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Chapter 7: Question 48 E (page 398)

In terms of the bonds present, explain why acetic acid, \(C{H_3}C{O_2}H\), contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, formed by loss of a hydrogen ion from acetic acid, only contains one type of carbon-oxygen bond. The skeleton structures of these species are shown:

Short Answer

Expert verified

Acetic acid, \(C{H_3}C{O_2}H\), contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, only contains one type of carbon-oxygen bond as there is resonance happening in acetate ion.

Step by step solution

01

Concept Introduction

Chemical bonding is a formation of chemical compound by initiating a chemical link between two or more atoms, molecules, or ions. The atoms in the consequent molecule are retained together by chemical bonds.

02

Bonds in Acetic Acid and Acetate Ion

The acetic acid molecule contains a\({\rm{C - O}}\)double bond and a\({\rm{C - O}}\)single bond.

There is resonance happening in case of acetate ion and it is described by two resonance structures that average the two\({\rm{C - O}}\)bonds.

So, it is because of resonance that acetate ion contains only one type of carbon-oxygen bond (average of two\({\rm{C - O}}\)bonds).

Therefore, both the acetate compounds contain different number of bonds due to resonance.

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Most popular questions from this chapter

Write the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols of the atom from which they are formed: (a) \({\rm{MgS}}\) (b) \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\) (c) \({\rm{GaC}}{{\rm{l}}_{\rm{3}}}\) (d) \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) (e) \({\rm{L}}{{\rm{i}}_{\rm{3}}}{\rm{N}}\) (f) \({\rm{KF}}\) .

Which of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions:\({\rm{P, I, Mg, Cl, In, Cs, O, Pb, Co}}\)?

The lattice energy of \({\rm{KF}}\) is \({\rm{794kJ/mol}}\), and the interionic distance is \({\rm{269 pm}}\). The \({\rm{Na - F}}\) distance in \({\rm{NaF}}\), which has the same structure as \({\rm{KF}}\), is \({\rm{231 pm}}\). Which of the following values is the closest approximation of the lattice energy of \({\rm{NaF}}\): \({\rm{682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol,}}\) or \({\rm{3175 kJ/mol}}\)? Explain your answer.

Predict the electron pair geometry and the molecular structure of each of the following ions:

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\,\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}{\rm{ - }}\)
  3. \({\rm{SnC}}{{\rm{l}}_{\rm{3}}}^{\rm{ - }}\)
  4. \({\rm{BrC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)

The arrangement of atoms in several biologically important molecules is given here. Complete the Lewis structures of these molecules by adding multiple bonds and lone pairs. Do not add any more atoms.
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