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Physical and Chemical Properties of Hydrogen

What is the a...

Question

What is the average bond order of $N - N$ bond in $N_{2} O$ ?

A

3

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B

1.5

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C

2

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D

2.5

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Solution

The correct option is D $2.5$
The resonating structures for $N_{2} O$ are given below:
In $1 s t$ structure, there are three bonds between both nitrogen and in $2 n d$ structure, there are two bonds. So a total of $6$ bonds is present in $5$ resonating structures.

Average bond order is given by $\frac{Total no. of bonds}{Total No. of canonical structures} = \frac{5}{2} = 2.5$
Hence, (d) is correct.

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Similar questions

Q. Calculate resonance energy of

N_{2} O

from the following data
Hence,

△ H^{\circ} (N_{2} O) = 82 k J m o l^{- 1}

Assume structure

N^{Θ} = N^{⨁} = O

(N \equiv N) b o n d = 950 k J m o l^{- 1}

(N = N) b o n d = 420 k J

^{- 1}

O = O) b o n d = 500 k J m o l^{- 1}

(O = N) b o n d = 610 k J m o l^{- 1}

Q. Calculate resonance energy of

N_{2} O

from the following data
Hence,

△ H^{\circ} (N_{2} O) = 82 k J m o l^{- 1}

Assume structure

N^{Θ} = N^{⨁} = O

(N \equiv N) b o n d = 950 k J m o l^{- 1}

(N = N) b o n d = 420 k J

^{- 1}

O = O) b o n d = 500 k J m o l^{- 1}

(O = N) b o n d = 610 k J m o l^{- 1}

Δ H_{f}^{o}

N_{2} O

82 k J / m o l

and bond energy for

N_{2}, N = N, O = O

N = O

946, 418, 498

607 k J / m o l

respectively. Resonance energy of

N_{2} O

Q. The nitrogen oxides that contain N – N bond(s) is:

Q. Calculate the resonance energy of

N_{2} O

from the following data:

△_{f} H^{\circ}

N_{2} O = 82 k J m o l^{- 1}

, standard bond enthalpies of

N = N, N = N, O = O

N = O

946, 418, 498

607 k J m o l^{- 1}

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