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The energy required to remove an electron from an isolated gaseous
atom in its ground state is known as ionisation enthalpy. Despite the fact that
the atoms are far separated in the gaseous state, there are some attraction
forces between them. It is impossible to isolate a single atom to calculate the
ionisation enthalpy. However, by lowering the pressure, the power of attraction
can be reduced much more. As a result, in the definition of ionisation
enthalpy, the term "isolated gaseous atom" is employed.
The most stable state of an atom is called the ground state. If an
isolated gaseous atom is in its ground state, removing an electron from it will
need less energy. As a result, ionisation enthalpy and electron gain enthalpy
for an ‘isolated gaseous atom' and its ‘ground state' must be established for
comparison reasons.
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