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Presentation of 12 pages for the course Unit 13 - Applications of Inorganic Chemistry at PEARSON (distinction level)
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2021-23 Unit 13 LA C Transition Metal ComplexesIntroduction
I work as an analytical technician for Yorkshire Water. I've been asked to create a reaction
scheme that my department may use to test water during the wastewater treatment
process in order to identify specific transition metal complexes that may be present. To
demonstrate the accuracy of my reaction scheme, I will deliver it to your colleagues in a
presentation with an accompanying report.
Transition metals
The periodic table's d-block contains a group of metallic elements known as transition
metals. They differ from other elements in that they have partially filled d orbitals in their
atomic electron configuration. One of their distinctive qualities is the capacity for many
oxidation states, which enables them to produce ions with various charges. Their ability to
adapt in chemical reactions results from this characteristic. Due to the availability of their
partially filled d orbitals, transition metals are also well recognised for their high propensity to
form complex ions and compounds. These compounds frequently exhibit bright colours and
have many uses in industries like pigments, dyes, and catalysis. Additionally, transition
metals have metallic qualities such a metallic sheen, high melting and boiling temperatures,
and great thermal and electrical conductivity. They can be applied in a variety of industrial
settings as a result. Their ability to serve as catalysts in a variety of chemical reactions is
another important characteristic. As a result, they are essential in industries like chemical
manufacture and energy production. Overall, transition metals demonstrate their distinctive
electrical configurations and varied features by playing key roles in a variety of sectors.
a propensity to create complicated ions and compounds because their partially filled d
orbitals are available.
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Vanadium (transition metal) Mercury (not a transition metal)
Solid Liquid
[Ar] 4s2 3d3 [Xe] 4f14 5d10 6s2
Forms at least 1 ion with partially filled D Forms 1 ion with full D subshell
subshell
Yellow flame Red flame
Mercury, a non-transition metal, is the only metal that is a liquid at room temperature,
whereas vanadium, a transition metal, exhibits multiple oxidation states, forms coloured
compounds, and exhibits catalytic activity. Mercury and vanadium are classified differently
and have different properties within the periodic table. Vanadium exhibits the normal
characteristics of transition metals, such as complex formation and varied magnetic
behaviour, while mercury exhibits low electropositive character and restricted reactivity.
Certain distinctions bring attention to how certain elements differ from one another in terms
of their electrical structure, chemistry, and uses.
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Ligands- A species that possesses a single pair of electrons that it can donate to a certain
metal ion in order to form a coordinate or dative bond in a complex ion for example water is
a ligand.
, 2021-23 Unit 13 LA C Transition Metal Complexes
Complex ion- A complex is made up of a metal ion in the centre surrounded by ligands that
have formed coordinate bonds with the metal for example hexaaquacopper is a complex ion.
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Complex ions
When transition chemicals are present in a solution, complex ions are created. A complex
ion is a metal ion that is surrounded by ligands (Clark, J., 2003). The term "ligand" means
molecules or ions that may form coordinate, covalent, or dative bonds with the metal ion by
donating a single pair of electrons. Every ligand works as a Lewis base (Clark, J., 2003).
According to the Lewis theory of acids and bases, a base is an electron pair donor (Clark. J,
2002) and an acid is an electron pair acceptor (Clark. J, 2003).
When there are covalent bonds between two atoms and one of the atoms gives both sets of
electrons to form a dative link (Clark. J., 2003), the bond is known as a coordinate bond or a
dative covalent bond. Water (H2O) is a common example of a ligand because it includes two
lone pairs of electrons that are donated to the metal ion. However, other ligands, such as
ammonia, chloride, and hydroxide ions, follow the same pattern (Brainscape, no date). One
thing that all ligands have in common is that they all have at least one lone pair of electrons
in their outer shell or energy level (Clark. J, 2003).
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Shape and bonding
For instance, [Co(H2O)6]2+ is the complex ion formed when cobalt (II) salts dissolve in
water. In this example, Co stands in for cobalt, and the ligands are shown in brackets. The
coordination number, which is indicated by the number outside the brackets, counts the
number of coordinate links. The overall charge is presented outside the square brackets,
indicating that this example is a complex ion. The diagram below gives a good example of
this.
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Images demonstrating complex ion shapes
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