Download Inorganic Nomencalture - UCO

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Composed of a Cation (+ charge) and an Anion
(- charge).
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Ionic compounds are electrically neutral.
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Ionic compounds are composed of:
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A metal and a non-metal
A metal and a polyatomic anion
A polyatomic cation and a non-metal
A polyatomic cation and a polyatomic anion
NaCl
NaNO3
NH4Cl
NH4NO3
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Metals form cations with + charges.
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Group 1 metals form cations with a 1+ charge.
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Cations are named with the metal’s name plus
ion.
Li1+ Na1+ K1+ Rb1+ Cs1+ Fr1+.
Lithium ion, Sodium ion, Potassium ion,
Rubidium ion, Cesium ion, Francium ion.
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Group 2 metals form cations with a 2+
charge.
Be2+
Mg2+
Ca2+
Sr2+
Ba2+
Ra2+
Beryllium ion, Magnesium ion, Calcium
ion, Strontium ion, Barium ion, Radium
ion.
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Other metals with only one oxidation
state (charge):
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Al3+
Aluminum ion
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Zn2+
Zinc ion
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Ag1+
Silver ion
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Cd2+
Cadmium ion
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Transition Metals (Group 3-12) may have
more than one oxidation state.
The oxidation state of the transition metal
is indicated by a Roman numeral in
parenthesis after the metals name (e.g.,
copper(I) ion is Cu1+).
This is important: Iron(III) DOES NOT
mean Fe3, it means Fe3+.
Determining the charge on the transition
metal means you have to know the names
and charges of anions.
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Monoatomic anions take the root of the element
and add “-ide” (i.e., Cl1- is chloride, O2- is oxide).
Halogens (Group 17), when combined with metals,
always form a negative 1 charged ion but may form
positive oxidation states when combined with
oxygen and other non-metals.
Chalcogens (Group 16), when combined with
metals, always form a negative 2 charged ion (O2-,
S2-, Se2-).
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Group 15, when combined with metals, always form
a negative 3 charged ion (N3-, P3-, As3-).
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Group 14, when combined with metals, always form
a negative 4 charged ion (C4-, Si4-).
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Hydrogen, when combined with metals, always
form a negative 1 ion (H1-) When combined with
non-metals will form a plus 1 ion (H1+) .
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The ion with the most oxygen atoms takes
the suffix –ate following the root of the first
element (i.e., nitrate for NO3-).
The ion with the least oxygen atoms takes
the suffix –ite following the root of the first
element (i.e., nitrite for NO2-).
Other examples:
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SO42PO43-
Sulfate
Phosphate
SO32PO33-
Sulfite
Phosphite
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Other important polyatomic oxygen containing
ions:
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Carbonate
CO32-
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Oxalate
C2O42-
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Acetate
C2H3O21-
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Manganate
MnO42−
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Permanganate MnO41−
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Chromate
CrO42−
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Dichromate
Cr2O729
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The ion with the most oxygen's takes the suffix –ate
following the root of the first element (i.e., chlorate
for ClO3-).
The ion with the least oxygen's takes the suffix –ite
following the root of the first element (i.e., chlorite
for ClO2-).
The ion with the one more oxygen than the –ate ion
takes the prefix per before the root of the first
element and the suffix –ate following the root of the
first element (i.e., perchlorate for ClO4-).
The ion with one less oxygen than the –ite ion takes
the prefix hypo before the root of the first element
and takes the suffix –ite following the root of the
first element (i.e., hypochlorite for ClO-).
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Diatomic Acids
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Halogen containing acids:
 These acids are named by adding hydro before
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the root of the halogen, adding –ic after the
root, and adding acid
HF(aq)
Hydrofluoric acid
HCl(aq)
Hydrochloric acid
HBr(aq)
Hydrobromic acid
HI(aq)
Hydroiodic acid
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The acid with the most oxygen's takes the suffix –ic
following the root of the first element (i.e., chloric
for HClO3) and adding acid. For HClO3 the name is
chloric acid.
