This presentation has brief deatils for nomenclature of inorganic compounds. Anyone can easily learn nomenclature from this ppt quickly.

1. NOMENCLATURE OF INORGANIC
COMPOUNDS
Submitted By:
 Darshan Kotadiya (16BCH028)
 Dhaval Bhimbha (16BCH008)
 Arpit Patel (16BCH038)

2. What is Inorganic Compound ?
 An Inorganic compound is a chemical compound that lacks C-H bonds.
 Inorganic compounds can be defined as any compound that is not organic
compound.
 Ex: CaCl2
NaCl

3.  IUPAC nomenclature of inorganic chemistry is a systematic method of
naming inorganic chemical compounds

5. Ionic Compounds
 Compounds made of a metal and non-metal are commonly known
as Ionic Compounds.
 Where the compound name has an ending of –ide.
 Cations have positive charges while anions have negative charges.
 The net charge of any ionic compound must be zero which also
means it must be electrically neutral.

6.  These rules are for those cation having only one oxidation charge.
 There are two rules that must be followed through:
• The cation (metal) is always named first with its name unchanged.
• The anion (nonmetal) is written after the cation, modified to end in –ide.
Na+ + Cl- = NaCl
Sodium + Chlorine = Sodium Chloride
Ca2+ + 2Br- = CaBr2
Calcium + Bromine = Calcium Bromide

7.  These are oxidation charges for some metal and non-metal.
1A 2A 3A 4A 5A 6A 7A 8A
Li+ Be+2 N-3 O-2 F-
Na+ Mg+2 Al+3 P-3 S-2 Cl-
K+ Ca+2 As-3 Se-2 Br-
Rb+ Sr+2 I-
Cs+ Ba+2

8.  The transition metals may form more than one ion, thus it is needed to be
specified which particular ion we are talking about.
 This is indicated by assigning a Roman numeral after the metal. The
Roman numeral denotes the charge and the oxidation state of the
transition metal ion.
 For example, iron can form two common ions Fe2+ would be named iron
(II) and Fe3+ would be named iron (III).
 However, some of the transition metals charges have specific Latin
names.

9.  Instead of using Roman numerals, the different ions can also be
presented in plain words. The metal is changed to end in –ous or –ic.
• -ous ending is used for the lower oxidation state
• -ic ending is used for the higher oxidation state
Cu+ cuprous ion Fe2+ ferrousion
Cu2+ cupric ion Fe3+ ferricion

10. Formulasand namesof common metal ionswith morethan one ionic charge.
Formula StockName ClassicalName
Cu+ Copper (I) ion Cuprous ion
Cu2+
Copper (II) ion Cupric ion
Fe2+
Iron (II) ion Ferrous ion
Fe3+
Iron (III) ion Ferric ion
Hg+
Mercury (I) ion Mercurous ion
Hg2+ Mercury (II) ion Mercuric ion
Pb2+
Lead (II) ion Plumbous ion
Pb4+
Lead (IV) ion Plumbic ion
Sn2+
Tin (II) ion Stannous ion
Sn4+
Tin (IV) ion Stannic ion
Cr2+
Chromium (II) ion Chromousion
Cr3+
Chromium (III) ion Chromic ion
Mn2+
Manganese (II) ion Manganous ion
Mn3+
Manganese (III) ion Manganic ion
Co2
Co3
Cobalt (II) ion
Cobalt (III) ion
Cobaltousion
Cobaltic ion

11. Names of ionic compounds consist of the cation name
followed by the anion name.
CaCl2 Calciumchloride
Al(NO3)3 Aluminum nitrate

12. However, this -ous/-ic system is inadequate in some cases, so the Roman numeral
system is preferred.
This method is used commonly in naming acids, where H2SO4 is commonly known as
Sulfuric Acid, and H2SO3 is known as Sulfurous Acid.
EXAMPLE
Compound Cu2O CuO FeCl2 FeCl3
Charge Charge of copper is Charge of copper is Charge of iron is +2 Charge of iron is +3
Nomenclature Cuprous Oxide Cupric Oxide Ferrous Chloride Ferric Chloride

13. Polyatomic Ion
 Polyatomic (many-atoms) anions containing oxygen have names ending in –ate or
–ite
 These are called oxyanions
 -ate is used for the most common oxyanion of an element
 -ite is used for an oxyanion that has the same charge but one less O atoms
NO3
- Nitrate ion
SO4
2- Sulfate ion
NO2
- Nitrite ion
SO3
2- Sulfite ion

14.  Some nonmetals form a series of polyatomic ions with oxygen (all having the same
charge)
• The -ate forms (formula and charge) must be memorized. In some cases, the - ate form has
three oxygens, and in some cases four oxygens.
• The -ite form has one less oxygen that the -ate form.
• The hypo- stem -ite form has two less oxygens than the -ate form.
• The per- stem -ate form has one more oxygen than the -ate form.
• The -ide form is the monatomic anion
Formula Name
XOn
y- stem + -ate
XOn-1
y- stem + -ite
XOn-2
y- hypo- + stem + -ite
XOn+1
y- per- + stem + -ate
Xy- stem + -ide
Examples
SO4
2- sulfate
SO3
2- sulfite
SO2
2- hyposulfite
SO5
2- persulfate
S2- sulfide

