Transition metals and Transition
elements
Learning Outcomes
Revision
1. Recall the different
physical and chemical
properties of TM to other
metals
You must be able to
• Calculate oxidation
states
• Write Electron
configurations
• Recall Metallic bonding
• Recall properties of
group 2 elements
2. Write Electron
Configurations for
elements and their ions
3. Apply variable oxidation
states to explain the
properties of the TM
THE FIRST ROW TRANSITION ELEMENTS
Using your periodic table, not of the internet
Location of Transition metals band position on the periodic table
•
•
•
Located between S-block elements and P-block elements
Central of the periodic table
Starting with Sc and ending with Zn in the first row
THE FIRST ROW TRANSITION ELEMENTS
Definition
D-block elements forming one or more stable ions with
partially filled (incomplete) d-sub shells.
The first row runs from scandium to zinc filling the 3d orbitals.
Properties arise from an incomplete d sub-shell in atoms or ions
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
m. pt / °C
63
850
1400
1677
1917
1903
1244
1539
1495
density /
g cm-3
0.86
1.55
3
4.5
6.1
7.2
7.4
7.9
8.9
Physical and chemical properties of transition
metals compared to other metals on the periodic
table
S-block metals compared to d-block metals are remarkably
opposite. If you use your periodic table to identify some d-block
metals, you should be able to recall the properties of these
metals. For instance recall the physical properties Fe, which is
used to make buildings and cars etc. How do the properties
compare to group 1 and 2 metals?
Furthermore the chemical properties varies with the transition
metals. Group 1 and 2 metals have fixed corresponding oxidation
states. Their ions form colourless solutions and rarely are used
for industrial processes compared to transition metals. When
reacted with anions they usually form ionic compounds that are
white solids.
Chemical
Physical
Group 1
and 2
Appearance
Density
Melting/boiling
points
Hard or Soft
Tensile strength
Mechanical
properties
Oxidation states
Colour of ion
solutions
Colour of ionic solids
Industrial uses
Transition
metals
Chemical
Physical
Group 1 and 2
Appearance
Density
Melting/boiling
points
Hard or Soft
Tensile strength
Mechanical
properties
Oxidation states
Colour of ion
solutions
Colour of ionic solids
Industrial uses
Transition
metals
Shiny
Low
Shiny
High
Low
High
Soft
Low
Hard
High
Poor
Good
1 or 2
Variable
Colourless
Coloured
White
Some
Coloured
A lot
THE FIRST ROW TRANSITION ELEMENTS
Why is there a difference in the physical properties between
transition and other metals of the periodic tables?
Metallic
properties
all the transition elements are metals
strong metallic bonds due to small ionic size and close packing
higher melting, boiling points and densities than s-block metals
THE FIRST ROW TRANSITION ELEMENTS
Why is there a difference in the physical properties between
transition and other metals of the periodic tables?
Metallic
properties
all the transition elements are metals
strong metallic bonds due to small ionic size and close packing
higher melting, boiling points and densities than s-block metals
e-
e-
Effect of Alloying on TM’s
SS CI 11.5 The d block
9
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, …..
Location
of 3dacross
elements
bandtable,
position
on the periodic table
However, it can be
easier to read
the periodic
but remember
that the first transition metal row is 3d:
1s
1s
2s
2p
3s
3p
4s
3d
4s fills and
empties before 3d
4p
Located between 4s and 4p elements
Recall the electron configurations of the follow elements using your periodic table
and finger:
How does a glass fill with a liquid (e.g. Water or beer)?
1) Li
2) N
3) F
10) Co
11)Cu
12) Zn
4)Mg
5)Cl
6)Ca
7) V
8) Cr
9) Mn
1) Li
2) N
3) F
10) Co
11)Cu
12) Zn
4)Mg
5)Cl
6)Ca
7) V
8) Cr
K
1s2 2s2 2p6 3s2 3p6 4s1
Ca
1s2 2s2 2p6 3s2 3p6 4s2
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
V
1s2 2s2 2p6 3s2 3p6 4s2 3d3
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
9) Mn
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
POTASSIUM
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s1
‘Aufbau’
Principle
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
CALCIUM
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
SCANDIUM
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d1
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
TITANIUM
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d2
HUND’S RULE OF
MAXIMUM MULTIPLICITY
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
VANADIUM
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d3
HUND’S RULE OF
MAXIMUM MULTIPLICITY
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
CHROMIUM
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s1 3d5
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
MANGANESE
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d5
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
IRON
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d6
HUND’S RULE OF
MAXIMUM MULTIPLICITY
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
COBALT
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d7
HUND’S RULE OF
MAXIMUM MULTIPLICITY
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
NICKEL
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d8
HUND’S RULE OF
MAXIMUM MULTIPLICITY
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
COPPER
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s1 3d10
HUND’S RULE OF
MAXIMUM MULTIPLICITY
ELECTRONIC CONFIGURATIONS OF THE FIRST ROW TRANSITION METALS
ZINC
INCREASING ENERGY /
DISTANCE FROM
NUCLEUS
4f
4
4d
4p
3d
4s
3
3p
1s2 2s2 2p6 3s2 3p6 4s2 3d10
The electron goes into the 4s to restore its filled state and complete the 3d and 4s
orbital filling.
