Upon absorption of a quantum of light, the energy of the atom changed by 6 eV. Find the wavelength of the absorbed light?

The energy of a photon is proportional to the frequency of light: E = h * V, where h = 6.6 * 10 ^ -34 J * s is Planck’s constant, V is the frequency. Thus, the maximum wavelength of light that can cause ionization of an oxygen atom is:
λ = c / V = c / E / h = (c * h) / E.
In the data, the energy is given in eV, it is necessary to convert to joules 1 eV = 1.6 * 10 ^ -19 J.
We substitute the data into the formula and calculate.
λ = (6.6 * 10 ^ -34 * 3 * 10 ^ 8) / (6 * 1.6 * 10 ^ -19) = 2.0625 * 10 ^ -7 m = 206.25 * 10 ^ -9 m = 206.25 nm.