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प्रश्न
Compare the relative stability of the following species and indicate their magnetic properties;
`"O"_2, "O"_2^+, "O"_2^-`(superoxide), `"O"_2^(2-)`(peroxide)
उत्तर
There are 16 electrons in a molecule of dioxygen, 8 from each oxygen atom. The electronic configuration of oxygen molecule can be written as:
`[sigma - (1"s")]^2[sigma^"*"(1"s")]^2[sigma(2"s")]^2[sigma(1"p"_"z")]^2[pi(2"p"_x)]^2[pi(2"p"_"y")]^2[pi^"*"(2"p"_x)]^1[pi^"*"(2"p"_"y")]^1`
Since the 1s orbital of each oxygen atom is not involved in boding, the number of bonding electrons = 8 = Nb and the number of anti-bonding orbitals = 4 = Na.
Bond order = `1/2("N"_"b" - "N"_"a")`
`= 1/2(8-4)`
= 2
Similarly, the electronic configuration of `"O"_2^+` can be written as:
`"KK"[sigma(2"s")]^2[sigma^"*"(2"s")]^2[sigma(2"p"_"z")]^2[pi(2"p"_x)]^2[pi(2"p"_"y")]^2[pi^"*"(2"p"_x)]^1`
`"N"_"b" = 8`
`"N"_"a" = 3`
Bond order of `"O"_2^+ = 1/2(8-3)`
= 2.5
Electronic configuration of `"O"_2^-` ion will be:
`KK[sigma(2"s")]^2[sigma^"*"("2s")]^2[sigma(2"p"_"z")]^2[pi(2"p"_x)]^2[pi(2"p"_"y")]^2[pi^"*"(2"p"_x)]^2[pi^"*"(2"p"_"y")]^1`
Nb = 8
Na = 5
Bond order of `"O"_2^-` = `1/2 (8-5)`
= 1.5
Electronic configuration of `"O"_2^(2-)` ion will be:
`"KK"[sigma(2"s")]^2[sigma^"*"("2s")]^2[sigma("2p"_"z")]^2[pi("2p"_x)]^2[pi("2p"_"y")]^2[pi^"*"("2p"_x)]^2[pi^"*"(2"p"_"y")]^2`
Nb = 8
Na = 6
Bond order of `"O"_2^(2-) = 1/2(8 - 6)` =1
Bond dissociation energy is directly proportional to bond order. Thus, the higher the bond order, the greater will be the stability. On this basis, the order of stability is `"O"_2^+ > "O"_2 > "O"_2^- >"O"_2^(2-)`
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संबंधित प्रश्न
How do you express the bond strength in terms of bond order?
Calculate the bond order of N2, O2, `"O"_2^+`and `"O"_2^-`?
What is meant by the term bond order?
Which of the following options represents the correct bond order?
Which of the following have identical bond order?
(i) \[\ce{CN-}\]
(ii) \[\ce{NO+}\]
(iii) \[\ce{O^{-}2}\]
(iv) \[\ce{O^{2-}2}\]
Species having same bond order are:
(i) \[\ce{N2}\]
(ii) \[\ce{N^{-}2}\]
(iii) \[\ce{F^{+}2}\]
(iv) \[\ce{O^{-}2}\]
Using molecular orbital theory, compare the bond energy and magnetic character of \[\ce{O^{+}2}\] and \[\ce{O^{-}2}\] species.
What is the effect of the following processes on the bond order in \[\ce{N2}\] and \[\ce{O2}\]?
(i) \[\ce{N2 -> N^{+}2 + e-}\]
(ii) \[\ce{O2 -> O^{+}2 + e-}\]
Match the species in Column I with the bond order in Column II.
| Column I | Column II |
| (i) \[\ce{NO}\] | (a) 1.5 |
| (ii) \[\ce{CO}\] | (b) 2.0 |
| (iii) \[\ce{O^{-}2}\] | (c) 2.5 |
| (iv) \[\ce{O2}\] | (d) 3.0 |
Which of the following pair is expected to have the same bond order?
In which of the following pairs, the two species have identical bond order?
