Transition elements are defined as elements that
have partially filled d or f electron sub shells
in any common oxidation state
Properties of the transition metals
1 They are metals
High NP BP
Shiny
Malleable and ductile
2 Multiple oxidation states
Manganese Mn has oxidation States from 2 to it
3 They all have coloured ions
Due to electron movement within d orbital
4 Form stable Paramagnetic compounds
Periodic Properties of Transition metals
Revising Quantum numbers
, Top row of
electron configuration due to extra stability gained
fM
transition metals do not have 3d 4s
from half filled 3ds and 4s orbital
i e Chromium Cr Ar 3d54s
Copper Ca Ar 3d 4s
stabilisation from half filled orbital are due to energy
of the orbitals as well as other factors such as
spin pairing energy
Thus 4s electrons are always lost first when
forming cations
Physical Properties of Transition metalsi
These two properties are
determined by the
strength of the metal
metal bonding
As expected atomic radii
decreases from left to right
with Mn being a clear
anomaly
Effective Nuclear Charge
Slight increase at the end
of each Period
, Effects of Effective Nuclear Charge ENC
For an electron in 3d orbital
Shielding by an electron in core orbital I
Shielding by an electron in its orbital O
Shielding by an electron in 3d orbital 0.35
i e ENC for Vanadium V
Ar 453rd 18 1.0 2 0 3 0.35
19.05
ENC 23 19.0
3.95
This explains the general
trendinperiodictable
However Ud and 5d
elements are almost
identical in terms of radius
Due to Lanthanide
Contraction
Lanthanides are 4f elements
which radii decreases
across period as expected
have partially filled d or f electron sub shells
in any common oxidation state
Properties of the transition metals
1 They are metals
High NP BP
Shiny
Malleable and ductile
2 Multiple oxidation states
Manganese Mn has oxidation States from 2 to it
3 They all have coloured ions
Due to electron movement within d orbital
4 Form stable Paramagnetic compounds
Periodic Properties of Transition metals
Revising Quantum numbers
, Top row of
electron configuration due to extra stability gained
fM
transition metals do not have 3d 4s
from half filled 3ds and 4s orbital
i e Chromium Cr Ar 3d54s
Copper Ca Ar 3d 4s
stabilisation from half filled orbital are due to energy
of the orbitals as well as other factors such as
spin pairing energy
Thus 4s electrons are always lost first when
forming cations
Physical Properties of Transition metalsi
These two properties are
determined by the
strength of the metal
metal bonding
As expected atomic radii
decreases from left to right
with Mn being a clear
anomaly
Effective Nuclear Charge
Slight increase at the end
of each Period
, Effects of Effective Nuclear Charge ENC
For an electron in 3d orbital
Shielding by an electron in core orbital I
Shielding by an electron in its orbital O
Shielding by an electron in 3d orbital 0.35
i e ENC for Vanadium V
Ar 453rd 18 1.0 2 0 3 0.35
19.05
ENC 23 19.0
3.95
This explains the general
trendinperiodictable
However Ud and 5d
elements are almost
identical in terms of radius
Due to Lanthanide
Contraction
Lanthanides are 4f elements
which radii decreases
across period as expected
