• Source: IUPAC nomenclature of inorganic chemistry 2005

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




Summary


The 2005 edition replaces their previous recommendations Nomenclature The Red Book of Inorganic Chemistry, IUPAC Recommendations 1990 (Red Book I), and "where appropriate" (sic) Nomenclature of Inorganic Chemistry II, IUPAC Recommendations 2000 (Red Book II).
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 (PIN), 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 (e.g. sodium chloride)
substitutive naming based on parent hydrides (GeCl2Me2 dichlorodimethylgermane)
additive naming ([MnFO3] fluoridotrioxidomanganese)
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 (stoichiometrically) or dialuminium hexachloride (dimer)
substitutional: trichloralumane
additive: trichloridoaluminium; hexachloridodialuminium (dimer without structural information); di-μ-chlorido-tetrachlorido-1κ2Cl,2κ2Cl-dialuminium (dimer with structural information)




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Throughout the recommendations the use of the electronegativity of elements for sequencing has been replaced by a formal list which is loosely based on electronegativity.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" (with the addition of elements 112 through 118, that had not yet been named in 2005, to their respective groups):

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 (which could be diamond, graphite etc or a mixture) would be named carbon.




= Specific allotrope

=



Molecular

O2 dioxygen (acceptable name oxygen)
O3 trioxygen (acceptable name ozone)
P4 tetraphosphorus (acceptable name white phosphorus)
S6 hexasulfur (acceptable name ε-sulfur)
S8 cyclo-octasulfur (acceptable names for the polymorphic forms are α-sulfur, β-sulfur, γ-sulfur)



Crystalline form

This is specified by the element symbol followed by the Pearson symbol for the crystal form. (Note that the recommendations specifically italicize the second character.)

Cn carbon(cF8) (acceptable name diamond)
Snn tin(tI4) (acceptable name β- or white tin)
Mnn manganese(cI58) (acceptable name α-manganese)



Amorphous recognised allotropes

Examples include
Pn,. red phosphorus ; Asn, 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. (See IUPAC numerical multiplier.) 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:

PBrClI phosphorus bromide chloride iodide (phosphorus is the most electropositive, the others are all designated as electronegative and are sequenced alphabetically)
The ternary 2:1:5 compound of antimony, copper and potassium can be named in two ways depending on which element(s) are designated as electronegative.

CuK5Sb2 copper pentapotassium diantimonide, (both copper and potassium are designated as electropositive and are sequenced alphabetically)
K5CuSb2 pentapotassium diantimonide cupride (only potassium is designated as electropositive and the two electronegative elements are sequenced alphabetically) (Note the red book shows this example incorrectly)




= 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

Na+ sodium(1+)
Cr3+ chromium(3+)
Sometimes an abbreviated form of the element name has to be taken, e.g. germide for germanium as germanide refers to GeH−3.
Polyatomic cations of the same element are named as the element name preceded by di-, tri-, etc., e.g.:

Hg2+2 dimercury(2+)
Polyatomic cations made up of different elements are named either substitutively or additively, e.g.:

PH+4 phosphanium
SbF+4 tetrafluorostibanium (substitutive) or tetrafluoridoantimony(1+)
Note that ammonium and oxonium are acceptable names for NH+4 and H3O+ respectively. (Hydronium is not an acceptable name for H3O+)



Anions

Monatomic anions are named as the element modified with an -ide ending. The charge follows in brackets, (optional for 1−) e.g.:

Cl− chloride(1−) or chloride
S2− sulfide(2−)
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(2−) (or peroxide as an acceptable name)
C22− dicarbide(2−) (or acetylide as an acceptable name)
S22− disulfide(2−)
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 (substitutive), or trihydridogermanate(1−) (additive)
TeH3− tellanuide substitutive where -uide specifies anion composed of additional hydride attached to parent hydride
[PF6]− hexafluoro-λ5-phosphanuide (substitutive), or hexafluoridophosphate(1−) (additive)
SO32− trioxidosulfate(2−) (additive), or sulfite (acceptable non-systematic name)
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(·+)
N2(2·)2+ dinitrogen(2·2+)



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(1/10). Similarly other examples of lattice compounds are:

CaCl2·8NH3, calcium chloride— ammonia (1/8)
2Na2CO3·3H2O2, sodium carbonate—hydrogen peroxide (2/3)
AlCl3·4EtOH, aluminium chloride—ethanol (1/4)




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 (groups 13–17) 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.




