Draw the resonance structures of $N_2O_5$,state its shape,and indicate the bond angles and bond lengths.
(N/A) $N_2O_5$ (dinitrogen pentoxide) exists as a covalent molecule in the gas phase with the structure $O_2N-O-NO_2$.
Its shape is planar with $C_{2v}$ symmetry.
The central $N-O-N$ bond angle is approximately $112^{\circ}$.
The terminal $N=O$ bonds are shorter (approximately $1.19 \ \mathring{A}$) compared to the $N-O$ bonds connected to the bridging oxygen (approximately $1.35 \ \mathring{A}$).
Resonance structures involve the delocalization of $\pi$-electrons across the $O-N-O$ framework,resulting in partial double bond character for the $N-O$ bonds.
Its shape is planar with $C_{2v}$ symmetry.
The central $N-O-N$ bond angle is approximately $112^{\circ}$.
The terminal $N=O$ bonds are shorter (approximately $1.19 \ \mathring{A}$) compared to the $N-O$ bonds connected to the bridging oxygen (approximately $1.35 \ \mathring{A}$).
Resonance structures involve the delocalization of $\pi$-electrons across the $O-N-O$ framework,resulting in partial double bond character for the $N-O$ bonds.
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$(b)$ The formal charge on $N$ is $+1$.
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$(d)$ The average bond order of the $NO$ bond is $4/3$.
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$(a)$ The coordination number of $N$ is $3$,and the structure is trigonal planar.
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$(c)$ The average formal charge on each $O$ atom is $-2/3$.
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View SolutionGiven that:
$(i) \Delta_f H^o$ of $N_2O$ is $82 \ kJ \ mol^{-1}$
$(ii)$ Bond energies of $N \equiv N, N = N, O = O$ and $N = O$ are $946, 418, 498$ and $607 \ kJ \ mol^{-1}$ respectively.
The resonance energy of $N_2O$ is $...... \ kJ \ mol^{-1}$.
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$(ii)$ Bond energies of $N \equiv N, N = N, O = O$ and $N = O$ are $946, 418, 498$ and $607 \ kJ \ mol^{-1}$ respectively.
The resonance energy of $N_2O$ is $...... \ kJ \ mol^{-1}$.
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