Transition element
A metal that can form one or more stable ions with an incomplete d sub-level
Which d block elements are not transition elements?
Zn and Sc
Chemical properties of transition metals
Form complex ions
Variable oxidation states
Coloured ions
Catalysts
Complex ion
A central metal ion surrounded by ligands
Ligand
A molecule or ion that forms a dative covalent bond with a central metal ion by donating a pair of electrons
Dative covalent bond
A covalent bond where the shared pair of electrons have been donated by the same atom/molecule
Co-ordination number
The number of dative bonds to the central metal
Cations which form complex ions must have two feature....
1.they must have a high charge density, and thus be able to attract electrons from ligands. 2.they must have empty orbitals of low energy, so that they can accept the lone pair of electrons from the ligands.
Monodentate ligands
Ligands which donate pair of electrons to make a dative covalent bond to the central metal ion.
Bidentate ligands
Ligands which donate 2 lone pairs of electrons forming 2 coordinate bonds each.
Multidentate ligands
A molecule with forms more than 2 co-ordinate bonds
Co-ordination number of an octahedral
6
Co-ordination number of a tetrahedral
4
Chloride ions and other large ions form
Tetrahedral complexes with a coordination number of 4
Silver ions form
Linear complexes with a coordination number of 2
Which 2 ions form a square planar shape?
Platinum and Nickel
Stereoisomerism
A molecule with the same structural formula but its atoms are arranged differently in space
Optical isomer
These are non superimposable mirror images
Cis ligands
2 ligands are at 90o to each other
Trans ligands
2 ligands are at 180o to each other
Optical isomers occur with what shape of molecule?
Octahedral with 3 bidentate ligands
Ligand substitution
Where one ligand substitutes another.
Why can CO be deadly?
CO can bind to haemoglobin sites, the same way oxygen can
However, CO forms stronger dative covalent bonds
The CO cannot be removed
With CO, the stability constant is greater than with complex in O2
When monodentate ligands are replaced with bi/multidentate ligands, there is an increase in...
Entropy
Metal aqua ions
Has 6 water ligands
Octahedral shape
Has the same charge as the metal (as water is neutral)
Cu2+ metal aqua ion colour
Blue solution
Co2+ metal aqua ion colour
Pink solution
Fe2+ metal aqua ion colour
Green solution (pale)
Fe3+ metal aqua ion colour
Yellow solution
Cr3+ metal aqua ion colour
Green solution
Mn2+ metal aqua ion colour
Pale pink solution
Cu2+ metal aqua ion with OH- colour
Blue precipitate
Co2+ metal aqua ion with OH- colour
Blue precipitate
Fe2+ metal aqua ion with OH- colour
Green precipitate
Mn2+ metal aqua ion with OH- colour
Brown precipitate
Cr3+ metal aqua ion with OH- colour
Green precipitate
Fe3+ metal aqua ion with OH- colour
Brown precipitate
Cu2+ metal aqua ion with NH3 colour
Blue precipitate
Co2+ metal aqua ion with NH3 colour
Blue precipitate
Fe2+ metal aqua ion with NH3 colour
Green precipitate
Mn2+ metal aqua ion with NH3 colour
Brown precipitate
Cr3+ metal aqua ion with NH3 colour
Green precipitate
Fe3+ metal aqua ion with excess NH3 colour
Brown precipitate
Cu2+ metal aqua ion with excess NH3 colour
Blue precipitate
Co2+ metal aqua ion with excess NH3 colour
Yellow/Brown solution
Cr3+ metal aqua ion with excess NH3 colour
Purple/Violet solution
Amphoteric
A molecule that is able to react both as a base and as an acid
Reaction with Chloride ions
Co-ordination number of 4
Tetrahedral
Oxidation of Iron (II)
Fe2+ can be oxidised to Fe3+ Usually use potassium manganate (VII)
Reduction of Iron (III)
Fe3+ can be reduced to Fe2+ Commonly use potassium iodide solution
Reduction of Chromium
(Cr2O7)2- can be reduced by Zn in acid solution Forms Cr3+ and Cr2+
True or False: It is easier to remove an electron from a negatively charged ion
True
Reduction of Cu2+
Cu2+ can be reduced to Cu+ using potassium iodide
Disproportionation of Copper (I) ions
Copper (I) ions will react with sulfuric acid to form Cu2+ and Cu metal
Testing for presence of a carbonate
Add any dilute acid (ideally nitric acid)
Observe for effervescence
Testing for presence of a sulphate
Add BaCl2
If present, white precipitate will form
Testing for presence of halide ions
Add silver nitrate (AgNO3)
Precipitates will form if present
Chloride: white precipitate
Bromide: cream precipitate
Iodide: yellow precipitate
Silver chloride will dissolve in
Dilute ammonia
Silver bromide will dissolve in
Concentrated ammonia
Sequence of testing for negative ions
Carbonate, sulphate, halide
Test for ammonium ions
React with warm NaOH
Ammonia gas formed can be identified by turning red litmus paper blue