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Coordination Nomenclature (Worksheet)

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    Name: ______________________________

    Section: _____________________________

    Student ID#:__________________________

    Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.


    Transition metal ions and some main block elements form coordination compounds which typically consist of a coordinate complex and counter ions. Coordination complexes are composed of ligands surrounding a central metal atom or ion. The coordinate complex itself consists of a transition metal atom or ion and the surrounding ligands. The coordinate complex is always enclosed in square brackets, [ ]. The coordinate complex can be an ion, cation or anion, or a neutral complex. Counter ions are needed to produce a neutral coordinate compound if the complex is an ion.

    Ligands possess one or more donor atoms, atoms that donate the lone pair of electrons. Donor atoms may possess more than one lone pair of electrons, but only one pair is involved in the bond. An electron pair donor is referred to as a Lewis Base. The central metal atom or ion accepts the lone pair of electrons involved in the bond. An electron pair receptor is referred to as a Lewis Acid. Bonds that are formed between the ligands and the central metal atom or ion are distinctive in that the bonds of the molecule are formed with both of the electrons involved in the bond being donated by just one of the atoms involved in the bond; this is known as a coordinate covalent bond.

    Example: [Fe(OH2)6]Cl2: Hexaaquairon (II), [Fe(OH2)6]+, is a complex ion consisting of the transition metal ion Fe+2 and six attached neutral water, OH2, ligands. The oxygen atom of each water molecule has two lone pairs of electrons one of which the neutral ligand donates to the coordinate covalent bond. The oxygen atom is referred to as the donor atom. The donor atom is listed first in the chemical formula of the ligand in contrast with the normal pattern for the ordering of atoms in a chemical formula: cation then anion. Also, note that when bringing together the complex ion with the counter ion, the complex ion is always enclosed in brackets [ ] while names of common ligands are enclosed in parenthesis ( ). The counter ion in for this example is the chloride anion, Cl-.

    Many transition metal complexes are neutral, e.g., [Cu(NH3)4Cl2], and do not require counter ions.


    Determine: (1) the oxidation number for each of the transition metal atoms, (2) the charge of each cation, and (3) the charge of each anion in these compounds (if existing). You will have to consult Tables \(\PageIndex{1}\) and \(\PageIndex{2}\).

    1. [V(OH2)6](NO3)3
    2. (NH4)2[CoCl4]
    3. [Co(py)4]Br2
    4. K4[Mn(CN)6]
    5. [Co(P(CH3)3)4]2(SO4)3
    6. Ni(NH3)4Cl2

    Complex Ion Nomenclature

    The chemical formula and the chemical name for Complex cations have different rules. The complex cation chemical formula follows traditional rules for naming ionic compounds with the cation listed first. For example [Cu(OH2)6]2+, the cationic copper II ion is listed first and the neutral water ligand is listed second. Complex cation chemical names are assembled by alphabetically listing the number and name of the ligands attached to the central metal atom or ion followed by the name of the central atom and its oxidation number indicated by a Roman numeral in parenthesis, for example, hexaaquacopper (II).

    The chemical names and formulas for Complex anions follow the same rules as complex cations with one additional step. The name of the central atom is changed by adding an –ate ending and then the oxidation number in parentheses. For example: [FeF6]3-, hexafluoroferrate (III). Note here also that the Latin name for iron is used to avoid an awkward sounding name. A list of such transition metals follows in the section on naming rules.

    Ligands are ions, ionic molecules, or neutral molecules that have atoms which possess lone pairs and thus act as Lewis bases. Ligand is derived form the Latin legare meaning to bind. The lone electron pairs are donated to empty d orbitals of the transition metal atom or ion creating a coordinate covalent bond. When a ligand donates only a single pair of electrons to the metal center the ligand is referred to as monodentate. Dentate comes from the Latin dens meaning tooth. Monodentate then figuratively means single toothed. Ligands that donate two, three, four, five, or six lone pairs of electrons are collectively referred to as polydentate, and bidentate, tridentate, tetradentate, pentadentate, and sexadentate respectively. Polydentate ligands typically form five- and six-membered rings and are referred to as chelating agents and the complex is referred to as chelate. Chelate comes from the Greek chela meaning claw.

