Explain why the spin splitting is not observed in
spectrum?
In a (^{13}\text{C})-NMR spectrum, spin–spin splitting due to (^{13}\text{C}–^{13}\text{C}) coupling is generally not observed because of the extremely low natural abundance of the (^{13}\text{C}) isotope. Carbon exists predominantly as ________ ______ _______ ______ _____ ______ _____ __________ ________ __________ ______ ____.
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What is meant by polarizability of a molecule?
A photoelectron spectrum of a compound containing nitrogen (N), aluminium (Al), and fluorine (F) shows three strong peaks at the following binding energies:
Peak X: ~686 eV
Peak Y: ~399 eV
Peak Z: ~73 eV
Find the best option from the choices given below that best explains the relative positioning of these peaks in terms of binding energy.
(i) Peak X corresponds to F 1s electrons, which have the highest binding energy because fluorine’s high electronegativity and small size give its 1s electrons a large effective nuclear attraction. Peak Y is N 1s and Peak Z is Al 2p.
(ii) Nitrogen has more valence electrons than fluorine or aluminium, therefore its peak appears at the highest binding energy.
(iii) The spectrum shows more aluminium atoms than nitrogen or fluorine, so its peak appears at the lowest binding energy due to dilution.
(iv) Aluminium has the highest nuclear charge, so its 2p peak should have the largest binding energy, but shielding effects reverse this trend.
Justify your answer.
Explain why the atomic spectra are line spectra whereas the molecular spectra are band spectra.
In what way is NMR spectrometry different from other molecular spectroscopic methods?
What are different mechanisms that contribute to the relaxation of nuclear spins in the excited state? Explain any one of them.
has bond length
. Calculate the wavenumbers of the first four lines in its microwave spectrum.
[Given: mass of C=12.000 u and mass of N=14.007 u]
A photon of visible light has a wavelength of . Calculate its
(i) wavenumber
(ii) frequency
(iii) energy per mol