1. Determine the Electron Configuration:
* Atomic Number: Germanium has an atomic number of 32, meaning it has 32 electrons.
* Electron Configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p²
2. Understand the Orbital Filling Rules:
* Aufbau Principle: Electrons fill orbitals in order of increasing energy.
* Hund's Rule: Within a subshell, electrons individually occupy each orbital before doubling up in any one orbital.
* Pauli Exclusion Principle: Each orbital can hold a maximum of two electrons, with opposite spins.
3. Draw the Orbital Diagram:
* Represent Orbitals: Use boxes to represent each orbital.
* Label Subshells: Label the subshells (1s, 2s, 2p, etc.)
* Fill Orbitals: Place arrows (representing electrons) within the boxes, following the filling rules.
Orbital Diagram for Germanium:
```
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑↓
3s: ↑↓
3p: ↑↓ ↑↓ ↑↓
4s: ↑↓
3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p: ↑ ↑
```
Explanation:
* 1s, 2s, 2p, 3s, 3p: These orbitals are completely filled with two electrons each.
* 4s: This orbital is also filled with two electrons.
* 3d: The 3d subshell has five orbitals and is completely filled with 10 electrons.
* 4p: The 4p subshell has three orbitals. Germanium has only two electrons in the 4p subshell, which occupy separate orbitals according to Hund's Rule.
Important Note: The orbital diagram shows the arrangement of electrons in the ground state of Germanium. The actual electron configuration in excited states may differ.
