Question:
The outer electronic configuration of \(\mathrm{Pd}\) is
The outer electronic configuration of \(\mathrm{Pd}\) is
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Palladium is a well-known exception in electronic configuration. Its actual configuration is
\[
[\mathrm{Kr}]\,4d^{10}\,5s^0
\]
instead of the expected
\[
[\mathrm{Kr}]\,4d^8\,5s^2.
\]
A completely filled \(d\)-subshell provides additional stability.
Updated On: Jun 26, 2026
- \(4d^8\,5s^2\)
- \(4d^9\,5s^1\)
- \(4d^{10}\,5s^0\)
- \(4d^{10}\,5s^1\)
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The Correct Option is C
Solution and Explanation
Step 1: Identify the element.
Palladium (\(\mathrm{Pd}\)) has atomic number \[ Z=46 \] It belongs to the \(4d\)-series of transition elements.
Step 2: Write the expected electronic configuration.
According to the Aufbau principle, the expected configuration would be \[ [\mathrm{Kr}]\,4d^8\,5s^2 \] However, palladium is an exception to the expected filling order.
Step 3: Understand the exceptional configuration.
A completely filled \(d\)-subshell possesses extra stability due to symmetrical distribution and maximum exchange energy.
Therefore, two electrons from the \(5s\) orbital shift to the \(4d\) orbital, giving a completely filled \(4d\)-subshell.
Thus, the actual electronic configuration of palladium is \[ [\mathrm{Kr}]\,4d^{10}\,5s^0 \]
Step 4: Determine the outer electronic configuration.
Hence, the outer electronic configuration of \(\mathrm{Pd}\) is \[ 4d^{10}\,5s^0 \]
Step 5: Final conclusion.
Therefore, \[ \boxed{4d^{10}\,5s^0} \] Hence, the correct option is \[ \boxed{(3)} \]
Palladium (\(\mathrm{Pd}\)) has atomic number \[ Z=46 \] It belongs to the \(4d\)-series of transition elements.
Step 2: Write the expected electronic configuration.
According to the Aufbau principle, the expected configuration would be \[ [\mathrm{Kr}]\,4d^8\,5s^2 \] However, palladium is an exception to the expected filling order.
Step 3: Understand the exceptional configuration.
A completely filled \(d\)-subshell possesses extra stability due to symmetrical distribution and maximum exchange energy.
Therefore, two electrons from the \(5s\) orbital shift to the \(4d\) orbital, giving a completely filled \(4d\)-subshell.
Thus, the actual electronic configuration of palladium is \[ [\mathrm{Kr}]\,4d^{10}\,5s^0 \]
Step 4: Determine the outer electronic configuration.
Hence, the outer electronic configuration of \(\mathrm{Pd}\) is \[ 4d^{10}\,5s^0 \]
Step 5: Final conclusion.
Therefore, \[ \boxed{4d^{10}\,5s^0} \] Hence, the correct option is \[ \boxed{(3)} \]
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