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DISTINCTION - BTEC Applied Science Unit 13 Applications of Inorganic Chemistry LA C - Investigate practically a range of reactions involving solutions of transition metal ions in order to understand the basis for their qualitative analysis.R258,14
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DISTINCTION - BTEC Applied Science Unit 13 Applications of Inorganic Chemistry LA C - Investigate practically a range of reactions involving solutions of transition metal ions in order to understand the basis for their qualitative analysis.
DISTINCTION LEVEL - BTEC Applied Science Unit 13 Applications of Inorganic Chemistry LA C - Investigate practically a range of reactions involving solutions of transition metal ions in order to understand the basis for their qualitative analysis.
Introduction: I have been requested to create a report as an analytical technician for
Yorkshire Water that devises a reaction scheme that can be used to analyse water
throughout the wastewater treatment process to detect certain transition metal complexes
that may be present.
Transition metal:
A transition metal, according to the IUPAC (International Union of Pure and Applied
Chemistry), is any element with a partly filled d electron subshell (Transition Elements | A-Level Chemistry
Revision Notes, 2022). Although the f-block elements (lanthanides and actinides, below the main
body of the periodic chart) are also transition metals, this term refers to groups 3 through 12
on the periodic table (Transition Elements | A-Level Chemistry Revision Notes, 2022). Transition metals are the
d-block elements, while lanthanides and actinides are "inner transition metals” (Transition Elements |
A-Level Chemistry Revision Notes, 2022).
Figure 01: Periodic table of elements
Mercury vs vanadium:
The symbol of Mercury is Hg and the symbol for vanadium is V. Regardless of the fact that
mercury belongs to group 12 (which is a transition metal), it is not considered a transition
metal since all of its atoms and ions have entirely filled d-orbitals (www.zigya.com, n.d.), i.e., it has
no partly filled d-orbitals in atomic state or common oxidation state (www.zigya.com, n.d.) (Hg2+).
Vanadium is considered a transition metal because there are 5 valence electrons in
vanadium that can be lost (A-LEVEL NOTES, n.d.). The capacity of transition metals to adopt
numerous oxidation states is one of their properties (A-LEVEL NOTES, n.d.). The melting point of
mercury is -38.9 °C and the boiling point is 356.7 °C (Government of Canada, 2013) ,whereas the
melting point of vanadium is 1890 °C and the boiling point is 3380 °C (Encyclopedia Britannica, n.d.).
Figure 02: Vanadium complex ion
Ligand:
1
, Unit 13 LA C Applications of Inorganic Chemistry
A ligand is a molecule or ion that donates a lone pair of electrons to establish a coordinate
bond with a transition metal. The number of coordinate bonds to the core metal atom or ion
is the coordination number (A-LEVEL NOTES, n.d.). There are three types of ligands: simple,
complex, and coordinative unsaturation (A-LEVEL NOTES, n.d.). Water, ammonia, and chloride ions
are examples of simple ligands (Clark, 2003). All of these have active lone pairs of electrons in
the outer energy level in common. The metal ion is employed to establish coordinate bonds
with them (Clark, 2003).
Figure 03: Examples of ligands.
Complex ion:
A complex ion is a species created when a central metal ion interacts with one or more
ligands, molecules, or ions that contain at least one lone pair of electrons (Chemistry LibreTexts, 2015).
The potential for small, highly charged metal ions to behave as Lewis acids and produce
complex ions is highest (Chemistry LibreTexts, 2015). The most common octahedral complexes formed
by complex ions with tiny ligands are octahedral complexes with small ligands (e.g. H2O and
NH3) (A-LEVEL NOTES, n.d.). With monodentate ligands, octahedral complexes can exhibit
cist-trans isomerism and optical isomerism with bidentate ligands (A-LEVEL NOTES, n.d.). Al(H 2O)6
is an example of a complex ion.
Figure 04: Example of a complex ion - Al(H 2O)6
Examples of transition metal complex ions formulae:
[Fe(H2O)6]2+ is an example of a complex ion. Fe2+ is the central metal ion (A-LEVEL NOTES, n.d.).
The ligands are water molecules (A-LEVEL NOTES, n.d.). Each water provides a pair of electrons
from the oxygen atom to the metal ion to create a coordination connection (A-LEVEL NOTES, n.d.).
The number of atoms, ions, or molecules that a central atom or ion retains as its closest
neighbours in a complex or coordination compound or in a crystal is known as the
coordination number (Coordination number | chemistry | Britannica, 2019). The coordination number of a
complex ion specifies how many coordinate bonds are established with the core ion. The
coordination number in [Fe(H2O)6]2+ is 6 (Coordination number | chemistry | Britannica, 2019). The overlap of an
orbital carrying a lone pair of electrons with an empty orbital on the transition metal forms the
coordinate bonds in complex ions. Complex ions can take on a variety of distinct forms
(Coordination number | chemistry | Britannica, 2019). The coordination number of a cation is the maximum
number of lone pairs of electrons it can receive (Coordination number | chemistry | Britannica, 2019). It is
determined by the size and electrical configuration of the cation, as well as the size and
charge of the ligand (Coordination number | chemistry | Britannica, 2019). The number 6 is the most popular
coordination number, however 4 and 2 are also acceptable (Coordination number | chemistry | Britannica,
2019).
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