Given:

Ground State Energy = 2.18 × 10^–18 J atom^–1

The energy of hydrogen atom is given by the following equation:

En = -2n²me⁴Z²/n²h²

Where

m = mass of electrons

Z = atomic mass of atom

E = charge of electron

h = Planck’s constant

For the process mentioned in the question, energy required = E_n– E₁

= 0 – [-2n²me⁴ / 1²h²]

= 4 × 2n²me⁴/h²

But we know 2n²me⁴/h² = 2.18 × 10^-18J

= 4 × 2.18 × 10^-18

= 8.72 × 10^-18J

Therefore, the energy required for the process is 8.72 × 10^-18J