Question

The general electronic configuration of d block elements is $$(\text{n}-1){\text{d}}^{1-10}\text{n}{\text{s}}^{1-2}$$, where n is the outermost shell. However Palladium does not follow this general electronic configuration. It has an electronic configuration $${{\left[\text{Kr}\right]}^3}^{6}4{{\text{d}}^1}^{0}5{\text{s}}^0$$ in order to have stability. Give a reason behind it.

Answer 1

Hint: In order to make d orbital half filled or fully filed, electron from s subshell jumps to d subshell. As half and fully filled orbitals are more stable.

Complete step by step solution:
In modern periodic tables the elements are organized in such a way that physical and chemical properties of the periodic function of its atomic number. Modern periodic table has 18 groups, 7 periods and 4 blocks. Generally elements of a group have similar outer shell electronic configuration. S block is from group 1 to group 2. Group 1 is known as alkali metal & have $$\text{n}{\text{s}}^1$$ electronic configuration. Group 2 is known as alkaline earth metal & has $$\text{n}{\text{s}}^2$$ valence electronic configuration. Group 13 to group 18 belongs to the p block & have $$\text{n}{\text{s}}^2\text{n}{\text{p}}^{1-6}$$ general electronic configuration. Group 3 to group 12 belong to d block & have $$(\text{n}-1){\text{d}}^{1-10}\text{n}{\text{s}}^{1-2}$$ .
It is important to note that in d block is that in third period of d block $$3{\text{d}}^4\text{ and }3{\text{d}}^9$$are not possible, in fourth period of d block $$4{\text{d}}^3,4{\text{d}}^6\text{ and }4{\text{d}}^9$$ is not possible and in fifth period of d block $$5{\text{d}}^8$$ is not possible. This is due to the reason of stability. In order to make d orbital half filled or fully filled; electron from s subshell jump to the d sub shell.

Note:
Lanthanides or 4f series are from atomic number 58-71. Actinides or 5f series are from atomic number 90-103. The d block elements are as follow: