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Chapter 10: Problem 47

Through appropriate Lewis structures, show that the phenomenon of resonance is involved in the nitrite ion.

Short Answer

Expert verified
The Nitrite ion shows resonance. Drawing the associated Lewis structures, we get two structures that differ only by the location of the double bond. It indicates the electrons are delocalized and shift between the two Oxygen atoms.

Step by step solution

01

Determining the Total number of valence electrons

Firstly, find the total number of valence electrons for Nitrogen (N) and Oxygen (O). Nitrogen has 5 valence electrons and each Oxygen atom has 6 valence electrons. Since Nitrite has a negative charge, add an extra electron. So the total number of valence electrons is \(5 + (2 \times 6) + 1 = 18\).
02

Drawing the skeletal structure

Next, draw the skeletal structure of the molecule with Nitrogen (N) at the center and two Oxygen (O) atoms attached to it.
03

Distributing the electrons

Distribute the 18 electrons around the atoms, prioritizing the fulfilment of the octet rule (eight electrons around each atom). Since 2 electrons have been used to bond the Nitrogen (N) with the two Oxygen (O) atoms, 16 electrons are left. These can be distributed as lone pairs around Oxygen atoms (6 electrons each) and the remaining 4 will go to Nitrogen.
04

Identifying the need for resonance

Notice that the Nitrogen atom only has 4 electrons around it, which doesn’t fulfil the octet rule. Thus, one of the Oxygen atoms forms a double bond with Nitrogen, shifting a lone pair from Oxygen to be a bonding pair. This can happen with either of the Oxygen atoms, leading to two possible structures. Both these structures represent the Nitrite ion and oscillate between each other, which is called resonance.
05

Drawing resonance structures

Finally, draw both resonance structures, showing the shifting double bond. The structures are represented with a double-headed arrow between them. Also, don’t forget to add the brackets and the negative charge on the outside to represent an ion.

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Most popular questions from this chapter

Write a plausible Lewis structure for crotonaldehyde, $\mathrm{CH}_{3} \mathrm{CHCHCHO},$ a substance used in tear gas and insecticides.

Hydrogen azide, \(\mathrm{HN}_{3}\), is a liquid that explodes violently when subjected to physical shock. In the \(\mathrm{HN}_{3}\) molecule, one nitrogen- to-nitrogen bond length is \(113 \mathrm{pm},\) and the other is \(124 \mathrm{pm} .\) The \(\mathrm{H}-\mathrm{N}-\mathrm{N}\) bond angle is \(112^{\circ} .\) Draw Lewis structures and a sketch of the molecule consistent with these facts.

The greatest bond length is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{Br}_{2} ;\) (d) BrCl.

Alternative strategies to the one used in this chapter have been proposed for applying the VSEPR theory to molecules or ions with a single central atom. In general, these strategies do not require writing Lewis structures. In one strategy, we write (1) the total number of electron pairs \(=[\) (number of valence electrons) \(\pm\) (electrons required for ionic charge) \(] / 2\) (2) the number of bonding electron pairs \(=\) (number of atoms) -1 (3) the number of electron pairs around central atom \(=\) total number of electron pairs \(-3 \times[\) number of terminal atoms (excluding \(\mathrm{H}\) )] (4) the number of lone-pair electrons = number of central atom pairs - number of bonding pairs After evaluating items \(2,3,\) and \(4,\) establish the VSEPR notation and determine the molecular shape. Use this method to predict the geometrical shapes of the following: (a) \(\mathrm{PCl}_{5} ;\) (b) \(\mathrm{NH}_{3} ;\) (c) \(\mathrm{ClF}_{3} ;\) (d) \(\mathrm{SO}_{2} ;\) (e) \(\mathrm{ClF}_{4}^{-}\); (f) \(\mathrm{PCl}_{4}^{+}\). Justify each of the steps in the strategy, and explain why it yields the same results as the VSEPR method based on Lewis structures. How does the strategy deal with multiple bonds?

Assign formal charges to the atoms in the following species, and then select the more likely skeletal structure. (a) \(\mathrm{H}_{2} \mathrm{NOH}\) or \(\mathrm{H}_{2} \mathrm{ONH}\) (b) SCS or CSS (c) NFO or FNO (d) \(\mathrm{SOCl}_{2}\) or \(\mathrm{OSCl}_{2}\) or \(\mathrm{OCl}_{2} \mathrm{S}\) (e) \(\mathrm{F}_{3} \mathrm{SN}\) and \(\mathrm{F}_{3} \mathrm{NS}\)
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