An octahedral complex of a d¹ transition metal complex has D = 203 kJ/mol. At what wavelength does this complex absorb light?

Question

Quizplus · Accepted Answer

The energy of the absorbed light (D) is related to the wavelength (λ) by the equation $E = \frac{hc}{\lambda}$, where $h$ is Planck's constant (6.626 x 10^-34 J·s) and $c$ is the speed of light (3.00 x 10^8 m/s). Rearranging for $\lambda$, we get $\lambda = \frac{hc}{E}$. Substituting $E = 203 \times 10^3 J/mol$ (or 203 kJ/mol), $h = 6.626 \times 10^{-34} J·s$, and $c = 3.00 \times 10^8 m/s$ into the equation gives a wavelength in the range of option B, which is approximately 5.90 x 10^-7 m or 590 nm.

An Octahedral Complex of a D1 Transition Metal Complex Has

An Octahedral Complex of a D¹ Transition Metal Complex Has