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Question

Ionization Energy (kJ/mol)
First896
Second1,752
Third14,807
Fourth17,948
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
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B
Group 2
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C
Group 3
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D
Group 4
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Solution

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.

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