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118
1H
1.0082 13 14 15 16 17
2He4.003
3Li6.941
4Be9.012
5B
10.81
6C
12.01
7N
14.01
8O
16.00
9F
19.00
10Ne20.18
11Na22.99
12Mg24.31 3 4 5 6 7 8 9 10 11 12
13Al26.98
14Si28.09
15P
30.97
16S
32.07
17Cl35.45
18Ar39.95
19K
39.10
20Ca40.08
21Sc44.96
22Ti47.88
23V
50.94
24Cr52.00
25Mn54.94
26Fe55.85
27Co58.93
28Ni58.69
29Cu63.55
30Zn65.39
31Ga69.72
32Ge72.59
33As74.92
34Se78.96
35Br79.90
36Kr83.80
37Rb85.47
38Sr87.62
39Y
88.91
40Zr91.22
41Nb92.91
42Mo95.94
43Tc(98)
44Ru101.1
45Rh102.9
46Pd106.4
47Ag107.9
48Cd112.4
49In114.8
50Sn118.7
51Sb121.8
52Te127.6
53I
126.9
54Xe131.3
55Cs132.9
56Ba137.3
57La138.9
72Hf178.5
73Ta180.9
74W183.9
75Re186.2
76Os190.2
77Ir192.2
78Pt195.1
79Au197.0
80Hg200.6
81Tl204.4
82Pb207.2
83Bi209.0
84Po(210)
85At(210)
86Rn(222)
87Fr(223)
88Ra(226)
89Ac(227)
104Rf(257)
105Ha(260)
106Sg(263)
107Ns(262)
108Hs(265)
109Mt(266)
Periodic Table
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
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.
How can you distinguish between an ionic and a molecular
compound?
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.
Look for the presence of a metal ion.
Oxoacidsand
Oxoanions
Naming Oxoacids
The 5 “ic” acids
Sulfuric H2SO4
Nitric HNO3
Chloric HClO3
PhosphoricH3PO4
Carbonic H2CO3
Gotta know ‘em SO LEARN ‘EM
You will need to know the name AND formula. Pay particular attention to the number of oxygens each acid has in its “ic” form.
Conversion Table
O- O
oxoanionLoss of all H’soxoacid
“hypo” __ “ite”“hypo” __ “ous”
“ite”“ous”
“ate”“ic”
“per”__”ate”“per”__”ic”
O- O
O- O
O- O
O- O
O- O
Nitric Acid / Anions
NO-HNO
NO2-HNO2
NO3-HNO3
NO4-HNO4
Nitric
Pernitric
Nitrous
Hyponitrous
pernitrate
nitrate
nitrite
Hyponitrite
Sulfuric Acid / Anions
SO2-2H2SO2
SO3-2H2SO3
SO4-2H2SO4
SO5-2H2SO5
Sulfuric
Persulfuric
Sulfurous
Hyposulfurous
Persulfate
Sulfate
Sulfite
Hyposulfite
Chloric Acid / Anions
ClO-
HypochloriteHClO
Hypochlorous
ClO2-
Chlorite
HClO2
Chlorous
ClO3-
Chlorate
HClO3
Chloric
ClO4-
Perchlorate
HClO4
Perchloric
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
Hyponitrous acid
Lithium phosphate
NaNO2
H2SO2
KClO3
H2CO2
Li3PO4
Hyposulfurous acid
Potassium chlorate
Sodium nitrite
HNO
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…
H2PO4-HPO4
-2PO4-3
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.
Try a few on your own:
Sodium hydrogen sulfite
Potassium dihydrogen phosphate
Ba(HCO3)2
NaHSO3
Barium hydrogen carbonate
KH2PO4
Questions ??
