The energy difference between two electronic states is 43.56 kcal/mo. The frequency of light emitted when the electron drops from higher orbit to lower orbit, is
(Planck's constant`=9.52xx10^(-14)kcal//mol`)

The energy difference between two electronic states is 46.12 "kcal"//"mol" . What will be the freqency of the light emitted when an electron drops from the higher to the lower energy state ? (Planck' constant = 9.52 xx 10^-14 kcal sec mol^-1 )

If the energy difference between the electronic states is 214.68 kJmol^(-1) calculate the frequency of light emitted when an electron drop form the higher to the lower state planks constant , h = 39.79 xx 10^(-14)kJmol^(-1)

The energy difference between two electronic states is 399.1 kJ mol^(-1) . Calculate the wavelength and frequency of light emitted when an electron drops from a higher to a lower state. (Planck's constant, h = 3.98 xx 10^(-13) kJ mol^(-1)) .

If the energy different between the electronic stazte in 214.68 mol^(-1) calculate the frequency of light emited when an electron drop form the hight to the lower state planks constant , h = 39,79 xx 10^(-14)kJmol^(-1)

Two energy levels of an electron in an atom are separated by 2.3 eV. The frequency of radiation emitted when the electrons go from higher to lower level is

Calculate the frequency nad wave length of the energy emitted when the electron jumps from 4th orbit to 1st orbit of a H-atom.

when a certain energy is applied to an hydrogen atom, an electron jumps from n =1 to n = 3 state. Find (i) the energy absorbed by the electron. (ii) wavelength of radiation emitted when the electron jump back to its initial state. ( Energy of electron in first orbit = - 13.6 eV , Planck's constant = 6.6225 xx10^(-34) Js, Charge on electron = 1.6 xx10^(-19) C, speed of light in vacuum = 3xx10^(8)ms^(-1)