Here are my revision notes for the Transition Metals section of the course.
Feel free to check out my other computer typed notes for parts of the 2nd year course on here.
I also have hand written notes of matching quality for pretty much the rest of the course (1st and 2nd year) if you're inter...
2.6. Isomerism
1. General Properties 2.5. Shapes of Complex Ions
• Isomer – compound with same mole
Transition Metal—Forms at least 1 stable ion with a part full “d” shell • Differences in shape occur due to varying ligand
different structural formula
of electrons sizes – a larger ligand means that less can fit in
Geometrical:
Scandium and Zinc are not transition metals the space around the central metal ion
• Occurs in octahedral and square planar
Properties: good heat and electricity conductors e.g. Cl ligand is larger than NH3 ligand
Example is platin (square pl
hard, strong, shiny
There are a few trans-platin
high mpt and bpt
examples of square Optical:
low chemical reactivity
planar: • Occurs when 2 or more bidentate ligands
variable oxidation states
[Ni(CN)4]2- present in complex
catalytic action
[Pt(Cl)4]2- • They are chiral
coloured complexes
[Pt(Cl)2(NH3)2] PLATIN • Distinguished by effect on plan polarized l
formation of complexes
2.1. Aqua Ions
1.1. Electron Configuration Dissolving a salt of a T.M in water, the positively 2.4. Haemoglobin
➢ 4s fills before 3d, 4s also empties before 3d charged metal ion is surrounded by polar water • Carries oxygen around body
❖ Chromium has config of [Ar] 4s1 3d5 molecules acting as ligands • Molecule has an Fe2+ ion with coordination number of 6 (octahedral)
❖ Copper has config of [Ar] 4s1 3d10 They replace the salt and form an aqua ion • Complex ion called haem
➢ It’s believed that a half full “d” orbital level makes the atom more • Globin is the complex protein
stable
Inorganic Chemistry: Transporting O2:
Transition Metals • Oxygen substitutes the water ligands forming oxyhaemoglobin
2. Complex Ion Formation and their Shapes • Oxygen then given up to where it’s needed
All T.M ions can form coordinate bonds by accepting electron pairs from other • Water replaces oxygen again and goes back to lungs
ions/molecules
Ligand—particle with lone pair that bonds to metals via coordinate bond Bonding:
Complex—metal ion with coordinately bonded ligands • Fe2+ to O2 bond is weak, so Oxygen can be given off easily
Coordination Number—no. of coordinate bonds from ligands to non-metal • CO is a better ligand and stronger bond, which prevents oxygen transfer
Lewis Base—lone pair doner
Lewis Acid—lone pair acceptor
2.3. Chelate Effect
Chelation – process by which a multidentate liga
Ligand examples include: H2O, NH3, Cl, CN, EDTA and they all • H2O, NH3 and Cl are monodentate ligands, the H2O and NH3 monodentate ligands in forming a co
vary in their coordination number ligands are similar in size and uncharged, so an exchange of transition metal ion
these 2 will have no effect on coordination number. • When chelation occurs, there are more moles of p
6 bonds = octahedral • But the Cl ligand is larger so will cause a decrease in reactants used, this causes an increase in entropy
4 bonds = tetrahedral or square planar coordination number – more shielding than oxygen, higher to the right. More molecules = increases entropy
2 bonds = linear mass . Entropy - measure of disorder within a system
• NH2CH2CH2NH2 (each N has a lone pair) [shown above] and
Monodentate Ligands—form 1 coordinate bonds with a T.M C2O4 are bidentate ligands • Complex ions with larger stability constants are mo
Bidentate Ligands—form 2 coordinate bonds • EDTA is polydentate (forms 6 coordinate bonds, lone pairs on smaller ones
Polydentate Ligands—form more than 2 coordinate bonds 4 oxygen atoms and 2 nitrogen atoms • EDTA is a chelating agent and used to prevent pois
Complex ions with polydentate ligands are
called chelates. Chelates are used to
remove “d” block metal ions from solution
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