Chapter : 7. Periodic Classification of Element
Variation of Ionisation energy
Variation of Ionisation energy down a Group :
Ionisation energy goes on decreasing down a group.
Reason : It is due to the increase in the distance between the valence electrons and the nucleus as the atomic size increase down a group, the force of attraction between the nucleus and the valence electrons decrease, therefore, the energy required to remove the electrons, i.e., the ioisation energy goes on decreasing.
Example :
Variation of Ionisation energy along a Period :
It goes on increasing generally along a period from left to right with decrease in atomic size.
Reason : Due to decrease in atomic size, the force of attraction between the valence electrons and the nucleus increase and, therefore, more energy is required to remove electron.
Example :
There is a decrease in ionisation energy from Be to B and from N to O, the reason of which you will study in higher classes.
Group 18 elements (noble gases) have the highest ionisation energy in respective periods due to stable electronic configuration, i.e., 8 electrons in their valence shells except He which has 2 electrons.
Ionisation energy goes on decreasing down a group.
Reason : It is due to the increase in the distance between the valence electrons and the nucleus as the atomic size increase down a group, the force of attraction between the nucleus and the valence electrons decrease, therefore, the energy required to remove the electrons, i.e., the ioisation energy goes on decreasing.
Example :
Variation of Ionisation energy along a Period :
It goes on increasing generally along a period from left to right with decrease in atomic size.
Reason : Due to decrease in atomic size, the force of attraction between the valence electrons and the nucleus increase and, therefore, more energy is required to remove electron.
Example :
There is a decrease in ionisation energy from Be to B and from N to O, the reason of which you will study in higher classes.
Group 18 elements (noble gases) have the highest ionisation energy in respective periods due to stable electronic configuration, i.e., 8 electrons in their valence shells except He which has 2 electrons.
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