The successive 5 ionisation energies of an element are $800,2427,3658,25024$ and $32824 \mathrm{~kJ} / \mathrm{mol}$, respectively. By using the above values predict the group in which the above element is present :

<p>We can determine the number of valence electrons by looking for a large jump in successive ionization energies. Here's how we can analyze the data:</p> <p>The ionization energies given are:</p> <p><p>$IE_1 = 800 \, \text{kJ/mol}$ </p></p> <p><p>$IE_2 = 2427 \, \text{kJ/mol}$ </p></p> <p><p>$IE_3 = 3658 \, \text{kJ/mol}$ </p></p> <p><p>$IE_4 = 25024 \, \text{kJ/mol}$ </p></p> <p><p>$IE_5 = 32824 \, \text{kJ/mol}$</p></p> <p>Notice that:</p> <p><p>The first three ionization energies are relatively low.</p></p> <p><p>There is a significant jump between the third and fourth ionization energy. </p></p> <p>What does the gap indicate?</p> <p><p>The large jump from $IE_3$ to $IE_4$ means that after removing the first three electrons (which are the valence electrons), the next electron to be removed (a core electron) is much more strongly bound.</p></p> <p><p>This implies that the element has 3 valence electrons.</p></p> <p>Which group does an element with 3 valence electrons belong to?</p> <p>Elements with 3 valence electrons are found in Group 13 of the periodic table.</p> <p>Thus, the element most likely belongs to Group 13.</p> <p>Correct Answer: Option C (Group 13).</p>