Atomic spectra Flashcards
How is the spin quantum number defined?
s
s = 1/2
What is the consequence of spatial and spin wavefunctions not being allowed to be the same?
Two electrons with a symmetric spin wavefunction (i.e. two parallel spins, triplet state) cannot occupy the same spatial wavefunction (orbital)
What is an added complication for spin-orbit coupling?
the magnetic dipoles from the spin angular momentum and the orbital angular momentum also interact
What are we concerned about in atomic spectroscopy?
with one state of an atom (defined by an electronic configuration) absorbing or emitting a quantum of light to generate another state via a transition
What are orbitals?
They are wavefunctions for the electrons - they describe the space which electrons occupy
Degenerate states
Different states with the same energy
Term
Represents one or more states with the same energy
Spin multiplicity
The number of potential orientations of the spin angular momentum corresponding to a given total quantum number (S), for the same spatial electronic wavefunction
Microstate
The arrangement of atoms or molecules in a single instant
Why is the hydrogen atom unusual in atomic spectra?
It only has one electron so the energies of the ns, np and nd orbitals are degenerate - simplifies the spectra
Triplet state of He
Cannot decay back to the ground state by the emission of light - but it can occur by collisions with one another or other species
Russell- Saunders Coupling
The determination of J forms and L (it is an approximation that only works for light atoms)
What is needed for a pure rotational spectrum to be observed?
a permanent electric dipole in the molecule as this interacts with the electric dipole of the electromagnetic radiation
What happens to a rotational spectrum with the changing of isotopes?
𝜇 increases with increasing isotope mass, bond length is unaffected so B decreases
Raman spectroscopy
works on the process of inelastic photon scattering
