Transition metals
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What is a transition metal
A d- block element that can form at least one stable ion with an incomplete d-subshell, or exists as an atom which has an incomplete d-subshell
Why do Cr and Cu have electron configurations (Ar)3d5,4s1 and (Ar)3d10,4s1 respectively
An e- from the 4s orbital moving into the 3d orbital to create a more stable half full or full 3d subshell
Why is Zn not a transition metal
Forms only 1 stable ion: Zn2+ which has a full-subshell
Give 4 properties of transition metals
Variable oxidation states Coloured ions in solution Good catalysts Complex formation
Why do transition metals have variable oxidation states
Electrons sit in the 4s and 3d subshells which are very close, therefore electrons are gained and lost using a similar amount of energy when they form ions
What is the Pneumonic to remember the colours of vanadium
You (VO₂⁺) Better (VO²⁺) Get (V³⁺) Vanadium (V²⁺)
What colour is VO₂⁺(aq)
Yellow
What colour is VO²⁺(aq)
Blue
What colour is V³⁺(aq)
Green
What colour is V²⁺ (aq)
Violet
What colour is Cr³⁺(aq)
Green/Violet
When is Cr³⁺(aq) violet
When surrounded by water ligands, however commonly substituted with other molecules and so usually green
What colour is Cr₂O₇⁻(aq)
Orange
What colour is Mn²⁺(aq)
Pale pink
What colour is MnO₄⁻(aq)
Purple
What colour is Fe²⁺(aq)
Pale green
What colour is Fe³⁺(aq)
Yellow-brownish
What colour is CO²⁺(aq)
Pink
What colour is Ni²⁺(aq)
Green
What colour is Cu²⁺(aq)
Blue
What colour are Zn²⁺(aq) and Sc³⁺(aq)
Colourless
What is a complex ion
A central transition metal ion is surrounded by ligands bonded by dative covalent bonds
What is a ligand
A molecule/ion that forms a covalent bond with a central metal atom by donating a pair of e-
What is a monodentate ligand
Ligands which only donate 1 pair of e- (to a transition metal ion) from one atom on the molecule/ion, forming 1 coordinate bond