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How many electrons occupy the bonding mo...

How many electrons occupy the bonding molecular orbitals of a C:N triple bond?

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To determine how many electrons occupy the bonding molecular orbitals of a carbon-nitrogen (C:N) triple bond, we can follow these steps: ### Step 1: Determine the total number of valence electrons Carbon has 4 valence electrons, and nitrogen has 5 valence electrons. In a CN triple bond, we also need to consider the negative charge (CN^-), which adds an extra electron. - Valence electrons from Carbon: 4 - Valence electrons from Nitrogen: 5 - Additional electron due to the negative charge: 1 **Total valence electrons = 4 + 5 + 1 = 10 electrons** ### Step 2: Understand the molecular orbital configuration In a triple bond, the molecular orbitals are filled in a specific order. For the C:N triple bond, the order of filling is as follows: 1. σ(1s) 2. σ*(1s) 3. σ(2s) 4. σ*(2s) 5. π(2px) = π(2py) 6. σ(2pz) 7. π*(2px) = π*(2py) 8. σ*(2pz) ### Step 3: Fill the molecular orbitals with the total number of electrons We will fill the molecular orbitals with the 10 valence electrons we calculated: 1. σ(1s) - 2 electrons 2. σ*(1s) - 0 electrons 3. σ(2s) - 2 electrons 4. σ*(2s) - 0 electrons 5. π(2px) - 2 electrons 6. π(2py) - 2 electrons 7. σ(2pz) - 2 electrons Now, let's count the total number of electrons in the bonding molecular orbitals: - Electrons in bonding orbitals: - σ(1s): 2 - σ(2s): 2 - π(2px): 2 - π(2py): 2 - σ(2pz): 2 **Total bonding electrons = 2 + 2 + 2 + 2 + 2 = 10 electrons** ### Step 4: Conclusion The number of electrons that occupy the bonding molecular orbitals of a C:N triple bond is **10 electrons**. ---
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The distribution of electrons among molecular orbitals is called the electronic configuration of the molecule which provides us the following very important informations about the molecule. (A)Stability of molecule : The molecule is stable if number of bonding moleculer orbital electrons (N_b) is greater than the number of antibonding molecular orbital electrons (N_a) . (B) Bond order : Bond order =1/2(N_b-N_a) A positive bond order means a stable molecule while a negative or zero bond order means an unstable molecule. ( C)Nature of the bond : Bond order 1,2 and 3 corresponds to single , double and triple bonds respectively. (D)Bond length: Bond length decreases as bond order increases. (E)Magnetic nature: Molecular orbitals in a molecule are doubly occupied , the substance is diamagnetic and if one or more molecular orbitals are singly occupied, it is paramagnetic. Which of the following statements is incorrect ?

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L.C.A.O. Principle is involved in the formation of the molecular orbitals according to molecular orbital theory. The energy of the bonding molecular orbital is less than that of the combining atomic orbitals while that of the antibonding molecular orbitals while that of the order (B.O.)=1/2(N_(b)-N_(a)) helps in predicting formation of molecules/molecular ions, bond dissociation energy, stability and bond length. Only the molecules or ions with positive B.O. can be formed. These will be diamagnetic if all molecular orbitals are dilled and paramagnetic if one of more are half filled. The atomic orbitals at the time of overlap must have the same symmetry as well. In the formation of N_(2)^(+) from N_(2), the electron is removed from a

L.C.A.O. Principle is involved in the formationof the molecular orbitals according ot molecular orbital theory. The energy of the bonding molecular orbital is less than that of thecombining atomic orbitals while that of the antibonding molecular orbitals while that of the order (B.O.)=1/2(N_(b)-N_(a)) helps in predicting (i) formation of molecules/molecular ions, bond dossociation energy, stability and bond length. Only the molecules or ions with positive B.O. can be formed. These will be diamagnetic if all molecular orbitals are dilled and paramagnetic if one of more are half filled. The atomic prbitals at the time of overlap must have the same symmetry as well. Bond arder is :

L.C.A.O. Principle is involved in the formation of the molecular orbitals according to molecular orbital theory. The energy of the bonding molecular orbital is less than that of the combining atomic orbitals while that of the antibonding molecular orbitals while that of the order (B.O.)=1/2(N_(b)-N_(a)) helps in predicting (i) formation of molecules/molecular ions, bond dissociation energy, stability and bond length. Only the molecules or ions with positive B.O. can be formed. These will be diamagnetic if all molecular orbitals are dilled and paramagnetic if one of more are half filled. The atomic orbitals at the time of overlap must have the same symmetry as well. In the homonuclear molecule which of the following sets of M.O. orbitals are degenerate ?