# Find the Ionisation Potential and Electron affinity of X

$$N_0/2$$ atoms of $$X_{(g)}$$ are converted into $$\ce{X^+_{(g)}}$$ by energy $$E_1$$. $$N_0/2$$ atoms of $$X_{(g)}$$ are converted into $$\ce{X^-_{(g)}}$$ by energy $$E_2$$. Hence ionisation potential and electron affinity of $$\ce{X_{(g)}}$$ per atom are:

I tried solving this by unitary method, which gave ionisation potential and electron affinity as, $${2E_1/N_0}$$, $${2E_2/N_0}$$ respectively.

But the answer given is $${2E_1/N_0}$$, $${2(E_2-E_1)/N_0}$$

Can anyone please tell me where I went wrong and help me with the solution. Thanks in advance!

The Ionisation Energy of an atom is defined as the minimum amount of energy required to remove the most loosely bound electron of an isolated neutral gaseous atom or molecule. In this case, since $$E_1$$ amount of energy is used to ionise $$N_0/2$$ atoms, the ionisation energy of each atom is $$\frac{E_1}{N_0/2} = \frac{2E_1}{N_0}$$.
The Electron Affinity is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion. In this case, $$E_2$$ amount of energy is released when $$N_0/2$$ atoms accept electrons to form negative ions, hence electron affinity of each atom is $$\frac{E_2}{N_0/2} = \frac{2E_2}{N_0}$$.
$$N_0/2$$ atoms of $$\ce{X+_{(g)}}$$ are converted into $$\ce{X−_{(g)}}$$ by energy $$E_2$$
This gives the answer as $$\frac{E_2 - E_1}{N_0/2} = \frac{2(E_2 - E_1)}{N_0}$$ for electron affinity.