To solve the problem of identifying a pair of isoelectronic species with a bond order of one, we need to understand the concepts of isoelectronic species and bond order.
Isoelectronic Species:
Isoelectronic species are molecules or ions that have the same number of electrons. For example, if two species have the same total number of electrons, they are considered isoelectronic.
Bond Order Calculation:
The bond order is a measure of the number of bonds between a pair of atoms. It can be calculated using the Molecular Orbital Theory:
\(Bond \ Order = \frac{(Number \ of \ Bonding \ Electrons) - (Number \ of \ Antibonding \ Electrons)}{2}\)
Solution:
O22− (Peroxide ion): The electronic configuration is the same as O2 but with 2 extra electrons, making it isoelectronic with F2.
F2 (Fluorine molecule): Has 18 electrons (9 per fluorine atom) which matches the total number of electrons in O22−.
For both O22− and F2:
Number of bonding electrons (σ2s, σ2s*, π2px, π2py): 10
Number of antibonding electrons (σ*2s, σ2p, σ*2p, π*2px, π*2py): 8
\(Bond \ Order = \frac{10 - 8}{2} = 1\)
Thus, both O22− and F2 have a bond order of one and are isoelectronic, making O22−, F2 the correct answer.
Conclusion:
The correct pair of isoelectronic species with a bond order of one is O22− and F2. The other options are eliminated because either they are not isoelectronic, or their bond orders do not satisfy the condition.
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