Base hydrides






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 (hydrogen peroxide is an acceptable name)
H2PPH2, diphosphane
H3SiSiH2SiH2SiH3, tetrasilane




Rings and chains


The recommendations describe three ways of assigning "parent" names to homonuclear monocyclic hydrides (i.e single rings consisting of one element):

the Hantzsch–Widman nomenclature (the method preferred for rings of size 3–10)
"skeletal replacement nomenclature"—specifying the replacement of carbon atoms in the corresponding carbon compound with atoms of another element (e.g. silicon becomes sila, germanium, germa) and a multiplicative prefix tri, tetra, penta etc)( the method preferred for rings greater than 10)
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(6). 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 diiodo(phenyl)bismuthane
For organometallic compounds of groups 1–2 can use additive (indicating a molecular aggregate) or compositional naming. Examples are:

[BeEtH] named ethylhydridoberyllium or ethanidohydridoberyllium
[Mg(η5-C5H5)2] named bis(η5-cyclopentadienyl)magnesium, or bis(η5-cyclopentadienido)magnesium
Na(CHCH2) sodium ethenide (compositional name)
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:

Si(OH)4 tetrahydroxidosilicon (additive), or silanetetrol (substitutive) (note silicic acid is an acceptable name—orthosilicic has been dropped).
[CoCl(NH3)5]Cl2 pentaamminechloridocobalt(2+) 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"




= Examples of ligand names

=




= 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:

[CoCl(NH3)5]Cl2 pentaamminechloridocobalt(3+) chloride where ammine (NH3)precedes chloride. The central atom name(s) come after the ligands. Where there is more than one central atom it is preceded by di- tri-, tetra- etc.
Os3(CO)12, dodecacarbonyltriosmium
Where there are different central atoms they are sequenced using the electronegativity list.

[ReCo(CO)9] 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:

Al2Cl4(μ-Cl)2
di-μ-chlorido-tetrachlorido-1κ2Cl,2κ2Cl-dialuminium
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:

[Be4(μ4-O)(μ-O2CMe)6]
hexakis(μ-acetato-κO:κO′)-μ4-oxido-tetrahedro-tetraberyllium
The μ4 describes the bridging of the central oxide ion. (Note the use of the kappa convention to describe the bridging of the acetate ion where both oxygen atoms are involved.) 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(III) 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:

aqua[(ethane-1,2-diyldinitrilo-κ2N,N′)tris(acetato-κO)acetato]cobaltate(1-), 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,N′. The three bonds from oxygen are specified by tris(acetato-κO), 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. (This is formally dealt with in the recommendations). 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:

di-μ-chlorido-tetrachlorido-1κ2Cl,2κ2Cl-dialuminium, (aluminium trichloride).
tetrachlorido-1κ2Cl,2κ2Cl specifies that there are two chloride ligands on each aluminium atom.
decacarbonyl-1κ3C,2κ3C,3κ4C-di-μ-hydrido-1:2κ2H;1:2κ2H-triangulo-(3 Os—Os), (Decacarbonyldihydridotriosmium).
decacarbonyl-1κ3C,2κ3C,3κ4C shows that there are three carbonyl groups on two osmium atoms and four on the third.
di-μ-hydrido-1:2κ2H;1:2κ2H specifies that the two hydride bridge between the osmium atom 1 and osmium atom 2.




= 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:

Cr(η6-C6H6)2, named as bis(η6-benzene)chromium as all of the (contiguous) atoms in the benzene ligands are involved their position does not have to be specified
[(1,2,5,6-η)-cycloocta-1,3,5,7-tetraene](η5-cyclopentadienyl)cobalt in this only two (at positions 1 and 5) 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 (SP-4-3)-(acetonitrile)dichlorido(pyridine)platinum(II) the (SP-4-3) 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 (transition metals and zinc, cadmium and mercury).




