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In order to write the electron configuration for each element, we have to first find their atomic numbers. The atomic number (Z) of an element is equal to the number of electrons in a neutral atom of that element. Oxygen has an atomic number (Z) of 8, which means it has 8 electrons. Sulfur has an atomic number (Z) of 16, which means it has 16 electrons. Now, we will write the electron configuration and orbital notation for these atoms.

Using the Aufbau principle and remembering the Pauli Exclusion Principle, we will fill the orbitals in increasing order of energy. Oxygen (Z = 8): 1s^2 2s^2 2p^4 Sulfur (Z = 16): 1s^2 2s^2 2p^6 3s^2 3p^4

Keeping Hund's Rule in mind, which states that electrons will fill degenerate orbitals singly before pairing up, we will represent the electron configuration in the orbital notation. For Oxygen (Z = 8): ``` 1s: [↑↓] 2s: [↑↓] 2p: [↑ ↑ ↑ ] [↓ ↓ (empty)] ``` For Sulfur (Z = 16): ``` 1s: [↑↓] 2s: [↑↓] 2p: [↑ ↑ ↑ ] [↓ ↓ ↓ ] 3s: [↑↓] 3p: [↑ ↑ ↑ ] [↓ ↓ (empty)] ``` In conclusion, the electron configuration for oxygen is 1s^2 2s^2 2p^4, and its orbital notation is as shown above. The electron configuration for sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4, and its orbital notation is also shown above.