Summary
HL IB Chemistry Summary notes on Periodicity topic
- Module
- HL IB Chemistry
- Institution
- Loughborough University (LU)
Includes: - Complex ions - Magnetism - Oxides - Periodic trends - Transition metals
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Complex ions- Metal ion surrounded by ligands
- Ligands are neutral or negative species that form coordinate bonds by donating a lone pair
of electrons
Coordinate covalent bonds are formed between the ligand and the transition metal
- All transition metals (excluding titanium) form an octahedral complex with the form
[M(H2O)6]2+ in an aqueous solution
- Complex ions can undergo substitution reactions in which (e.g.) H 2O ligand can be replaced
with another ligand
Factors affecting colour:
Anything that affects the energy gap between the d-orbitals
Greater split >> greater the energy difference >> greater frequency >> shorter wavelength
METAL
Magnetism
PARAmagnetism is caused by unpaired electrons
- Paramagnetic materials are attracted to a magnetic field
- The more unpaired electrons, the greater then magnetic moment
DIAmagnetism is caused by paired electrons and are repelled slightly by a magnetic field
CATALYSTS:
- Transition metals make good catalysts
- Provide an alternative reaction pathway
- Fe >> Haber proces
, Transition Metals
= an element that forms at least one stable ion with a partially filled d orbital
1st row d-
block
- Variable/different oxidation states
- coloured solutions
- form complex ions >> e.g. [Cu(H2O)6]2+
- can have magnetic properties
- good catalysts
4s fills before 3d, but 3d is at a higher energy level than 4s – BUT – the electrons in 3d are inside
the 4s and repels it out ∴ 4s are the outermost electrons and are lost first
- stability associated with a half full or full d-orbital
- All transition metals show oxidation number +2, usually as a result of the 2 electrons in the
4s subshell
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