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7/22/2019 Report on Transition Metals
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Physical and chemical properties of transition metals and differences between
the transition metals complexes.
Preparation of a transition metal complex with a knowledge about physical
and chemical features of the transition metals and their complexes.
Aims
The main aim of this experiment is preparation of the transition metal complex. For starters, the
physical and chemical features of transition metals and their complexes need to be determined.
to determine physical properties of the transition metals,
how the transition metal complexes behave in contact with ammonia,
differences between Chromium( III) Chloride Anhydrous and Chromium (III) Chloride,
prepare a simple transition metal complex.
Introduction
The transition metals they are metals which make the transition to using the d-orbital for their
bonding . The first row d-block elements are all to reactive to occur naturally as free metals and they
form compounds with oxide ores and sulphide ores. Transition metals form one or most stable ions
which has incompletely filled d-orbital. Lewis bases which bond to metal ion and donate an electronpair to the metal are called ligands. The ligand is generally neutral, such as H2O, NH3or anionic such
as Cl-. The ligand coordinate to the metal ion to give a complex. In the first part of the experiment
the properties of the example of the transition metals will demonstrated. It will be also observed
and recorded how the transition metals complexes react with ammonia and water. In the last part of
the experiment the transition metal complex will be prepared and IR spectrum will be recorded.
Methods
Part 1
On the laboratory bench there were samples of the transition metals: Zinc, Copper, Nickel and
Iron. The physical features of the metals (colours and forms ) were recorded. Their magnetic
properties were checked using magnetic stirrer and noted. Finally, a small sample of each metal was
tested how it react with water.
Part 2
Solution of Zn, Cu, Ni and Fe sulphates and chlorides were provided on the laboratory bench. A small
sample of each of these metals were taken and a few drops of the ammonia solution were added at
a time. The physical characteristics of the solutions were recorded. Then ammonia solution was
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added until no further change were observed. Samples of Chromium (III) chloride and Chromium (III)
Chloride Anhydrous were provided on the laboratory desk. The differences between them were
studied and recorded. Firstly 1.006g of CrCl3.6H2O was added to 50ml of water, then the solution
was stirred using a stirrer hot plate. The observed details, what happens with solution were
recorded. Then an examination of 1.036 g of CrCl3 and an ammonia solution was repeated.
Part 3
In this section of the experiment, a simple transition metal complex was prepared. First, in 25 ml
conical flask, 3.084g of Ni (II) nitrate hexahydrate was dissolved in 4.0 ml of hot industrial
methylated spirits (IMS) under stirring. In a separate flask, 2.026 g of KSCN was also dissolved in 4ml
of IMS. Then, two solution were combined under stirring and 10 ml of IMS were added to them. The
mixture were cooled and a solid material was formed. Next, the resultant solid was isolated by
vacuum filtration and washed with a small volume of IMS. The filtrate ( green liquid ) was retained.
In a third conical flask, a 1:1 (by volume) mixture OF IMS and water was made and heated up gently.3.804 g KSCN was dissolved in a small volume of the IMS/water mixture. Once the KSCN has
dissolved completely, the filtrate from the previous experiment was added and the mixture was
transferred to a large beaker. The beaker was placed on a steam bath in the fume cupboard until the
solvent volume has been reduced to around 5ml. Then, the solution was cooled in an ice bath and
after a few minutes, crystals were started to form. The solution was left for 20 minutes in the ice
bath to form crystals and then were recovered by vacuum filtration. The mass of the product and the
IR spectrum were recorded.
Results 1
Part 1
Table 1. Physical characteristics of transition metals.
Elements Appearance of
elements
Magnetic properties Reactivity with water
Zn Form: bars
Colour: Silver
No magnetic No reactive
Cu Form: bars
Colour: Orange-brown
No magnetic No reactive
Ni Form: powder
Colour: Metallic- grey
Magnetic Forms a layer.
Fe Form: powder
Colour: Grey
Magnetic React very slowly
Part 2
Table 2. Physical characteristic of the transition metal solutions.
Solution (formula) Colour of solution Reaction with ammoniasolution
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Zinc chloride (ZnCl2 ) Colourless White precipitate
Ferric chloride (FeCl3) Yellow Brown-orange precipitate
Nickel chloride (NiCl2) Green Light blue precipitate
Copper sulphate (CuSO4) Light blue Light blue precipitate with a
few drops of ammonia. Adding
more ammonia changes thecolour into more blue and
solution dissolve in ammonia.
As indicates the table 2 all solutions not dissolve in ammonia. Only Copper sulphate dissolve
completely in ammonia making blue solution.
ZnCl2+NH3
Table 3. The differences between CrCl3and CrCl3.6H2O.
Complex Colour of complex Reaction with water
CrCl3 Purple, glitter, shinny Not dissolve in water
CrCl3.6H2O Green, not shinny Dissolve in water into green
solution
Regarding to the table 3, CrCl3complex not dissolve in water. Instead, CrCl3.6H2O dissolve in water
completely.
Part 3
Analysis:
As indicates the table 1 all transition metal not react with water or react very, very slowly.
Considering magnetism data, Zinc and Copper do not indicate magnetic features but Nickel and Iron
are magnetic. The magnetic properties of elements depend on their electronic configuration. Atoms
and molecules with unpaired electrons are paramagnetic and are not magnetic. Electron
configuration of Cu: 1s22s
22p
63s
23p
64s
13d
10points that Cu has an unpaired electron and is not
magnetic. Electron configuration of Zn: 1s22s22p63s23p64s23d10indicates that this metal is
diamagnetic because has paired electron and should be magnetic but is not. Electron configuration
of Ni: 1s22s
22p
63s
23p
64s
23d
8and Fe: 1s
22s
22p
63s
23p
64s
23d
6indicate that these metals are
diamagnetic because have paired electrons and they expect to be not attracted into magnetic field
but according to my results they are magnetic.
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Structure of the starting material (Ni (II) nitrate hexahydrate )
Conclusion
In this laboratory experiment, the physical characteristic of the transition metals were determined.
Our result indicates that some of the metals should have different properties (magnetizm) accordingto their electron configuration.