Naming and formula writing are essential skills in future chapters. It is important that you
practice independently until you are good at these skills. Use your flow chart for every
problem until you know the chart and the system. Start at the top of the appropriate side of
the flowchart (naming or formula writing) and ask yourself each question about the
compounds so you follow the correct rules for naming. This worksheet includes summaries
of information from the flowchart.
A SAD STORY OF CHEMICAL IGNORANCE
Johnny was a chemist’s son.
But Johnny is no more.
What Johnny thought was H2O
Was H2SO4
SECTION A: BINARY IONIC COMPOUNDS: (metal and non-metal)
Name the metal. Name the non-metal with an –ide ending.
If you see an –ide ending in a name, it is often a binary ionic compound. Reverse the naming process,
determine charges from the periodic table and do criss-cross to write the formula.
1
Al2O3
Potassium bromide
2
CsCl
Aluminum chloride
3
NaBr
Barium oxide
4
CaF2
Barium fluoride
5
ZnF2
Magnesium sulfide
6
K3N
Calcium phosphide
7
Ag2O
Boron iodide
8
RbCl
Potassium nitride
9
Li3P
Radium nitride
10 BP
11 AlI3
12 NaF
13 Ba3N2
14 BeO
15 Mg3N2
Lithium bromide
SECTION B: BINARY MOLECULAR COMPOUNDS (non-metals)
Prefixes are used to indicate the number of atoms of each element. Use a prefix for more than one of the
first element. Always use a prefix for the second element, and end the second element with –ide.
The prefixes to memorize:
1 mono, 2 di, 3 tri, 4 tetra, 5 penta, 6 hexa, 7 hepta, 8 octa, 9 nona, 10 deca
Use the prefixes to write the formulas. Do not criss-cross; the prefix refers to the element it is with.
16
N2O5
17
CCl4
Dihydrogen
monoxide
Carbon disulfide
SECTION C: BINARY IONIC AND MOLECULAR MIXED
Decide if compounds are ionic or covalent and name according the appropriate rules.
Ionic: Metal and non-metal
Molecular: 2 non-metals
For formula writing, prefixes indicate a molecular compound.
18
Li2S
Beryllium bromide
19
Al2O3
Dinitrogen triiodide
20
GaP
Calcium sulfide
21
S3F6
Francium carbide
22
Be3N2
Rubidium telluride
23
RaTe
Trisilicon monoxide
24
InCl3
Nitrogen monoxide
25
CaO
Radium carbide
26
P3N2
Strontium phosphide
27
Rb2Se
Barium bromide
28
MgH2
29
F4O
30
PO7
31
Cs3P
32
As2S9
SECTION D: IONIC COMPOUNDS WITH TRANSITION METALS
The charges (oxidation numbers) of transition metals may vary. The charge is determined from the known
charge of the anions. (This seems like reverse criss-cross.) The charge is shown with a Roman numeral.
Ag is always 1+ Zn and Cd are always 2+ no Roman numeral used
Pb, Sb, and Sn vary and require Roman numerals.
In writing formulas from names, the Roman numeral gives the cation’s charge. Use it in criss-cross.
33
Fe2S3
Lead (IV) iodide
34
Cu3N2
35
ZnF2
Antimony (III)
sulfide
Cadmium iodide
SECTION E: MIXED COMPOUNDS: BINARY IONIC, MOLECULAR, TRANSITION METALS
36
Cl3O5
37
S6F2
Diphosphorus
trichloride
Carbon pentachloride
38
CuO
Sodium carbide
39
B2Cl10
Dihydrogen dioxide
40
Ra3N2
Copper (II) sulfide
41
SnO2
Xenon heptafluoride
42
P3O6
Dinitrogen
octabromide
SECTION F: TERNARY COMPOUNDS have more than 2 kinds of elements. They may be composed
of ionic bonds involving polyatomic ions. Check your list for names, formulas, and charges.
Endings other than –ide (except for hydroxide) indicate polyatomic ions. Look at your polyatomic ion list
and criss-cross.
