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In chemical nomenclature , the IUPAC NOMENCLATURE OF INORGANIC CHEMISTRY is a systematic method of naming inorganic chemical compounds , as recommended by the International Union of Pure and Applied Chemistry (IUPAC). It is published in _Nomenclature of Inorganic Chemistry _ (which is informally called the Red Book). Ideally, every inorganic compound should have a name from which an unambiguous formula can be determined. There is also an IUPAC nomenclature of organic chemistry .

CONTENTS

* 1 System

* 2 Traditional naming

* 2.1 Naming simple ionic compounds

* 2.1.1 List of common ion names

* 2.2 Naming hydrates

* 2.3 Naming molecular compounds

* 2.3.1 Common exceptions

* 3 2005 revision of IUPAC\'s nomenclature for inorganic compounds * 4 Nomenclature of Inorganic Chemistry * 5 See also * 6 References * 7 External links

SYSTEM

The names "caffeine " and " 3,7-dihydro-1,3,7-trimethyl-1H-purine-2,6-dione " both signify the same chemical. The systematic name encodes the structure and composition of the caffeine molecule in some detail, and provides an unambiguous reference to this compound, whereas the name "caffeine" just names it. These advantages make the systematic name far superior to the common name when absolute clarity and precision are required. However, for the sake of brevity, even professional chemists will use the non-systematic name almost all of the time, because caffeine is a well-known common chemical with a unique structure. Similarly, H2O is most often simply called water in English, though other chemical names do exist .

* Single atom anions are named with an _-ide_ suffix: for example, H− is hydride . * Compounds with a positive ion (cation ): The name of the compound is simply the cation's name (usually the same as the element's), followed by the anion. For example, NaCl is _sodium chloride _, and CaF2 is _calcium fluoride _. * Cations which have taken on more than one positive charge are labeled with Roman numerals in parentheses. For example, Cu+ is copper(I), Cu2+ is copper(II). An older, deprecated notation is to append _-ous_ or _-ic_ to the root of the Latin name to name ions with a lesser or greater charge. Under this naming convention, Cu+ is cuprous and Cu2+ is cupric. For naming metal complexes see the page on complex (chemistry) .

* Oxyanions (polyatomic anions containing oxygen) are named with _-ite_ or _-ate_, for a lesser or greater quantity of oxygen, respectively. For example, NO− 2 is nitrite, while NO− 3 is nitrate. If four oxyanions are possible, the prefixes _hypo-_ and _per-_ are used: hypochlorite is ClO−, perchlorate is ClO− 4. * The prefix _bi-_ is a deprecated way of indicating the presence of a single hydrogen ion, as in "sodium bicarbonate " (NaHCO3). The modern method specifically names the hydrogen atom. Thus, NaHCO3 would be pronounced sodium hydrogen carbonate.

Positively charged ions are called cations and negatively charged ions are called anions. The cation is ALWAYS named first. Ions can be metals or polyatomic ions. Therefore, the name of the metal or positive polyatomic ion is followed by the name of the non-metal or negative polyatomic ion. The positive ion retains its element name whereas for a single non-metal anion the ending is changed to _-ide_. Example: sodium chloride, potassium oxide , or calcium carbonate .

When the metal has more than one possible ionic charge or oxidation number the name becomes ambiguous . In these cases the oxidation number (the same as the charge) of the metal ion is represented by a Roman numeral in parentheses immediately following the metal ion name. For example, in uranium(VI) fluoride the oxidation number of uranium is 6. Another example is the iron oxides. FeO is iron(II) oxide and Fe2O3 is iron(III) oxide.

An older system used prefixes and suffixes to indicate the oxidation number, according to the following scheme:

OXIDATION STATE CATIONS AND ACIDS ANIONS

Lowest _hypo- -ous_ _hypo- -ite_

_-ous_ _-ite_

_-ic_ _-ate_

_per- -ic_ _per- -ate_

Highest _hyper- -ic_ _hyper- -ate_

Thus the four oxyacids of chlorine are called hypochlorous acid (HOCl), chlorous acid (HOClO), chloric acid (HOClO2) and perchloric acid (HOClO3), and their respective conjugate bases are the hypochlorite, chlorite, chlorate and perchlorate ions. This system has partially fallen out of use, but survives in the common names of many chemical compounds : the modern literature contains few references to "ferric chloride" (instead calling it "iron(III) chloride"), but names like "potassium permanganate" (instead of "potassium manganate(VII)") and "sulfuric acid" abound.

TRADITIONAL NAMING

NAMING SIMPLE IONIC COMPOUNDS

An ionic compound is named by its cation followed by its anion. See polyatomic ion for a list of possible ions.

For cations that take on multiple charges, the charge is written using Roman numerals in parentheses immediately following the element name. For example, Cu(NO3)2 is _copper(II) nitrate _, because the charge of two nitrate ions (NO− 3) is 2 × −1 = −2, and since the net charge of the ionic compound must be zero, the Cu ion has a 2+ charge. This compound is therefore copper(II) nitrate. In the case of cations with a +4 oxidation state, the only acceptable format for the Roman numeral 4 is IV and not IIII.

