1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p²
Here's how it breaks down:
* 1s²: The first energy level (n=1) has 2 electrons in the s orbital.
* 2s²: The second energy level (n=2) has 2 electrons in the s orbital.
* 2p⁶: The second energy level (n=2) has 6 electrons in the p orbital.
* 3s²: The third energy level (n=3) has 2 electrons in the s orbital.
* 3p⁶: The third energy level (n=3) has 6 electrons in the p orbital.
* 4s²: The fourth energy level (n=4) has 2 electrons in the s orbital.
* 3d¹⁰: The third energy level (n=3) has 10 electrons in the d orbital.
* 4p²: The fourth energy level (n=4) has 2 electrons in the p orbital.
This configuration reflects the order in which electrons fill orbitals, following the Aufbau principle and Hund's rule.
