Chemistry-Ions(1)_150818_01

© Art Traynor 2011
Chemistry
Inorganic Binary Ionic Compounds ( Type I ) Section 2.8 (Pg. 61)
 Cation ( Positive Ion ) is named First
 Name a constituent positive Ion ( Cation ) principally
( in the progression of the formula evolving from the LHS → RHS )
after which the negative Ion ( Anion ) is named, and further specified by
the following conventions :
Atomic Combinations
Nomenclature Conventions
Compounds in this Equivalency Class share the following characteristics
 Anion ( Negative Ion ) is named Secondly
 Monatomic Ions
Cation takes its name from the Elementn
Anion takes its name from the root of the
Element appending an “ –ide ” suffix
n
 Type I IBIC’s are Singular – only one species of Ion can be formed from
the constituent element(s)
Inorganic Binary Ionic Compounds
( IBIC )

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Hydrogen
Hydrogen
1
1
1.00794
GIA (1): Alkali Metal
P1
1s1
Non-Metal
H
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
 Nobel Gas Configuration ( NGC )
H → He1s21s1
 Hydrogen wants the electron
configuration of Helium
It can achieve this by Donating or
Receiving an Electron Cation ↑↓ Hydrogen 1+
H+
+
–
H1
Anion ↑↓ Hydride 1 –
H–

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Lithium
Lithium
2
3
6.941
P2
[He] 2s1
Metal
Li
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
Li → He1s22s1
 Lithium wants the electron
configuration of Helium –
–
–
Cation
↑↓ Lithium +
+
Li
n = 2 ↑↓
1
+
+ +
↑↓
Li3

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Sodium
Sodium ( Natrium )
2
11
22.98976
P3
[Ne] 3s1
Metal
Na
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
Na → Ne2s2 2p63s1
 Sodium wants the electron
configuration of Neon –
–
–
Cation
↑↓
Sodium +
+
Na
n = 2 ↑↓
8
↑↓
1
–
–
11
+ 11
Ø
n = 3 ↑↓
↑↓
Na11

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Potassium
Potassium ( Kalium )
2
19
39.0983
P4
[Ar] 4s1
Metal
K
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
K → Ar3s23p64s1
 Potassium wants the electron
configuration of Argon –
–
–
Cation
3↑↓
Potassium +
+
K
n = 2 ↑↓
8
↑↓
1
–
–
19
+ 19
Ø
n = 3 ↑↓
8
n = 4 ↑↓
We haven’t quite hit the d-block yet
–
–
K19

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Caesium
Caesium
2
55
132.9054519
P6
[Xe] 6s1
Metal
Cs
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
 Nobel Gas Configuration
( NGC )
→ Xe5s24d105p6
 Cesium wants the electron
configuration of Xenon –
–
–
Cation
5↑↓
Caesium +
n = 2 ↑↓
8
↑↓
8
–
–
55
+ 55
Ø
n = 3 ↑↓
18
n = 4 ↑↓
–
–
Cs →
6s1
18
1
–
–
n = 5 ↑↓
n = 6 ↑↓
–
–
+
Cs
Cs55

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Beryllium
Beryllium
2
4
9.012182
GIIA (2): Alkaline Earth Metal
P2
[He] 2s2
Metal
Be
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
Be → He1s22s2
 Beryllium wants the electron
configuration of Helium –
–
–
Cation
↑↓ Beryllium 2+
2+
Be
n = 2 ↑↓
2
+ +
↑↓
–
++
Be4

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Magnesium
Magnesium
2
12
24.3050
P3
[Ne] 3s2
Metal
Mg
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
Mg → Ne2s2 2p63s2
 Magnesium wants the electron
–
–
Cation
↑↓
Magnesium 2+
2+
Mg
n = 2 ↑↓
8
↑↓
2
–
–
12
+ 12
Ø
n = 3 ↑↓
↑↓
–
Mg12

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Calcium
Calcium
2
20
40.078
P4
[Ar] 4s2
Metal
Ca
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
Ca → Ar3s23p64s2
 Calcium wants the electron
–
–
Cation
3↑↓
Calcium 2+
n = 2 ↑↓
8
↑↓
2
–
–
20
+ 20
Ø
n = 3 ↑↓
8
n = 4 ↑↓
–
–
–
2+
Ca
Ca20

