Copper is a transition metal with an atomic number of 29. What is the ground-state electro… — JAMB UTME

Copper is a transition metal with an atomic number of $29$ . What is the ground-state electronic configuration of the copper(II) ion ( $Cu^{2+}$ ) present in copper compounds such as copper(II) tetraoxosulfate(VI)?

$[Ar] 3d^9$ Answer
B
$[Ar] 3d^8 4s^1$
C
$[Ar] 3d^7 4s^2$
D
$[Ar] 3d^{10} 4s^1$

Answer

The ground-state electronic configuration of the copper(II) ion (

Cu^{2+}

) is

[Ar] 3d^9

The correct answer specifies

[Ar] 3d^9

. Neutral copper has a ground-state configuration of

[Ar] 3d^{10} 4s^1

. Ionization to form

Cu^{2+}

requires losing two electrons; the first comes from the outermost

4s

orbital, and the second comes from the

3d

subshell, leaving

[Ar] 3d^9

Step-by-Step Solution

Determine the electronic configuration of a neutral copper atom (

Cu, Z=29

Neutral copper has the ground-state configuration

[Ar] 3d^{10} 4s^1

(anomalous filling for extra stability of a full d-subshell).

A completely filled

3d^{10}

subshell provides lower overall energy than a

3d^9 4s^2

arrangement.

Identify which electrons are removed when forming the

Cu^{2+}

ion.

Two electrons must be removed: 1 electron from the

4s

orbital and 1 electron from the

3d

orbital.

Electrons in the outermost principal quantum level (

n=4

) are always removed first during cation formation.

Write the final electronic configuration of

Cu^{2+}

[Ar] 3d^9

Subtracting

1

electron from

4s

and

1

electron from

3d^{10}

leaves

9

electrons in the

3d

subshell and

0

4s

Key Concept

Electronic configuration of transition metal cations and anomalous electron filling in copper.

Estimated Time:1m 0s

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Answer

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