Question

How ionisation enthalpy and the electron gain enthalpy affect the formation of an ionic bond .

Answer 1

Ionisation energy is the amount of energy, which is required to remove the most loosely bound electrons from an isolated gaseous atom to form a positive ion.
In forming an ionic bond, one atom must form a cation by losing one or more electrons. That is xelements having low ionisation energies have a more favourable chance to form a cation, thereby having a greater tendency to form ionic bonds.
Thus, lower ionization energy of metallic elements favours the formation of an ionic bond

It is defined as the amount of energy released when an extra electron is added to an isolated gaseous atom t o form gaseous anion.

higher the electron gain enthalpy ,more is the quantity of energy released and easier the formation of ionic bond.


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Answer 2

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⇒Atoms of same elements gain electrons while forming ionic compounds. An atom is able to gain an electron only when the electron outside the atom is attracted by its nucleus. Attraction involves the liberation of energy..

⇒The electron affinity or electron gain enthalpy of an element is defined as the energy liberated when an electron is added to its neutral gaseous atom...

⇒The energy required to remove an electron from the outermost orbit or shell of a neutral gaseous atom is called ionization enthalpy/ potential/ energy...it is expressed in kJ mol⁻¹.....Always I₁ < I₂

→The Condition required for the formation of an ionic bond between two Elements are: Two elements must be of opposite charge. An element must have its less Ionisation Enthalpy(Cation). Another element must have high negative electron gain enthalpy(Anion).

→Thus, the low ionization energy of a metal atom and high electron affinity of a non-metal atom facilitate the formation of an ionic bond between them.

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