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Caesium
Barium
2
56
137.327
P6
[Xe] 6s2
Metal
Ba
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
( NGC )
→ Xe5s24d105p6
 Barium wants the electron
–
–
Cation
5↑↓
Barium 2+
n = 2 ↑↓
8
↑↓
8
–
–
56
+ 56
Ø
n = 3 ↑↓
18
n = 4 ↑↓
–
–
Ba →
6s2
18
2
–
–
n = 5 ↑↓
n = 6 ↑↓
–
–
2+
Ba
–
Ba56

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Aluminum
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
n = 2 ↑↓
n = 3 ↑↓ ↑↓
Aluminum
2
13
26.9815386
GIIIA (13): Post-Transition Metal
P3
8
[Ne]3s23p1
3
Metal
AlAl → Ne2s2 2p63s2 3p1
 Aluminum wants the electron
configuration of Neon
Cation
↑↓
Aluminum 3+
3+
Al↑↓
↑↓
–
–
–
–
–
13
+ 13
Ø
–
p
Al13

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
Atomic Combinations
Ionic species of Silver
Silver ( Argentum )
2
47
107.8682
GIB (11): Transition Metal
P5
[Kr] 4d10 5s1
Metal
Ag
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
( NGC )
Kr 3d104s24p6
 Silver wants the electron
configuration of Krypton –
–
–
Cation
4↑↓
Silver +
n = 2 ↑↓
8
↑↓
1
–
–
47
+ 47
Ø
n = 3 ↑↓
18
n = 4 ↑↓
–
–
Ag →
4d105s1
18
–
n = 5 –
+
Ag
↑↓
d
↑↓↑↓↑↓
↑↓↑↓
Ag47

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Fluorine
Fluorine
2
9
18.9984032
GVIIA (17): Halogen
P2
[He] 2s2 2p5[2]
F
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
F → Ne2s2 2p62s22p5[2]
 Fluorine wants the electron
–
–
Anion
↑↓
Fluoride –
–
F
n = 2 ↑↓
7
–
9
+ 9
Ø
↑↓
Non-Metal
p
↑↓↑↓↑↓
↑↓↑↓↑↓
F9

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Chlorine
Chlorine
2
17
35.453
GVIIA (17): Halogen
P3
[Ne] 3s22p5
Cl
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
Cl → Ar3s23p63s2 2p5
 Chlorine wants the electron
–
–
n = 2 ↑↓
8
–
–
17
+ 17
Ø
n = 3 ↑↓
7
–
Non-Metal
p
↑↓↑↓↑↓
↑↓↑↓↑↓
Anion ↑↓ Chloride –
–
Cl↑↓ ↑↓↑↓↑↓
↑↓
Cl17

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
p
↑↓↑↓↑↓
↑↓↑↓↑↓
Atomic Combinations
Ionic species of Bromine
Bromine
2
35
79.904
GVIIA (17): Halogen
[Ar] 4s2 3d10 4p5
Br
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
Kr
 Bromine wants the electron
configuration of Krypton
–
–
–
n = 2 ↑↓
8
7
–
–
35
+ 35
Ø
n = 3 ↑↓
18
n = 4 ↑↓
–
–
Br →
18
–
P4
Non-Metal
3d104s24p64s2 3d10 4p5
↑↓↑↓↑↓
Anion
↑↓
Bromide –
–
Br
↑↓ ↑↓↑↓↑↓
↑↓
↑↓
Br35

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
p
Atomic Combinations
Ionic species of Iodine
Iodine
2
53
126.90477
GVIIA (17): Halogen
[Kr] 4d10 5s2 5p5
I
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
( NGC )
Xe5s24d105p6
 Iodine wants the electron
–
–
n = 2 ↑↓
8
7
–
–
53
+ 53
Ø
n = 3 ↑↓
18
n = 4 ↑↓
–
–
I →
4d10 5s2 5p5
18
–
–
n = 5 ↑↓ –
P5
Non-Metal
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
4↑↓Anion Iodide –
–
I↑↓↑↓↑↓
I53

