Question

	Ionization Energy $\left(kJ/mol\right)$
First	$896$
Second	$1,752$
Third	$14,807$
Fourth	$17,948$

The table above shows the first four ionization energies of an element. This element is located in which group of the periodic table?

• A. Group $1$
• B. Group $2$
• C. Group $3$
• D. Group $4$

Answer 1

The correct option is A Group $1$

The third IE is very much higher than second IE. Thus the element attains inert gas configuration on removal of $2$ electrons. Thus the element belongs to group $2$; because the group $2$ elements have $2$ valence electrons and on removal of those, the element attains inert gas configuration.