Question

Which type of molecular orbital has a maximum electron density along the internuclear axis but zero density in a plane perpendicular to the internuclear axis? oo on Which type of molecular orbital is used to describe a buildup of electron density along the axis connecting two atomic nuclei to form a bond? On OO on Which type of molecular orbital has a maximum electron density above and below the internuclear axis but zero density in a plane perpendicular to the internuclear axis? O " Ons on Thes 0/2 What is the valence electron molecular orbital electron configuration of C2? (2)(*2s)(n2p)*(02p) (0*2p)?(n*2p)2 (02)2(0*2s) (nap) (02)2(0*2s) (720) (02)2(0* 2s)(02p) (2p)2 ant e s 0/2 What is the valence electron molecular orbital electron configuration of N2? (02)(0*2s)?(n2p) ?(n*2p)2 (02)2(72p)*(0*2p)2 (2)(*2s) (72p)*(02p)2 (02)2(0*2s) (72p)*(02p) (n*2p)2 The 2 Which type of molecular orbital is used to describe a buildup of electron density above and below the axis connecting two atomic nuclei to form a bond? on On ОО What is the bond order for O2? 00 2.5 0.5 O2 Tres 2

Answer 1

1.   Sigma star (σ*) orbital : antibonding molecular orbital in have a region of zero electron probability / density (a nodal plane) perpendicular to the internuclear axis. For sigma orbital electron density along the internuclear axis and between the nuclei has cylindrical symmetry :  all cross-sections perpendicular to the internuclear axis are in this cylinder.

2.  Sigma (σ) orbital : are used to describe build up electron density along two nuclei forming bond. It denotes a bonding orbital :  nuclei are attracted to the accumulation of electron density in the internuclear region.

3. pi ($\pi$) orbital :Sum of these side-to-side interactions increases the electron probability in the region above and below a line connecting the nuclei, so it is a bonding molecular orbital that is called a pi (π) orbital.It has a nodal plane along inter-nuclear axis.

4. C(6) : valence electron : 2s2,2p2

C₂ = ( σ_2s)2 (σ*_2s)2 (π_2p)4

5. N(7) : valence electron : 2s2,2p3

N₂ = ( σ_2s)2 (σ*_2s)2 (π_2p)4( σ_2p)2

6. pi ($\pi$) orbital :  It is result of side-to-side interaction which  increases the electron density in the region above and below axis connecting the nuclei, it is a bonding molecular orbital that is called a pi (π) orbital.

7.

O(8) : valence electron : 2s2,2p4

O₂ = ( σ_2s)2 (σ*_2s)2 ( σ_2p)2 (π_2p)4 (π*_2p)2   

So, bond order is = 1/2(8-4) = 2

8.

F(9) : valence electron : 2s2,2p5

F₂ = ( σ_2s)2 (σ*_2s)2 ( σ_2p)2 (π_2p)4 (π*_2p)4

9 .   O(8) : valence electron : 2s2,2p4

O₂ = ( σ_2s)2 (σ*_2s)2 ( σ_2p)2 (π_2p)4 (π*_2p)2

10. Of these O₂ is paramagnetic , as it has 2 electrons in degenerate π*_2p orbitals, as per hund's rule these are filled : so, two unpaired electrons make is paramagnetic.

others have no electron unpaired ,thus are diamagnetic.

11. N₂ = ( σ_2s)2 (σ*_2s)2 (π_2p)4( σ_2p)2

bond order is = 1/2(8-2) = 3

12. C₂ = ( σ_2s)2 (σ*_2s)2 (π_2p)4

bond order is = 1/2(6-4) = 2.