Question

Given that the wavelength of maximum absorption for chromium is 574.7 nm, what is the energy per Cr atom of the transition for an electron to move from one d orbital to another of higher energy? (h = 6.626 x 10-34 Js/particle, c = 3x108 m/s)

Answer 1

`E=3.46* 10^(-19)\ J/atom`

Step-by-step explanation:

`E=\frac {h* c}{\lambda}`

Where,

h is Plank's constant having value
`6.626* 10^(-34)\ Js/atom`

c is the speed of light having value
`3* 10^8\ m/s`

`\lambda` is the wavelength of the light

Given,
`\lambda=574.7\ nm=574.7* 10^(-9)\ m`

Thus, applying values as:

`E=(6.626* 10^(-34)* 3* 10^8)/(574.7* 10^(-9))\ J`

`E=(10^(-26)* \:19.878)/(10^(-9)* \:574.7)\ J/atom`

`E=3.46* 10^(-19)\ J/atom`