Value of `IE_(1), IE_(2), IE_(3)` of an element are `9.3, 18.2` and `553.8 eV`. Predict group number in Modern Periodic Table.

Answer

To determine the group number of the element based on its ionization energies (IE1, IE2, IE3), we can follow these steps:

### Step 1: Analyze the Given Ionization Energies
We have the following ionization energies:
- IE1 = 9.3 eV
- IE2 = 18.2 eV
- IE3 = 553.8 eV

### Step 2: Understand the Trend in Ionization Energies
Ionization energy generally increases as more electrons are removed from an atom. The first ionization energy (IE1) is the energy required to remove the first electron, the second ionization energy (IE2) is for removing the second electron, and so on.

### Step 3: Identify the Significant Jump in Ionization Energy
Notice that there is a significant jump between IE2 (18.2 eV) and IE3 (553.8 eV). This large increase suggests that after removing the second electron, the atom achieves a stable electronic configuration, likely resembling that of a noble gas.

### Step 4: Determine the Implication of the Jump
The large jump in ionization energy indicates that the element can lose two electrons relatively easily but requires a lot more energy to remove a third electron. This is characteristic of elements that have two valence electrons, which typically belong to Group 2 of the periodic table (the alkaline earth metals).

### Step 5: Conclusion
Since the element can lose two electrons to achieve a stable noble gas configuration and the third ionization energy is significantly higher, we conclude that the element belongs to Group 2 of the modern periodic table.

### Final Answer
The element belongs to Group 2 of the modern periodic table.

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