The document summarizes key concepts about transition elements including: 1. Transition elements are defined as elements that can form at least one stable ion with a partially filled d subshell. Common errors in defining transition elements are also discussed. 2. The electronic configurations of transition elements and their ions are covered, noting exceptions like Cr and Cu. 3. Physical properties of transition elements discussed include atomic/ionic radii, ionization energy, melting points and how they vary within the period and group.

1. Transition Elements

2. Transition Elements
The focus for Inorganic Chemistry (Gp II, VII, Transition
Elements) is the trends for the physical and chemical
properties of the elements.

3. Overview
Transition Elements
• definition
• electronic configuration
Physical Properties
• atomic/ ionic radii
• ionisation energy
• mp
Chemical Properties (4C)
• catalysts
- give examples of TE as
homo/heterogeneous catalysts
• complex ion
- definition
- ligand exchange
• coordination compound
• colour
- account for colour using CFT

4. Transition Elements
Definition
A transition element is an element that can form at least one
stable ion that has a partially filled d subshell.
Common Errors:
1. … that has partially filled d orbitals
2. define in terms of characteristics of transition elements e.g.
element that can form coloured complexes/ that can exhibit
varying oxidation states.

5. Transition Elements
Electronic Configuration
• Fill up 4s before 3d.
e.g. Ti: 1s2 2s2 2p6 3s2 3p6 3d2 4s2
• Remove from 4s before 3d.
e.g. Ti+: 1s2 2s2 2p6 3s2 3p6 3d2 4s1
• Remember the exceptions (Cr, Cu)

6. Transition Elements
Electronic Configuration
For transition metal ions, write config for the metal atom first
before removing from 4s.
e.g. Fe3+
Fe
:1s2 2s2 2p6 3s2 3p6 3d6 4s2
Fe3+ :1s2 2s2 2p6 3s2 3p6 3d5
Wrong: 1s2 2s2 2p6 3s2 3p6 3d3 4s2

7. Physical Properties
Atomic Radii
Note that in this chapter, there are 2 comparisons that we can
make where the explanations are different:
1. transition element with main group metal in same Period
2. transition element with another transition element in the
same Period.
Students often get confused and give the wrong explanation.

8. Physical Properties
A transition element has a smaller atomic radius than a main
group metal in the same period e.g. Ca and Fe
Explanation:
- Fe has more protons than Ca  nuclear charge of Fe is
higher
- Although Fe has more e–, the e– are added to the 3d
orbitals which provide poor shielding
- Increase in nuclear charge outweighs the increase in
shielding effect
 effective nuclear charge is higher for Fe

9. Physical Properties
Across the Period, the atomic radii of transition elements
remains relatively constant.
Explanation:
- Across the Period, no. of protons increases, nuclear charge
increases
- e– are added to an inner d subshell, shielding effect
increases significantly
- Increase in nuclear charge is about equal to the increase in
shielding effect  effective nuclear charge remains constant

10. Q: For TM complexes e.g. [Cu(NH3)4(H2O)2]2+, how can the 3d
and 4s accommodate all the lone pairs from the ligands?
A: TM can also use the energetically accessible 4p orbitals for
bonding.
i.e. 3d, 4s and 4p orbitals are available for bonding
 9 orbitals that can accommodate up to 18 e–

11. Q: Is TiO2+ a complex ion? How do I identify complex ions?
A: A complex ion contains ligands that are datively bonded to
the metal.
Oxo ions (ions containing the metal and oxygen only) are not
complex ions
Example: TiO2+, VO2+, Cr2O72–, MnO4–
Reason: oxygen is covalently bonded to the metal

12. Q: How do I identify ligands that are not datively bonded to the
metal?
1. Erase all the bonds between the metal and the ligands.
2. Determine if the ligands are stable chemically i.e.
stable
: H2O, NH3
unstable : OH, Cl, O (incomplete octet)
3. Ligands that are stable form dative bonds to the metal
4. Ligands that are unstable form ionic/ covalent bonds to
the metal

13. Q: How do I determine the charge on the metal in a complex?
1. Erase all the bonds between the metal and the ligands.
2. Determine if the ligands are stable chemically i.e.
stable : H2O, NH3
unstable : OH, Cl, O (incomplete octet)
3. Ligands that are stable have no charge
4. For unstable ligands, determine the charge on it
i.e. OH–, Cl–, O2–
5. Use algebraic method to determine charge on metal.

14. Example:
2+
dative bond
ionic bond
stable
unstable

15. Q: How do I identify the donor atom in polyatomic ligands?
A: Memorise. Some generalisations:
Ligands containing COO–, use oxygen with –ve charge.
For CO, CN–, SCN–, use the less electro–ve atom (in red).
In research, the donor atom is determined through (i)
quantum calculations and (ii) single crystal X-ray diffraction.

16. Q: For aq. metal ions, when do we write out the aqua ligands
and when do we not?
A: It is actually acceptable both ways i.e.
Fe2+ (aq) ≡ [Fe(H2O)6]2+
Cu2+ (aq) ≡ [Cu(H2O)6]2+

17. The aqua ligands are only shown when they are directly involved
in the reaction to emphasise their presence e.g.
Hydrolysis of water
[Fe(H2O)6]3+ + H2O  [Fe(H2O)5(OH)]2+ + H3O+
Ligand exchange
[Fe(H2O)6]3+ + 6NH3  [Fe(NH3)6]3+ + 6H2O

18. Q: Do strong ligands and strong field ligands mean the
same thing?
A: No.
Strong ligands:
- form strong bonds to the metal
- can displace weaker ligands from their complexes
(ligand
exchange reactions)

19. Q: Do strong ligands and strong field ligands mean the same
thing?
A: No.
Strong field ligands:
- cause big crystal field splitting.
However, ligands that can bind strongly to the metal usually
causes bigger splitting.