IUPAC nomenclature of inorganic chemistry 2005

Nomenclature of Inorganic Chemistry, IUPAC Recommendations 2005 is the 2005 version of Nomenclature of Inorganic Chemistry. It is a collection of rules for naming inorganic compounds, as recommended by the International Union of Pure and Applied Chemistry.

Summary

The 2005 edition replaces their previous recommendations Nomenclature The Red Book of Inorganic Chemistry, IUPAC Recommendations 1990 , and "where appropriate" Nomenclature of Inorganic Chemistry II, IUPAC Recommendations 2000 .
The recommendations take up over 300 pages and the full text can be downloaded from IUPAC. Corrections have been issued.
Apart from a reorganisation of the content, there is a new section on organometallics and a formal element list to be used in place of electronegativity lists in sequencing elements in formulae and names. The concept of a preferred IUPAC name, a part of the revised blue book for organic compound naming, has not yet been adopted for inorganic compounds. There are however guidelines as to which naming method should be adopted.

Naming methods

The recommendations describe a number of different ways in which compounds can be named. These are:

compositional naming
substitutive naming based on parent hydrides
additive naming

Additionally there are recommendations for the following:

naming of cluster compounds
allowed names for inorganic acids and derivatives
naming of solid phases e.g. non-stoichiometric phases

For a simple compound such as AlCl₃ the different naming conventions yield the following:

compositional: aluminium trichloride or dialuminium hexachloride
substitutional: trichloralumane
additive: trichloridoaluminium; hexachloridodialuminium ; di-μ-chlorido-tetrachlorido-1κ²Cl,2κ²Cl-dialuminium

Sequencing elements—the "electronegativity" list

Throughout the recommendations, the use of the electronegativity of elements for sequencing has been replaced by a formal list which is loosely based on electronegativity. The recommendations still use the terms electropositive and electronegative to refer to an element's relative position in this list.
A simple rule of thumb, ignoring lanthanides and actinides, is:

for two elements in different groups—then the element in the higher numbered group has higher "electronegativity"
for two elements within the same group the element with the lower the atomic number has the higher "electronegativity"
Hydrogen is fitted in to be less electronegative than any chalcogen and more electronegative than any pnictogen. Hence the formulae of water and ammonia can be written H₂O and NH₃ respectively.

The full list, from highest to lowest "electronegativity" :

Group 17 in atomic number sequence i.e. F–Ts followed by
Group 16 in atomic number sequence i.e. O–Lv followed by
H, hydrogen, followed by
Group 15 in atomic number sequence i.e. N–Mc followed by
Group 14 in atomic number sequence i.e. C–Fl followed by
Group 13 in atomic number sequence i.e. B–Nh followed by
Group 12 in atomic number sequence i.e. Zn–Cn followed by
Group 11 in atomic number sequence i.e. Cu–Rg followed by
Group 10 in atomic number sequence i.e. Ni–Ds followed by
Group 9 in atomic number sequence i.e. Co–Mt followed by
Group 8 in atomic number sequence i.e. Fe–Hs followed by
Group 7 in atomic number sequence i.e. Mn–Bh followed by
Group 6 in atomic number sequence i.e. Cr–Sg followed by
Group 5 in atomic number sequence i.e. V–Db followed by
Group 4 in atomic number sequence i.e. Ti–Rf followed by
Group 3 in atomic number sequence i.e. Sc–Y followed by
the lanthanoids in atomic number sequence i.e. La–Lu followed by
the actinoids in atomic number sequence i.e. Ac–Lr followed by
Group 2 in atomic number sequence i.e. Be–Ra followed by
Group 1 (excluding H) in atomic number sequence i.e. Li–Fr followed by
Group 18 in atomic number sequence i.e. He–Og

Determining the nomenclature to use

Note "treat separately" means to use the decision table on each component

Element names

Sample of indeterminate structure

An indeterminate sample simply takes the element name. For example a sample of carbon would be named carbon.

Specific allotrope

Molecular

O₂ dioxygen
O₃ trioxygen
P₄ tetraphosphorus
S₆ hexasulfur
S₈ cyclo-octasulfur

Crystalline form

This is specified by the element symbol followed by the Pearson symbol for the crystal form.

C_n carbon
Sn_n tin
Mn_n manganese

Amorphous recognised allotropes

Examples include
P_n,. red phosphorus ; As_n, amorphous arsenic.

Compounds

Compositional names impart little structural information and are recommended for use when structural information is not available or does not need to be conveyed.
Stoichiometric names are the simplest and reflect either the empirical formula or the molecular formula. The ordering of the elements follows the formal electronegativity list for binary compounds and electronegativity list to group the elements into two classes which are then alphabetically sequenced. The proportions are specified by di-, tri-, etc. Where there are known to be complex cations or anions these are named in their own right and then these names used as part of the compound name.

