Question

Answer the questions below for the diatomic species

A)   O₂^–

B)   O₂⁺

C)   O₂^–2

What is the bond order for the O₂^–2 ion? Bond Order =

Which of the species has the shortest bond?

How many of the above molecules/ions are paramagnetic?

Answer 1

Molecular orbitals and their order of energy will be used to write the electronic configuration of each specie of dioxygen.

Note that the bond order = (# of bonding electrons - # of antibonding electrons) /2

Also, If there are equal number of electrons is bonding and antibonding electrons, we can cancel them while counting the total electrons. Only the remaining i.e. uncancelled bonding electrons and antibonding electrons will be counted.

The higher the bond order, the shorter the bond-length and the stronger the bond is.

See the attached image:

Since O₂⁺ has highest bond-order of 2.5, It will have the shortest bond length.

And the bond order of O₂^-2 is 1.

gives obital Theony (MOT) Mote culas The Molecular obi tals (Mo's) ehder tolemuwing TT 2PY Mo's: is, 1s,s,2 695 S degenerate Mo Py, Pz ahe in eath case 8+8 = 16 elechons 02 has = 17 electaons 16+ has A) 02 1 wpained elechen pasanagnehe tilling eMD's would be 2 T 2py 2 6 2 Pr Thpz (b-0) band oder 6-3) = 15 Panamagnehe, unpais elechim 15 elechons B) 0 has 16 1 1 2 25 2S 2 2 2 , . (b.0.)6-1) 25 diamagnehe, al pained T2y -2 16+2 18 e - C) 0,has 2 2 , . 2 2S (b-0.)=0-

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