Chromium and Copper
• Cr and Cu don’t fit the pattern of building up the
3d sub-shell, why?
• In the ground state electrons are always arranged
to give lowest total energy
• Electrons are negatively charged and repel each
other
• Lower total energy is obtained with e- singly in
orbitals rather than if they are paired in an
orbital
• Energies of 3d and 4s orbitals very close
together in Period 4
SS CI 11.5 The d block
25
Chromium and Copper
• At Cr
– Orbital energies such that putting one e- into
each 3d and 4s orbital gives lower energy than
having 2 e- in the 4s orbital
• At Cu
– Putting 2 e- into the 4s orbital would give a
higher energy than filling the 3d orbitals
SS CI 11.5 The d block
26
ELECTRONIC CONFIGURATIONS
K
1s2 2s2 2p6 3s2 3p6 4s1
Ca
1s2 2s2 2p6 3s2 3p6 4s2
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
V
1s2 2s2 2p6 3s2 3p6 4s2 3d3
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
ELECTRONIC CONFIGURATIONS of metal ions
What is a transition metal?
• Transition metals [TM’s] have characteristic
properties
– e.g. coloured compounds, variable oxidation states
• These are due to presence of an inner incomplete d
sub-shell
• Electrons from both inner d sub-shell and outer s
sub-shell can be involved in compound formation
SS CI 11.5 The d block
29
THE FIRST ROW TRANSITION ELEMENTS
Definition
D-block elements forming one or more stable ions with
partially filled (incomplete) d-sub shells.
The first row runs from scandium to zinc filling the 3d
orbitals.
Chemical properties arise from an incomplete d sub-shell in
atoms or ions
This definition leads to the properties of the transitions metals
ELECTRONIC CONFIGURATIONS
Write electron configuration for Cr and Cu
K
1s2 2s2 2p6 3s2 3p6 4s1
Ca
1s2 2s2 2p6 3s2 3p6 4s2
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
V
1s2 2s2 2p6 3s2 3p6 4s2 3d3
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
5.4.1 – PROPERTIES OF TRANSITION METALS?
1) They exhibit variable oxidation states.
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
+1
+3
+2
+2
+2
+2
+2
+2
+2
+3
+3
+3
+3
+3
+3
+3
+3
+4
+4
+2
+4
+5
+6
+6
+6
+7
SS CI 11.5 The d block
32
5.4.1 – PROPERTIES OF TRANSITION METALS?
2) They form coloured ions.
COLOURED IONS
A characteristic of transition metals is their ability to form coloured compounds
COLOURED IONS
A characteristic of transition metals is their ability to form coloured compounds
Theory
ions with a d10 (full) or d0 (empty) configuration are colourless
ions and partially filled d-orbitals tend to be coloured
it is caused by the ease of transition (jumping) of electrons between
energy levels
energy is absorbed when an electron is promoted to a higher level
the frequency of light is proportional to the energy difference
COLOURED IONS
A characteristic of transition metals is their ability to form coloured compounds
Theory
ions with a d10 (full) or d0 (empty) configuration are colourless
ions and partially filled d-orbitals tend to be coloured
it is caused by the ease of transition (jumping) of electrons between
energy levels
energy is absorbed when an electron is promoted to a higher level
the frequency of light is proportional to the energy difference
ions with
or
d10 (full) Cu+,Ag+ Zn2+
d0 (empty) Sc3+ configuration are colourless
e.g. titanium(IV) oxide TiO2 is white
colour depends on ...
