Ineed asap come and asap. describe the trends in first ionization energy within groups and across periods in the periodic table. provide examples.

Solution:- Ionization energy increases on going left to right and decreases on going top to bottom in the periodic table.

Explanations:- Ionization energy is the energy required to remove the electron from outer most shell of a gaseous atom. It increases left to right in periodic table as the size of the atom decreases and it's hard to remove electron from outer most shell.

The size decreases on going left to right because the electrons are keep added to the same energy shell and so the effective nuclear charge increases . Due to the more effective nuclear charge, more energy is required to remove the electron from outer most shell.

For example, Ionization energy of F is greater than O. electron configuration of O is and for F it is . From electron configurations, both the elements have valence electrons in the second shell but F has more protons means more nuclear charge. So, the size of F is smaller and hence it's harder to remove electron from F than O.

On going too to bottom in periodic table, the new shell is added and so the size of atom increases. It's easy to remove electron from a bigger atom and hence the ionization energy decreases.

Example:- Ionization energy for Li is greater than Na. electron configurations for Li and Na are and . From electron configurations it is clear that Li has valence electron in second shell where as Na has valence electron in third shell. So, the size of Na is bigger than Li, and it needs less energy to remove valence electron from Na as compared to Li.

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