Question

1. Explain why the spectral lines (wavelengths) associated with the energy released when the electron returns to the n = 1 level were not measured using any method. 2. Describe another method for identifying the metal ions (for the unknowns in the flame test portion) besides simply observing the colors of the flames. 3. For hydrogen, discuss what present quantum theory predicts for the position of the 1s electron?

Answer 1

1. The reason is that n = 1 corresponds to the ground state and the energy of an electron in an atom in its ground state is well established.

2. Based on the ionization energy value of the metal, one can easily predict what the metal is.

I.E. = 13.6*n²/Z, where Z is the atomic no. of the metal.

3. For hydrogen, the quantum mechanical model of the atom predicts for the position of the 1s electron.