To understand the orbital diagrams for Titanium (Ti), Oxygen (O), and Silicon (Si), we need to look at their electron configurations and how the electrons occupy different atomic orbitals.
Titanium (Ti)
Titanium has an atomic number of 22. Its electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d² 4s². The orbital diagram for Titanium will look like this:
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑ 3s: ↑↓ 3p: ↑↓ ↑↓ ↑ 4s: ↑↓ 3d: ↑↓ ↑
Oxygen (O)
Oxygen has an atomic number of 8. Its electron configuration is 1s² 2s² 2p⁴. The orbital diagram for Oxygen is as follows:
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑ ↑
Silicon (Si)
Silicon has an atomic number of 14. Its electron configuration is 1s² 2s² 2p⁶ 3s² 3p². The orbital diagram for Silicon appears as:
1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑ 3s: ↑↓ 3p: ↑↓ ↑
In these diagrams, each box represents an atomic orbital, while the arrows indicate electrons. An upward arrow (↑) signifies an electron with a spin of +1/2, and a downward arrow (↓) indicates an electron with a spin of -1/2. Electrons fill orbitals according to the Aufbau principle, Hund’s rule, and the Pauli Exclusion Principle.