Question

What is the electronic configuration of palladium?

• A. \([Kr]\,5s^2\,4d^8\)
• B. \([Kr]\,5s^1\,4d^9\)
• C. \([Kr]\,4d^{10}\)
• D. \([Kr]\,5s^2\,4d^{10}\)

Hint:

Palladium is a famous exception. Its ground-state configuration is \([Kr]\,4d^{10}\) with an empty \(5s\) orbital.

Answer 1

The Correct Option is C

Concept: Palladium is one of the exceptional transition elements that does not follow the expected Aufbau filling pattern. Its atomic number is: \[ Z=46 \] The expected configuration would be: \[ [Kr]\,5s^2\,4d^8 \] However, greater stability is achieved when the \(4d\) subshell becomes completely filled.

Step 1: Determine the atomic number. Palladium contains: \[ 46 \text{ electrons} \] The first 36 electrons constitute the krypton core. \[ [Kr] \]

Step 2: Apply the exceptional configuration rule. Instead of \[ [Kr]\,5s^2\,4d^8 \] electrons rearrange to produce a completely filled \(4d\) subshell. \[ [Kr]\,4d^{10} \]

Step 3: Identify the correct option. The accepted electronic configuration of palladium is: \[ \boxed{[Kr]\,4d^{10}} \] Therefore, the correct option is \[ \boxed{(C)} \]