Introduction to Transition Metals
Transition Metals are metals that can form one or more stable ions with an incomplete d-
subshell.
A d block element can contain up to 10 electrons so transition metals must form at least one ion
that has between 1 and 9 electrons in the d-subshell. This includes elements from Titanium to
Copper.
All period 4 d-block elements are transition metals apart from Scandium and Zinc as they do
not have a complete d-subshell.
Scandium forms one ion which is Sc3+ which has an empty 3d-subshell.
Zinc forms only one stable ion of Zn2+ where it loses two electrons from the 4s
subshell and still has a full 3d orbital.
Physical Properties:
The properties of the transition metals do not gradually change across the periodic table, they
all have similar physical properties.
High Density.
High boiling/high melting point.
Chemical Properties:
Complexed Ions - causes by their property of variable oxidation states so the central metal
ions can form a variable number of ligands and bonds.
Coloured Ions - compounds of transition metals are coloured.
Catalysts - the transition metals can change to variable oxidation states by gaining or
donating electrons from a reagent in a reaction, substances can be adsorbed onto the
surface and activated.
Variable Oxidation States - form more than one positive ion which is shown by the roman
numerals which showcase the oxidation states.
Oxidation State of the Metal Ion = The total charge of the complex - The sum of the
charges of the ligands
Complex A central bonded atom surrounded by coordinately bonded ligands.
Complexed Ion Central metal ion surrounded by coordinately bonded ligands.
Ligands An atom, ion or molecule that forms a co-ordinate bond with a central
transition metal ion by donating a pair of electrons. It surrounds the metal
ion. It is the same as a nucleophile and it has a negative charge.
Monodentate Ligands that can only form one co-ordinate bond
Ligand
Bidentate ligand Ligands that can only form two coordinate bonds.
Transition Metals are metals that can form one or more stable ions with an incomplete d-
subshell.
A d block element can contain up to 10 electrons so transition metals must form at least one ion
that has between 1 and 9 electrons in the d-subshell. This includes elements from Titanium to
Copper.
All period 4 d-block elements are transition metals apart from Scandium and Zinc as they do
not have a complete d-subshell.
Scandium forms one ion which is Sc3+ which has an empty 3d-subshell.
Zinc forms only one stable ion of Zn2+ where it loses two electrons from the 4s
subshell and still has a full 3d orbital.
Physical Properties:
The properties of the transition metals do not gradually change across the periodic table, they
all have similar physical properties.
High Density.
High boiling/high melting point.
Chemical Properties:
Complexed Ions - causes by their property of variable oxidation states so the central metal
ions can form a variable number of ligands and bonds.
Coloured Ions - compounds of transition metals are coloured.
Catalysts - the transition metals can change to variable oxidation states by gaining or
donating electrons from a reagent in a reaction, substances can be adsorbed onto the
surface and activated.
Variable Oxidation States - form more than one positive ion which is shown by the roman
numerals which showcase the oxidation states.
Oxidation State of the Metal Ion = The total charge of the complex - The sum of the
charges of the ligands
Complex A central bonded atom surrounded by coordinately bonded ligands.
Complexed Ion Central metal ion surrounded by coordinately bonded ligands.
Ligands An atom, ion or molecule that forms a co-ordinate bond with a central
transition metal ion by donating a pair of electrons. It surrounds the metal
ion. It is the same as a nucleophile and it has a negative charge.
Monodentate Ligands that can only form one co-ordinate bond
Ligand
Bidentate ligand Ligands that can only form two coordinate bonds.
