CHEM 1100 Lecture Notes - Lecture 1: Transition Metal, Paramagnetism, Reaction Rate
22 May 2018
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Malleable - shape can be change
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Coloured complexes
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Conductive - conducts electricity and heat
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Used as catalyst - increases reaction rate
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Strong positively charged ions
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Easily oxidised
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Ie Fe, Cr
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Multiple oxidation states
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Features of transition metal
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Transition metal
Ultra-electro plastic
metal
Semi metal
When neutral, nd orbitals of (n+1) period are HIGHER in energy than (n+1)s orbital
Oxidation
Electrons comes out of 4s orbital
4s orbitals are more radially diffuse than 3d orbitals
1s< 2s< 2p< 3s< 3p< 4s< 3d< 4p< 5s< 4d< 5p< 6s< 5d< 6p< 7s< 6d
Reason for special features
The special features of complexes are due to 5 valence d orbitals
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Therefore, they do poor shielding nuclear charge
The orbitals are highly directional
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Early metals have higher oxidation states
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3+ oxidation state is more common for early metals ( left hand side)
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2+ is more common for late metals (right hand side)
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RELATED TO Z(eff) --> effective nuclear charge
Oxidation states
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Oxidation state in transition metals increase by 1 or -1, unlike p-block or s-block metals
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This results in unpair electrons in the orbitals and paramagnetism
Paramagnetism
Lecture 1 Week 10 Monday
Tuesday, 22 May 2018
10:43 PM
New Section 1 Page 1
Document Summary
When neutral, nd orbitals of (n+1) period are higher in energy than (n+1)s orbital. 4s orbitals are more radially diffuse than 3d orbitals. The special features of complexes are due to 5 valence d orbitals. Oxidation states: early metals have higher oxidation states, 3+ oxidation state is more common for early metals ( left hand side, 2+ is more common for late metals (right hand side, related to z(eff) --> effective nuclear charge. Paramagnetism: oxidation state in transition metals increase by 1 or -1, unlike p-block or s-block metals, this results in unpair electrons in the orbitals and paramagnetism.
