To determine the electronic configuration for the most stable ion of Tungsten (W), let's follow the steps below:
1. Identify the Atomic Number of Tungsten:
- The atomic number of Tungsten (W) is 74. This means a neutral atom of Tungsten has 74 electrons.
2. Determine the Electronic Configuration for the Neutral Atom:
- We distribute the 74 electrons into the available orbitals using the Aufbau principle (increasing energy order), Pauli Exclusion Principle, and Hund's Rule:
- 1s: 2 electrons (1s2)
- 2s: 2 electrons (2s2)
- 2p: 6 electrons (2p6)
- 3s: 2 electrons (3s2)
- 3p: 6 electrons (3p6)
- 4s: 2 electrons (4s2)
- 3d: 10 electrons (3d10)
- 4p: 6 electrons (4p6)
- 5s: 2 electrons (5s2)
- 4d: 10 electrons (4d10)
- 5p: 6 electrons (5p6)
- 6s: 2 electrons (6s2)
- 4f: 14 electrons (4f14)
- 5d: 4 electrons (5d4)
So, the electronic configuration for a neutral Tungsten atom (W) is:
```plaintext
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d4
```
3. Determine the Most Stable Ion for Tungsten:
- The most stable ion for Tungsten is commonly W^6+, which means Tungsten loses 6 electrons to become stable.
4. Adjust the Electronic Configuration for the W^6+ Ion:
- To form W^6+, we need to remove 6 electrons from the neutral state's electron configuration, starting from the outermost orbitals:
- 6s2: Remove 2 electrons (since these are the highest energy electrons)
- 5d4: Next, remove 4 electrons from the 5d orbital
After removing 6 electrons (2 from 6s and 4 from 5d), we get the electronic configuration for W^6+:
```plaintext
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 4f14
```
Therefore, the electronic configuration for the most stable ion of Tungsten (W^6+) is:
```plaintext
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 4f14
```
