1)Briefly outline how the line spectra contributed to the evolution of the atomic model.
2)write a COMPLETE set of quantum numbers for i)the highest energy electron(s) in a hafnium(Hf) atom
II)the lowest energy and highest energy electron(s) in a gallium(Ga) atom.
Tags: Atom, Contribute, Evolution, Line, Spectra
The line spectra, which is the spectrum of light emitted or absorbed in transitions, confirmed the theory that there are various energy levels in an atom. When the electron falls from one level to a lower one, it releases photons which are unique to that transition in that atom. The measurement of the frequencies of the photons released in the transitions confirmed the formulae that we had got of the energy of the electron in various orbits etc. Further, when the atoms were in a magnetic or an electric field, the lines we used to get were further divided very finely into three, the effects are called zeeman effect for magnetic field and stark effect for the electric field. this further division led to the idea that the orbits are further divided into orbitals, which behave in the same way without external field but their energies change in an outside electric or magnetic field. All this profoundly influenced the atomic model and shaped it to as we see it today.
Hafnium’s configuration is [Xe] 4f14 5d2 6s2.
As much as I know, the highest energy electrons in it should be the 6s2 electrons which have the quantum nos
6, 0, 0, -½ and 6, 0, 0, +½
Gallium’s configuration is [Ar] 3d10 4s2 4p1
having the highest energy electron of the 4p orbital the quantum nos. of which should be
4, 1, -1, -½
the lowest energy electrons are always the 1s electrons. so the quantum nos. of the lowest energy electrons will be 1, 0, 0, -½ and 1, 0, 0, +½