Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
Answers
All the metals display +2 oxidation states except Sc.
On moving from the Sc to the Mn, the atomic numbers increase from 21 to the 25.
It means the number of electrons in the 3d-orbital also increases from 1 to 5. Sc (+2) = d1, Ti (+2) = d2, V (+2) = d3, Cr (+2) = d4 and Mn (+2) = d5.
The +2 oxidation state is achieved by loss of the 2 4s electrons by the metals.
Answer:
+2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number as 3d orbitals acquire only one electron in each of five 3d orbitals (remain half-filled) and the electronic repulsion is least and the nuclear charge increases. In the second half of the first row transition series, electrons pair up in 3d orbitals. This increases the electronic repulsion
Explanation: