Ionization energy and ionization potential

Ionization energy is defined as the amount of energy required to remove the most loosely bound electron from an isolated gaseous atom in its ground state to produce a cation. Ionization energy is the smallest potential difference necessary to remove the most loosely bound electron from an isolated gaseous atom. It is also known as ionization potential. This process is represented as:

First (1st) ionization energy

The first ionization energy is the energy required to remove the first electron and convert M to M⁺.

Second (2nd) Ionization energy

The second ionization energy is the energy required to remove the second electron and convert M⁺ to M²⁺.

Third (3rd) Ionization energy

The third ionization energy is the energy required to remove the third electron and convert M²⁺ to M³⁺.

I.E₁ < I.E₂ < I.E₃ < I.E₄

Periodic table trends : Ionization energy

Along the period

In general, when we move from left to right in a period, the ionization energy increases with increasing atomic numbers. This tendency is explained by the combined impact of greater nuclear charge and decreasing atomic size, which causes electrons to become increasingly strongly linked to the nucleus. This results in a gradual increase in ionization energies.

Along the group

The ionization energy decreases in a group from top to bottom in a group. A gradual increase in atomic size is due to the addition of a new shell in each element as a result of an increase in nuclear charge. This factor tries to increase the ionization energy along with the group.

Factor affecting Ionization Energy

Atomic Size

Ionization energy decreases with an increase in atomic size. In a bigger atom, outer electrons are held less firmly and it becomes easier to remove the electron.

Magnitude of Nuclear Charge

The ionization energy increases with an increase in nuclear charge. The attractive force is directly proportional to the product of charges of the nucleus and that on electrons, therefore it becomes comparatively difficult to remove the electron.

Screening Effect or Shielding effect

The ionization energy decreases when the shielding or screening effect of the inner electrons increases.

In multi-electron atoms, the electrons in the valance shell are pulled by the nucleus and repelled by electrons of inner shells. Thus, outermost electrons experience less attraction from the nucleus under the combined effect of attractive and repulsive force acting on valance electrons. This effect is called the screening effect.

The actual charge felt by the valance shell electron as a result of this is called an effective nuclear charge (Z_eff).

Penetration Effect of Electron based on Shape of Orbital

If the electrons have a greater penetrating ability, they will be closer to the nucleus and will be held firmly by the nucleus. More energy is required to pull out the electron from the s-orbital than p, d, f orbitals. Hence ionization energy decreases in order s> p> d> f orbital.

Electronic Configuration

Half-filled or completely filled orbitals are more stable than others and hence more energy is needed to remove an electron from such atoms. Thus the more stable the electronic configuration, the greater will be the ionization energy.

p⁶ > d¹⁰ > p³ > d ⁵

Ionizaton energy of K, Li, Mg, Na, Ca, F, O and other Elements

FAQs / MCQs