(a)

(i)

Use the above diagrams to explain why $\mathrm{Fe}^{2+}(\mathrm{aq})$ ions are coloured, whereas $\mathrm{Zn}^{2+}(\mathrm{aq})$ ions are colourless.

[ 4 ]

[Maximum number: 1]

Copper is a transition element and has atomic number 29.

(a)

The following equilibrium exists between two complex ions of copper in the +2 oxidation state.

\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}+4 \mathrm{Cl}^{-} \rightleftharpoons\left[\mathrm{CuCl}_{4}\right]^{2-}+6 \mathrm{H}_{2} \mathrm{O}

[ 1 ]

(i)

State the colours of these two complex ions.
$\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ $\left[\mathrm{CuCl}_{4}\right]^{2-}$

[ 1 ]

(a)

(i)

State the colour of the solutions containing the following ions.
- $\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}(\mathrm{aq})$
- $\left[\mathrm{CuCl}_{4}\right]^{2-}(\mathrm{aq})$

[ 1 ]

(ii)

Octahedral complexes of $\mathrm{Cu}^{2+}$ with different ligands can have different colours.

Explain why.

[ 2 ]

[Maximum number: 6]

Iron is a transition element in the fourth period. Iron forms compounds containing the ions $\mathrm{Fe}^{2+}$ and $\mathrm{Fe}^{3+}$ .

(a)

(i)

Aqueous $\mathrm{Fe}^{3+}$ ions form coloured complexes.

Explain the origin of the colour in transition element complexes.

[ 4 ]

(b)

When an excess of $\mathrm{CN}^{-}(\mathrm{aq})$ ions is added to green $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}(\mathrm{aq})$ ions, yellow $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ complex ions are formed.

Heating $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ with dilute nitric acid and then neutralising the product with $\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})$ produces red crystals, containing the $\left[\mathrm{Fe}(\mathrm{CN})_{5} \mathrm{NO}\right]^{2-}$ complex ion.

NO is a neutral, monodentate ligand.

[ 2 ]

(i)

The two complex ions $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ and $\left[\mathrm{Fe}(\mathrm{CN})_{5} \mathrm{NO}\right]^{2-}$ are different colours.

Explain why the colours of the two complex ions are different.

[ 2 ]

(a)

$\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Cr}_{2}\left(\mathrm{O}_{2} \mathrm{CCH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]$ are both complexes of chromium(II) and have different colours.

Explain why the colours of these complexes are different.

[ 2 ]

(a)

A solution of $\mathrm{Cr}^{3+}(\mathrm{aq})$ and a solution of $\mathrm{Fe}^{3+}(\mathrm{aq})$ have different colours.

Explain why the two complexes have different colours.

[ 2 ]

(a)

Explain why chromium complexes are coloured.

[ 4 ]

(a)

The 3d orbitals in an isolated $\mathrm{Ag}^{+}$ ion are degenerate.

[ 1 ]

(i)

Define degenerate d orbitals.

[ 1 ]

(a)

The presence of electrons in d orbitals is responsible for the colours of transition element compounds.

[ 4 ]

(i)

The d orbitals in an isolated transition metal atom or ion are all at the same energy level. What term is used to describe orbitals that are at the same energy level?

(ii)

Complete the diagram to show the splitting of the d orbital energy levels in an octahedral complex ion.

(iii)

On the axes below, sketch the shapes of one d orbital from the lower energy level and one d orbital from the higher energy level.

lower energy level

higher energy level

[ 4 ]

(b)

The octahedral complex $\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ is green. Explain the origin of the colour of this complex.

[ 3 ]

(a)

(i)

The 3d orbitals in an isolated $\mathrm{Cu}^{2+}$ ion are degenerate.

Explain what is meant by the term degenerate in this context.

[ 1 ]

(ii)

Complete the diagram to describe the splitting of the 3d orbital energy levels in an octahedral complex.

$\mathrm{Cu}^{2+}$ in octahedral complex

[ 1 ]