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Chapter 2: Problem 39

Consider the Lewis structures for the following molecules: $$\begin{equation} \mathrm{CO}_{2}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-}, \text {and } \mathrm{NO}_{3}^{-} \end{equation}$$ Which molecules are best represented by multiple resonance structures? (A) \(\mathrm{CO}_{2}\) and \(\mathrm{CO}_{3}^{2-}\) (B) \(\mathrm{NO}_{2}^{-}\) and \(\mathrm{NO}_{3}^{-}\) (C) \(\mathrm{CO}_{3}^{2-}\) and \(\mathrm{NO}_{3^{-}}^{-}\) (D) \(\mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-},\) and \(\mathrm{NO}_{3}^{-}\)

Short Answer

Expert verified
(D) \(\mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-},\) and \(\mathrm{NO}_{3}^{-}\)

Step by step solution

01

Identify Resonance in CO2

The Lewis Structure of \(\mathrm{CO}_2\) includes one carbon atom and two oxygen atoms. The carbon atom is in the middle while the two oxygen atoms are on each side of carbon. Each oxygen forms double bonds with carbon, indicating no unpaired electron is left in any atom. Thus, \(\mathrm{CO}_2\) cannot have a resonance, as it is best represented by a single Lewis Structure. Hence, \(\mathrm{CO}_2\) is not included in the answer.
02

Identify Resonance in CO32-

\(\mathrm{CO}_3^{2-}\) includes one carbonate atom and three oxygen atoms. One of the three oxygen atoms forms a double bond with carbon, and the rest two form a single bond and have one additional electron to satisfy the octet rule. Therefore, there are multiple ways to show bonding in \(\mathrm{CO}_3^{2-}\) making it best represented by multiple resonance structures. So, \(\mathrm{CO}_3^{2-}\) is included in the answer.
03

Identify Resonance in NO2-

\(\mathrm{NO}_2^{-}\) includes one nitrogen atom and two oxygen atoms. One oxygen atom forms a double bond with nitrogen, and the other one forms a single bond to satisfy the octet rule. Therefore, there are multiple ways to show bonding making it best represented by multiple resonance structures. Thus, \(\mathrm{NO}_2^{-}\) is included in our answer.
04

Identify Resonance in NO3-

\(\mathrm{NO}_3^{-}\) contains one nitrogen atom and three oxygen atoms, each oxygen forming a single bond with nitrogen. As \(\mathrm{NO}_3^{-}\) includes a charge, there is a necessity for the electrons to move for resonance. Thus, \(\mathrm{NO}_3^{-}\) is also best represented by multiple resonance structures and is included in the answer.

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Most popular questions from this chapter

Aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2},\) is a weak base with \(K_{\mathrm{b}}=3.8 \times 10^{-10}\) (a) Write out the reaction that occurs when aniline reacts with water. (b) (i) What is the concentration of each species at equilibrium in a solution of 0.25\(M \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} ?\) (ii) What is the pH value for the solution in (i)?

A sample of \(\mathrm{H}_{2} \mathrm{S}\) gas is placed in an evacuated, sealed container and heated until the following decomposition reaction occurs at \(1000 \mathrm{K} :\) \(2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}\) (A) \(K_{\mathrm{c}}=\frac{\left[\mathrm{H}_{2}\right]^{2}\left[\mathrm{S}_{2}\right]}{\left[\mathrm{H}_{2} \mathrm{S}\right]^{2}}\) (B) \(K_{\mathrm{c}}=\frac{\left[\mathrm{H}_{2} \mathrm{S}\right]^{2}}{\left[\mathrm{H}_{2}\right]^{2}\left[\mathrm{S}_{2}\right]}\) (C) \(K_{\mathrm{c}}=\frac{2\left[\mathrm{H}_{2}\right]\left[\mathrm{S}_{2}\right]}{2\left[\mathrm{H}_{2} \mathrm{S}\right]}\) (D) \(K_{\mathrm{c}}=\frac{2\left[\mathrm{H}_{2} \mathrm{S}\right]}{2\left[\mathrm{H}_{2}\right]\left[\mathrm{S}_{2}\right]}\)

London dispersion forces are caused by (A) temporary dipoles created by the position of electrons around the nuclei in a molecule (B) the three-dimensional intermolecular bonding present in all covalent substances (C) the uneven electron-to-proton ratio found on individual atoms of a molecule (D) the electronegativity differences between the different atoms in a molecule

Which of the following is true for all bases? (A) All bases donate \(\mathrm{OH}^{-}\) ions into solution. (B) Only strong bases create solutions in which \(\mathrm{OH}^{-}\) ions are present. (C) Only strong bases are good conductors when dissolved in solution. (D) For weak bases, the concentration of the \(\mathrm{OH}^{-}\) ions exceeds the concentration of the base in the solution.

A stock solution of 12.0 M sulfuric acid is made available. What is the best procedure to make up 100.0 mL of 4.0 M sulfuric acid using the stock solution and water prior to mixing? (A) Add 33.3 mL of water to the flask, and then add 66.7 mL of 12.0 M acid. (B) Add 33.3 mL of 12.0 M acid to the flask, and then dilute it with 66.7 mL of water. (C) Add 67.7 mL of 12.0 M acid to the flask, and then dilute it with 33.3 mL of water. (D) Add 67.7 mL of water to the flask, and then add 33.3 mL of 12.0 M acid.
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