43
Li3PO4
Aluminum sulfate
44
KClO3
Barium carbonate
45
Rb2SO4
46
AgHCO3
Magnesium
dichromate
Silver nitrate
47
Ca(OH)2
Barium nitrite
48
B2(SO3)3
Potassium hydroxide
49
MgCrO4
Calcium chromate
50
NH4Cl
Zinc perchlorate
51
NH4OH
Ammonium iodide
52
Na2SO3
Sodium bicarbonate
53
BaCO3
Boron phosphate
54
Li2SO4
Zinc sulfate
55
Ba(C2H3O2)2
Sodium hydroxide
56
Al2(Cr2O7)3
57
ZnCrO4
Ammonium
carbonate
Silver hydroxide
58
K2SO3
Calcium acetate
59
Al(HCO3)3
Lithium chromate
60
RbClO3
Ammonium chlorite
61
NaHClO
Strontium
perchlorate
SECTION G: ACIDS
The cation is H+ in an acid. The anion is indicated by the form of the name following 3 guidelines.
1. If the anion ends in -ide…hydro + the name of anion with –ic ending acid
2. If the anion ends in -ate… name of anion with –ic ending acid
3. If the anion ends in -ite… name of anion with –ous ending acid
Use these rules in reverse if you see the word “acid” in the name.
Work in future chapters will be easier if you memorize the acids in bold.
62
HF
Hydrochloric acid
63
H2SO4
Nitric acid
64
HNO2
Sulfurous acid
65
H2S
Carbonic acid
66
HClO
Phosphoric acid
67
H3P
Phosphorous acid
SECTION H: ALL TYPES
Name or write the formulas for the following compounds. All types are included as a real test of your
ability! Identify each type of compound and refer to your naming and formula writing outline to
determine what rules to follow for each compound.
68
ZnS
Tin (II) nitrate
69
MgCl2
Zinc phosphate
70
Ca(ClO3)2
Lithium sulfide
71
BaSO4
Silver sulfate
72
AgNO3
Potassium nitrite
73
CaO
Copper (I) sulfite
74
Mg3(PO4)2
Carbon disulfide
75
KCl
Calcium oxide
76
K2O
Barium carbonate
77
Al(NO2)3
Silicon dioxide
78
MgO
Carbon tetrachloride
79
SnI2
Sodium hydride
80
AsCl5
Cesium fluoride
81
CuSO3
Aluminum oxide
82
FeSO4
83
SnCl4
Ammonium
phosphate
Boron trifluoride
84
AsCl3
Radium sulfate
85
NH4OH
Calcium bicarbonate
86
HNO3
Magnesium nitride
87
CS2
Silver oxide
88
CuCl2
Lead (IV) sulfite
89
PCl5
Calcium chlorate
MORE MIXED:
90
LiNO3
Sodium phosphate
91
KHCO3
Sodium fluoride
92
HCl
93
CuSO3
Diphosphorus
pentoxide
Sulfur dichloride
94
MgSO4
Aluminum sulfate
95
CuCl
Dinitrogen trioxide
96
NaBr
Sulfur dichloride
97
P2O3
Sulfuric acid
98
HClO
Ammonium chloride
99
N2O5
Strontium carbonate
100
AlN
Nitrous acid
101
Pb(NO3)2
102
CaH2
103
NaH
104
KClO2
Cobalt (II) chloride hexahydrate CoCl2 6H2O
Copper (II) sulfate forms a hydrate with 5 water molecules. Complete
its formula and name below.
105
SiO2
CuSO4 ______________
EXTRA
NAMING HYDRATES
Hydrates are compounds with water in the structure in a defined ratio.
A dot separates the water molecule. A coefficient tells how many
water molecules. In the name, a prefix and the word hydrate indicate
how many water molecules are present.
A compound that forms hydrates, but has no water is called the
anhydrous form.
Copper (II) sulfate
________________
If you worked carefully and thoughtfully, you should have a good foundation in
CHEMICAL NOMENCLATURE.
Yes, there is even a name for naming!
THE HAPPY ENDING
Johnny got a second chance
He studied hard in school
Johnny learned his chemistry,
And now he is no fool.
Johnny knows ‘bout nomenclature
He knows what not to drink
He knows no matter what he does…
It’s always smart to THINK!