Video Tutorial on Properties of Transition Metals, Complex ions and splitting of d orbitals for colour formation . Prepared by Lawrence Kok http://lawrencekok.blogspot.com.

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Presentation transcript:

Video Tutorial on Properties of Transition Metals, Complex ions and splitting of d orbitals for colour formation . Prepared by Lawrence Kok http://lawrencekok.blogspot.com

Transition Metals – d block elements with half/partially filled d orbitals

Properties of Transition metals Variable oxidation states Coloured Complexes Variable oxidation states Catalytic Properties Complex ions Taken from:http://www.chemguide.co.uk/inorganic/transition/features.html Taken from:http://alevelchem.com/aqa_a_level_ chemistry/unit3.5/s354/02.htm Taken from:http://elementalolympics.wordpress.com/2011/02/28/variable-oxidation- states-and-catalysts/

Properties of Transition Metals – Variable Oxidation State

Properties of Transition Metals – Complex ions formation Drawing complex ion Overall charged on complex ion metal Metal ion in the center (+ve charged) Ligands attached Dative bonds from ligands

Complex ions with diff metal ions, diff ligands, oxidation state and overall charged

How to name Complex ions and its ligands Naming of Copper (II) Complexes

Strong ligand displaces weaker ligand Complex ions with different ligands – different colours Copper with ligand water – Blue Copper with ligand ammonia – Deep Blue Copper with ligand chloride - Yellow Cobalt with ligand water – Pink Cobalt with ligand chloride - Blue

Properties of Transition Metals – Coloured Complexes Why transition metals ion complexes have different colour? Why Titanium (III) ion is violet ? Taken from: http://www.chm.bris.ac.uk/webprojects2003/rogers/998/chemlab.htm

Colour formation due to splitting of 3d orbitals by ligands Splitting of 3d orbitals by ligands – allow electronic transition from lower to higher state

Ti 3+ transmit blue/violet region BUT absorb green/orange/red Ti 3+ violet due to absorption of green/yellow region to excite electrons to higher orbital level

Cu 2+ transmit blue/violet region BUT absorb green/orange/red Cu 2+ blue due to absorption of green/yellow to excite electrons to higher level

Transition metal have different colours due to splitting of 3d orbitals presence of ligands which causes splitting partially filled 3d orbitals Why some are colourless ? Cu 2+ anhydrous – colourless Cu 1+ hydrous – colourless Zn 2+ hydrous – colourless Sc 3+ hydrous – colourless Cu 2+ hydrous - colour CuSO4 (anhydrous) without ligands - Colourless

Sc 3+ ion with ligand water - Colourless Zn 2+ ion with ligand water - Colourless

Cu 1+ ion with ligand water - Colourless Cu 2+ ion with ligand water – Colour Blue

Catalyst speed up reaction by Taken from:http://comp.chem.umn.edu/itccd/Catalytics.html Taken from:http://gcserevision101.wordpress.com/chemistry-c3/

Uses of catalyst Video on colour formation due to different ligands with different metals ion Click here to view

Acknowledgements Thanks to source of pictures and video used in this presentation Thanks to Creative Commons for excellent contribution on licenses http://creativecommons.org/licenses/ Prepared by Lawrence Kok Check out more video tutorials from my site and hope you enjoy this tutorial http://lawrencekok.blogspot.com