Ionization Energy Trends in Periodic Table
Ionization Energy follows a specific trend while moving from Left to Right and Top to Bottom in the periodic table.
The image given below shows the trend of variation of Ionization Energy while moving left to right and top to bottom in the periodic table.
Left to Right in a Period
As we move from left to right in a period in the periodic table the atomic radius decreases. It is due to the reason that the elements start gaining near noble gas configuration as we move across the period. Due to this interelectronic repulsion is reduced and the atomic radius decreases. Hence the electrons are more tightly held by the nucleus. Hence a higher amount of energy is required to remove the electrons. Thus IE increases as we move across a period.
Top to Bottom in a Group
As we move from top to bottom in a group, new shells are added up and the electrons start to occupy higher orbitals and shells. Thus the atomic radius also increases. The electrons are now far away from the nucleus. So lesser amount of energy is required to remove the electron. Thus IE decreases as moves down a group.
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Ionization Energy
Ionization energy can be defined as the minimum amount of energy required to remove the valence electron i.e. the most loosely bound electron from an isolated gaseous atom or ion. It is important to note the term isolated gaseous atom as if the atom is not isolated, then the energy required may be more due to the interatomic forces.
Let’s learn about Ionization Energy in detail in this article.
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