Binary compounds

In binary compounds the more electropositive element is placed first in the formula. The formal list is used. The name of the most electronegative element is modified to end in -ide and the more electropositive elements name is left unchanged.
Taking the binary compound of sodium and chlorine: chlorine is found first in the list so therefore comes last in the name. Other examples are

PCl₅ phosphorus pentachloride
Ca₂P₃ dicalcium triphosphide
NiSn nickel stannide
Cr₂₃C₆ tricosachromium hexacarbide

Ternary compounds and beyond

The following illustrate the principles.
The 1:1:1:1 quaternary compound between bromine, chlorine, iodine and phosphorus:

phosphorus bromide chloride iodide

The ternary 2:1:5 compound of antimony, copper and potassium can be named in two ways depending on which are designated as electronegative.

CuK₅Sb₂ copper pentapotassium diantimonide,
K₅CuSb₂ pentapotassium diantimonide cupride

Naming of ions and radicals

Cations

Monatomic cations are named by taking the element name and following it with the charge in brackets e.g

sodium
chromium

Sometimes an abbreviated form of the element name has to be taken, e.g. germide for germanium as germanide refers to.
Polyatomic cations of the same element are named as the element name preceded by di-, tri-, etc., e.g.:

dimercury

Polyatomic cations made up of different elements are named either substitutively or additively, e.g.:

phosphanium
tetrafluorostibanium or tetrafluoridoantimony
Note that ammonium and oxonium are acceptable names for and respectively.

Anions

Monatomic anions are named as the element modified with an -ide ending. The charge follows in brackets, e.g.:

Cl⁻ chloride or chloride
S²⁻ sulfide

Some elements take their Latin name as the root e.g

silver, Ag, argentide
copper, Cu, cupride
iron, Fe, ferride
tin, Sn, stannide

Polyatomic anions of the same element are named as the element name preceded by di-, tri-, etc., e.g.:

O₂²⁻ dioxide
C₂²⁻ dicarbide
S₂²⁻ disulfide

or sometimes as an alternative derived from a substitutive name e.g.

S₂²⁻ disulfanediide

Polyatomic anions made up of different elements are named either substitutively or additively, the name endings are -ide and -ate respectively e.g. :

GeH₃⁻ germanide, or trihydridogermanate
TeH₃⁻ tellanuide substitutive where -uide specifies anion composed of additional hydride attached to parent hydride⁻ hexafluoro-λ⁵-phosphanuide, or hexafluoridophosphate
SO₃²⁻ trioxidosulfate, or sulfite

A full list of the alternative acceptable non-systematic names for cations and anions is in the recommendations.
Many anions have names derived from inorganic acids and these are dealt with later.

Radicals

The presence of unpaired electrons can be indicated by a "·". For example:

He^·+ helium
N₂²⁺ dinitrogen

Naming of hydrates and similar lattice compounds

The use of the term hydrate is still acceptable e.g. Na₂SO₄·10H₂O, sodium sulfate decahydrate. The recommended method would be to name it sodium sulfate—water. Similarly other examples of lattice compounds are:

CaCl₂·8NH₃, calcium chloride— ammonia
2Na₂CO₃·3H₂O₂, sodium carbonate—hydrogen peroxide
AlCl₃·4EtOH, aluminium chloride—ethanol

Specifying proportions using charge or oxidation state

As an alternative to di-, tri- prefixes either charge or oxidation state can be used. Charge is recommended as oxidation state may be ambiguous and open to debate.

Substitutive nomenclature

This naming method generally follows established IUPAC organic nomenclature. Hydrides of the main group elements are given -ane base names, e.g. borane, BH₃. Acceptable alternative names for some of the parent hydrides are water rather than oxidane and ammonia rather than azane. In these cases the base name is intended to be used for substituted derivatives.
This section of the recommendations covers the naming of compounds containing rings and chains.

Hydrides with non-standard bonding—lambda convention

Where a compound has non standard bonding as compared to the parent hydride for example PCl₅ the lambda convention is used. For example:

PCl₅ pentachloro-λ⁵-phosphane
SF₆ hexafluoro-λ⁶-sulfane

Polynuclear hydrides

A prefix di-, tri- etc. is added to the parent hydride name. Examples are:

HOOH, dioxidane
H₂PPH₂, diphosphane
H₃SiSiH₂SiH₂SiH₃, tetrasilane

Rings and chains

The recommendations describe three ways of assigning "parent" names to homonuclear monocyclic hydrides :

the Hantzsch–Widman nomenclature
"skeletal replacement nomenclature"—specifying the replacement of carbon atoms in the corresponding carbon compound with atoms of another element
by adding the prefix cyclo to the name of the corresponding unbranched, unsubstituted chain

Boron hydrides

The stoichiometric name is followed by the number of hydrogen atoms in brackets. For example B₂H₆, diborane. More structural information can be conveyed by adding the "structural descriptor" closo-, nido-, arachno-, hypho-, klado- prefixes.

