Transcript Chemical Naming & Formulas

1)
2)
3)
Covalent
Ionic
Organic
◦ Entire unit in Chem 30S
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Generally a bond between 2 non-metal elements
General Rules
◦ First element is named as listed on periodic table
◦ Second element has the suffix –ide
◦ Prefix used for each element to indicate the # of atoms
 If only one atom of first element → No prefix used
Number
1
2
3
4
5
6
7
8
9
10
Prefix
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
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Name the following
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CO2
CO
CCl4
N2O4
SF6
P2Cl5
PI3
P5Cl8
Carbon dioxide
Carbon oxide
Carbon tetrachloride
Dinitrogen tetraoxide
Sulfur hexafluoride
Diphosphorus pentachloride
Phosphorus triodide
Pentaphosphorus octachloride
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Write the formulas for the following
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Tetranitrogen decaoxide
Disulfur pentafluoride
Hexaselenium tribromide
Nitrogen monoxide
Aluminum Chloride
N4O10
S2F5
Se6Br3
NO
IONIC
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3 subcategories
◦ Monatomic Ions
◦ Polyatomic Ions
◦ Transitional Metals
 Can use both monatomic and polyatomic
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Rules
◦ Formula must be neutral
◦ No # prefixes used as only one possible combination
with ions involved
◦ Cation (+ve) listed first, Anion (-ve) listed second
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Monatomic ions are ions that contain only 1 atom
Anion has suffix –ide
Examples
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NaCl
AlCl3
MgO
Ga2P3
HF
NaH
Sodium Chloride
Aluminum Chloride
Magnesium Oxide
Gallium Phosphide
Hydrogen Fluoride
Sodium Hydride
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Entire unit MUST be neutral
◦ Add appropriate # of each ion to balance charges
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Example
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Aluminum Fluoride
Al3+
F-
+3
-1
Al3+
3F-
+3
-3
AlF3
=
+2
=
0
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Example
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Gallium Oxide
Ga3+
O2-
+3
-2
Ga3+
2O2-
+3
-4
2Ga3+
2O2-
+6
-4
2Ga3+
3O2-
+6
-6
Ga2O3
=
+1
=
-1
=
+2
=
0
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Examples
◦ Write the formulas for the following
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Lithium Sulfide
Magnesium Bromide
Hydrogen Nitride
Aluminum Phosphide
Boron Sulfide
Li2S
MgBr2
H3N
AlP
B2S3
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Ions with more than one atom
◦ Eg)
 NO3 PO43 NH4+
(Nitrate)
(Phosphate)
(Ammonium)
◦ The entire item has a charge, not each element in the
polyatomic ion
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Look at page. 257
The exact ion name is used
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Examples
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NaBrO3
Na2C2O4
Ca(NO3)2
NH4Cl
Al2(SO3)3
Sodium Bromate
Sodium Oxalate
Calcium Nitrate
Ammonium Chloride
Aluminum Sulfite
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Entire unit MUST be neutral
◦ Add appropriate # of each ion to balance charges
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Example
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Potassium Permanganate
K+
MnO4-
+1
-1
KMnO4
=
0
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Example
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Magnesium Nitrite
Mg2+
+2
NO2-1
=
Mg2+
2NO2-
+2
-2
Mg(NO2)2
=
+1
0
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Transitional Metals can have different charges
◦ Depends on the situation
◦ Example
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Fe2+
Fe3+
Ti2+
Ti4+
When naming, must determine what the charge is
◦ Indicated by using Roman numerals
 Must know Roman numerals 1-10
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Example
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Fe2+
+2
FeO
O2-2
Iron (II) Oxide
=
0
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Example
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Fe2(CO3)3
2Fe 3+
+6
3CO32-6
=
Iron (III) Carbonate
0
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Write the names for the following
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TiS2
CuCl
AgNO3
CuSO4
V(ClO4)5
Titanium (IV) Sulfide
Copper (I) Chloride
Silver (I) Nitrate
Copper (II) Sulfate
Vanadium (V) Perchlorate
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The name indicates the charge
◦ Balance as normal
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Example
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Zinc (II) Chloride
Zn2+
Cl-
+2
-1
Zn2+
2Cl-
+2
-2
ZnCl2
=
=
+1
0
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Examples
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Nickel (II) Nitride
Chromium (IV) Oxalate
Iron (III) Cyanide
Mercury (I) Acetate (careful)
Ni3N2
Cr(C2O4)2
Fe(CN)3
Hg2(CH3COO)2
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Peroxide
◦ A polyatomic ion with 2 oxygen atoms with a 2- charge
◦ Very reactive ion
◦ Explosive in some cases
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H20
H2O2
Dihydrogen Monoxide (Covalent)
Hydrogen peroxide (Ionic)
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Example
MgO2
If the oxygen is an oxide ion, then we would have
-4
The Mg is +2
This is not balanced
Therefore the O2 item must have a -2 charge
Peroxide (O22-)
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P.282 #’s 65-70
◦ Omit #67 d)
& #69 i)
& #66 h)