Draw orbital box diagram to represent electronic configuration for Manganese.
This site does not support diagrams or drawings. Here is the orbital notation for 25Mn
25Mn 1s2 2s2 2p6 3s2 3p6 3d5 4s2
For the box diagram, note that all of the orbitals are FULL except 3d5 so place two electrons in each box for all except 3d5. For the 3d box place 1 electron in each of the 5 boxes.
To draw the orbital box diagram for Manganese (Mn), we need to understand its electronic configuration.
1. Determine the atomic number of Manganese: The atomic number of Manganese is 25, which means it has 25 electrons.
2. Follow the Aufbau principle: According to the Aufbau principle, electrons fill the orbitals from the lowest energy level to the highest. The orbitals are labeled as 1s, 2s, 2p, 3s, 3p, and so on.
3. Fill up the orbitals with electrons: Starting from the lowest energy level, fill up each orbital with the appropriate number of electrons, following the Pauli exclusion principle and Hund's rule.
The electronic configuration of Manganese (Mn) is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5
Now, let's draw the orbital box diagram:
1s: ↑↓
2s: ↑↓
2p: ↑↓ ↑↓ ↑
3s: ↑↓
3p: ↑↓ ↑↓ ↑
4s: ↑↓
3d: ↑↓ ↑↓ ↑↓ ↑↓ ↑
In the box diagram, each box represents an orbital, and the arrows represent electrons. The direction of the arrow indicates the spin of the electron, either up (↑) or down (↓).
Note: Manganese has an exception in its electronic configuration. Normally, the 4s orbital is filled before the 3d orbital. However, in Manganese, the 3d orbital gets filled before the 4s orbital, which results in the configuration 3d^5 4s^2. This anomaly occurs because half-filled or fully filled d orbitals are more stable than partially filled d orbitals.