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Chapter 7: Question 45 E (page 397)

(a) sulphur dioxide, \({\rm{S}}{{\rm{O}}_{\rm{2}}}\)

(b) carbonate ion, \({\rm{CO}}_{\rm{3}}^{{\rm{2 - }}}\)

(c) hydrogen carbonate ion, \({\rm{HCO}}_{\rm{3}}^{\rm{ - }}\) (\({\rm{C}}\) is bonded to an \({\rm{OH}}\) group and two \({\rm{O}}\) atoms)

(d) pyridine:

(e) the allyl ion:

Short Answer

Expert verified

The resonance forms for the following compounds are as follows –

(a) Sulphur dioxide –

(b) Carbonate Ion –

(c) Hydrogen Carbonate Ion –

(d) Pyridine –

(e) Allyl Ion –

Step by step solution

01

Concept Introduction

Resonance is a term used to describe delocalized electrons within molecules or polyatomic ions. Several resonance structures portray a molecule or ion with delocalized electrons.

02

Resonance form of Sulphur Dioxide

(a)

Below are the resonance forms of \({\rm{S}}{{\rm{O}}_{\rm{2}}}\)

Therefore, the resonance forms of \({\rm{S}}{{\rm{O}}_{\rm{2}}}\) are obtained.

03

Resonance form of Carbonate Ion

(b)

Below are the resonance forms of \({\rm{CO}}_{\rm{3}}^{{\rm{2 - }}}\)–

Therefore, the resonance forms of \({\rm{CO}}_{\rm{3}}^{{\rm{2 - }}}\) are obtained.

04

Resonance form of Hydrogen Carbonate Ion

(c)

Below are the resonance forms of \({\rm{HCO}}_{\rm{3}}^{\rm{ - }}\) –

Therefore, the resonance forms of\({\rm{HCO}}_{\rm{3}}^{\rm{ - }}\) are obtained.

05

Resonance form of Pyridine

(d)

Below are the resonance forms of pyridine –

Therefore, the resonance forms of pyridine are obtained.

06

Resonance form of Allyl Ion

(e)

Below are the resonance forms of allyl ion –

Therefore, the resonance forms of allyl ions are obtained.

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Most popular questions from this chapter

Methanol,\({{\text{H}}_{\text{3}}}{\text{COH}}\), is used as the fuel in some race cars. Ethanol,\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH}}\), is used extensively as motor fuel in Brazil. Both methanol and ethanol produce\({\text{C}}{{\text{O}}_{\text{2}}}\)and\({{\text{H}}_{\text{2}}}{\text{O}}\)when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

Question: Using the standard enthalpy of formation data in Appendix G, show how the standard enthalpy of formation of \({\rm{HCl(g)}}\) can be used to determine the bond energy.

Write the electron configuration for each of the following ions: (a) \({\rm{A}}{{\rm{s}}^{{\rm{3 - }}}}\) (b) \({{\rm{I}}^{\rm{ - }}}\) (c) \({\rm{B}}{{\rm{e}}^{{\rm{2 + }}}}\) (d) \({\rm{C}}{{\rm{d}}^{{\rm{2 + }}}}\)(e) \({{\rm{O}}^{{\rm{2 - }}}}\) (f) \({\rm{G}}{{\rm{a}}^{{\rm{3 + }}}}\) (g) \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\) (h) \({{\rm{N}}^{{\rm{3 - }}}}\) (i) \({\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}\) (j) \({\rm{C}}{{\rm{o}}^{{\rm{2 + }}}}\) (k) \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}\) (l) \({\rm{A}}{{\rm{s}}^{{\rm{3 + }}}}\) .

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity: (a)\({\rm{C, F, H, N, O}}\)(b)\({\rm{Br, Cl, F, H, I }}\)(c)\({\rm{F, H, O, P, S }}\)(d)\({\rm{Al, H, Na, O, P}}\)(e)\({\rm{Ba, H, N, O, As}}\).

Write the Lewis structure for the diatomic molecule \({{\rm{P}}_{\rm{2}}}\), an unstable form of phosphorus found in high temperature phosphorus vapor.
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