The acid with the least oxygen's takes the suffix –
ous following the root of the first element (i.e.,
chlorous for HClO2) and adding acid. For HClO2 the
name is chlorous acid.
The acid with the one more oxygen than the –ic
acid takes the prefix per before the root of the first
element and the suffix –ic following the root of the
first element (i.e., perchloric for HClO4) and adding
acid. For HClO4 the name is perchloric acid.
The acid with one less oxygen than the –ous acid
takes the prefix hypo before the root of the first
element and takes the suffix –ous following the
root of the first element (i.e., hypochlorous for
HClO). For HClO the name is hypochlorous acid. 12

The acid with the most oxygen's takes the
suffix –ic following the root of the first element
and adding acid.
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Nitrate forms
Sulfate forms
Phosphate forms
HNO3(aq)
H2SO4 (aq)
H3PO4 (aq)
nitric acid
sulfuric acid
phosphoric acid
HNO2 (aq)
H2SO3 (aq)
H3PO3 (aq)
nitrous acid
sulfurous acid
phosphorous acid
The acid with the least oxygen's takes the
suffix –ous following the root of the first
element and adding acid.
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Nitrite forms
Sulfite forms
Phosphate forms
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
Carbonate ion forms H2CO3 (aq)
Carbonic acid
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Oxalate ion forms H2C2O4 (aq)
Oxalic acid
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Acetate ion forms
Acetic acid
HC2H3O2 (aq)
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Hydrates are ionic compounds with
loosely bound water molecules.
Examples:
MgSO4·2H2O, magnesium sulfate dihydrate
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MgSO4·7H2O, magnesium sulfate
heptahydrate (epsom salts)
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Na2CO3·10H2O, sodium carbonate
decahydrate (washing soda).
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The number of water molecules is given
by Greek prefixes:
Incorrect examples:
MgSO4-2H2O
Magnesium diwater
Magnesium di(dihydrogen oxide)
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Molecular (or covalent) compounds consist of two
non metal elements.
Prefixes are used to indicate the number of atoms.
The less electronegative element is named first in
covalent compounds.
The name of the second nonmetal ends in –ide.
Some nonmetals can form more than one compound.
Mono is never used if there is only 1 atom of the
first nonmetal.
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STEP 1 Name the first nonmetal by its element name.
STEP 2 Name the second nonmetal with an ide ending.
STEP 3 Prefixes to indicate the number (from
subscripts) of atoms of each nonmetal. Mono is usually
omitted.
Name P4S3
STEP 1 The first nonmetal P is phosphorus.
STEP 2 The second nonmetal S is sulfide.
STEP 3 The subscript 4 of P is shown as tetra.
The subscript 3 of O is shown as tri.
P4S3 → tetraphosphorus trisulfide
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Write the formula for carbon disulfide.
STEP 1 Elements are C and S
STEP 2 No prefix for carbon means 1 C
Prefix di = 2 means 2 S
Formula: CS2
Other Examples:
Phosphorus pentachloride:
1P
penta = 5Cl
PCl5
Dinitrogen trioxide:
di = 2N
tri = 3 O
N2O3
Xenon tetrafluoride:
1Xe
tetra = 4F
XeF4
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Identify each compound as ionic or molecular, and give its
correct name:
A. SO2
B. BaCl2
C. N2O4
D. Cu2CO3
E. Ca3(PO4)2
molecular: 1 S, 2 O sulfur dioxide
ionic: Ba2+, Cl− barium chloride
molecular: 2 N, 4 O dinitrogen tetroxide
ionic: copper(I) carbonate
ionic: Ca2+, PO43− calcium phosphate
F. FeBr3
ionic: Fe3+, Br −
G. SCl2
molecular: 1 S, 2 Cl
H. Cl2O
molecular: 2 Cl, 1 O dichlorine oxide
iron(III) bromide
sulfur dichloride
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