Ionisation potential or ionisation energy
The electrons in an atom are attracted by the nucleus. At the time when an electron is to be removed then work is done against this nuclear attraction. Or we can say that the energy is required to remove an electron from an atom. To understand the details of chemical behaviour of an element we must have an indication of the energy with which an atom binds its electrons. This is obtained by the measurement of ionisation potential or ionisation energy. It may be defined as the energy needed to remove the electron from the outermost orbit of an isolated gaseous atom in its ground state. It is expressed in electron volts (eV) or kilo calories per gram atom. In an atom, the energy needed to remove first electron from a gaseous atom is known as first ionisation energy. The energy needed to eliminate one electron from a unipositive ion to form a bipositive ion is called second ionisation energy. Second ionisation energy is higher than the first. The cause is that in unipositive ion left after the removal of one electron from the atom, the electrons are more tightly bound to the nucleus than in the atom. Therefore more energy is needed to remove the second electron.
Similarly, third ionisation energy is even more than second ionisation energy.
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