OO
③
●●
④
⑤
●●
●●
●●
●●
●●
●●
●●

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
=Cl 2
=O – 1
Cl
O
①
②
OO
③
●●
●●
●●
●●
[ClO3 ]
–
 Chlorate
Cl
O ①
②
OO
③
●●
⑥
④
⑤
●●
●●
●●
●●
=Cl – 1
=O 2
Cl
O
①
②
OO
③
●●
④
=Cl 1
=O 1
=O 0
Cl
O
①
②
OO
③
●●
④
⑤
●●
●●
●●
●●
Two Double Bonds
●●
●●
●●
=Cl 0
=O – 1
=O 0 Section 7.4 (Pg. 206)
McQuarrie, et al.
Zumdahl
Note that the sum of
the MC FC’s in this
configuration conforms
to the net ionic charge
1 (Cl) · 0 = 0
1 (O) · ( – 1) = 0
2 (O) · 0 = 0

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
O
Cl
Molecular
Constituent
Element
Group
( Elemental )
2
G17 (7)
Valence
Electron
Configuration
[He] 3s23p5
MCVE’s
Valence
Electrons
( VE’s )
·
Molecular
Constituents
( MC’s )
6 x 4 = 24
=
7 x 1 = 7
Σ MCVE’s
q
32
Molecular Ion
V.E.’s
( MIVE’s )
=
= 1
[He] 2s22p4G16 (6)
Single Bond
( Trial )
Lewis Skeleton
Molecular
Ion Bonds = 4
( MIB’s )
Cl17
17
3
O8
16
Cl
O
①
②
O
[ClO4 ]
–
 Perchlorate
O
③
–
O
④

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
4 x 2 = 8
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
24
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O4 x 6 = 24
Σ ODMC’s 24
Molecular
Ion Bonds = 4
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Molecular
Ion Bonds = 4
( MIB’s )
Cl
O
①
②
OO
③
–
O
④
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Cl
O
①
②
OO
③
–
O
④
◌◌
◌◌
◌ ◌
◌◌
◌◌
◌ ◌
◌◌
◌◌
◌ ◌
◌◌
◌◌
[ClO4 ]
–
 Perchlorate
◌ ◌

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
6
1
2
1
2
Shared Pair
Electrons
( SPE’s )
2
1·
7
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
7
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
– 1
0
1
2
8
1
· 4 7 4=+ – = 3
[ClO4 ]
–
 Perchlorate
Cl
O
①
②
OO
③
–
O
④
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
Cl
O
①
②
OO
③
–
O
④
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
A FC of – 1 ain’t so bad and is the usual result of .
Oxygen in a Molecular Ensemble with a SB to
adjacent species The FC on the remaining species
in the molecular ensemble will dictate whether
alternate structures need be explored.
An FC of +3 is honking awful, so we will
definitely need to seek an alternative structure
for this molecular ensemble to arrive at a more
closely descriptive structure

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Double Bond
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
=Cl 3
=O – 1
[ClO4 ]
–
 Perchlorate
Cl
O
①
②
OO
③
–
O
④
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
O
Cl
O ①
②
OO
③
⑥
④
⑤
●●
●●
●●
●●
⑦
––
⑧
1 (Cl) · 3 = 3
4 (O) · ( – 1) = – 4
Though the individual
species FC’s are

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
8 x 2 = 16
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
16
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O4 x 4 = 16
Σ ODMC’s 16
Molecular
Ion Bonds = 8
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Molecular
Ion Bonds = 8
( MIB’s )
[ClO4 ]
–
 Perchlorate
O
Cl
O ①
②
OO
③
⑥
④
⑤
●●
●●
●●
●●
⑦
––
⑧
O
Cl
O ①
②
OO
③
⑥
④
⑤
◌ ◌
◌◌
◌ ◌
◌◌
⑦
––
⑧

