Periodic Table
1
18
1
H
1.008
2
13
14
15
16
17
2
He
4.003
3
Li
6.941
4
Be
9.012
5
B
10.81
6
C
12.01
7
N
14.01
8
O
16.00
9
F
19.00
10
Ne
20.18
11
Na
22.99
12
Mg
24.31
3
4
5
6
7
8
9
10
11
12
13
Al
26.98
14
Si
28.09
15
P
30.97
16
S
32.07
17
Cl
35.45
18
Ar
39.95
19
K
39.10
20
Ca
40.08
21
Sc
44.96
22
Ti
47.88
23
V
50.94
24
Cr
52.00
25
Mn
54.94
26
Fe
55.85
27
Co
58.93
28
Ni
58.69
29
Cu
63.55
30
Zn
65.39
31
Ga
69.72
32
Ge
72.59
33
As
74.92
34
Se
78.96
35
Br
79.90
36
Kr
83.80
37
Rb
85.47
38
Sr
87.62
39
Y
88.91
40
Zr
91.22
41
Nb
92.91
42
Mo
95.94
43
Tc
(98)
44
Ru
101.1
45
Rh
102.9
46
Pd
106.4
47
Ag
107.9
48
Cd
112.4
49
In
114.8
50
Sn
118.7
51
Sb
121.8
52
Te
127.6
53
I
126.9
54
Xe
131.3
55
Cs
132.9
56
Ba
137.3
57
La
138.9
72
Hf
178.5
73
Ta
180.9
74
W
183.9
75
Re
186.2
76
Os
190.2
77
Ir
192.2
78
Pt
195.1
79
Au
197.0
80
Hg
200.6
81
Tl
204.4
82
Pb
207.2
83
Bi
209.0
84
Po
(210)
85
At
(210)
86
Rn
(222)
87
Fr
(223)
88
Ra
(226)
89
Ac
(227)
104
Rf
(257)
105
Ha
(260)
106
Sg
(263)
107
Ns
(262)
108
Hs
(265)
109
Mt
(266)
Review of Naming Ionic Compounds
• Cation first in name and formula
• Monatomic anion name ends in “ide”
• Monatomic cation (metal) name remains same as its atom
• Give charge for transition metals (i.e. Fe, Cr, Mn)
Examples:
Manganese (III) oxide
Mn2O3
Mn+3 O-2
Potassium dichromate
K2Cr2O7
K+1
Cr2O7-2
Magnesium nitrate
Mg(NO3)2
Mg+2
NO3-1
Review of Naming Molecular Compounds
• First element listed in name or formula keeps its atomic
name. Second element ends with “ide”.
• Must state the number of each element in the name
using the Greek prefixes. (i.e. mono, di, tri, tetra…)
Examples:
Xenon hexafluoride
XeF6
Carbon disulfide
CS2
Trisilicon pentabromide
Si3Br5
Remember that something like K2SO4 is NOT dipotassium
sulfate. Why? K2SO4 is ionic and NOT molecular.
How can you distinguish between an
ionic and a molecular compound?
Look for the presence of a metal ion.
If there is a metal ion, the compound is ionic and you
should use the rules for naming ionic compounds. If
there are only nonmetals present, the compound is
molecular and you should use the rules for naming
molecular compounds.
Oxoacids
and
Oxoanions
Naming Oxoacids
The 5 “ic” acids
Sulfuric
Nitric
Chloric
Phosphoric
Carbonic
H2SO4
HNO3
HClO3
H3PO4
H2CO3
You will need to know the name AND formula. Pay
particular attention to the number of oxygens each acid
has in its “ic” form.
Gotta know ‘em
SO LEARN ‘EM
Conversion Table
oxoacid
“per”__”ic”
O 
 -O
“ic”
O 
 -O
“ous”
O 
 -O
“hypo” __ “ous”
Loss of all H’s
oxoanion
“per”__”ate”
O 
 -O
“ate”
O 
 -O
“ite”
O 
 -O
“hypo” __ “ite”
Nitric Acid / Anions
HNO4
NO4pernitrate
HNO3
NO3nitrate
HNO2
Nitrous
NO2nitrite
HNO
Hyponitrous
NOHyponitrite
Pernitric
Nitric
Sulfuric Acid / Anions
H2SO5
SO5-2
Persulfuric
Persulfate
H2SO4
Sulfuric
SO4-2
Sulfate
H2SO3
SO3-2
Sulfurous
Sulfite
H2SO2
Hyposulfurous
SO2-2
Hyposulfite
Chloric Acid / Anions
HClO4
Perchloric
ClO4Perchlorate
HClO3
Chloric
ClO3Chlorate
HClO2
Chlorous
ClO2Chlorite
HClO
Hypochlorous
ClOHypochlorite
Phosphoric Acid / Anions
H3PO5
Perphosphoric
PO5-3
Perphosphate
H3PO4
Phosphoric
PO4-3
Phosphate
H3PO3
Phosphorous
PO3-3
Phosphite
H3PO2
Hypophosphorous
PO2-3
Hypophosphite
Carbonic Acid / Anions
H2CO4
Percarbonic
CO4-2
Percarbonate
H2CO3
Carbonic
CO3-2
Carbonate
H2CO2
Carbonous
CO2-2
Carbonite
H2CO
Hypocarbonous
CO-2
Hypocarbonite
Try a few on your own:
Carbonous acid
H2CO2
Hyponitrous acid
HNO
Lithium phosphate
Li3PO4
NaNO2
Sodium nitrite
H2SO2
Hyposulfurous acid
KClO3
Potassium chlorate
Now what about cases like these…
H2PO4-
HPO4-2
PO4-3
From what we know so far all of these would be ???
phosphate
Well they can’t all be phosphate so we need a
method to deal with multiple hydrogens…
PO4-3
phosphate
Example:
HPO4-2
Hydrogen phosphate
Na2HPO4
H2PO4Dihydrogen phosphate
Sodium hydrogen phosphate
Note: These are the ONLY examples of where there will be three parts
of a name.
Try a few on your own:
Sodium hydrogen sulfite
NaHSO3
Potassium dihydrogen
phosphate
KH2PO4
Ba(HCO3)2
Barium hydrogen
carbonate
Questions ??