    Table \(\PageIndex{1}\): Neutral Ligands
    aqua OH2 monodentate
    ammine NH3 monodentate
    benzene C6H6 monodentate
    carbonyl CO monodentate
    nitrosyl NO monodentate
    methylamine CH3NH2 monodentate
    dimethylamine (CH3)2NH2 monodentate
    trimethylamine N(CH3)3 monodentate
    ethylenediamine or en H2NCH2CH2NH2 bidentate
    diethylenetriamine or dien NH(CH2CH2NH2)2 tridentate
    triethylenetetraamine or trien N(CH2CH2NH2)3 tetradentate
    Pyridine or py C5H5N monodentate
    2,2 ′-bipyridine or bipy (C5H4N)2 bidentate
    2,2 ′,6 ′ ,2 ′′terpyridine or terpy (C5H4N)3 tridentate
    bis(diphenylphosphine) ethylene or dppe (C6H5)2P(CH2)2P(C6H5)2 bidentate
    bis(dimethylphosphino) ethylene or dmpe (CH3)2P(CH2)2P(CH3)2 bidentate
    trimethylphosphine (PMe3) P(CH3)3 monodentate

    Many of the ligands have different protonation states when unbound, so the charge of the unbound ligands will vary depending on pH. Many of these ligands make dative bonds to the transition metal with lone pairs on nitrogens. At low pHs, these nitrogens are protonated and the ligands will not be able to bind.

    Table \(\PageIndex{2}\): Anionic Ligands
    fluoro F- monodentate
    chloro Cl- monodentate
    bromo Br- monodentate
    iodo I- monodentate
    carbonato CO32- monodentate
    cyano CN- monodentate
    hydrido H- monodentate
    hydroxo OH- monodentate
    nitro NO2- monodentate
    nitrito ONO- monodentate
    nitrato NO3- monodentate
    oxalate (ox) C2O42- bidentate
    oxo O2- monodentate
    sulfato SO42- monodentate
    thiocyanato SCN- monodentate
    azido N3- monodentate
    thiosulfato S2O32- monodentate
    acetylacetonate (acac) CH(COCH3)2- bidentate
    ethylenediaminetetraacetato (EDTA)* (COO)2N(CH2)N(COO)2-4 hexadentate

    *EDTA has multiple protonation states. For the carboxyl protons of pKa, the pKa's are pKa1 = 0.0 , pKa2 = 1.5 , pKa3 = 2.0 and Ka4 = 2.69. For the ammonium protons the pKa's are pKa5 = 6.13 and pKa6 = 10.37. At pHs below 10.24, most EDTA molecules are partially or fully protonated and is not in the anionic form that binds to metal ions.

    Coordination Number

    The number of coordinate covalent bonds formed typically ranges from two to eight depending on the charge, size, and electron configuration of the transition metal atom or ion. The coordination number may also be as low as 1 and as high as 12. The number of coordinate covalent bonds is the coordination number (CN) with two, four and six the most common coordination numbers. This may be different than the number of ligands bound to the metal since ligands may also bond via multiple sites (polydendate).


    Identify the coordination number for each transition metal in the coordination compounds below.

    1. [V(OH2)6](NO3)3
    2. (NH4)2[CoCl4]
    3. [Co(py)4]Br2
    4. K4[Mn(CN)6]
    5. [Co(P(CH3)3)4]2(SO4)3
    6. Ni(NH3)4Cl2

