1s² 2s² 2p⁶ 3s² 3p⁴

Here's a breakdown:

* 1s²: The first energy level (n=1) has one subshell (s), which can hold 2 electrons.

* 2s²: The second energy level (n=2) has one s subshell, which can hold 2 electrons.

* 2p⁶: The second energy level (n=2) also has three p subshells, each holding 2 electrons, for a total of 6 electrons.

* 3s²: The third energy level (n=3) has one s subshell, which can hold 2 electrons.

* 3p⁴: The third energy level (n=3) has three p subshells, but only 4 electrons occupy them.

Important Note: This is the ground state electron configuration. It's possible for sulfur to have an excited state configuration where electrons are temporarily promoted to higher energy levels.