Chapter 7.6, Problem 6Q

Interpretation Introduction

Interpretation:

The electron configuration for the placement of La or Lu below Y has to be explained.

Concept Introduction:

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

General electronic configuration of d-block: These elements having common formula $\left(\text{n-1}\right){\text{d}}^{\text{1–10}}{\text{ ns}}^{\text{1–2}}$. The (n–1) stands for the inner d orbitals which may have one to ten electrons and the outermost ns orbital may have one or two electrons.

General electronic configuration of f-block: The general the electronic configuration of these elements is $\left(\text{n-2}\right){\text{f}}^{\text{1-14}}\left(\text{n-1}\right){\text{d}}^{\text{1–10}}{\text{ns}}^{\text{1–2}}$. The two rows of elements present at the bottom of the periodic table are called the (4f) series or lanthanides and actinides (5f). They are also called inner transition elements.