factors effecting ionization energy,first,second third ionization energy complete article must follow link- googlegalaxychemistry.com /search ionization energy trend The ionization energy trend changes when move across period and group. It is quite evident that ionization enthalpy of elements are linked with their electronic configurations .in each period ionization energy maximum are found at noble gases while minimum energy to remove electron notice at the alkali metals

1. Periodic table
Trends and patterns of
properties in the periodic table

2. Nuclear Charge(protons)
What its function?
●
The attraction that an outer shell
electron feels towards the nucleus.
What effect down a group?
●
Remain Same
What effect across a period?
●
Increases; there are more electrons in the outer
shell which are greatly attracted to the nucleus.

3. Ionisation Energy
●
What is it?
●
Amount of energy required to
remove the highest energy electron
from an atom. (or steal one electron)
●
What happens down a group?
●
Decreases; since the size of the atom is increasing,
the attraction is weaker between the outer shell
electrons and the nucleus. Therefore electrons are
easier to remove.
●
What happens across a period?
●
Increases; since there is an increase in core charge,
the attraction is greater between the outer shell
electrons and the nucleus. Therefore electrons are
harder to remove.

4. Trends in Ionization energy
●
The ionization energy is the amount of energy it takes
to detach one electron from a neutral atom
●
Or How much energy it takes to steal an electron!!
●
If its easy to steal a electron it has low ionisation energy
●
If its hard to steal an electron it has a high ionisation
energy
●
The smaller the atom the harder to steal an electron
●
The larger the atom the easier it is to steal an electron

6. ●
As the period begins it does not take a lot of
energy to remove an electron from Li but as
you go across the period it takes more and
more energy to take an electron away

7. ●
b