Question

Among the following which one will have the largest O-O bond?
A.$KO_{2}$
B.$O_{2}$
C.$O_2 ^{+}AsF^-$
D.$K_{2}O_{2}$

Answer 1

We will discuss the various properties and exceptional points about the bond order. We will find out how to compare the bond length of each compound stated in the above question.

Complete step by step answer:
Bond order is described as the distinction between the range of bonds and antibonds. The bond variety itself is the wide variety of electron pairs (bonds) among a pair of atoms. Bond number offers an indication of the steadiness of a bond. Isoelectronic species have the same bond quantity. In molecular geometry, bond duration or bond distance is described as the common distance among nuclei of two bonded atoms in a molecule. It is a transferable property of a bond among atoms of fixed kinds, noticeably independent of the relaxation of the molecule. Bond duration is related to bond order: whilst more electrons participate in bond formation the bond is shorter. Bond duration is also inversely associated with bond electricity and the bond dissociation electricity: all other factors being identical, a more potent bond can be shorter. In a bond between equal atoms, half of the bond distance is identical to the covalent radius. Thus, the bond order is lowest in $K_{2}O_{2}$. Hence, the O−O bond period is maximum in $K_{2}O_{2}.$
Hence option D is correct.

Additional Information:
In molecular orbital principle, bond order is defined as 1/2 the difference between the number of bonding electrons and the variety of antibonding electrons as per the equation underneath. This regularly however not continually yields comparable consequences for bonds close to their equilibrium lengths, however it does not now work for stretched bonds. Bond order is also an index of bond energy and is likewise used notably in valence bond concept.

Note:
In molecular orbital principle, bond order is described as half of the distinction between the quantity of bonding electrons and the quantity of antibonding electrons as in step with the equation underneath. This frequently but now not always yields similar outcomes for bonds close to their equilibrium lengths, but it does not work for stretched bonds. Bond order is also an index of bond power and is also used considerably in valence bond principle.