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1. Transition metals: Ti – Cu = incomplete d sub-level in atoms/ions
form positive ions: s electrons removed before d electrons
not Sc & Zn: Sc3+ & Zn2+ = empty/full 3d subshell
Physical Properties – similar (don’t change across period)
- High density
- High melting point
- Similar ionic radius
Chemical Properties
complex formation
formation of coloured ions
variable oxidation states (unlike s-block metals)
catalytic activity
Ligand: molecule/ion that forms co-ordinate bond with transition metal by donating pair
Complex: central metal atom/ion surrounded by co-ordinately-bonded ligands
Co-ordination number: number of co-ordinate bonds to central metal atom/ion
4. Formation of coloured ions by visible light
- ligands split 3d orbitals into 2 energy levels = ground state & excited state = energy gap ∆E
- electrons absorb energy from visible light frequencies = excite electrons
- transmitted/reflected visible light frequencies: combine = complementary colour – seen
∆E = hν = hc
λ
- ∆E: energy gap between ground & excited state d electrons
o larger = absorbs higher frequency
- h: Planck’s constant 6.63x10-34 J s
- v: frequency absorbed Hz
- c: speed of light 3x108 ms-1
- λ: wavelength absorbed m
things that cause a change in ∆E (that causes a colour change)
- oxidation state
- co-ordination number
- ligand
spectroscopy: find concentration of coloured ions in solution by measuring how much light absorbed
1. Colorimetry
- white light
- filter – colour of light sample absorbs
- solution
- colorimeter: calculates how much light absorbed by sample
2. Calibration curve: relative absorbance / concentration
3. Find concentration from absorbance of sample
Absorbs more light = more concentrated
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