1. Tutorial on Properties of Transition Metals, Complex ions and splitting of 3d orbitals by ligands.
Review Lessons

2. Transition Metals (d block elements)Ca
4s2

3. Transition Metals (d block elements)Ca
4s2
Across period
Cr - 4s13d5
half filled more stable
Cu - 4s13d10
fully filled more stable

4. Transition Metals (d block elements)Ca
4s2
Across period
Cr - 4s13d5
half filled more stable
Cu - 4s13d10
fully filled more stable
Transition metal have partially filled 3d orbitals
3d and 4s electrons can be lost easily
electrons filled from 4s level first then 3d level

5. Transition Metals (d block elements)Ca
4s2
Across period
Cr - 4s13d5
half filled more stable
Cu - 4s13d10
fully filled more stable
Transition metal have partially filled 3d orbitals
3d and 4s electrons can be lost easily
electrons filled from 4s level first then 3d level
electrons lost from 4s level first then 3d level 4s 3d
Filling electrons- 4s level lower, filled first
Losing electrons- 4s higher, lose first

6. Transition Metals (d block elements)Ca
4s2
Across period
Cr - 4s13d5
half filled more stable
Cu - 4s13d10
fully filled more stable
Transition metal have partially filled 3d orbitals
3d and 4s electrons can be lost easily
electrons filled from 4s level first then 3d level
electrons lost from 4s level first then 3d level
3d and 4s energy level close together (similar in energy) 4s 3d
Filling electrons- 4s level lower, filled first
Losing electrons- 4s higher, lose first

7. Transition Metals (d block elements)
d block elements with half/partially filled d orbitals/sublevels in one or more of its oxidation states
Lose Ions
Electrons formation
Incomplete filled d orbitals

8. Transition Metals (d block elements)
d block elements with half/partially filled d orbitals/sublevels in one or more of its oxidation states
Lose Ions
Electrons formation
Sc3+
4s03d0
Zn2+
4s03d10
Incomplete filled d orbitals
Sc not transition elements.
Sc → Sc3+ - (empty d orbital)
4s23d s03d0
Zn not transition elements.
Zn → Zn2+ - (fully filled d orbital)
4s23d s03d10

9. Transition Metals (d block elements)
d block elements with half/partially filled d orbitals/sublevels in one or more of its oxidation states
Lose Ions
Electrons formation
Sc3+
4s03d0
Zn2+
4s03d10
Incomplete filled d orbitals
Sc not transition elements.
Sc → Sc3+ - (empty d orbital)
4s23d s03d0
Zn not transition elements.
Zn → Zn2+ - (fully filled d orbital)
4s23d s03d10

10. Transition Metals (d block elements)
Formation coloured complexes
Formation complex ions
Properties of Transition metals
Formation of complex ions
Formation coloured complexes
Variable oxidation states
Catalytic activity
Catalytic activity
Variable Oxidation states
Sci-Media/Images/Catalytic-converter-catalyst

11. Transition Metals (d block elements) – Variable Oxidation States
Oxidation state +2 more common on right (Co → Zn)
Harder to lose electron as Nuclear charge of Co - Zn is getting higher (NC ↑)
Oxidation state +3 more common on left (Sc → Fe)
Easier to lose electron as Nuclear charge of Sc – Fe is lower (NC ↓)
Oxidation state for Mn is highest +7
Higher oxidation state exist when elements bond to oxygen – oxides/oxyanions
(MnO4)- +7 +6
Cr2O7
(MnO4)2-
oxides
oxyanion +5
V2O5 +4
TiCI4
(VO2)2+
MnCI4 +3
ScCI3
TiCI3
VCI3
CrCI3
MnCI3
FeCI3
chlorides +2
CrCI2
MnCI2
FeCI2
CoCI2
NiCI2
CuCI2
ZnCI2 +7 +6 +6 +5 +4 +4 +3 +3 +3 +3 +3 +3 +2 +2 +2 +2 +2 +2 +2

12. Transition Metals (d block elements) – Variable Oxidation States
Oxidation state +2 more common on right (Co → Zn)
Harder to lose electron as Nuclear charge of Co - Zn is getting higher (NC ↑)
Oxidation state +3 more common on left (Sc → Fe)
Easier to lose electron as Nuclear charge of Sc – Fe is lower (NC ↓)
Oxidation state for Mn is highest +7
Higher oxidation state exist when elements bond to oxygen – oxides/oxyanions
(MnO4)- +7 +6
Cr2O7
(MnO4)2-
oxides
oxyanion +5
V2O5 +4
TiCI4
(VO2)2+
MnCI4 +3
ScCI3
TiCI3
VCI3
CrCI3
MnCI3
FeCI3
chlorides +2
CrCI2
MnCI2
FeCI2
CoCI2
NiCI2
CuCI2
ZnCI2 +7
Oxidation number increases +6 +6 +5 +4 +4 +3 +3 +3 +3 +3 +3 +2 +2 +2 +2 +2 +2 +2
+3 oxidation state more common
+2 oxidation state more common

