d-block Elements PPT Chemistry Class 12

 Page 1


SS CI 11.5 The d block 1
1s
2s
3s
4s
2p
3p
3d
Energy
Ar
1s
2  
2s
2 
2p
6 
3s
2 
3p
6
4p
Page 2


SS CI 11.5 The d block 1
1s
2s
3s
4s
2p
3p
3d
Energy
Ar
1s
2  
2s
2 
2p
6 
3s
2 
3p
6
4p
SS CI 11.5 The d block 2
1s
2s
3s
4s
2p
3p
3d
Energy
Sc
1s
2  
2s
2 
2p
6 
3s
2 
3p
6 
3d
1 
4s
2
4p
Page 3


SS CI 11.5 The d block 1
1s
2s
3s
4s
2p
3p
3d
Energy
Ar
1s
2  
2s
2 
2p
6 
3s
2 
3p
6
4p
SS CI 11.5 The d block 2
1s
2s
3s
4s
2p
3p
3d
Energy
Sc
1s
2  
2s
2 
2p
6 
3s
2 
3p
6 
3d
1 
4s
2
4p
Electronic Arrangement
Element Z 3d 4s
Sc 21 [Ar] ? ??
Ti 22 [Ar] ? ? ??
V 23 [Ar] ? ? ? ??
Cr 24 [Ar] ? ? ? ? ? ?
Mn 25 [Ar] ? ? ? ? ? ??
Fe 26 [Ar] ?? ? ? ? ? ??
Co 27 [Ar] ?? ?? ? ? ? ??
Ni 28 [Ar] ?? ?? ?? ? ? ??
Cu 29 [Ar] ?? ?? ?? ?? ?? ?
Zn 30 [Ar] ?? ?? ?? ?? ?? ??
SS CI 11.5 The d block 3
Page 4


SS CI 11.5 The d block 1
1s
2s
3s
4s
2p
3p
3d
Energy
Ar
1s
2  
2s
2 
2p
6 
3s
2 
3p
6
4p
SS CI 11.5 The d block 2
1s
2s
3s
4s
2p
3p
3d
Energy
Sc
1s
2  
2s
2 
2p
6 
3s
2 
3p
6 
3d
1 
4s
2
4p
Electronic Arrangement
Element Z 3d 4s
Sc 21 [Ar] ? ??
Ti 22 [Ar] ? ? ??
V 23 [Ar] ? ? ? ??
Cr 24 [Ar] ? ? ? ? ? ?
Mn 25 [Ar] ? ? ? ? ? ??
Fe 26 [Ar] ?? ? ? ? ? ??
Co 27 [Ar] ?? ?? ? ? ? ??
Ni 28 [Ar] ?? ?? ?? ? ? ??
Cu 29 [Ar] ?? ?? ?? ?? ?? ?
Zn 30 [Ar] ?? ?? ?? ?? ?? ??
SS CI 11.5 The d block 3
Chromium and Copper
• Cr and Cu don’t fit the pattern of 
building up the 3d sub-shell, why?
– In the ground state electrons are always 
arranged to give lowest total energy
– Electrons are negatively charged and repel 
each other
– Lower total energy is obtained with e
-
singly 
in orbitals rather than if they are paired in 
an orbital
– Energies of 3d and 4s orbitals very close 
together in Period 4
Page 5


SS CI 11.5 The d block 1
1s
2s
3s
4s
2p
3p
3d
Energy
Ar
1s
2  
2s
2 
2p
6 
3s
2 
3p
6
4p
SS CI 11.5 The d block 2
1s
2s
3s
4s
2p
3p
3d
Energy
Sc
1s
2  
2s
2 
2p
6 
3s
2 
3p
6 
3d
1 
4s
2
4p
Electronic Arrangement
Element Z 3d 4s
Sc 21 [Ar] ? ??
Ti 22 [Ar] ? ? ??
V 23 [Ar] ? ? ? ??
Cr 24 [Ar] ? ? ? ? ? ?
Mn 25 [Ar] ? ? ? ? ? ??
Fe 26 [Ar] ?? ? ? ? ? ??
Co 27 [Ar] ?? ?? ? ? ? ??
Ni 28 [Ar] ?? ?? ?? ? ? ??
Cu 29 [Ar] ?? ?? ?? ?? ?? ?
Zn 30 [Ar] ?? ?? ?? ?? ?? ??
SS CI 11.5 The d block 3
Chromium and Copper
• Cr and Cu don’t fit the pattern of 
building up the 3d sub-shell, why?
– In the ground state electrons are always 
arranged to give lowest total energy
– Electrons are negatively charged and repel 
each other
– Lower total energy is obtained with e
-
singly 
in orbitals rather than if they are paired in 
an orbital
– Energies of 3d and 4s orbitals very close 
together in Period 4
Chromium and Copper
• At Cr
– Orbital energies such that putting one 
e
-
into each 3d and 4s orbital gives 
lower energy than having 2 e
-
in the 
4s orbital
• At Cu
– Putting 2 e
-
into the 4s orbital would 
give a higher energy than filling the  
3d orbitals
SS CI 11.5 The d block 5