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प्रश्न
Calculate the bond order of N2, O2, `"O"_2^+`and `"O"_2^-`?
उत्तर
If Na is equal to the number of electrons in an anti-bonding orbital, then Nb is equal to the number of electrons in a bonding orbital.
Bond order = `1/2 ("N"_"b" - "N"_"a")`
If Nb > Na, then the molecule is said be stable. However, if Nb ≤ Na, then the molecule is considered to be unstable.
Bond order of N2 can be calculated from its electronic configuration as:
`[sigma(1"s")]^2[sigma^"*"(1"s")]^2[sigma("2s")]^2[sigma^"*"("2s")]^2[pi(2"p"_x)]^2[pi(2"p"_"y")^2[sigma(2"p"_"z")]]^2`
Number of bonding electrons, Nb = 10
Number of anti-bonding electrons, Na = 4
Bond order of nitrogen molecule = `1/2(10 - 4)`
= 3
There are 16 electrons in a dioxygen molecule, 8 from each oxygen atom. The electronic configuration of oxygen molecule can be written as:
`[sigma-(1"s")]^2[sigma^"*"("1s")]^2[sigma("2s")]^2[sigma^"*"("2s")]^2[sigma("1p"_"z")]^2[pi("2p"_x)]^2[pi^"*"("2p"_"y")]^2[pi^"*"("2p"_x)]^1[pi^"*"("2p"_"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 electrons = 4 = Na.
Bond order ` = 1/2("N"_"b" - "N"_"a")`
`= 1/2 (8-4)`
= 2
Hence, the bond order of oxygen molecule is 2.
Similarly, the electronic configuration of `"O"_2^+` can be written as:
`"KK"[sigma("2s")]^2[sigma^"*"("2s")]^2[sigma("2p"_"z")]^2[pi("2p"_x)]^2[pi("2p"_"y")]^2[pi^"*"("2p"_x)]^1`
Nb = 8
Na = 3
Bond order of `"O"_2^+ = 1/2 (8 -3)`
= 2.5
Thus, the bond order of `"O"_2^+` is 2.5.
The electronic configuration of `"O"_2^-` ion will be:
`"KK"[sigma("2s")]^2[sigma^"*"("2s")]^2[sigma("2p"_"z")]^2[pi("2p"_x)]^2[pi("2p"_"y")]^2[pi^"*"("2p"_x)]^2[pi^"*"("2p"_y)]^1`
Nb = 8
Na = 5
Bond order of `"O"_2^- = 1/2 (8-5)`
= 1.5
Thus, the bond order of `"O"_2^-` ion is 1.5.
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संबंधित प्रश्न
How do you express the bond strength in terms of bond order?
Compare the relative stability of the following species and indicate their magnetic properties;
`"O"_2, "O"_2^+, "O"_2^-`(superoxide), `"O"_2^(2-)`(peroxide)
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?
