Chapter 15.9, Problem 7P

Interpretation Introduction

Interpretation:

The number of $4d$ electrons present in ${\text{Pd}}^{2+}$ and the $+2$ ion in the fourth and the sixth period having the same number of $3d$ electrons as ${\text{Pd}}^{2+}$ are to be determined

Concept Introduction:

The elements in group $\text{3-12}$ are called d-block elements.

For d-block elements, the number of electrons in valence shell is same as the group number. The number of d-electrons is two less than the group number.

The first sequence of d-block elements starts with the element scandium which has one $\text{3d}$-electron and continues to zinc which has ten $\text{3d}$-electrons. The same trend holds true for the second ($\text{4d}$) and third ($\text{5d}$) sequence of d-block elements.

For the elements, in the same group, the number of valence electrons as well as d-electrons remains the same.