© Art Traynor 2011
Chemistry
Atomic Combinations
( Trial )
Lewis Structure
Lone Pair
Electrons
( LPE’s )
4
1
2
1
2
Shared Pair
Electrons
( SPE’s )
4
1·
6
Free Element
VE’s
( FEVE’s )
6
Formal Charge
VE’s
( FCVE’s )
6
FCVE’s
=
=
+
+
–
–
=
=
Formal
Charge
( FC )
0
0
1
2
16
1
· 8
7 8
=+
– = – 1
[ClO4 ]
–
 Perchlorate
The familiar configuration of Oxygen in a Molecular
Ensemble with a DB to adjacent species leads to
an optimized FC of zero. The FC on the remaining
species in the molecular ensemble will dictate
whether alternate structures need be explored.
An FC of –1 ain’t bad (insofar as it can only be
improved by a single unit of FC) if this FC can
be further improved – without any diminution to
the FC’s of the other constituent species in the
molecular ensemble – then some mixture of
bonds may be further FC optimized.
O
Cl
O ①
②
OO
③
⑥
④
⑤
●●
●●
●●
●●
⑦
––
⑧
O
Cl
O ①
②
OO
③
⑥
④
⑤
●●
●●
●●
●●
⑦
––
⑧
Further improvement however is unlikely
as in an all-DB configuration we have
arrived at the net ionic charge.

© Art Traynor 2011
Chemistry
Atomic Combinations
Trial
Lewis
Structures
One Single Bond
All Else Double Bonds
Chlorine
Fc ( Cl )
Oxygen
Fc ( O )6LPE
Oxygen
Fc ( O )4LPE
=Cl 3
=O – 1
[ClO4 ]
–
 Perchlorate
Cl
O
①
②
OO
③
–
O
④
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
●●
O
Cl
O ①
②
OO
③
⑥
④
⑤
●●
●●
●●
●●
⑦
––
⑧
1 (Cl) · 3 = 3
4 (O) · ( – 1) = – 4
The Cl FC of +3 is a
bit of a give-away,
indicating that 3 DBs
might improve the
ionic FC
=Cl 0
=O – 1
1 (Cl) · 0 = 0
4 (O) · ( – 1) = – 4
O
Cl
O ①
②
OO
③
⑥
④
⑤
●●
●●
●●
●●
⑦
–
●●
●●
●●

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
MIB’s Single Bond
Electrons
MIB-VE’s
7 x 2 = 14
=· – MIVE’s
– 32 =
Molecular
Unbound VE’ s
( MUVE’s )
18
=
OD7
OD6
OD5
OD4
OD3
OD2
OD1
O3 x 4 = 12
Σ ODMC’s 18
Molecular
Ion Bonds = 7
( MIB’s )
Lewis Structure
( Postulated )
2
Cl17
17
3
O8
16
Molecular
Ion Bonds = 7
( MIB’s )
[ClO4 ]
–
 Perchlorate
O
Cl
O ①
②
OO
③
⑥
④
⑤
●●
●●
●●
●●
⑦
–
●●
●●
●●
O
Cl
O ①
②
OO
③
⑥
④
⑤
◌ ◌
◌◌
◌ ◌
◌◌
⑦
–
◌ ◌
◌◌
◌◌
O1 x 6 = 6

© Art Traynor 2011
Chemistry
Molecules
Bonding
Molecular Dipole Section 2.5 (Pg. 55)
 Molecular dipoles[edit]
For molecules there are three types of dipoles:
Permanent dipoles: These occur when two atoms in a molecule have substantially
different electronegativity: One atom attracts electrons more than another, becoming
more negative, while the other atom becomes more positive. A molecule with a
permanent dipole moment is called a polar molecule. See dipole-dipole attractions.
Instantaneous dipoles: These occur due to chance when electrons happen to be more
concentrated in one place than another in a molecule, creating a temporary dipole. See
instantaneous dipole.
Induced dipoles: These can occur when one molecule with a permanent dipole repels
another molecule's electrons, inducing a dipole moment in that molecule. A molecule
is polarized when it carries an induced dipole. See induced-dipole attraction.
Wiki: “ Chemical Bond”

© Art Traynor 2011
Chemistry
Molecules
Bonding
Molecular Dipole Section 2.5 (Pg. 55)
 Any scalar or other field may have a dipole moment.
Dipoles can be characterized by their dipole moment, a vector quantity. For the simple
electric dipole given above, the electric dipole moment points from the negative charge
towards the positive charge, and has a magnitude equal to the strength of each charge
times the separation between the charges. (To be precise: for the definition of the
dipole moment, one should always consider the "dipole limit", where e.g. the distance
of the generating charges should converge to 0, while simultaneously the charge
strength should diverge to infinity in such a way that the product remains a positive
constant.)
Wiki: “ Chemical Bond”

Chemistry-Ions(2)_150824_01

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