1. If the overlap integral for two atomic orbitals is found to be ~0.1, what doe
ID: 908551 • Letter: 1
Question
1. If the overlap integral for two atomic orbitals is found to be ~0.1, what does this imply?
Question options:
There is substantial overlap between the two atomic orbitals.
There is a little overlap between the two atomic orbitals.
There is no overlap between the two atomic orbitals.
There is complete overlap between the two atomic orbitals.
2. When light scatters off a rotating molecule and the molecule makes a transition with J = -2, the resulting photon
Question options:
has increased energy and is called Stokes radiation.
has decreased energy and is called Rayleigh radiation.
has increased energy and is called anti-Stokes radiation.
has decreased energy and is called anti-Stokes radiation.
has decreased energy and is called Stokes radiation.
has increased energy and is called Stokes radiation.
has decreased energy and is called Rayleigh radiation.
has increased energy and is called anti-Stokes radiation.
has decreased energy and is called anti-Stokes radiation.
has decreased energy and is called Stokes radiation.
Explanation / Answer
1. the overlap integral between two atomic orbitals means there is little overlap between them. Overlap integral meausures the lack of orthogonality between two orbitals. If two are orthogonal then the integral is zero as there is no overlap. Substantial values lie between .2 to .3
3.This question is based on the rotational Raman spectral selection rule.
del J= 0 Rayleigh scattering
del J= +2 stokes line with increased energy
del J= -2 antistokes line with decreased energy
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.