N2 does not show pure vibrat ional spectral because:a)Triple bond in N2 is very strongb)The dipo le mo ment of N2 is zeroc)Both a and bd)None of the above.Correct answer is option 'B'. Can you explain this answer?

Question

Answer

Explanation:

Zero Dipole Moment:
The reason why N2 does not show a pure vibrational spectral is because the molecule has a zero dipole moment. A dipole moment is a measure of the separation of positive and negative charges in a molecule. In the case of N2, the molecule is linear and symmetrical, with the two nitrogen atoms sharing the electrons equally. This results in a cancellation of the dipole moments of the two N-N bonds, leading to a zero overall dipole moment for the molecule.

Implications for Spectroscopy:
In vibrational spectroscopy, the interaction of a molecule with electromagnetic radiation results in changes in the vibrational energy levels of the molecule. In molecules with a non-zero dipole moment, such as HCl or CO2, these changes can be observed in the form of vibrational spectra. However, in the case of N2, the absence of a dipole moment means that there is no significant interaction with electromagnetic radiation in the infrared region, which is typically used to study vibrational transitions in molecules.

Strong Triple Bond:
While the presence of a strong triple bond in N2 does contribute to the lack of vibrational spectral features, it is not the primary reason for the absence of pure vibrational spectra. The zero dipole moment of N2 is the main factor that prevents the molecule from exhibiting characteristic vibrational transitions in the infrared region.
Therefore, the correct answer is option B, as the zero dipole moment of N2 is the key factor that explains why the molecule does not show a pure vibrational spectral.

Top Courses for Chemistry

Suggested Free Tests

Related Content

Schools

Competitive Examinations

Quick Access Links

Technical Exams