Transition Metals Flashcards
D block elements properties
All metallic, so have high melting and boiling points, shiny in appearance and conduct electricity and heat.
Copper, silver, nickel and zinc have been used in coinage.
Iron used in construction and production of tools.
Copper used in electrical cables and water pipes.
Titanium has great strength and is used in aerospace industry and medical applications eg joint replacement.
When forming an atom the 4s orbital….
When forming an ion the 4s orbital….
Fills before the 3d orbitals.
Empties before the 3d orbitals.
A species containing a transition element in its highest oxidation state
Is often a strong oxidant agent.
Iron 2+ and iron 3+ ions electron configurations and colours
Iron (II) ion: Fe2+ 1s2 2s2 2p6 3s2 3p6 3d6 -pale green
Iron (III) ion: 1s2 2s2 2p6 3s2 3p6 3d10 - yellow
The contact process
Production of sulcus trioxide from oxidation of sulfur dioxide. Reaction catalysed by vanadium oxide V2O5
2SO2 (g) + O2 (g) -> 2SO3 (g)
Decomposition of hydrogen peroxide
2H2O2 (aq) -> 2H2O (l) + O2 (g)
Fe2+ catalyst in reaction between S2O8 2- and Fe 2+
S2O8 2- (aq) +Fe2+ (aq) -> 2SO4 2- (aq) + Fe3+ (aq)
Fe3+ (aq) + 2I- (aq) -> I2 (aq) + Fe2+ (aq)
Bidentate ligands
These ligands can donate two lone pairs of electrons to the central metal ion, forming two coordinate bonds.
Most common ligands
See card 1
Octahedral shape and bond angle
90 degrees
See card 2
Tetrahedral shape and bond angle
109.5 degrees
See card 3
Square planar shape and bond angle
Platinum (II) and palladium (II) and gold (III) and tend to form square planar shapes.
90 degrees
See card 4
In the cis isomer the bond angle between identical ligands are..
In trans isomer the coordinate bonds between the identical ligands are..
90 degrees
180 degrees
Do cis or trans isomers form optical isomers
Cis, trans cannot form optical isomers as mirror image is exactly same and can be superimposed.
Two different reactions of ligand substitution of Cu with ammonia
Pale blue precipitate of Cu(OH)2 is formed in the first stage of the reaction. The Cu(OH)2 precipitate then dissolves in excess ammonia to form a dark blue solution.
Ligand substitution with chloride ions
Conc HCL added to [Cu(H2O)6]2+ pale blue solution becomes yellow.
If water added to yellow solution, blue solution formed (more dilute and paler in colour than original blue solution).
Intermediate is green solution (result of yellow mixing with blue)
See card 5
Chromium potassium sulfate also known as
Chrome alum
Reaction of [Cr(H2O)6]3+ with ammonia equation
See card 6
Carbon monoxide and ligand substitution
Can bind to Fe2+ ion in haem, called carboxyhaemoglobin.
If CO breathed in, ligand substitution takes place where oxygen in haemoglobin replaces by CO.
Bond is so strong that process is irreversible, if conc of carboxyhaemoglobin becomes too high, O2 transport is prevented leading to death.
Transition metal ions in aq solution react with
Aq sodium hydroxide and aq ammonia to form precipitates.
Some of these precipitates dissolve in excess NaOH or NH3 to form complex ions in solution.
Cu2+ reaction equation with NaOH
See card 7
Fe2+ reaction with NaOH
Pale green solution reacts to form green precipitate.
Precipitate insoluble in excess NaOH but turns brown at surface on standing in air as iron (II) is oxidised to iron (III)
See card 8
Reaction of Fe3+ with NaOH
Pale yellow solution reacts to form an orange-brown precipitate of iron (III) hydroxide. Precipitate insoluble in excess NaOH
See card 9
Reaction of Mn2+ with NaOH
Pale pink solution reacts to form light brown precipitate of manganese hydroxide which darkens on standing in air. Precipitate is insoluble in excess NaOH.
See card 10
Cr3+ with NaOH
Violet solution reacts to form a grey green precipitate of chromium (III) hydroxide.
Precipitate is soluble in excess NaOH forming a dark green solution.
See card 11
Redox reaction involving transition metal Fe2+ and Mn
See card 12
Reduction of Fe3+ to Fe2+
See card 13
Reaction of dichromate and chromium
See card 14
Oxidation of Cr3+ to CrO4 2-
See card 15
Reduction of Cu2+ to Cu+
See card 16
Disproportionation of Cu+ ions
See card 17
Identifying ammonium ions
See card 18
Test for ammonium ion ; aq NaOH heated gently with solution. If ammonia evolved damp red pH indicator paper will turn blue.