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Oxygen
Oxygen
2
8
15.9994
GVIA (16): Chalcogen
[He] 2s2 2p4
O
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
O → Ne2s2 2p62s2 2p4
 Oxygen wants the electron
–
–
n = 2 ↑↓
6
–
8
+ 8
Ø
P2
Non-Metal
p
↑↓↑↓↑↓
Oxide 2 –
2 –
O↑↓↑↓↑↓2↑↓Anion
O8

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Sulfur
Sulfur
2
16
32.065
GVIA (16): Chalcogen
P3
[Ne] 3s22p4
S
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
S → Ar3s23p63s2 3p4
 Sulfur wants the electron
–
–
n = 2 ↑↓
8
–
–
16
+ 16
Ø
n = 3 ↑↓
6
–
Non-Metal
p
↑↓↑↓↑↓
↑↓↑↓↑↓
Sulfide 2 –
2 –
S↑↓↑↓↑↓3↑↓Anion
S16

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Nitrogen
Nitrogen
2
7
14.0067
GVIA (15): Pnictogen
[He] 2s2 2p3
N
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
N → Ne2s2 2p62s2 2p3
 Nitrogen wants the electron
–
–
n = 2 ↑↓
5
–
7
+ 7
Ø
P2
Non-Metal
p
↑↓↑↓↑↓
Nitride 3 –
3 –
N↑↓↑↓↑↓2↑↓Anion
N7

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
Atomic Combinations
Ionic species of Phosphorus
Phosphorus
2
15
30.973762
GVA (15): Pnictogen
P3
[Ne] 3s23p3
P
G
r
o
u
p
O r b i t a l s
n = 1
s
↑↓
P → Ar3s23p63s2 3p3
 Phosphorus wants the electron
–
–
n = 2 ↑↓
8
–
–
15
+ 15
Ø
n = 3 ↑↓
5
–
Non-Metal
p
↑↓↑↓↑↓
↑↓↑↓↑↓
Phosphide 3 –
3 –
P↑↓↑↓↑↓3↑↓Anion
P15

© Art Traynor 2011
Chemistry
Inorganic Binary Ionic Compounds ( Type II – Monatomic ) Section 2.8 (Pg. 62)
 Type II IBIC’s are composed of Transition and Post-Transition Metals
Atomic Combinations
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
Inorganic Binary Ionic Compounds ( Type II ) Section 2.8 (Pg. 61)
Atomic Combinations
Ionic species of Iron
Iron ( Ferrum )
2
26
55.845
GVIIIB (98): Transition Metal
P4
[Ar] 3d64s2
Metal
FeG
r
o
u
p
O r b i t a l s
 NGC : Iron has a “ d ” orbital that
is just over half-filled and will ionize
by relenting one to achieve an evenly
half-filled “ d ” orbital and one of
its “ s ” valence electrons ( to achieve
a configuration similar to the native
state of Copper ) , and further
ionizing by yielding its remaining
8
14
21
s
↑↓
2 ↑↓
3 ↑↓
4 ↑↓
n p
↑↓↑↓↑↓
↑↓↑↓↑↓
d –1
↑↓↑↓↑↓
↑↓↑↓
Ferrous
Iron (II) 2 +
2 +
Fe4↑↓Cation
Ferric
Iron (III) 3 +
3 +
Fe4↑↓Cation
–
–
–
–
–
26
+ 26
Ø
–
–
↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
↑↓↑↓↑↓
–
“s” valence electron to assume
the configuration of Argon
→ Fe3d54s1
Fe 3d64s2
→ Ar3s23p6
Fe 3d64s2 Fe26

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
Atomic Combinations
Ionic species of Cobalt
Cobalt
2
27
58.933195
GVIIIB (9): Transition Metal
P4
[Ar] 3d74s2
Metal
CoG
r
o
u
p
O r b i t a l s
 Cobalt has a “ d ” orbital that is
just over half-filled and will ionize
by relenting two to achieve an
evenly half-filled “ d ” orbital, it
will ionize still further yielding one
of its “ s ” valence electrons
( to achieve a configuration similar
to the native state of Copper )
8
15
21
s
↑↓
2 ↑↓
3 ↑↓
4 ↑↓
n p
↑↓↑↓↑↓
↑↓↑↓↑↓
d –1
↑↓↑↓↑↓
↑↓↑↓
Cobalt (II) 2 +
2 +
Co4↑↓Cation
Cobalt (III) 3 +
3 +
Co4↑↓Cation
–
–
–
–
–
27
+ 27
Ø
–
–
↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
↑↓↑↓↑↓
–
→ Co3d54s2
Co3d74s2
→ Co3d54s1
Co3d74s2
Co27

