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Complex Ions: Structure, Coordination, Shapes, Ligands, and Spectrochemical Series, Study notes of Applied Chemistry

The Royal Conservatoire of Scotland (RCS)Applied Chemistry

The topic of complex ions, including their structure, coordination number, shapes, definition of ligands, coordinate covalent bonds, and the role of ligands as Lewis bases. Additionally, it explains why certain ligands cause specific d orbital splittings and wavelengths of light absorption, leading to the colors of complex ions. Topics include the hexaaquaaluminium (III) ion, EDTA4-, and the spectrochemical series.

Typology: Study notes

2021/2022

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MSJChem – Topic 3 – Complex ions
Complex ions
1) Describe the structure of a complex ion.
2) A complex ion has a coordination number of 6 – how many
coordinate bonds are formed to the central metal ion?
3) Deduce the shape of the complex ion below:
4) Define the term
ligand.
5) How does a coordinate covalent bond differ from a conventional
covalent bond?
6) Explain how ligands are also able to act as Lewis bases.
7) Explain why EDTA4- is classified as a hexadentate ligand.
8) Explain why the Tetrachlorocuprate(II) ion has a charge of 2-
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MSJChem – Topic 3 – Complex ions

Complex ions

  1. Describe the structure of a complex ion.
  2. A complex ion has a coordination number of 6 – how many coordinate bonds are formed to the central metal ion?
  3. Deduce the shape of the complex ion below:
  4. Define the term ligand. 5 ) How does a coordinate covalent bond differ from a conventional covalent bond? 6 ) Explain how ligands are also able to act as Lewis bases. 7 ) Explain why EDTA^4 -^ is classified as a hexadentate ligand. 8 ) Explain why the Tetrachlorocuprate(II) ion has a charge of 2 -

MSJChem – Topic 3 – Complex ions Answers:

  1. A complex ions consists of a central metal ion bonded to ligands by coordinate covalent bonds.
  2. The coordination number is the number of coordinate bonds from the ligands to the central metal ion. A coordination number of 6 means that there are 6 coordinate bonds between the ligands and central metal ion.
  3. The hexaaquaaluminium (III) ion has a coordination number of 6, therefore its shape is octahedral.
  4. A ligand is a species with a lone pair of electrons that forms a coordinate bond to a central metal ion. Ligands can be negative ions (CN-) or neutral molecules (NH 3 ). 5 ) In a coordinate covalent bond, both atoms in the bond come from one atom. In a conventional covalent bond, each atom supplies one electron in the bond. 6 ) Ligands have lone pairs of electrons, therefore they can act as Lewis bases. The central metal ion is classed as the Lewis acid. 7 ) EDTA^4 -^ has 6 lone pairs of electrons, therefore it can form 6 coordinate bonds with the central metal ion. 8 ) The ligands (Cl-) bonded to the copper ion have a charge of - 1. The charge on the copper ion is 2+ (oxidation number +2). There are 4 Cl-^ ligands giving a total charge of 4 - , therefore (2+) + (4-) = 2-

MSJChem – Topic 3 – Spectrochemical series **Answers:

  1. CN-**^ > H 2 O > OH-^ > S^2 -^ > I- Decreasing d orbital splitting The higher the ligand is in the electrochemical series, the greater the splitting of the d orbitals. Therefore CN-^ would produce the greatest splitting of the d orbitals, and I

- **the least.

  1. CN-**^ < H 2 O < OH-^ < S^2 -^ < I- Decreasing wavelength of light absorbed x The higher up in the electrochemical series, the greater the splitting of the d orbitals and the greater energy difference between the two sets of d orbitals. x As energy increases, wavelength decreases, therefore a complex ion with CN-^ ligands would absorb the shortest wavelength (greatest energy) of light and I-^ the longest wavelength (lowest energy). 3) x As the ligand changes from H 2 O to NH 3 , the wavelength of light absorbed decreases. x NH 3 is higher up in the spectrochemical series, therefore it produces the greatest splitting of the d orbitals, and the greatest energy difference between the 2 sets of d orbitals. x The energy that the electrons absorb to transition between the two sets of d orbitals increases from H 2 O to NH 3 , therefore the wavelength of light absorbed decreases.

MSJChem – Topic 3 – Colour of complex ions

Colour of complex ions

**1) Explain why copper (II) sulfate (CuSO4(aq)) forms a blue solution but a solution of zinc sulfate (ZnSO4(aq)) is colourless.

  1. [Fe(H 2 O) 6 ]3+**^ (hexaaquairon (III) ion) forms a yellow solution. Use the colour wheel below to explain why the hexaaquairon (III) ion is coloured.