Question:

The stability of ferric ion is due to

Updated On: Jul 5, 2022

half-filled d-orbitals
half-filled f-orbitals
completely filled d-orbitals
completely filled f-orbitals

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The Correct Option is A

Solution and Explanation

$E.C$. of $Fe ^{3+}$ ion i.e., $Fe ^{3+}=1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{6}, 3 d^{5} .$ Therefore, ferric ion is quite stable due to half-filled $d$-orbitals.

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Concepts Used:

Subshell Electronic Configuration

Electron Configuration is referred to as the distribution of electrons in an atom's orbitals. An electron in an atom is defined by a set of four quantum numbers (n), the most important of which defines the main energy level known as a shell. The filling of electrons into different subshells, also known as orbitals (s, p, d, f) in an atom. The position of an element in the periodic table is determined by the quantum numbers of the last orbital filled.

Subshells:

The azimuthal quantum number (denoted by 'l') determines the subshells into which electrons are distributed.
The value of this quantum number is determined by the value of the principal quantum number, n. As a result, when n equals 4, four different subshells are possible.
When n = 4, The s, p, d, and f subshells correspond to l=0, l=1, l=2, and l=3 values, respectively.
The formula 2*(2l + 1) gives the maximum number of electrons that a subshell can accommodate.
As a result, the s, p, d, and f subshells can each hold a maximum of 2, 6, 10, and 14 electrons.