13. Transition Metal ion + Ligands = Complex Ions
Transition Metals (d block elements) – Formation Complex Ions
Transition Metal ion + Ligands = Complex Ions
Transition Metal ion
High charged density metal ion, partially filled 3d orbital
Attract ligand (neutral, anion with lone pair electron)
Form dative/co-ordinate bond – lone pair from ligands
Ligands
Neutral/anion species that donate
lone pair/non bonding electron pair to metal ion
Lewis base, lone pair donor – dative bond with metal ion
Coordination number – number of ligands around central ion
[Cu(H2O)4]CI [Cu(H2O)4] CI- +2

14. Transition Metal ion + Ligands = Complex Ions
Transition Metals (d block elements) – Formation Complex Ions
Transition Metal ion + Ligands = Complex Ions
Transition Metal ion
High charged density metal ion, partially filled 3d orbital
Attract ligand (neutral, anion with lone pair electron)
Form dative/co-ordinate bond – lone pair from ligands
Ligands
Neutral/anion species that donate
lone pair/non bonding electron pair to metal ion
Lewis base, lone pair donor – dative bond with metal ion
Coordination number – number of ligands around central ion
[Cu(H2O)4]CI [Cu(H2O)4] CI- 2+ +
2CI-
CI2
water
Complex ion – [Cu(H2O)4]CI2 also written as CuCI2
Complex ion
4 water ligands attached
4 dative bonds
Coordination number = 4
Anion +2

15. Transition Metal ion + Ligands = Complex Ions
Transition Metals (d block elements) – Formation Complex Ions
Transition Metal ion + Ligands = Complex Ions
Transition Metal ion
High charged density metal ion, partially filled 3d orbital
Attract ligand (neutral, anion with lone pair electron)
Form dative/co-ordinate bond – lone pair from ligands
Ligands
Neutral/anion species that donate
lone pair/non bonding electron pair to metal ion
Lewis base, lone pair donor – dative bond with metal ion
Coordination number – number of ligands around central ion
[Cu(H2O)4]CI [Cu(H2O)4] CI- 2+ +
2CI-
CI2
water
Complex ion – [Cu(H2O)4]CI2 also written as CuCI2
Complex ion
4 water ligands attached
4 dative bonds
Coordination number = 4
Anion
Drawing complex ion
Overall charged on complex ion
Metal ion in the center (+ve charged)
Ligands attached
Dative bonds from ligands +2

16. Overall charge on complex ion
Complex ions with different metal ions, ligands, oxidation state and overall charged
Coordination number
Shape
Complex ion
(metal + ligand)
Ligand
(charged)
Metal ion
(Oxidation #)
Overall charge on complex ion 2
linear
[Cu(CI2)]-
CI = -1 +1 -1
[Ag(NH3)2]+
NH3 = 0
[Ag(CN)2]-
CN = -1 4
Square planar
[Cu(CI)4]2-
CI =-1 +2 -2
[Cu(NH3)4]2+
NH3=0
[Co(CI)4]2-
CI=-1
[Ni(CI)4]2-
Tetrahedral
[Zn(NH3)4]2+
NH3 =0
[Mn(CI)4]2- 6
Octahedral
[ Cu(H2O)6] 2+
H2O =0
[Fe(OH)3(H2O)3]
OH =-1
H2O = 0 +3 o
[Fe(CN)6]3-
CN =-1 -3
[Cr(NH3)4CI2]+
Types of ligands:
Monodentate – 1 lone pair electron donor – H2O, F-, CI-, NH3, OH-, CN-
Bidentate – 2 lone pair electron donor –1,2 diaminoethane H2NCH2CH2NH2, ethanedioate (C2O4)2-

17. Naming Complex ions Chloride
Step in naming complex ion - [Co(NH3)4CI2]+CI-
Tetraamine dichloro cobalt (III)
(cation part)
Cation part first → anion part later
Within a complex metal – ligands named first followed by metal ion
Name - Tetraamine dichloro cobalt (III) chloride
Chloride
(anion part)