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
Atomic Combinations
Ionic species of Copper
Copper ( Cuprum )
2
29
63.546
GIB (11): Transition Metal
P4
[Ar] 3d104s2
Metal
Cu
G
r
o
u
p
O r b i t a l s
 NGC : Copper wants the electron
configuration of Argon, with its 2nd
“ s ” electron occupying the 3d
orbital (to fill the 3d) its single “ s ”
electron is easily relented, with a
second yielded from the 3d orbital
→ Ar3s23p6
8
18
11
s
↑↓
2 ↑↓
3 ↑↓
4 ↑↓
n p
↑↓↑↓↑↓
↑↓↑↓↑↓
d –1
↑↓↑↓↑↓
↑↓↑↓
Cu3d104s1
Cuprous Copper (I) +
+
Cu4↑↓Cation
Cupric Copper (II) 2 +
2 +
Cu4↑↓Cation
–
–
–
–
–
29
+ 29
Ø
–
–
↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
↑↓↑↓↑↓
Cu29

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
Atomic Combinations
Ionic species of Tin
Tin ( Stannum )
2
50
118.710
GIVA (14): Post Transition Metal
P5
[Kr] 4d105s25p2
Metal
SnG
r
o
u
p
O r b i t a l s
 NGC : Tin wants the electron
configuration of Krypton, but
is also stable with that of
Strontium
→ Kr 3d104s24p6
8
18
18
4
1
s
↑↓
2 ↑↓
3 ↑↓
4 ↑↓
5 ↑↓
n p
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
d –1
↑↓↑↓↑↓
↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
Sr 5s2
→Sn4d105s2 5p2
Sn4d105s2 5p2
Tin (II) 2 +
2 +
Sn↑↓5↑↓Cation
Tin (IV) 4 +
4 +
Sn↑↓5↑↓Cation
–
–
–
–
–
50
+ 50
Ø
–
–
–
–
–
Sn50

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
F-Block
Atomic Combinations
Ionic species of Lead
Lead ( Plumbum )
2
82
207.02
GIVA (14): Post Transition Metal
P6
[Xe] 6s24f145d106p2
Metal
Pb
G
r
o
u
p
O r b i t a l s
 NGC : Lead wants the electron
configuration of Xenon , but is
also stable with that of Barium
→ Xe5s24d105p6
– –
8
18
82
+ 82
Ø
18
→
32
4
1
s
↑↓
2 ↑↓
3 ↑↓
4 ↑↓
5 ↑↓
6 ↑↓
n p
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
d –1
↑↓↑↓↑↓
↑↓↑↓
f – 2
↑↓↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
Ba6s2
→Pb6s2 6p2
Pb6s2 6p2
Lead (II) 2 +
2 +
Pb↑↓6↑↓Cation
Lead (IV) 4 +
4 +
Pb↑↓6↑↓Cation
6s
6p
5d
4f
Pb82

© Art Traynor 2011
Chemistry
S-Block
S
P-Block
D-Blocks
F-Block
Atomic Combinations
Ionic species of Mercury
Mercury (Hydrargyrum )
2
80
200.59
GIVA (26): Transition Metal
P6
[Xe] 4f145d106s2
Metal
HgG
r
o
u
p
O r b i t a l s
 NGC : Mercury wants the
electron configuration of
Xenon, ( but will only ionize
as a Diatomic molecule )
→ Xe5s24d105p6
– –
8
18
80
+ 80
Ø
18
→
32
2
1
s
↑↓
2 ↑↓
3 ↑↓
4 ↑↓
5 ↑↓
6 ↑↓
n p
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
d –1
↑↓↑↓↑↓
↑↓↑↓
f – 2
↑↓↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
↑↓↑↓↑↓
↑↓↑↓
Hg4f14 5d10 6s2
Mercury (II) Mercuric 2 + 2 +
Hg6↑↓Cation
Mercury (I) Mercurous 2 +
2 +
Hg2
6s
5p
5d
4f
Known as a Dimeric Cation
Hg80

Chemistry-Ions(1)_150818_01

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