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# How do you calculate the ionization energy of an element?

Last updated date: 13th Jun 2024
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Hint: The minimum amount of energy required to remove an electron from the valence shell of a gaseous atom is called ionization energy. If we remove the first electron by using a certain amount of energy then it is called first ionization energy and vice versa.

- In the question it is asked to write the formula to calculate the ionization energy of an element.
- The formula to calculate the ionization energy of an element is as follows.
$\Delta {{E}_{i}}=A\left( \dfrac{1}{n_{f}^{2}}-\dfrac{1}{n_{i}^{2}} \right)$
Where $\Delta {{E}_{i}}$ = ionization energy
A = $2.18\times {{10}^{-18}}$ joules
${{n}_{f}}$ = final energy level
${{n}_{i}}$ = starting energy level
- By using the above formula we can calculate the ionization of any electron from any orbit in the element.
- By using ionization energy values we can easily find the stability of the atom or element.
- If the ionization value is too high means the atom or element is more stable means not interested to lose electrons easily.
- The ionization energy is inversely proportional to atomic radii.
- If the atomic radius of an atom or element is too high then the ionization energy will be less and vice versa.

Note:
Ionization energy value is going to decrease as we are moving from left to right in the periodic table due to decrease of the atomic radii along the periods. Ionization energy is going to increase along the groups means as we are moving from top to bottom in the periodic table.