18. Naming Complex ions Chloride Tetraaqua copper (II) Chloride
Step in naming complex ion - [Co(NH3)4CI2]+CI-
Tetraamine dichloro cobalt (III)
(cation part)
Cation part first → anion part later
Within a complex metal – ligands named first followed by metal ion
Name - Tetraamine dichloro cobalt (III) chloride
Chloride
(anion part)
Step in naming complex ion - [Cu(H2O)4]2+CI2
Tetraaqua copper (II)
(cation part)
Cation part first → anion part later
Within a complex metal – ligands named first followed by metal ion
Name - Tetraaqua copper(II) chloride
Chloride
(anion part)

19. Naming Complex ions Chloride Tetraaqua copper (II) Chloride
Step in naming complex ion - [Co(NH3)4CI2]+CI-
Tetraamine dichloro cobalt (III)
(cation part)
Cation part first → anion part later
Within a complex metal – ligands named first followed by metal ion
Name - Tetraamine dichloro cobalt (III) chloride
Chloride
(anion part)
Step in naming complex ion - [Cu(H2O)4]2+CI2
Tetraaqua copper (II)
(cation part)
Cation part first → anion part later
Within a complex metal – ligands named first followed by metal ion
Name - Tetraaqua copper(II) chloride
Chloride
(anion part)
Step in naming complex ion - [Co(H2O)6]2+SO4
Hexaaqua cobalt(II)
(cation part)
Cation part first → anion part later
Within a complex metal – ligands named first followed by metal ion
Name – Hexaaqua cobalt (II) sulphate
Sulphate
(anion part)
Step in naming complex ions with TWO different ligands
1. Name ligand (alphabetical order)
2. [Cu(NH3)4(H2O)2]2+ - tetraammine diaqua copper(II) ion. (1st ligand- ammine, 2nd ligand aqua)
3. [Al(H2O)2(OH)4]- - diaqua tetrahydroxo aluminate ion. (1st ligand – aqua, 2nd ligand hydroxo)

20. Ligand displacement Stronger ligand displace weaker ligand
Tetrachloro copper (II) ion
Tetraaqua copper (II) ion
CI- displace H2O
[Cu(H2O)4] CI → [Cu(CI)4]2-

21. Ligand displacement Stronger ligand displace weaker ligand
Tetrachloro copper (II) ion
Tetraaqua copper (II) ion
Tetraamine copper (II) ion 2+
CI- displace H2O
NH3 displace H2O
[Cu(H2O)4] CI → [Cu(CI)4]2-
[Cu(H2O)4] NH3 → [Cu(NH3)4]2+

22. Ligand displacement Stronger ligand displace weaker ligand
Tetrachloro copper (II) ion
Tetraaqua copper (II) ion
Tetraamine copper (II) ion 2+
CI- displace H2O
NH3 displace H2O
[Cu(H2O)4] CI → [Cu(CI)4]2-
[Cu(H2O)4] NH3 → [Cu(NH3)4]2+
Hexaaqua cobalt (II) ion
Tetrachloro cobalt(II) ion
CI- displace H2O
[Co(H2O)6] CI → [Cu(CI)4]2-
Tetrachloro copper (II) ion
Hexaaqua iron (III) ion

23. Why transition metals ion complexes have different colour?
Transition Metals (d block elements) – Coloured Complexes
Why transition metals ion complexes have different colour?
Taken from:

24. Why Titanium (III) ion is violet ?
Transition Metals (d block elements) – Coloured Complexes
Why transition metals ion complexes have different colour?
Why Titanium (III) ion is violet ?
Taken from:

25. Transition Metals (d block elements) – Coloured Complexes
Colour formation due to splitting of 3d orbitals of metal ion by ligands
Absence of ligands
3d orbitals same energy level
five 3d orbitals are equal in energy
Five 3d orbitals

26. Transition Metals (d block elements) – Coloured Complexes
Colour formation due to splitting of 3d orbitals of metal ion by ligands
Absence of ligands
3d orbitals same energy level
five 3d orbitals are equal in energy
Presence of ligands
3d orbitals split
five 3d orbitals unequal in energy
Five 3d orbitals
Five 3d orbitals
Splitting 3d orbitals

27. Transition Metals (d block elements) – Coloured Complexes
Colour formation due to splitting of 3d orbitals of metal ion by ligands
Absence of ligands
3d orbitals same energy level
five 3d orbitals are equal in energy
Presence of ligands
3d orbitals split
five 3d orbitals unequal in energy
Five 3d orbitals
Five 3d orbitals
Splitting 3d orbitals
Why Titanium (III) ion solution is violet ?
violet
No ligands
No splitting of 3d orbitals
3d orbitals equal energy

