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  • Define ionization enthalpy discuss the factor affecting ionization enthalpy of the element and its trend in the periodic table   

Define ionization enthalpy. Discuss the factor affecting ionization enthalpy of the element and its trend in the periodic table.

 

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Ionization enthalpy is the amount of energy required to remove the most loosely bound electron from an isolated gaseous atom in its ground state.

Factors affecting Ionization Enthalpy

  1. Atomic size: Larger the atomic radius → outer electrons are farther → lower IE.

  2. Nuclear charge: Higher nuclear charge → stronger attraction → higher IE.

  3. Shielding effect: More inner electrons → stronger shielding → lower IE.

  4. Penetration effect of orbitals: Electrons in orbitals with greater penetration (s > p > d > f) are held more strongly → higher IE.

  5. Electronic configuration: Atoms with stable configurations (noble gases, half-filled or fully filled orbitals) have exceptionally high IE.

Trends in the Periodic Table

Across a period (left → right):

  • Atomic size decreases, nuclear charge increases.

  • Ionization enthalpy increases.

Down a group (top → bottom):

  • Atomic size increases, shielding effect increases.

  • Ionization enthalpy decreases.

 

Posted by

Saumya Singh

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