Question

you do a calculation on a molecule and determined that the energy of the highest occupied molecular orbital (homo) is -2.42 hartree, and the energy of the lowest unoccupied molecular orbital (lumo) is 0.65 hartree. what is the wavelength of the photon required to excite this molecule from its ground state, to its first excited state?

Answer 1

The wavelength of the photon required to excite this molecule from its ground state, to its first excited state is 1240 nm.

This is given by the equation:

wavelength = hc/(E_homo - E_lumo)

where h is Planck's constant =6.626070 * 10^-34 J.m , c is the speed of light = 3.0 x 10^8 m/s^2, and E_homo and E_lumo are the energies of the highest occupied molecular orbital and the lowest unoccupied molecular orbital, respectively.

In this particular case, the wavelength of the required photon would be:

wavelength = hc/(-2.42 hartree - 0.65 hartree)

= 6.626070 * 10^-34 X 3.0 x 10^8 / (-3.07)

= 1240 nm

Hence , The wavelength of the photon required to excite this molecule from its ground state, to its first excited state is 1240 nm.

Learn more about wavelength at : brainly.com/question/13533093

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