Question

Post-Laboratory Questions What is the identity of a HYDROGEN-LIKE cation that has the following energy levels? (show calculations) E -3,485 x 10-17 E -8.712 x 10-18 E = -3.872 x 10-J Refer to the diagram below. a) Complete the diagram below to show all possible transitions when electrons go from the n-5 state to the n-2 state in hydrogen? b) Based on the number of transitions, which transition in to n) leads to the most intense line in the line spectrum? E n=5 n=4 - n=3 n=2 3. The L ion has a ground state electron energy of -1.960-10-J. a) Determine the energy, in units of kJ mol, required to raise 1.00 mol of Li ions each from their ground state to a final state of n = 3. b) Calculate the wavelength of the light that would be required to ionize the LP+ ion if it is initially in its ground state. Give the answer in units of nanometres. In the first part of this experiment a Helium lamp is used to generate a calibration curve for scale reading vs. wavelength. a) Why is a Helium lamp used instead of a more traditional light source such as a standard Tungsten-filament light bulb? b) Would a white light source such as sunlight also be appropriate? Justify your answer.

Answer 1

solution As we know that Energy for the hydrogen like cation Ene - 2.179x1018 22 J E Therefore Enel =-2.149x1018 z2 g ū a T And given that Em-1 = -3.485x10175 Thus. 22 - 3.4858101 = - 2.179x108 z² = -3.4858 1017 - 2:17.9 x1512 2 15.99 ~ 16 - 4 - Be cation Huey Now consider 2 16 > = -2:199X10 nr. 2-.712X10 11 7 ( 1972 (JJ = z2z-4x8.712X1519 - 2/29 X 10-18

z² = 15.99 z² = 16 22 4 » Be cation Aus sin consider the last, En=3 = - 3,872 x 1000 ; = -2.179 x1018 z2 (332 z z-983.872 xlöll - 2.179X10-18 2² = 15.99 2²=16 Z =4 → Bestration