The value of `IE_(1), IE_(2), IE_(3)` and `IE_(4)` of an atom are respectively `7.5 eV, 25.6 eV, 48.6 eV` and `170.6 eV`. The electronic configuration of the atom will be

Options

A. `1s^(2), 2s^(2)2p^(6), 3s^(1)`
B. `1s^(2)2s^(2)2p^(6)3s^(2) 3p^(1)`
C. `1s^(2), 2s^(2)2p^(6)3s^(2)3p^(3)`
D. `1s^(2), 2s^(2)2p^(6)3s^(2)`

Explanation

To determine the electronic configuration of the atom based on the provided ionization energies (IE), we can follow these steps:

### Step 1: Analyze the Ionization Energies
We have the following ionization energies:
- \( IE_1 = 7.5 \, \text{eV} \)
- \( IE_2 = 25.6 \, \text{eV} \)
- \( IE_3 = 48.6 \, \text{eV} \)
- \( IE_4 = 170.6 \, \text{eV} \)

### Step 2: Calculate the Differences Between Ionization Energies
Next, we will calculate the differences between consecutive ionization energies to identify trends:
- Difference between \( IE_1 \) and \( IE_2 \):
\[ 25.6 - 7.5 = 18.1 \, \text{eV} \]
- Difference between \( IE_2 \) and \( IE_3 \):
\[ 48.6 - 25.6 = 23.0 \, \text{eV} \]
- Difference between \( IE_3 \) and \( IE_4 \):
\[ 170.6 - 48.6 = 122.0 \, \text{eV} \]

### Step 3: Identify the Significant Increase in Ionization Energy
From the differences calculated:
- The first and second ionization energies have a moderate increase.
- The second and third ionization energies also show a moderate increase.
- However, there is a significant jump in the energy required to remove the fourth electron (from 48.6 eV to 170.6 eV).

### Step 4: Conclusion on Valence Electrons
The large increase in ionization energy from \( IE_3 \) to \( IE_4 \) suggests that after removing three electrons, the atom reaches a stable electronic configuration, likely resembling that of a noble gas. This indicates that the atom has three valence electrons.

### Step 5: Determine the Electronic Configuration
Elements with three valence electrons typically belong to Group 13 of the periodic table. The electronic configuration for an element with three valence electrons (like Aluminum, which has the configuration of \( [Ne] 3s^2 3p^1 \)) can be represented as:
\[ \text{Electronic Configuration: } [Ne] 3s^2 3p^1 \]

### Final Answer
The electronic configuration of the atom is \( [Ne] 3s^2 3p^1 \).

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