The first `(IE_(1))` and second `(IE_(2))` ionisation energies `(k J mol^(-1))` of a new elements designated by roman numerals are shown below:
`{:(,,IE_(1),IE_(2),),(I,,2370,5250,),(II,,520,7300,),(III,,900,1800,),(IV,,1700,3400,):}`
Which of the above elements is likely to be :
a. A reactive metal
b. A reactive non-metal
c. a noble gas
d. A metal that forms a stable binary halide of the formula `AX_(2)` (`X=` the halogen).

Explanation

To solve the problem, we need to analyze the given ionization energies (IE) of the four elements and determine their chemical properties based on these values.

### Step-by-Step Solution:

1. **Identify the Ionization Energies:**
We have the following ionization energies for the four elements:
- Element I: IE₁ = 2370 kJ/mol, IE₂ = 5250 kJ/mol
- Element II: IE₁ = 520 kJ/mol, IE₂ = 7300 kJ/mol
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