Consider a N2 molecule in its first excited electronic state.(a) Identify the molecular orbitals involved and sketch a diagram to show the transition(b) Compare the bond order and bond length of N2* with N2, where the asterisk denotes the excited molecule. (c) Is N2* diagmagnetic or paramagnetic?(d) When N2* loses its excess energy and converts to the ground state N2, it emits a photon of wavelength 470 nm. Calculate the energy difference between these levels. thank you so much

Hello. Since the question contains multiple subparts, the first three subparts are solved. In case the solution for other subparts is required, then repost the entire question and specify the subparts that have to be solved.(a) In a Neutral N2 molecule, the outermost electrons are present in ?2pz orbitals in the ground state and the electron is excited to *2px or * 2py in the excited state. The transition takes place from ?2pz to *2px or * 2py orbitals. The MO diagram is shown as follows:Step 3: (b) The bond order for N2 is 3. The bond order for N2* is ½ (5-1) =2.0. N2* should have a longer bond length than N2. (c) N2* is paramagnetic due to the presence of two unpaired electrons.

Answered: Consider a N2 molecule in its first…

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Consider a N2 molecule in its first excited electronic state.

(a) Identify the molecular orbitals involved and sketch a diagram to show the transition

(b) Compare the bond order and bond length of N2* with N2, where the asterisk denotes the excited molecule.

(d) When N2* loses its excess energy and converts to the ground state N2, it emits a photon of wavelength 470 nm. Calculate the energy difference between these levels.

thank you so much

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