    Simplified IUPAC Nomenclature Rules

    1. Cations are always named before the anions.
    2. Ligands are named before the metal atom or ion.
    3. Ligand names are modified with an -o added to the root name of an anion. For neutral ligands the name of the molecule is used, with the exception of OH2, NH3, CO and NO. Names of common neutral ligands are listed in Table \(\PageIndex{1}\), and common anionic ligands are listed in Table \(\PageIndex{2}\).
    4. The prefixes mono-, di-, tri-, tetra-, penta-, and hexa- are used to denote the number of simple ligands.
    5. The prefixes bis-, tris-, tetrakis-, etc., are used for more complicated ligands or ones that already contain di-, tri-, etc.
    6. The oxidation state of the central metal ion is designated by a Roman numeral in parentheses.
    7. When more than one type of ligand is present, they are named alphabetically. Prefixes do not affect the order.
    8. If the complex ion has a negative charge, the suffix –ate is added to the name of the metal.
    9. (Advanced and not questioned in this worksheet) In the case of complex-ion isomerism the names cis, trans, fac, or mer may precede the formula of the complex-ion name to indicate the spatial arrangement of the ligands. Cis means the ligands occupy adjacent coordination positions, and trans means opposite positions just as they do for organic compounds. The complexity of octahedral complexes allows for two additional geometric isomers that are peculiar to coordination complexes. Fac means facial, or that the three like ligands occupy the vertices of one face of the octahedron. Mer means meridional, or that the three like ligands occupy the vertices of a triangle one side of which includes the central metal atom or ion.

    Nomenclature Examples:

    • [CrCl2(OH2)4]+ is the tetraaquadichlorochromium (III) ion
    • [CrCl4(OH2)2]- is the diaquatetrachlorochromate (III) ion
    • [Cr(OH2)(NH3)5]3+ is the pentaammineaquachromium (III) ion
    • [Ga(OH)Cl3]- is the trichlorohydroxogallate (III) ion
    • cis-[PtBrCl(NO2)2]2- is the cis-bromochlorodinitroplatinate (II) ion
    • trans-[Co(OH)Clen2]+ is the trans-chlorobis(ethylenediamine)hydroxo cobalt (III) ion
    • [Mn(CO)3(C6H6)]+ is the benzenetricarbonvlmanganese (I) ion
    • [Ni(CO)4] is tetracarbonylnickel (0)
    • NH4[AuCl4] is ammonium tetrachloroaurate (III)


    Put the following compounds together to give the formula of the compound.

    • Remember to use [ ] to identify the complex ion in ionic complexes.
    • Where you need a counter-ion to produce a neutral compound, use either K+ or Cl- (If you use SO4-2, you would need half amounts)
    • Remember to list the cation first, followed by anion for ionic compounds.

    Metal/charge Ligands Formula (note that the charge on the ligands are not shown; review Tables \(\PageIndex{2}\) and \(\PageIndex{2}\) to get ligand charge)

    1. V+3, four OH, and two SCN
    2. Co+2 and four Br
    3. Ru+3 and three oxalates
    4. Os+3 and three dppe ligands
    5. Ni+2 and two Br, two NH3, and two CN
    6. Fe+3 and six CN


    Name the following.

    1. K4[Ni(CN)4]
    2. (NH4)3[Fe(SCN)6]
    3. Na2[Ni(CN)4]
    4. [Fe(ox)3]3-
    5. [Co(NH3)5Cl]Br2
    6. [Cr(OH2)4Cl2]Cl
    7. [Pt(NH3)2]Cl2
    8. Na2[MoOCl4]
    9. [Cr(OH2)6](NO3)3
    10. [Fe(NH3)6]SO4
    11. (NH4)2[CoCl4]
    12. Cr(NH3)4Cl2
    13. [Co(P(CH3)3)4]2(SO4)3
    14. [Ni(OH2)6]Cl2


    Write formulas for the following.

    1. potassium hexacyanoferrate(III)
    2. sodium hexafluoroaluminate(III)
    3. pentaaquabromomanganese(III) sulfate
    4. hexaamminechromium(III) nitrate
    5. sodium tetrahydroxochromate(III)
    6. hexaammineruthenium(III) tetrachloronickelate(II)
    7. tetraamminecopper(II) pentacyanohydroxoferrate(III)
    8. potassium diaquatetrabromovanadate(III)


    Provide the name or chemical formula for the following complex compounds or ions.

    1. [Al(OH2)6]Br3
    2. [Cr(NH3)6]Cl3
    3. potassium hexafluoroferrate (III)
    4. tetrahydroxozincate (II) ion
    5. [Co(OH2)4Cl2]Cl
    6. [Cu(NH3)4]+2
    7. potassium hexachlorostannate (IV)
    8. tetraamminedichloroplatinum (IV) hexachloroplatinate (IV)

    This page titled Coordination Nomenclature (Worksheet) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Delmar Larsen via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request.