Question

write condensed electron configuration and partial diagram for Hf and explain how it gained or lost?

Answer 1

### Electron Configuration for Hafnium (Hf)

**Condensed Electron Configuration:**
\[ \text{[Xe]} \, 4f^{14} \, 5d^2 \, 6s^2 \]

**Explanation:**
Hafnium (atomic number 72) is located in the d-block of the periodic table and is classified as a transition metal. Here’s a breakdown of its electron configuration:

- The inner shell configuration up to xenon (Xe, atomic number 54) contains 54 electrons.
- Hafnium has a total of 72 electrons, so we take into account the additional electrons:
- The 4f subshell can hold 14 electrons, and in Hf, it is fully filled (\(4f^{14}\)).
- The 5d subshell has 2 electrons (\(5d^2\)).
- The 6s subshell has 2 electrons (\(6s^2\)).

### Partial Diagram

Here is a simplified energy level diagram illustrating the electron arrangement in Hafnium:

```
6s: ↑↓
5d: ↑↓
4f: ↑↑↑↑↑↑↑↑↑↑↑↑↑↑ (fully filled)
5p: (not occupied)
5s: (filled)
4d: (filled)
4p: (filled)
4s: (filled)
3d: (filled)
3p: (filled)
3s: (filled)
2p: (filled)
2s: (filled)
1s: (filled)
```

### Gaining or Losing Electrons

In typical chemical reactions and bonding contexts, hafnium usually tends to **lose electrons** to form positive ions. When Hf engages in bonding, especially in its compounds, it commonly achieves oxidation states of +4 (by losing the two \(5d\) and two \(6s\) electrons) or even +2 or +3 depending on the context.

- **Loss of Electrons:** When forming compounds, Hf typically loses its outermost electrons, which include both \(6s\) and \(5d\) electrons, given their higher energy and availability for bonding.

This tendency to lose electrons allows hafnium to participate in ionic or covalent bonding, contributing to its properties as a transition metal.