The ionization energy of the hydrogen atom is 13.6 eV. What is the wavelength of a photon having this much energy? (h = 6.63 * 10 ^- ³⁴J.s, c = 3.00 *10⁸ m/s, 1 eV = 1.6 *10 ^- ¹⁹ J, and 1 nm = 10 ^- ⁹ m) A) 91.4 nm B) 360 nm C) 136 nm D) 273 nm

Question

Quizplus · Accepted Answer

The energy of the photon is 13.6 eV, which is equivalent to 13.6 x 1.6 x 10^-19 J. Using the formula E = hc/λ, where h is Planck's constant and c is the speed of light, we can solve for λ (wavelength). Substituting the values, λ = (6.63 x 10^-34 J·s x 3.00 x 10^8 m/s) / (13.6 x 1.6 x 10^-19 J) = 91.4 nm.

The Ionization Energy of the Hydrogen Atom Is 13