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Transition metals produce a variety of coloured ions, complexes, and compounds.The colours are useful in the qualitative analysis since they provide information about the sample makeup. A transition metal is one that produces stable ions with partially filled d orbitals. Technically, not all of the periodic table’s d block elements are transition metals according to this definition. Zinc and scandium, for example, aren’t transition metals under this definition since Zn2+ have a full d level while Sc3+ have no d electrons. Different components may give colours that differ from one another. Furthermore, differing charges of the same transition metal can produce distinct hues. Another consideration is the ligand’s chemical makeup. A metal ion with the same charge can create a varied hue depending on the ligand to which it binds.
The flame colour of metal ions
Because transition metals contain empty d orbitals, they generate colourful solutions and compounds. Because the d orbitals are degenerate, the metal ions aren’t truly coloured on their own. In other words, they all have the same energy and hence the same spectral signal. Transition metal ions become coloured as they form complexes and compounds with other molecules. When a transition metal binds with one or more neutral or negatively charged nonmetals, a complex is formed (ligands). The ligand modifies the geometry of the d orbitals. Some of the d orbitals get more energy than previously, while others lose energy. This results in an energy gap. Those gaps would absorb UV light while having no effect on visible colour. Light wavelengths that have not been absorbed flow through a complex. A molecule also reflects some light back. The apparent hues of the complexes are the consequence of a mixture of absorption, reflection, and transmission. An electron, for example, may absorb red light and get excited at a higher energy level. We would perceive a green or blue colour since the non-absorbed light is the colour reflected. Complexes of a single metal can have varied hues depending on the element’s oxidation state.
Why don’t all transition metals show colours?
However, not all oxidation states result in colour. A colourless solution is formed by a transition metal ion with zero or ten d electrons.
So, by the exact definition, zinc and scandium aren’t transition metals since Zn2+ has a full d level while Sc3+ has no d electrons.
Colours of Transition Metal Complexity
Transition metal complexes’ hues frequently change in different solvents. The colour of the complex is determined by the ligand. In water, Fe2+ It is pale green, but in a concentrated hydroxide base solution, carbonate solution, or ammonia, it produces a dark green precipitate. Co2+ dissolves in water as a pink solution, but precipitates as a blue-green solution in hydroxide base solution, a straw-coloured solution in ammonia, and a pink precipitate in carbonate solution.
Lanthanide series elements can also create colourful complexes. Lanthanides are sometimes known as inner transition metals or simply as a transition metal subclass. The colourful complexes, on the other hand, are caused by 4f electron transitions. Lanthanide complexes have pale hues that are not as impacted by the type of their ligand as transition metal complexes.
Colours of common transition metal ions in aqueous solution.
Origin of Colour of transition metal ions
splitting of the d-d orbital
When a metal ion forms a complex with ligands, the surrounding ligands interact to varying degrees with the d-orbitals within the d-subshell.
This causes a d-d orbital splitting, with some d-orbitals having a greater energy level and others having a lower energy level.
The difference in energy between the two levels happens to match the energy level of a certain colour in the visible light zone.
d-subshell that is just half filled
When the d-subshell is partly occupied (d1 to d9), an electron can transition or be promoted from a lower energy state to a higher energy level.
Because there are no electrons when there are no electrons (d0), no d-d transition is feasible.
When the d-subshell is completely filled (d10), there is no room at the higher energy level for the d-d transition to occur.
Complex ions containing transition metals are frequently coloured, whereas non-transition metal ions are not. This implies that the partially filled d orbitals must be involved in the generation of colour in some way.
Factors Influencing Transition Colour Metal assemblages
In each scenario, we will select a different metal ion for the complex’s core and alter other parameters. Colour shifts haphazardly from metal to metal over a transition series.
The ligand’s composition
The metal’s oxidation state
The Ion’s coordination
Conclusion
The presence of an unfinished (n-1)d sub shell accounts for the colour. The d-ordinals of central metal break into multiple energy levels under the impact of approaching ions towards the core metal ion. This is known as crystal field splitting. When six ions or molecules approach a metal ion (octahedral field), the d-orbitals break into two sets: one set consisting of two d-orbitals of greater energy (dx2-y2 & dz2) and the other set consisting of d-orbitals of lower energy (dxy, dyz, & dxz). Electrons in the same d-sub shell are easily promoted from one energy level to another. There is something known as a d-d transition.
The amount of energy required to excite some electrons to higher energy states within the same d-subshell corresponds to the energy of specific visible-light colours. As a result, when white light strikes the compounds, a portion of its energy corresponding to a certain colour is absorbed, the electron is elevated from lower energy to higher energy, and the surplus colour is transmitted. The seen colour is complementary to the absorbed colour.
