Oxygen (O):

* Full configuration: 1s² 2s² 2p⁴

* Shorthand configuration: [He] 2s² 2p⁴

Sulfur (S):

* Full configuration: 1s² 2s² 2p⁶ 3s² 3p⁴

* Shorthand configuration: [Ne] 3s² 3p⁴

Explanation:

* Electron Configuration: Describes the arrangement of electrons in an atom's energy levels and orbitals.

* Principal Quantum Number (n): Indicates the energy level (e.g., 1, 2, 3).

* Sublevel (s, p, d, f): Indicates the shape of the orbital.

* s: Spherical

* p: Dumbbell-shaped

* d: More complex shapes

* f: Even more complex shapes

* Number of Electrons: The superscript indicates the number of electrons in that sublevel.

* Shorthand Configuration: Uses the previous noble gas to simplify the configuration.

Key Points:

* Oxygen and Sulfur are in the same group (Group 16, or the Chalcogens). This means they have similar valence electron configurations, leading to similar chemical properties.

* Valence Electrons: The outermost electrons (in the highest energy level) are responsible for an element's reactivity. For both oxygen and sulfur, their valence electrons are in the p sublevel.

Let me know if you have any other questions about electron configuration!