transition element
oxidation state
ligand
coordination number
3d ORBITALS
There are 5 different orbitals of the d variety
xy
xz
x2-y2
yz
z2
COLOURED IONS
The observed colour of a solution depends on the wavelengths absorbed
Absorbed colour
VIOLET
BLUE
BLUE-GREEN
YELLOW-GREEN
YELLOW
ORANGE
RED
nm
400
450
490
570
580
600
650
Observed colour
GREEN-YELLOW
YELLOW
RED
VIOLET
DARK BLUE
BLUE
GREEN
nm
560
600
620
410
430
450
520
How to measure the absorbance of white
light using a colorimeter
COLOURED IONS
a solution of copper(II)sulphate
COLOURED IONS
a solution of nickel(II)sulphate
5.4.1 – PROPERTIES OF TRANSITION METALS?
3) They form complexes (ligands form co-ordinate bonds to
the metal ion).
[Cu(H2O)6]2+
OH2
H2O
H2O
Cu
OH2
[CuCl4]2Cl
2+
OH2
OH2
2-
Cu
Cl
Cl
Cl
COMPLEX IONS - LIGANDS
Formation
ligands form co-ordinate bonds to a central transition metal ion
COMPLEX IONS - LIGANDS
Formation
ligands form co-ordinate bonds to a central transition metal ion
Ligands
atoms, or ions, which possess lone pairs of electrons
form co-ordinate bonds to the central ion
donate a lone pair into vacant orbitals on the central species
COMPLEX IONS - LIGANDS
Formation
ligands form co-ordinate bonds to a central transition metal ion
Ligands
atoms, or ions, which possess lone pairs of electrons
form co-ordinate bonds to the central ion
donate a lone pair into vacant orbitals on the central species
Ligand
chloride
cyanide
hydroxide
oxide
water
ammonia
Formula
Cl¯
NC¯
HO¯
O2H2O
NH3
Name of ligand
chloro
cyano
hydroxo
oxo
aqua
ammine
5.4.1 – PROPERTIES OF TRANSITION METALS?
4) They show catalytic activity.
e.g.
Ni
V2O5
Fe
Pt, Pd
margarine production
making SO3 for H2SO4
Haber process to make NH3
catalytic converters
Write an answer to the statement below.
Minimum of 500 words (one side of A4) and
include diagrams.
Font size 12 normal
Do not copy and paste of the internet!
Add references (not included in the word
count)
Using the concept of variable oxidation
states, explain the properties of the
Transition Metals
COMPLEX IONS - LIGANDS
Multidentate
form several co-ordinate bonds
HAEM
A complex containing iron(II) which
is responsible for the red colour in
blood and for the transport of
oxygen by red blood cells.
Co-ordination of CO molecules
interferes with the process
COMPLEX IONS - LIGANDS
some ligands attach themselves using two or more lone pairs
classified by the number of lone pairs they use
multidentate and bidentate ligands lead to more stable complexes
Multidentate
form several co-ordinate bonds
ISOMERISATION IN COMPLEXES
Some octahedral complexes can exist in more than one form
[MA4B2]n+
TRANS
[MA3B3]n+
CIS
ISOMERISATION IN COMPLEXES
GEOMETRICAL (CIS-TRANS) ISOMERISM
Square planar complexes of the form [MA2B2]n+ exist in two forms
trans platin
cis platin
An important anti-cancer drug. It
is a square planar, 4 co-ordinate
complex of platinum.
5.4.3 – SHAPES OF COMPLEX IONS
Geometric Isomerism
e.g. [PtCl2(NH3)2]
cis
Cl
Pt
Cl
trans
NH3
H3N
NH3
Cl
Pt
Cl
NH3
5.4.3 – SHAPES OF COMPLEX IONS
Geometric isomerism
e.g. [CoCl2(NH3)4]+
5.4.3 – SHAPES OF COMPLEX IONS
Optical Isomerism
e.g. [Co(en)3]3+
5.4.3 – SHAPES OF COMPLEX IONS
Optical Isomerism
ISOMERISATION IN COMPLEXES
OPTICAL ISOMERISM
Some octahedral complexes exist in two forms
ISOMERISATION IN COMPLEXES
OPTICAL ISOMERISM
Some octahedral complexes exist in two forms
Octahedral complexes with bidentate ligands can
exist as a pair of enantiomers (optical isomers)
ISOMERISATION IN COMPLEXES
OPTICAL ISOMERISM AND GEOMETRICAL ISOMERSIM
The complex ion [Co(en)2Cl2]+ exhibits both types of isomerism
OPTICAL
ISOMERISM
ISOMERISATION IN COMPLEXES
OPTICAL ISOMERISM AND GEOMETRICAL ISOMERSIM
The complex ion [Co(en)2Cl2]+ exhibits both types of isomerism
OPTICAL
ISOMERISM
GEOMETRICAL
ISOMERISM
CIS
TRANS
Naming complex ions
Naming complex ions is very similar to naming organic
compounds. My friends at IUPAC will help you…..
