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In general the electronic configuration of outer orbitals of t

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In general the electronic configuration of outer orbitals of these elements is $(n - 1) d^{110} n s^{1 - 2}$ . The $\underline{(n - 1) stands for the inner d orbitals which may}$ have one to ten electrons and the outermost ns orbital may haye one or two electrons. However, this generalisation has several exceptions because of very little energy difference between (n-1)d and ns.orbitals. Furthermore, half and completely filled sets of orbitals are relatively more stable. A consequence of this factor is reflected in the electronic configurations of $Cr$ and $Cu$ in the $3 d$ series. For example, consider the case of $Cr$ , which has $3 d^{5} 4 s^{'}$ configuration instead of $3 d^{4} 4 s^{2}$ ; the energy gap between the two sets ( $3 d$ and $4 s$ ) of orbitals is small enough to prevent electron entering the $3 d$ orbitals. Similarly in case of $Cu$ , the configuration is $3 d^{10} 4 s^{1}$ and not $3 d^{9} 4 s^{2}$ . The ground state electronic configurations of the outer orbitals of transition elements are given in Table 8.1.

Uploaded: 2023-09-01T14:39:17.000Z
Duration: 16 min

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Updated on: Sep 1, 2023

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Chloe Discussed

In general the electronic configuration of outer orbitals of these elements is

(n - 1) d^{110} n s^{1 - 2}

. The

\underline{(n - 1) stands for the inner d orbitals which may}

have one to ten electrons and the outermost ns orbital may haye one or two electrons. However, this generalisation has several exceptions because of very little energy difference between (n-1)d and ns.orbitals. Furthermore, half and completely filled sets of orbitals are relatively more stable. A consequence of this factor is reflected in the electronic configurations of

Cr

and

Cu

in the

3 d

series. For example, consider the case of

Cr

, which has

3 d^{5} 4 s^{'}

configuration instead of

3 d^{4} 4 s^{2}

; the energy gap between the two sets (

3 d

and

4 s

) of orbitals is small enough to prevent electron entering the

3 d

orbitals. Similarly in case of

Cu

, the configuration is

3 d^{10} 4 s^{1}

and not

3 d^{9} 4 s^{2}

. The ground state electronic configurations of the outer orbitals of transition elements are given in Table 8.1.

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Question Text	In general the electronic configuration of outer orbitals of these elements is $(n - 1) d^{110} n s^{1 - 2}$ . The $\underline{(n - 1) stands for the inner d orbitals which may}$ have one to ten electrons and the outermost ns orbital may haye one or two electrons. However, this generalisation has several exceptions because of very little energy difference between (n-1)d and ns.orbitals. Furthermore, half and completely filled sets of orbitals are relatively more stable. A consequence of this factor is reflected in the electronic configurations of $Cr$ and $Cu$ in the $3 d$ series. For example, consider the case of $Cr$ , which has $3 d^{5} 4 s^{'}$ configuration instead of $3 d^{4} 4 s^{2}$ ; the energy gap between the two sets ( $3 d$ and $4 s$ ) of orbitals is small enough to prevent electron entering the $3 d$ orbitals. Similarly in case of $Cu$ , the configuration is $3 d^{10} 4 s^{1}$ and not $3 d^{9} 4 s^{2}$ . The ground state electronic configurations of the outer orbitals of transition elements are given in Table 8.1.
Updated On	Sep 1, 2023
Topic	Qualitative Analysis
Subject	Chemistry
Class	Class 12
Answer Type	Video solution: 1
Upvotes	64
Avg. Video Duration	16 min

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