The Roman numerals in fact show the oxidation number , but in simple ionic compounds (i.e., not metal complexes ) this will always equal the ionic charge on the metal. For a simple overview see , for more details see selected pages from IUPAC rules for naming inorganic compounds.

List Of Common Ion Names

Monatomic anions: Cl− chloride S2− sulfide P3− phosphide

Polyatomic ions : NH+ 4 ammonium H 3O+ hydronium NO− 3 nitrate NO− 2 nitrite ClO− hypochlorite ClO− 2 chlorite ClO− 3 chlorate ClO− 4 perchlorate SO2− 3 sulfite SO2− 4 sulfate HSO− 3 hydrogen sulfite (or bisulfite ) HCO− 3 hydrogen carbonate (or bicarbonate ) CO2− 3 carbonate PO3− 4 phosphate HPO2− 4 hydrogen phosphate H 2PO− 4 dihydrogen phosphate CrO2− 4 chromate Cr 2O2− 7 dichromate BO3− 3 borate AsO3− 4 arsenate C 2O2− 4 oxalate CN− cyanide SCN− thiocyanate MnO− 4 permanganate

NAMING HYDRATES

Hydrates are ionic compounds that have absorbed water. They are named as the ionic compound followed by a numerical prefix and _-hydrate_. The numerical prefixes used are listed below (see IUPAC numerical multiplier ):

* mono- * di- * tri- * tetra- * penta- * hexa- * hepta- * octa- * nona- * deca-

For example, CuSO4·5H2O is "copper(II) sulfate pentahydrate".

NAMING MOLECULAR COMPOUNDS

Inorganic molecular compounds are named with a prefix (see list above) before each element. The more electronegative element is written last and with an _-ide_ suffix. For example, H2O (water) can be called _dihydrogen monoxide_. Organic molecules do not follow this rule. In addition, the prefix MONO- is not used with the first element; for example, SO2 is _sulfur dioxide_, not "monosulfur dioxide". Sometimes prefixes are shortened when the ending vowel of the prefix "conflicts" with a starting vowel in the compound. This makes the name easier to pronounce; for example, CO is "carbon monoxide" (as opposed to "monooxide").

Common Exceptions

There are a number of exceptions and special cases that violate the above rules. Sometimes the prefix is left off of the initial atom: I2O5 is known as _iodine pentoxide_, but it should be called _diiodine pentoxide_. N2O3 is called _nitrogen sesquioxide_ (_sesqui-_ means  1 1⁄2).

The main oxide of phosphorus is called _phosphorus pentoxide _. It should actually be _diphosphorus pentoxide_, but everyone knows that there are two phosphorus atoms (P2O5) needed in order to balance the oxidation numbers of the five oxygen atoms. However, people have known for years that the real form of the molecule is P4O10, not P2O5, yet it is not normally called _tetraphosphorus decaoxide_.

In writing formulas, _ammonia_ is NH3 even though nitrogen is more electronegative. Likewise, _methane_ is written as CH4 even though carbon is more electronegative.

2005 REVISION OF IUPAC\'S NOMENCLATURE FOR INORGANIC COMPOUNDS

Main article: IUPAC nomenclature of inorganic chemistry 2005

NOMENCLATURE OF INORGANIC CHEMISTRY

_ The front cover of the 2005 edition of the Red Book_

_Nomenclature of Inorganic Chemistry_, by chemists commonly referred to as the _RED BOOK_, is a collection of recommendations on IUPAC nomenclature, published at irregular intervals by the IUPAC. The last full edition was published in 2005, in both paper and electronic versions.

Published editions RELEASE YEAR TITLE PUBLISHER ISBN

2005 Recommendations 2005 (Red Book) RSC Publishing 0-85404-438-8

2001 Recommendations 2000 (Red Book II) (supplement) RSC Publishing 0-85404-487-6

1990 Recommendations 1990 (Red Book I) Blackwell 0-632-02494-1

1971 Definitive Rules 1970 Butterworth 0-408-70168-4

1959 1957 Rules Butterworth

1940/1941 1940 Rules Scientific journals

SEE ALSO

* IUPAC nomenclature * IUPAC nomenclature of organic chemistry * List of inorganic compounds * Water of Crystallization * IUPAC nomenclature of inorganic chemistry 2005 (the _Red Book_) * Nomenclature of Organic Chemistry (the _Blue Book_) * Quantities, Units and Symbols in Physical Chemistry (the _Green Book_) * Compendium of Chemical Terminology (the _Gold Book_) * Compendium of Analytical Nomenclature (the _Orange Book_)

REFERENCES

* ^ Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005 - Full text (PDF) 2004 version with separate chapters as pdf: IUPAC Provisional Recommendations for the Nomenclature of Inorganic Chemistry (2004) * ^ International Union of Pure and Applied Chemistry (2005). _Nomenclature of Inorganic Chemistry _ (IUPAC Recommendations 2005). Cambridge (UK): RSC –IUPAC . ISBN 0-85404-438-8 . Electronic version.

EXTERNAL LINKS

* Bibliography of IUPAC Recommendations on Inorganic

.