15. Name: Cation Anion Formula
Ammonium ion NH4
+
Hydronium ion H3O+
Acetate ion C2H3O2
-
Arsenate ion AsO4
3-
Carbonate ion CO3
2-
Hypochlorite ion ClO-
Chlorite ion ClO2
-
Chlorate ion ClO3
-
Perchlorate ion ClO4
-
Chromate ion CrO4
2-
Dichromate ion Cr2O7
2-
Cyanide ion CN-
Hydroxide ion OH-
Nitrite ion NO2
-
Nitrate ion NO3
-
Oxalate ion C2O4
2-
Permanganate ion MnO4
-
Phosphate ion PO4
3-
Sulfite ion SO3
2-
Sulfate ion SO4
2-
Thiocyanate ion SCN-
Thiosulfate ion S2O3
2-
Name: Cation Anion Formula
Ammonium ion NH4
+
Hydronium ion H3O+
Acetate ion C2H3O2
-
Arsenate ion AsO4
3-
Carbonate ion CO3
2-
Hypochlorite ion ClO-
Chlorite ion ClO2
-
Chlorate ion ClO3
-
Perchlorate ion ClO4
-
Chromate ion CrO4
2-
Dichromate ion Cr2O7
2-
Cyanide ion CN-
Hydroxide ion OH-
Nitrite ion NO2
-
Nitrate ion NO3
-
Oxalate ion C2O4
2-
Permanganate ion MnO4
-
Phosphate ion PO4
3-
Sulfite ion SO3
2-
Sulfate ion SO4
2-
Thiocyanate ion SCN-
Thiosulfate ion S2O3
2-

16.  To combine the topic of acids and polyatomic ions, there is nomenclature of
aqueous acids. Such acids include sulfuric acid (H2SO4) or carbonic acid (H2CO3).
 To name them, follow these quick, simple rules:
• If the ion ends in -ate and is added with an acid, the acid name will have an -
ic ending.
• Examples: nitrate ion (NO3
-) + H+ (denoting formation of acid) = nitric acid (HNO3)
• If the ion ends in -ite and is added with an acid, then the acid name will have an -
ous ending.
• Example: nitrite ion (NO2
-) + H+ (denoting formation of acid) = nitrous acid
(HNO2)

17. Binary Acids
 An acid is a substance that dissociates into hydrogen ions (H+) and anions in
water.
 A quick way to identify acids is to see if there is an H (denoting hydrogen) in front
of the molecular formula of the compound.
 To name acids, the prefix hydro- is placed in front of the nonmetal modified to
end with –ic. The state of acids is aqueous (aq) because acids are found in water.

18.  It is important to include (aq) after the acids because the same compounds can be
written in gas phase with hydrogen named first followed by the anion ending with –ide.
Some common binary acids include:
HF (g) = hydrogen fluoride --> HF (aq) = hydrofluoric acid
HBr (g) = hydrogen bromide --> HBr (aq) = hydrobromic acid
HCl (g) = hydrogen chloride --> HCl (aq) = hydrochloric acid
H2S (g) = hydrogen sulfide --> H2S (aq) = hydrosulfuricacid

19.  Anions whose name ends in –ate have associated acids with an –ic ending.
 Anions whose name ends in –ite have associated acids with an –ous ending.
 Prefixes in the name ofthe anionare retained in the name ofthe acid.
ClO-
Hypochlorite ion HClO hypochlorous acid
ClO2
-
Chlorite ion HClO2 chlorous acid
ClO3
-
Chlorate ion HClO3 chloric acid
ClO4
-
Perchlorate ion HClO4 perchloric acid

20. Compounds between Nonmetals and
Nonmetals
 Compounds that consist of a nonmetal bonded
to a nonmetal are commonly known
as Molecular Compounds, where the element
with the positive oxidation state is written
first.
 In many cases, nonmetals form more than one
binary compound, so prefixes are used to
distinguish them.

21. EXAMPLE
CO = carbon monoxide
BCl3 = boron trichloride
CO2 = carbon dioxide
N2O4 = dinitrogen tetroxide
N2O5 = dinitrogen pentoxide
 The prefix mono- is not used for the first element.
 If there is not a prefix before the first element, it is assumed that there is only
one atom of that element.

22. Exercise
Name of the following compunds :
 CuS
 K3N
 SnCl2
 K2S
 CaI2
 NaI

23.  CuS Copper (II) sulfide
 K3N Potassium Nitride
 SnCl2 Tin (II) chloride
 K2S Potassium sulfide
 CaI2 Calcium Iodide
 NaI Sodium Iodide