There is a fully systematic method of numbering the atoms in the boron hydride clusters, and a method of describing the position of bridging hydrogen atoms using the μ symbol.

Main group organometallic compounds

Use of substitutive nomenclature is recommended for group 13–16 main group organometallic compounds. Examples are:

AlH₂Me named methylalumane
BiI₂Ph named diiodobismuthane

For organometallic compounds of groups 1–2 can use additive or compositional naming. Examples are:

named ethylhydridoberyllium or ethanidohydridoberyllium
named bismagnesium, or bismagnesium
Na sodium ethenide

However the recommendation notes that future nomenclature projects will be addressing these compounds.

Additive nomenclature

This naming has been developed principally for coordination compounds although it can be more widely applied. Examples are:

Si₄ tetrahydroxidosilicon, or silanetetrol .
Cl₂ pentaamminechloridocobalt chloride

Recommended procedure for naming mononuclear compounds

The recommendations include a flow chart which can be summarised very briefly:

identify the central atom,
identify and name the ligands,
specify coordination mode of ligands i.e. using kappa and/or eta conventions
sequence the ligands
specify coordination geometry i.e polyhedral symbol, configuration index (using CIP rules and absolute configuration for optically active compounds.

Ligand names

Anionic ligands

If the anion name ends in -ide then as a ligand its name is changed to end in -o. For example the chloride anion, Cl⁻ becomes chlorido. This is a difference from organic compound naming and substitutive naming where chlorine is treated as neutral and it becomes chloro, as in PCl₃, which can be named as either substitutively or additively as trichlorophosphane or trichloridophosphorus respectively.
Similarly if the anion names end in -ite, -ate then the ligand names are -ito, -ato.

Neutral ligands

Neutral ligands do not change name with the exception of the following:

Water, "aqua"
Ammonia, "ammine"
Carbon monoxide bonded via carbon, "carbonyl"
Nitrogen monoxide bonded via nitrogen, "nitrosyl"

Sequence and position of ligands and central atoms

Ligands are ordered alphabetically by name and precede the central atom name. The number of ligands coordinating is indicated by the prefixes di-, tri-, tetra- penta- etc. for simple ligands or bis-, tris-, tetrakis-, etc. for complex ligands. For example:

Cl₂ pentaamminechloridocobalt chloride where ammine precedes chloride. The central atom come after the ligands. Where there is more than one central atom it is preceded by di- tri-, tetra- etc.
Os₃₁₂, dodecacarbonyltriosmium

Where there are different central atoms they are sequenced using the electronegativity list.

nonacarbonylrheniumcobalt

Bridging ligands—use of μ symbol

Ligands may bridge two or more centres. The prefix μ is used to specify a bridging ligand in both the formula and the name. For example the dimeric form of aluminium trichloride:
200px
This example illustrates the ordering of bridging and non bridging ligands of the same type. In the formula the bridging ligands follow the non bridging whereas in the name the bridging ligands precede the non bridging. Note the use of the kappa convention to specify that there are two terminal chlorides on each aluminium.

Bridging index

Where there are more than two centres that are bridged a bridging index is added as a subscript. For example in basic beryllium acetate which can be visualised as a tetrahedral arrangement of Be atoms linked by 6 acetate ions forming a cage with a central oxide anion, the formula and name are as follows:
The μ₄ describes the bridging of the central oxide ion. In the name where a ligand is involved in different modes of bridging, the multiple bridging is listed in decreasing order of complexity, e.g. μ₃ bridging before μ₂ bridging.

Kappa, κ, convention

The kappa convention is used to specify which ligand atoms are bonding to the central atom and in polynuclear species which atoms, both bridged and unbridged, link to which central atom. For monodentate ligands there is no ambiguity as to which atom is forming the bond to the central atom. However when a ligand has more than one atom that can link to a central atom the kappa convention is used to specify which atoms in a ligand are forming a bond. The element atomic symbol is italicised and preceded by kappa, κ. These symbols are placed after the portion of the ligand name that represents the ring, chain etc where the ligand is located. For example:

pentaamminenitrito-κO-cobalt specifies that the nitrite ligand is linking via the oxygen atom

Where there is more than one bond formed from a ligand by a particular element a numerical superscript gives the count. For example:

aquacobaltate, the cobalt anion formed with water and pentadentate edta, which links via two nitrogen atoms and three oxygen atoms. There are two bonds from nitrogen atoms in edta which is specified by -κ²N,''''. The three bonds from oxygen are specified by tris, where there is one ligation per acetate.

