1. 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
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)
Periodic Table

2. 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
Potassium dichromate
Magnesium nitrate
Mn2O3 Mn+3 O-2
K2Cr2O7 K+1 Cr2O7-2
Mg(NO3)2 Mg+2 NO3-1

3. 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
Carbon disulfide
Trisilicon pentabromide
XeF6
CS2
Si3Br5
Remember that something like K2SO4 is NOT dipotassium sulfate. Why?
K2SO4 is ionic and NOT molecular.

4. 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.

5. Oxoacids
and
Oxoanions

6. Naming Oxoacids The 5 “ic” acids Sulfuric H2SO4 Nitric HNO3
Chloric HClO3
Phosphoric H3PO4
Carbonic 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

7. Conversion Table oxoacid oxoanion “per”__”ic” “per”__”ate” “ic” “ate”
Loss of all H’s
oxoanion
“per”__”ic”
“per”__”ate”
“ic”
“ate”
“ous”
“ite”
“hypo” __ “ous”
“hypo” __ “ite”

8. Nitric Acid / Anions HNO4 NO4- pernitrate Pernitric HNO3 NO3- nitrate
nitrite
Nitrous
HNO
NO-
Hyponitrous
Hyponitrite

9. Sulfuric Acid / Anions H2SO5 SO5-2 Persulfuric Persulfate H2SO4 SO4-2
Sulfurous
Sulfite
H2SO2
SO2-2
Hyposulfurous
Hyposulfite

10. Chloric Acid / Anions HClO4 Perchloric ClO4- Perchlorate HClO3 Chloric
Chlorous
ClO2-
Chlorite
HClO
Hypochlorous
ClO-
Hypochlorite

11. Phosphoric Acid / Anions
H3PO5
Perphosphoric
PO5-3
Perphosphate
H3PO4
Phosphoric
PO4-3
Phosphate
H3PO3
Phosphorous
PO3-3
Phosphite
H3PO2
Hypophosphorous
PO2-3
Hypophosphite

12. Carbonic Acid / Anions H2CO4 Percarbonic CO4-2 Percarbonate H2CO3
Carbonous
CO2-2
Carbonite
H2CO
Hypocarbonous
CO-2
Hypocarbonite

13. Try a few on your own:
Carbonous acid
Hyponitrous acid
Lithium phosphate
NaNO2
H2SO2
KClO3
H2CO2
HNO
Li3PO4
Sodium nitrite
Hyposulfurous acid
Potassium chlorate

14. 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
HPO4-2
H2PO4-
phosphate
Hydrogen phosphate
Dihydrogen phosphate
Example: Na2HPO4
Sodium hydrogen phosphate
Note: These are the ONLY examples of where there will be three parts of a name.

15. Try a few on your own:
Sodium hydrogen sulfite
Potassium dihydrogen phosphate
Ba(HCO3)2
NaHSO3
KH2PO4
Barium hydrogen carbonate

16. Questions ??