= 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 bis(η5-cyclopentadienyl)metal (and ring-substituted analogues), 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 Ba(C5H5)2 or Sn(C5H5)2.
Examples of compounds that meet the criteria are:

vanadocene, [V(η5-C5H5)2]
chromocene, [Cr(η5-C5H5)2]
cobaltocene, [Co(η5-C5H5)2]
rhodocene, [Rh(η5-C5H5)2]
nickelocene, [Ni(η5-C5H5)2]
ruthenocene, [Ru(η5-C5H5)2]
osmocene, [Os(η5-C5H5)2]
manganocene, [Mn(η5-C5H5)2]
rhenocene, [Re(η5-C5H5)2].
Examples of compounds that should not be named as metallocenes are:

C10H10Ti
[Ti(η5-C5H5)2Cl2] is properly named dichloridobis(η5-cyclopentadienyl)titanium 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:
(3 Os—Os) in Decacarbonyldihydridotriosmium.
A pair of brackets contain a count of the bonds formed (if greater than 1), 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-(13)-Δ4-closo] can be used. this is determined by the complexity of the cluster. Some examples are shown below of descriptors and CEP equivalents. (The CEP descriptors are named for Casey, Evans and Powell who described the system.

Examples:
decacarbonyldimanganese
bis(pentacarbonylmanganese)(Mn—Mn)
dodecacarbonyltetrarhodium
tri-μ-carbonyl-1:2κ2C;1:3κ2C;2:3κ2C-nonacarbonyl-
1κ2C,2κ2C,3κ2C,4κ3C-[Td-(13)-Δ4-closo]-tetrarhodium(6 Rh—Rh)
or tri-μ-carbonyl-1:2κ2C;1:3κ2C;2:3κ2C-nonacarbonyl-
1κ2C,2κ2C,3κ2C,4κ3C-tetrahedro-tetrarhodium(6 Rh—Rh)




Inorganic acids






= Hydrogen names

=
The recommendations include a description of hydrogen names for acids. The following examples illustrate the method:

HNO3 hydrogen(nitrate)
H2SO4 dihydrogen(sulfate)
HSO−4 hydrogen(sulfate)(2−)
H2S dihydrogen(sulfide)
Note that the difference from the compositional naming method (hydrogen sulfide) 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 (hydrogen atoms). If this information is to be conveyed then the additive name should be used (see the list below for examples).




= 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:

iron(II) sulfide (iron deficient)
molybdenum dicarbide (carbon excess)




= 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.

BaTiO3 (perovskite type)




= 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:

~FeS (circa or approximately)
Where there is a continuous range of composition this can be written e.g., K(Br,Cl) for a mixture of KBr and KCl and (Li2,Mg)Cl2 for a mixture of LiCl and MgCl2.
The recommendation is to use the following generalised method e.g.

CuxNi1−x for (Cu,Ni)
KBrxCl1−x for K(Br,Cl)
Note that cation vacancies in CoO could be described by CoO1−x




= 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 (the element vanadium).




= Phase nomenclature

=
To specify the crystal form of a compound or element the Pearson symbol may be used. The use of Strukturbericht (e.g. A1 etc) or Greek letters is not acceptable. The Pearson symbol may be followed by the space group and the prototype formula. Examples are:

carbon(cF 8 ), diamond
RuAl(CP22, Pm3m)(CsCl type)




Polymorphism


It is recommended that polymorphs are identified (e.g. for ZnS where the two forms zincblende (cubic) and wurtzite (hexagonal)), as ZnS(c) and ZnS(h) respectively.




Notes and references

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• IUPAC nomenclature of inorganic chemistry
• IUPAC nomenclature of inorganic chemistry 2005
• Chemical nomenclature
• International Union of Pure and Applied Chemistry
• Chirality (chemistry)
• IUPAC Color Books
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• Salt (chemistry)
• Coordination geometry
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