Here's the breakdown:
* s orbitals: These are the lowest energy orbitals and are always filled first. Every element has electrons in s orbitals.
* p orbitals: These orbitals are higher in energy than s orbitals and are filled after the s orbitals. All elements from Boron (B) onwards have electrons in p orbitals.
* d orbitals: These are even higher in energy than p orbitals and are filled after the s and p orbitals. All elements from Scandium (Sc) onwards have electrons in d orbitals.
* f orbitals: These are the highest in energy and are filled after the s, p, and d orbitals. All elements from Lanthanum (La) onwards have electrons in f orbitals.
Therefore, any element with an atomic number greater than or equal to Lanthanum (La) will have electrons in all four types of orbitals (s, p, d, and f).
Examples:
* Lanthanum (La): [Xe] 5d¹ 6s²
* Gold (Au): [Xe] 4f¹⁴ 5d¹⁰ 6s¹
* Uranium (U): [Rn] 5f³ 6d¹ 7s²
Let me know if you'd like more specific examples or explanations!
