+2 Oxidation State Of Nickel explained in this presentation

2. Presentation On
+2 Oxidation State Of
Nickel

3. My todays talk about
Nickel & Its +2 oxidation state
Octahedral arrangement of Nickel +2

4. Nickel
• Discovered & named at 1754 by Axel Fredrik
• Ni +2 oxidation state involves wide variety of -
the halides, oxides, sulphide, selenide, telluride, salts
of common acids & oxidizing salts.
• Formed double salts.
• Formed complicated complex's.
Electronic configuration
Ni — [Ar] 𝟑𝒅 𝟖
𝟒𝒔 𝟐
N𝒊+𝟐
— [Ar] 𝟑𝒅 𝟖

5. Octahedral arrangement of Nickel +2
The reason they split is because of the electrostatic
interactions between the electrons of the ligand and the
lobes of the d orbital.
t2g
eg
Fig:d8
arrangement in octahedral field (weak)

6. Special case of 𝒅 𝟖
octahedral
Square-planar complex is formed, attempts to form
octahedral complexes become impossible.
If the ligand field is sufficiently strong, the difference in
energy between these two orbitals becomes larger
then the energy needed to pair the electrons.
Fig: 𝐝 𝟖
arrangement in strong octahedral field ( square planar formed)

7. • With ammonia [𝑵𝒊(𝑵𝑯 𝟑) 𝟔] 𝟐+,
[𝑵𝒊(𝑯 𝟐 𝑶) 𝟒(𝑵𝑯 𝟑) 𝟐] 𝟐+
• [𝑵𝒊(𝒆𝒕𝒉𝒚𝒍𝒆𝒏𝒆𝒅𝒊𝒂𝒎𝒊𝒏𝒆) 𝟑] 𝟐+
Examples of Octahedral complex's
Examples of square planar complex’s
• [𝑵𝒊(𝑪𝑵) 𝟒] 𝟐−
• Colour : generally red, brown
or yellow

8. 𝑵𝒊+𝟐
& Dimethylglyoxime in solid
• In solid the square planar molecules are stacked on top of
each other & a Ni-Ni(distance 3.25𝜜 𝝄
) interaction occurs.
• Dimethylglyoxime loses a proton, and stabilized by forming 2
five membered chelate ring and internal hydrogen bonding.
N
OH
OH
N
Ni
N
NN
N
H3C
H3C
HO O
H
CH3
CH3
O OH
H
+2 OH-
-2 H2O
2Ni2+
+
Fig: Nickel dimethylglyoxime complex

9. The reason for splitting is due to poor overlap between the
metal & the ligand orbitals. The orbitals are directed on
the axes, while the ligands not.
𝒅 𝟖
arrangement in tetrahedral field
Fig: Tetrahedral ligand field
surrounding a central metal
t2g
Fig:d8
arrangement in tetrahedral field
eg

10. That’s All
Thanks To All