13C
, Transition metals
Transition metals are d-block elements that form ions with an incomplete d-subshell.
Key properties of transition metals- • Varying stages of oxidation (vanadium: +2, +3, +4, +5).
• Colored compounds because of electron transitions and d-orbital splitting.
• Reaction catalytic activity (e.g., Fe in Haber process).
Mercury vs vanadium
• Mercury (Hg): Not a transition metal since d-orbital splitting is prevented by the entire dⁱ⁰
configuration of its usual oxidation states (+1, +2).
• Vanadium (V): A transition metal due to its various oxidation states (+2, +3, +4, +5) and incomplete
d-orbitals.
- Ligands and complex ions
Ligand: An ion or molecule that forms a coordination bond with a transition metal by giving it a lone
pair.
• Monodentate: H₂O, NH₃, Cl⁻, and other compounds that bind through a single atom.
• Bidentate: Forms a bond with two atoms (e.g., oxalate, ethylenediamine).
• Polydentate: Forms bonds with several atoms (EDTA⁴⁻, for example).
• Complex Ion: [Cu(H₂O) ₆] ²⁺ is an example of a core metal ion around by ligands.
Square backet notation of complex ions
To show metal-ligand coordination, complexes are written in square brackets (e.g., [Cr (NH₃) ₆] ³⁺, [Fe
(CN)₆] ³⁻).
Shapes of Transition Metal Complexes
• Octahedral (Coordination Number: 6) – Common for small ligands (e.g., H₂O, NH₃).
• Example: [Co(H₂O) ₆] ²⁺ (Hexaaquacobalt (II)).
• Tetrahedral (Coordination Number: 4) – Common for larger ligands (e.g., Cl⁻).
, Transition metals
Transition metals are d-block elements that form ions with an incomplete d-subshell.
Key properties of transition metals- • Varying stages of oxidation (vanadium: +2, +3, +4, +5).
• Colored compounds because of electron transitions and d-orbital splitting.
• Reaction catalytic activity (e.g., Fe in Haber process).
Mercury vs vanadium
• Mercury (Hg): Not a transition metal since d-orbital splitting is prevented by the entire dⁱ⁰
configuration of its usual oxidation states (+1, +2).
• Vanadium (V): A transition metal due to its various oxidation states (+2, +3, +4, +5) and incomplete
d-orbitals.
- Ligands and complex ions
Ligand: An ion or molecule that forms a coordination bond with a transition metal by giving it a lone
pair.
• Monodentate: H₂O, NH₃, Cl⁻, and other compounds that bind through a single atom.
• Bidentate: Forms a bond with two atoms (e.g., oxalate, ethylenediamine).
• Polydentate: Forms bonds with several atoms (EDTA⁴⁻, for example).
• Complex Ion: [Cu(H₂O) ₆] ²⁺ is an example of a core metal ion around by ligands.
Square backet notation of complex ions
To show metal-ligand coordination, complexes are written in square brackets (e.g., [Cr (NH₃) ₆] ³⁺, [Fe
(CN)₆] ³⁻).
Shapes of Transition Metal Complexes
• Octahedral (Coordination Number: 6) – Common for small ligands (e.g., H₂O, NH₃).
• Example: [Co(H₂O) ₆] ²⁺ (Hexaaquacobalt (II)).
• Tetrahedral (Coordination Number: 4) – Common for larger ligands (e.g., Cl⁻).
