*Response times vary by subject and question complexity. Again, Ne2-Here There are more number of Atoms then the Orbitals.. doesn't exist. Anonymous. The y axis of a mo diagram represents the total energy not potential nor gibbs energy of the orbitals. Ne2 = S1s(2),S*1s(2),S2s(2),S*2s(2),S2pz(2),P2px(2)=P2py(2),P*2px(2)=P*2py(2), S*2pz(2). Electron configuration of Ne2: (sigma)2s^2 (sigma*)2s^2 (sigma)2p^2 (pi)2p^4 (pi*)2p^4 (sigma*)2p^2 Bond order is zero since bonding an antibonding orbitals have … I can draw be2 but not this. Get 1:1 help now from expert Chemistry tutors If there existed a di-beryllium anion with one additional electron, Be2^-, then it would have a bond order of ½. So, obiously, it will not be Exist! Expert Answer 100% (11 ratings) Previous question Next question Get more help from Chegg. The bond order is 25. The bond order uses the number of electrons in bonding orbitals and anti-bonding orbitals to give a qualitative picture of the molecule's stability. Thus Ne2 molecule . The highest energy occupied molecular orbital in the Ne-Ne bond of the Ne_2 molecule is _____ sigma_2 s sigma_2p sigma*_2s sigma*_2p sigma*_1p. We we draw the molecular orbital diagram for neutral di-beryllium we find a bond order of zero since there are four bonding electrons and four anti-bonding electrons. Draw the molecular orbital diagram for ne2 and determine if the bond between the two atoms will be stable. again. Get more help from Chegg. Q: Cl2 (g) + H2 (g) → 2 HCl (g) ΔH0rxn = ‒184.6 kJ 8. 7 0. The bond order of any given molecule can be calculated from the difference of the electrons of bonding orbitals and electrons of antibonding orbitals. (IV) Amongst B 2 , C 2 , N 2 − and O 2 , N 2 − and O 2 on further ionization (losing single electron) form thermodynamically more stable species. It is Paramagnetic. B2 c2 n2 structure or o2 f2 ne2 structure. If the distribution of electrons in the molecular orbitals between two atoms is such that the resulting bond would have a bond order of zero, a stable bond … The order of a covalent bond is a guide to its strength; a bond between two given atoms becomes stronger as the bond order increases . Theory we will formalize a definition of bond order the number of bonds between atoms in a molecule. The addition of two more electrons to make Ne2 fills all the bonding and antibonding MOs. Therefore, the bond order of Ne2 is zero, and the molecule is not expected to exist. Apply molecular orbital theory to determine the bond order of Ne2. What is the bond order of Ne2 provided the following electron configuration? (III) In both crystalline N a H C O 3 and K H C O 3 , H C O 3 − forms only dimeric anion through a hydrogen bond. So, bond order: 10-9 /2 = 0.5. Median response time is 34 minutes and may be longer for new subjects. So, bond Order: 10 - 10 /2 = 0. we cant say anything about it. 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