The `IP_(1),IP_(2),IP_(3),IP_(4)` and `IP_(5)` of an element are `7.1, 14.3, 34.5, 46.8, 162.2V` respectively. The element is likely to be -

Options

A. `Na`
B. `Si`
C. `F`
D. `Ca`

Explanation

To determine the element based on the given ionization potentials (IP1, IP2, IP3, IP4, and IP5), we can analyze the provided values step by step.

### Step-by-Step Solution:

1. **Identify the Ionization Potentials**:
- The given ionization potentials are:
- IP1 = 7.1 V
- IP2 = 14.3 V
- IP3 = 34.5 V
- IP4 = 46.8 V
- IP5 = 162.2 V

2. **Analyze the Differences Between Ionization Potentials**:
- Calculate the differences between consecutive ionization potentials:
- Difference between IP1 and IP2: 14.3 - 7.1 = 7.2 V
- Difference between IP2 and IP3: 34.5 - 14.3 = 20.2 V
- Difference between IP3 and IP4: 46.8 - 34.5 = 12.3 V
- Difference between IP4 and IP5: 162.2 - 46.8 = 115.4 V

3. **Identify the Significant Increase**:
- Notice that the difference between IP4 and IP5 (115.4 V) is significantly larger than the differences between the previous ionization potentials. This indicates that removing the fifth electron requires a lot more energy, suggesting that the first four electrons are relatively easier to remove.

4. **Determine the Number of Electrons that Can Be Removed**:
- The large jump in energy required to remove the fifth electron suggests that the element has four valence electrons. After removing these four electrons, the element achieves a stable electronic configuration similar to that of a noble gas.

5. **Identify the Element**:
- Elements with four valence electrons are typically found in Group 14 of the periodic table. The most common element with four valence electrons is silicon (Si), which has the electronic configuration of:
- 1s² 2s² 2p⁶ 3s² 3p²
- After removing four electrons, silicon would achieve the configuration of neon (a noble gas).

6. **Conclusion**:
- Based on the analysis of the ionization potentials and the electronic configuration, the element is likely to be **Silicon (Si)**.