28. Transition Metals (d block elements) – Coloured Complexes
Colour formation due to splitting of 3d orbitals of metal ion by ligands
Absence of ligands
3d orbitals same energy level
five 3d orbitals are equal in energy
Presence of ligands
3d orbitals split
five 3d orbitals unequal in energy
Five 3d orbitals
Five 3d orbitals
Splitting 3d orbitals
Why Titanium (III) ion solution is violet ?
violet
No ligands
No splitting of 3d orbitals
3d orbitals equal energy
With ligands
Splitting of 3d orbitals
3d orbitals unequal energy
Splitting 3d orbitals
3d orbitals split into different energy level
Electronic transition possible
Photon of light absorbed to excite electrons

29. Ti3+ transmit blue/violet region BUT absorb green/yellow/red
Transition Metals (d block elements) – Coloured Complexes
Why Titanium (III) ion solution is violet ?
Ti3+ transmit blue/violet region BUT absorb green/yellow/red

30. Ti3+ transmit blue/violet region BUT absorb green/yellow/red
Transition Metals (d block elements) – Coloured Complexes
Why Titanium (III) ion solution is violet ?
Ti3+ transmit blue/violet region BUT absorb green/yellow/red
Light in vis region
Ti3+ transmit
blue/violet region
Electron excited
Ground state Ti3+ (3d1)
Ti3+ absorb green/yellow/red photons
to excite electrons to higher level

31. Transition Metals (d block elements) – Coloured Complexes
Why Copper (II) ion solution is blue ?
Cu2+ transmit blue/violet BUT absorb /orange/red region

32. Transition Metals (d block elements) – Coloured Complexes
Why Copper (II) ion solution is blue ?
Cu2+ transmit blue/violet BUT absorb /orange/red region
Light in vis region
Cu2+ transmit
blue/violet region
Electron excited
Ground state Cu2+ (3d9)
Cu2+ absorb orange/red photons
to excite electrons to higher level
Cu2+ appears blue
Complementary colour (Red/Orange) are absorbed to excite electron
Blue colour is transmitted

33. Transition Metals (d block elements) – Coloured Complexes
Transition metal have different colours due to
splitting of 3d orbitals by ligands
partially filled 3d orbitals for electron transition
Why some are colourless ?
Cu2+ anhydrous – colourless
Cu1+ hydrous – colourless
Zn2+ hydrous – colourless
Sc3+ hydrous – colourless

34. CuSO4 (anhydrous) without ligands - Colourless
Transition Metals (d block elements) – Coloured Complexes
Transition metal have different colours due to
splitting of 3d orbitals by ligands
partially filled 3d orbitals for electron transition
Why some are colourless ?
Cu2+ anhydrous – colourless
Cu1+ hydrous – colourless
Zn2+ hydrous – colourless
Sc3+ hydrous – colourless
CuSO4 (anhydrous) without ligands - Colourless
NO Colour
No ligands
No splitting of 3d orbitals
No electron transition
No colour

35. Transition Metals (d block elements) – Coloured Complexes
Transition metal have different colours due to
splitting of 3d orbitals by ligands
partially filled 3d orbitals for electron transition
Why some are colourless ?
Cu2+ anhydrous – colourless
Cu1+ hydrous – colourless
Zn2+ hydrous – colourless
Sc3+ hydrous – colourless
CuSO4 (anhydrous) without ligands - Colourless
NO Colour
No ligands
No splitting of 3d orbitals
No electron transition
No colour
CuSO4 (hydrous) with H2O ligands – Blue Colour
Colour
Ground state Cu2+ (3d9)
Electron transition from
lower to higher level by
absorbing ∆E
Ligands split the 3d orbitals
[Cu(H2O)6]2+ SO4 – splitting 3d orbitals by ligand – Blue colour

36. Sc 3+ ion with ligands - Colourless
Transition Metals (d block elements) – Coloured Complexes
Sc 3+ ion with ligands - Colourless
[Sc(H2O)6]3+ CI3
Empty 3d orbitals
No colour
NO Colour
No electrons in 3d orbital
No electron transition
Ground state Sc3+ (3d0)
Ligands split the 3d orbitals

37. Sc 3+ ion with ligands - Colourless Zn2+ ion with ligands - Colourless
Transition Metals (d block elements) – Coloured Complexes
Sc 3+ ion with ligands - Colourless
[Sc(H2O)6]3+ CI3
Empty 3d orbitals
No colour
NO Colour
No electrons in 3d orbital
No electron transition
Ground state Sc3+ (3d0)
Ligands split the 3d orbitals
[Zn(H2O)6]2+ SO4
Filled 3d orbitals
No colour
Zn2+ ion with ligands - Colourless
NO Colour
Fully filled in 3d orbital
No electron transition
Ground state Zn2+ (3d10)
Ligands split the 3d orbitals

