   Chapter 7.6, Problem 2.1ACP

Chapter
Section
Textbook Problem

Give the electron configurations for iron and the iron(II) and iron(III) ions.

Interpretation Introduction

Interpretation:

The electronic configuration given ion of iron (Fe), (Fe2+) and (Fe3+) has to be predicted.

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 (n-1)d1–10 ns1–2. 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.

Explanation
• Electronic configuration of iron (Fe):

Electronic configuration of iron (Fe) is d-block elements and its orbital filling method is shown below.

Here the iron (Fe) is a 8 group element and 4th periodic position in the periodic table, hence the (Fe) element first filling find the proceedings (Ar) noble gas and then note the number of (s, p, d, f) electrons that lead from the noble gas to the element.

Atomicnumber (Z)ofIron(Fe)=26spdfwith noble gas notation=[Ar]3d64s2Orbitalboxnotation       = [Ar]3d64s2

Therefore, the electronic configuration of iron (Fe) = [Ar]3d64s2

• Electronic configuration of iron (Fe2+):

Further the iron (Fe) was oxidized to (Fe2+) and (Fe3+) ions, it lost for two and three electrons in outermost (4s) and inner (3d) orbital shells. So these electronic configuration methods we discussed below.

Atomicnumber (Z)ofIron(Fe)=26Loss of two electrons in (Fe2+) ions=262=24spdfwith noble gas notation=[Ar]3d64s0Orbitalboxnotation       = [Ar]&#

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