Question

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

• A. Group 4
• B. Group 14
• C. Group 2
• D. Group 13

Hint:

A sharp increase in ionisation energy suggests that the element has reached a stable electron configuration (typically after the removal of the last valence electron).

Answer 1

The Correct Option is B

Ionisation energy increases with the removal of each electron, but there is a significant jump in ionisation energy when the element reaches a stable electron configuration. A sharp rise in ionisation energy, as seen after the second ionisation energy, indicates the removal of an electron from a stable configuration, which suggests that the element belongs to Group 14.

Final Answer: Group 14.

Answer 2

Step 1: Understand the concept of ionization energies.
Ionization energy refers to the energy required to remove an electron from a gaseous atom or ion. The successive ionization energies represent the energy required to remove each subsequent electron, starting from the outermost electron.

In general, as electrons are removed from an atom, the ionization energy increases because the remaining electrons experience a stronger attraction from the nucleus. However, there is often a significant increase in ionization energy when a new shell or energy level is reached, which corresponds to the removal of an electron from a more stable, more tightly bound core shell.

Step 2: Analyze the given ionization energies.
The successive ionization energies are:
1st: 800 kJ/mol
2nd: 2427 kJ/mol
3rd: 3658 kJ/mol
4th: 25024 kJ/mol
5th: 32824 kJ/mol
We observe a large jump in the ionization energy between the 3rd and 4th ionization energies (from 3658 kJ/mol to 25024 kJ/mol). This significant increase suggests that the 4th electron is being removed from a more stable core shell, indicating that the first three electrons are in the outermost shell, and the 4th is in a more tightly bound inner shell.

Step 3: Determine the group of the element.
The large jump in ionization energy between the 3rd and 4th ionizations suggests that the element has 4 valence electrons, which is characteristic of Group 14 elements in the periodic table (such as carbon, silicon, germanium, etc.).

Final Answer:
\[ \boxed{\text{Group 14}}. \]