1) Simple complex ions
2) Complex complex ions (more than one ligands involved)
Standard format:
Simple complex ions
Number of ligands Name of ligand
metal ion with (charge)
e.g. [Cu(H2O)6]2+ is called the hexaaquacopper(II) ion.
Standard format:
Complex ions
Name of ligand put in alphabetic order
Number of ligands
e.g. [Cu(NH3)4(H2O)2]2+ is called the
Metal ion with (charge)
tetraamminediaquacopper(II) ion.
Naming complex ions
However, numbers are not used only numbers in words.
Test your spelling….. any mistakes
An complex with an overall positive charge is called a
Cationic complex. An overall negative charge is called an
Anionic complex
e.g. tetrachlorocuprate(II) ion.
Naming complex ions
Using the strips of paper, write the ligand code name,
code of the number of ligands and then using the third
table the name of the cation or anion. For each x2
Task to follow…..
Task
http://www.chemguide.co.uk/inorganic/complexions/shapes.html#top
Using the cut out strips make some complex ions.
1) Name them
2) Draw their shapes
3) Name the shapes and angles
CATALYTIC PROPERTIES
Transition metals and their compounds show great catalytic activity
It is due to partly filled d-orbitals which can be used to form bonds with adsorbed
reactants which helps reactions take place more easily
Examples of catalysts
IRON
Manufacture of ammonia - Haber Process
NICKEL
Hydrogenation reactions - margarine manufacture
RHODIUM
Catalytic converters
VANADIUM(V) OXIDE
Manufacture of sulphuric acid - Contact Process
FINDING COMPLEX ION FORMULAE USING COLORIMETRY
• a change of ligand can change the colour of a complex
• this property can be used to find the formula of a complex ion
FINDING COMPLEX ION FORMULAE USING COLORIMETRY
•
•
•
•
a change of ligand can change the colour of a complex
this property can be used to find the formula of a complex ion
light of a certain wavelength is passed through a solution
the greater the colour intensity, the greater the absorbance
RED
LIGHT
WHITE
LIGHT
BLUE
FILTER
SOLUTION
COLORIMETER
FINDING COMPLEX ION FORMULAE USING COLORIMETRY
•
•
•
•
•
•
a change of ligand can change the colour of a complex
this property can be used to find the formula of a complex ion
light of a certain wavelength is passed through a solution
the greater the colour intensity, the greater the absorbance
the concentration of each species in the complex is altered
the mixture with the greatest absorbance identifies ratio of ligands and ions
RED
LIGHT
WHITE
LIGHT
BLUE
FILTER
SOLUTION
COLORIMETER
FINDING COMPLEX ION FORMULAE USING COLORIMETRY
•
•
•
•
•
•
a change of ligand can change the colour of a complex
this property can be used to find the formula of a complex ion
ight of a certain wavelength is passed through a solution
the greater the colour intensity, the greater the absorbance
the concentration of each species in the complex is altered
the mixture with the greatest absorbance identifies ratio of ligands and ions
Finding the formula of an iron(III) complex
White light is passed through
a blue filter. The resulting red
light is passed through
mixtures of an aqueous
iron(III) and potassium
thiocyanate solution.
Maximum absorbance occurs
first when the ratio of Fe3+
and SCN¯ is 1:1.
This shows the complex has
the formula [Fe(H2O)5SCN]2+
FINDING COMPLEX ION FORMULAE USING COLORIMETRY
•
•
•
•
•
•
a change of ligand can change the colour of a complex
this property can be used to find the formula of a complex ion
ight of a certain wavelength is passed through a solution
the greater the colour intensity, the greater the absorbance
the concentration of each species in the complex is altered
the mixture with the greatest absorbance identifies ratio of ligands and ions
Finding the formula of an nickel(II) edta complex
Filtered light is passed
through various mixtures of
an aqueous solution of
nickel(II) sulphate and edta
solution.
The maximum absorbance
occurs when the ratio of Ni2+
and edta is 1:1.