Defining complex ions

A complex ion is a central metal atom or ion surrounded by coordinately bonded ligands.

• A ligand is an atom, ion or molecule that donates a pair of electrons to the central metal ion.
• A coordinate bond (or dative covalent bond) is a covalent bond in which both electrons in the shared pair come from the same atom or ion.

An example of a complex ion is [Cr(H₂O)₆]³⁺; the oxygen atom of each water molecule donates a lone pair of electrons to the central Cr³⁺ ion:

Transition metal elements form complex ions because their partially filled, energetically accessible d-orbitals can accept lone pairs of electrons from ligands.

Representing complex ions

Complex ions are enclosed inside square brackets, with the overall charge of the complex shown outside the brackets.

Ligands are written in parentheses, with the number of ligands indicated as a subscript.

For example, the complex ion [Cu(NH₃)₄]²⁺ has:

• A central Cu ion.
• Four NH₃ ligands.
• An overall charge of +2.

Common coordination numbers and shapes

The number of coordinate bonds formed between the ligands and metal ion is called the coordination number.

Complex ions usually have coordination numbers of 6 or 4.

Some examples of complex ions with different coordination numbers are shown below:

The complex ion [Fe(H₂O)₆]²⁺ has a coordination number of 6 as the small water ligands can pack tightly around the central metal ion, while [CuCl₄]^2- only has a coordination number of 4 as the chloride ligands are larger, limiting the number that can fit around the copper ion.

Types of ligand

Ligands can be categorised by how many coordinate bonds they are capable of forming with metal ions:

1. Monodentate ligands - These have one lone electron pair available for bonding. Examples include H₂O, NH₃, Cl^-, and CN^-.

2. Bidentate ligands - These have two lone electron pairs available for bonding. Examples include 1,2-diaminoethane (en) and ethanedioate.

3. Multidentate ligands - These have more than two lone electron pairs available for bonding. An example includes the hexadentate ligand EDTA^2- which has six lone electron pairs available for bonding.

Ligands can also be categorised by their overall charge:

1. Neutral ligands - These are molecules or atoms such as H₂O, NH₃, and en.
2. Negatively charged ligands - These are anions such as Cl^-, CN^-, and OH^-.

Determining oxidation states

The overall charge on a complex ion is also called the total oxidation state.

The equation to calculate the oxidation state of the central metal cation is:

$\text{Oxidation state of metal cation }=\text{ Total oxidation state}-\text{ Sum of oxidation states of all ligands}$

Worked example 1 - Calculating the oxidation state of the metal cation

Determine the oxidation state of the central copper ion in the complex ion [Cu(NH₃)₄]²⁺.

Step 1: Calculate sum of oxidation states of all ligands

Each ammonia (NH₃) ligand is neutral.

There are 4 ammonia ligands, so the sum of the oxidation states of all ligands is $0\times 4=0$

Step 2: Equation

$\text{Oxidation state of metal cation }=\text{ Total oxidation state}-\text{ Sum of oxidation states of all ligands}$

Step 3: Substitution and correct evaluation

$\text{Oxidation state of Cu }=+2-0=+2$

So, the oxidation state of the central Cu ion in [Cu(NH₃)₄]²⁺is +2.

Worked example 2 - Calculating the oxidation state of the metal cation

Determine the oxidation state of the central chromium ion in the complex ion [Cr(H₂O)₄Cl₂]⁺.

Step 1: Calculate sum of oxidation states of all ligands

Each water (H₂O) ligand is neutral.

Each chloride (Cl) ligand has a charge of $-1$.

There are 4 water ligands and 2 chloride ligands, so the sum of the oxidation states of all ligands is $(0\times 4)+(-1\times 2)=-2$

Step 2: Equation

$\text{Oxidation state of metal cation }=\text{ Total oxidation state}-\text{ Sum of oxidation states of all ligands}$

Step 3: Substitution and correct evaluation

$\text{Oxidation state of Cr }=+1-(-2)=+3$

So, the oxidation state of the central Cr ion in [Cr(H₂O)₄Cl₂]⁺is +3.