In polynuclear complexes the use of the kappa symbol is extended in two related ways. Firstly to specify which ligating atoms bind to which central atom and secondly to specify for a bridging ligand which central atoms are involved. The central atoms must be identified, i.e. by assigning numbers to them.. To specify which ligating atoms in a ligand link to which central atom, the central atom numbers precede the kappa symbol, and numerical superscript specifies the number of ligations and this is followed by the atomic symbol. Multiple occurrences are separated by commas.
Examples:

Eta, η, convention

The use of η to denote hapticity is systematised. The use of η¹ is not recommended. When the specification of the atoms involved is ambiguous the position of the atoms must be specified. This is illustrated by the examples:

Cr₂, named as bischromium as all of the atoms in the benzene ligands are involved their position does not have to be specified
cobalt in this only two of the four double bonds are linked to the central atom.

Coordination geometry

For any coordination number above 2 more than one coordination geometry is possible. For example four coordinate coordination compounds can be tetrahedral, square planar, square pyramidal or see-saw shaped. The polyhedral symbol is used to describe the geometry. A configuration index is determined from the positions of the ligands and together with the polyhedral symbol is placed at the beginning of the name. For example in the complex -dichloridoplatinum the at the beginning of the name describes a square planar geometry, 4 coordinate with a configuration index of 3 indicating the position of the ligands around the central atom. For more detail see polyhedral symbol.

Organometallic groups 3–12

Additive nomenclature is generally recommended for organometallic compounds of groups 3-12.

Metallocenes

Following on from ferrocene—the first sandwich compound with a central Fe atom coordinated to two parallel cyclopentadienyl rings—names for compounds with similar structures such as osmocene and vanadocene are in common usage. The recommendation is that the name-ending ocene should be restricted to compounds where there are discrete molecules of bismetal, where the cyclopentadienyl rings are essentially parallel, and the metal is in the d-block. The terminology does NOT apply to compounds of the s- or p-block elements such as Ba₂ or Sn₂.
Examples of compounds that meet the criteria are:

Examples of compounds that should not be named as metallocenes are:

C₁₀H₁₀Ti
is properly named dichloridobistitanium NOT titanocene dichloride

Polynuclear cluster compounds

Metal-metal bonds

In polynuclear compounds with metal-metal bonds these are shown after the element name as follows:
in Decacarbonyldihydridotriosmium.
A pair of brackets contain a count of the bonds formed, followed by the italicised element atomic symbols separated by an "em-dash".

Polynuclear cluster geometry

The geometries of polynuclear clusters can range in complexity. A descriptor e.g. tetrahedro or the CEP descriptor e.g. Td--Δ⁴-closo] can be used. this is determined by the complexity of the cluster. Some examples are shown below of descriptors and CEP equivalents. -Δ⁴-closo]56octahedro6triprismo8antiprismo8dodecahedro12icosahedro
Examples:
decacarbonyldimanganese 200px
bis
dodecacarbonyltetrarhodium 200px
tri-μ-carbonyl-1:2κ²C;1:3κ²C;2:3κ²C-nonacarbonyl-
1κ²C,2κ²C,3κ²C,4κ³C--tetrarhodium

or tri-μ-carbonyl-1:2κ²C;1:3κ²C;2:3κ²C-nonacarbonyl-
1κ²C,2κ²C,3κ²C,4κ³C-tetrahedro-tetrarhodium

Inorganic acids

Hydrogen names

The recommendations include a description of hydrogen names for acids. The following examples illustrate the method:
Note that the difference from the compositional naming method as in hydrogen naming there is NO space between the electropositive and electronegative components.
This method gives no structural information regarding the position of the hydrons. If this information is to be conveyed then the additive name should be used.

List of acceptable names

The recommendations give a full list of acceptable names for common acids and related anions. A selection from this list is shown below.

Solids

Stoichiometric phases are named compositionally. Non-stoichiometric phases are more difficult. Where possible formulae should be used but where necessary naming such as the following may be used:
*

Mineral names

Generally mineral names should not be used to specify chemical composition. However a mineral name can be used to specify the structure type in a formula e.g.
*

Approximate formulae and variable composition

A simple notation may be used where little information on the mechanism for variability is either available or is not required to be conveyed:

Where there is a continuous range of composition this can be written e.g., for a mixture of and and for a mixture of and.
The recommendation is to use the following generalised method e.g.

Note that cation vacancies in could be described by

Point defects (Kröger–Vink) notation

Point defects, site symmetry and site occupancy can all be described using Kröger–Vink notation, note that the IUPAC preference is for vacancies to be specified by V rather than V.

Phase nomenclature

To specify the crystal form of a compound or element the Pearson symbol may be used. The use of Strukturbericht or Greek letters is not acceptable. The Pearson symbol may be followed by the space group and the prototype formula. Examples are:

, diamond

Polymorphism

It is recommended that polymorphs are identified and wurtzite ), as and respectively.