38. Cu1+ ion with H2O ligands - Colourless
Transition Metals (d block elements) – Coloured Complexes
[Cu(H2O)6]1+ CI
Filled 3d orbitals
No colour
Cu1+ ion with H2O ligands - Colourless
NO Colour
Fully filled in 3d orbital
No electron transition
Ground state Cu2+ (3d10)
Ligands split the 3d orbitals

39. Transition Metals (d block elements) – Coloured Complexes
[Cu(H2O)6]1+ CI
Filled 3d orbitals
No colour
Cu1+ ion with H2O ligands - Colourless
NO Colour
Fully filled in 3d orbital
No electron transition
Ground state Cu2+ (3d10)
Ligands split the 3d orbitals
Cu2+ ion without H2O ligands – Colourless
NO Colour
No ligands
No splitting of 3d orbitals
No electron transition
No colour

40. Transition Metals (d block elements) – Coloured Complexes
[Cu(H2O)6]1+ CI
Filled 3d orbitals
No colour
Cu1+ ion with H2O ligands - Colourless
NO Colour
Fully filled in 3d orbital
No electron transition
Ground state Cu2+ (3d10)
Ligands split the 3d orbitals
Cu2+ ion without H2O ligands – Colourless
NO Colour
No ligands
No splitting of 3d orbitals
No electron transition
No colour
Cu2+ ion with H2O ligands – Blue Colour
Colour
Ground state Cu2+ (3d9)
Electron transition from
lower to higher level by
absorbing ∆E
Ligands split the 3d orbitals
[Cu(H2O)6]2+ SO4 – splitting 3d orbitals by ligand – Blue colour

41. Transition Metals (d block elements) – Catalytic Activity
Catalytic Properties of Transition metal
Variable oxidation state - lose and gain electron easily
Acts as Homogeneous or Heterogenous catalyst – lower activation energy
Homogeneous catalyst – catalyst and reactants are in the same phase
Heterogeneous catalyst – catalyst and reactants are in different phase
Heterogenous catalyst- Metal surface provide active site (lower Ea )
Surface catalyst bring molecule together (close contact)
-bond breaking/making easier
Transition metal work as a catalyst with diff oxidation states
2 H2O2 + Fe2+ → 2H2O + O2 + Fe3+
H2O2 + Fe2+ → H2O + O2 + Fe3+
Fe3+ + I - → Fe2+ + I2
Fe2+ ↔ Fe3+
Reaction is slow if only I- is added H2O2 + I- → I2 + H2O + O2
Reaction speeds up if Fe2+/Fe3+ added
Fe2+ changes to Fe3+ and is change back to Fe2+ again
recycle 3+

42. Uses of transition metal as catalyst in industrial processes
Haber Process – Production of ammonia for fertilisers and agriculture
3H2 + N2 → 2NH3
Contact Process – Sulphuric acid for fertilisers, detergent, paints and batteries
2SO2 + O2 → 2SO3
Hydrogenation Process- Margerine and trans fats
C2H4 H2 → C2H6
Hydrogen peroxide decomposition – Oxygen production
2H2O2→ 2H2O + O2
Catalytic converter – Convertion of CO and NO to CO2 and N2
2CO + 2NO → 2CO2 + N2
Biological enzymes
Hemoglobin – transport oxygen
Vitamin B12 – RBC production

43. Manganese (IV) oxide, MnO2 Platinum/Palladium, Pt/Pd
Uses of transition metal as catalyst in industrial processes
Haber Process – Production of ammonia for fertilisers and agriculture
3H2 + N2 → 2NH3
Contact Process – Sulphuric acid for fertilisers, detergent, paints and batteries
2SO2 + O2 → 2SO3
Hydrogenation Process- Margerine and trans fats
C2H4 H2 → C2H6
Hydrogen peroxide decomposition – Oxygen production
2H2O2→ 2H2O + O2
Catalytic converter – Convertion of CO and NO to CO2 and N2
2CO + 2NO → 2CO2 + N2
Biological enzymes
Hemoglobin – transport oxygen
Vitamin B12 – RBC production
Iron , Fe
Vanadium (V) oxide, V2O5
Nickel, Ni
Manganese (IV) oxide, MnO2
Platinum/Palladium, Pt/Pd
Iron , Fe
Cobalt, Co

44. Video on transition metal
Click here to view nickel ion complexes
Click here to view vanadium ion complexes
Click here to view iron in hemoglobin
Click here to view oxidation states