The energy difference between the 5d and the 6s sublevels in gold accounts for its color. If this energy difference is about 2.7
eV (electron volt; 1 eV = 1.602 × 10−19 J), calculate the wavelength of light absorbed in the transition of an electron from the 5d subshell to the 6s subshell. Round the answer to the correct number of significant figures.
The light's wavelength absorbed during the transition is 459 nm. Energy difference between the 5-d and the 6-s sub-levels in gold is expressed as ΔE. Let the wavelength associated with the electron's transition from the 5-d to the 6-s state be λ. The relationship that describes the connection between energy and wavelength is defined as: E = hc/λ, where E stands for photon energy, h represents Planck's constant, c is the speed of light, and λ denotes the wavelength of the photon. Therefore, the absorption wavelength in this transition stands at 459 nm.
