* Atomic Number: 16

* Electronic Configuration: 1s² 2s² 2p⁶ 3s² 3p⁴

Explanation:

* 1s²: The first energy level (n=1) has 2 electrons in the 1s orbital.

* 2s²: The second energy level (n=2) has 2 electrons in the 2s orbital.

* 2p⁶: The second energy level (n=2) has 6 electrons in the 2p orbitals (2px, 2py, 2pz).

* 3s²: The third energy level (n=3) has 2 electrons in the 3s orbital.

* 3p⁴: The third energy level (n=3) has 4 electrons in the 3p orbitals (3px, 3py, 3pz).

Visual Representation:

You can represent this electronically with an orbital diagram:

```

1s 2s 2p 3s 3p

↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑

```

Key Points:

* Valence Electrons: Sulfur has 6 valence electrons (the electrons in the outermost energy level, n=3). These are the electrons involved in chemical bonding.

* Reactivity: The presence of only 4 electrons in the 3p orbitals makes sulfur reactive, seeking to gain 2 more electrons to achieve a stable octet configuration.

Let me know if you have any other questions!