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Summary Unit 13 - Applications of Inorganic Chemistry BTEC Unit 13 Assignment 3 all criteria
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Unit 13 - Applications of Inorganic Chemistry BTEC Unit 13 Assignment 3 all criteria/distinction received.
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Moreen Mero / Unit 13 Assignment 3 / BTEC Level 3 Extended Diploma – Applied ScienceLab Report – Properties and reactions of transition metal complexes
Experiment Date: 12/01/2022
Experiment Title: Reactions of Transition Metal Complex Ions
Introduction: p7
What are transition metals?
Transition metals are found in the d-block in the periodic table, and they form stable ions, with
incomplete d-subshells. For example, vanadium V, it has the electronic configuration
1s2 2s3 2p6 3s2 3P6 4s2 3d3, it shows that it fords a stable ion with incomplete d-subshell. However, some
elements in the d-block are not transition metals, such as Mercury which has an electronic figuration
1s2 2s3 2p6 3s2 3P6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10, which is not considered as a transition metal,
because it forms a full d-subshell, but it is considered as element in the d-block. Transition metals have
high boiling and melting point, as well as have high densities. They form multiple oxidation stated and
coloured compounds. Other physical properties include strength, as transition metals are harder, and
stronger than group 1 and 2 metals. And have high electrical and heat conductivity. Transition metals
can form complex ions, by reacting with ligands. A ligand is species which has one (at least) lone pair
of electrons, that can be donated to the metal ion, so therefore dative covalent bond will form due to
this reaction.
An example of a transition metal complex ion is hexaaquacopper(II) ion Cu(H2O)6]2+
(Octahedral complex ion) the Octahedral complex shapes form when ion, of central
metal ion is forming six coordinate bonds. It can be bond with six small monodentate
ligands that form small six coordinate bonds. The copper’s oxidation state is 2+ that’s
why it is called hexaaquacopper(II) ion, and the complex ion does not carry a charge
of 2+ but the uncomplexed original ion was 2+. This complex ion forms when CuSO4
(copper sulphate) dissolves in water, therefore the copper ions will break from the
sulphate ions away and form dative covalent bonds to 6 molecules of H2O (the ligands
are the water molecules). the 3D representation bond shows that there are 6 Coordination numbers,
which are the coordinate bonds towards the central metal ion. The group of the species is shown as
square brackets and the overall charge it is been written outside those square brackets. The overall
charge does show the sum of the metal ion charge and the ligands’ charge (if ligands did have a charge)
In the 3D representative diagrams, the simple straight line lines shows a bond that it lying in the surface
plane, a thick and wedge shaped represents bond in front of this plane, and a dashed or hatched
represents bond in the back of this plane.
Another examples of transition metals complex ions:
• Tetrahedral: the shape will be tetrahedral if there are 4 coordinate bonds, and the
bond angles in tetrahedral complexes are 109.5o. an example is [CuCl4]2-
tetrachlorocopper(II) ion, as the chlorine ligands are large, therefore only 4 will fit
around the metal ion central: which is copper.
• Square planar: these complexes also form 4 four coordinate bonds, but they adapt
as a square planar geometry shape, instead of the tetrahedral shape. And the bond angles
are 90o. an example is Cisplatin: [PtCl2(NH3)2]. This is an anticancer drug.
, Moreen Mero / Unit 13 Assignment 3 / BTEC Level 3 Extended Diploma – Applied Science
Method:
The following tests Carried out on separate samples of each transition metal ion solution that have
been selected:
1. Add 2M sodium hydroxide dropwise solution until an excess is present
2. Add 2M ammonium hydroxide solution dropwise until an excess is present
3. Add 1.0M sodium carbonate solution dropwise until an excess is present
4. Add concentrated ammonia solution dropwise until an excess is present
5. Add concentrated hydrochloric acid dropwise until an excess is present
A note been made of the colours of the transition metal complexes initially, the precipitation of
insoluble compounds and any colour changes. Also, whether any precipitates dissolve in an excess of
a reagent been noted.
Results of observations: P8
The observation after adding each solution to each transition metal ion
Transition Amount added
Concentration
metal ion to each Concentration
2M NaOH 2M NH4OH 1M Na2Co3 Hydrochloric
(In each transition Ammonia
acid
test tube) metal
Before adding: Light blue Light Blue Light Blue Light Blue Light Blue
Crystal blue light crystal Very dark blue
2+ Light blue
Cu Drops added: with solids at
bottom
blue with
solids
crystals.
at top, very light
blue at bottom
Light blue
Excessive Crystal blue, Light blue Very light blue,
Light blue Light green
added: not cleat with crystals not clear
Before adding: Light pink Light pink Light pink Light pink Light pink
Light purple at
Dark-blue at Dark blue-
Dark aqua top, light
2+ Drops added: bottom. Light green, lighter at Light blue
Co blue at top
blue crystal blue at
bottom
the bottom
Green-blue,
Excessive Dark blue and Light blue and
lighter at the Dark blue Green-blue
added: clear crystals light green
bottom
Light-Green Light-Green Light-Green Light-Green Light-Green
Before adding:
yellow yellow yellow yellow yellow
Dark brown
Drops added: Yellow Light yellow yellow with brown yellow
Fe2+ solid substances
Dark yellow
Excessive Dark yellow, Yellow-light
and brown Dark yellow yellow
added: light brown brown
solids
Before adding: Light green Light green Light green Light green Light green
Fe3+ Drops added: Light yellow
Very light
Dark yellow
Dark red-
Orange at top, Dark yellow
yellow
clear at bottom
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