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  • The successive ionization energies for an element is given below <img alt="\mathrm{ IE_1 : 590 kJ\: mol^{-1}}" src="/latex-im

The successive ionization energies for an element \mathrm{X} is given below

\mathrm{ IE_1 : 590 kJ\: mol^{-1}}
\mathrm{IE_2:1145 kJ\: mol^{-1}}
\mathrm{IE_3 : 4912 kJ \: mol^{-1}}
\mathrm{IE_4 : 6491 kJ\: mol^{-1}}
Find out the number of valence electrons for the element \mathrm{X.}

Option: 1

3


Option: 2

4


Option: 3

2


Option: 4

1


Answers (1)

best_answer

On close observation, it is evident that there is a big jump in IE2 and IE3 as compared to other successive IEs. It implies that it requires huge ionisation energy to remove a third electron from the element. The element must be belonging to Group 2 and has two valence shell electrons.

Hence Option 3 is correct.

Posted by

sudhir kumar

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