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Chapter 2: Problem 38

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 molecule would have the shortest bonds? (A) \(\mathrm{CO}_{2}\) (B) \(\mathrm{CO}_{3}^{2-}\) (C) \(\mathrm{NO}_{2}^{-}\) (D) \(\mathrm{NO}_{3}^{-}\)

Short Answer

Expert verified
The molecule with the shortest bonds is CO2 (Option A) because it has only double bonds.

Step by step solution

01

Lewis Structure of CO2

Carbon Dioxide (CO2) has a linear structure with double bonds between the Carbon and each Oxygen atom. Thus, there are two double bonds in CO2.
02

Lewis Structure of CO3 2-

The Carbonate ion (CO3 2-) has one double bond and two single bonds. It is structured in a way that the Carbon atom forms a double bond with one of the Oxygen atoms and single bonds with the other two.
03

Lewis Structure of NO2-

The Nitrite ion (NO2-) has one single bond and one double bond. The Nitrogen atom forms a double bond with one Oxygen atom and a single bond with the other.
04

Lewis Structure of NO3-

The Nitrate ion (NO3-) has three equivalent bonds which are somewhere between a single and double bond due to resonance. Each bond is equivalent and is 1.33, more than a single bond but less than a double bond.
05

Comparing the Bond Lengths

Because CO2 has double bonds only (2 bonds between atoms), CO2 has shortest bonds in comparison to others. More bonds equates to shorter bond lengths. So, CO2 is the answer.

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Most popular questions from this chapter

The average mass, in grams, of one mole of carbon atoms is equal to (A) the average mass of a single carbon atom, measured in amus (B) the ratio of the number of carbon atoms to the mass of a single carbon atom (C) the number of carbon atoms in one amu of carbon (D) the mass, in grams, of the most abundant isotope of carbon

\(2 \mathrm{Ag}^{+}(a q)+\mathrm{Fe}(s) \rightarrow 2 \mathrm{Ag}(s)+\mathrm{Fe}^{2+}(a q)\) Which of the following would cause an increase in potential in the voltaic cell described by the above reaction? (A) Increasing \(\left[\mathrm{Fe}^{2+}\right]\) (B) Adding more \(\mathrm{Fe}(s)\) (C) Decreasing \(\left[\mathrm{Fe}^{2+}\right]\) (D) Removing some \(\mathrm{Fe}(s)\)

Which of the following pairs of ions would make the best buffer with a pH between 6 and 7? \(K_{\mathrm{a}}\) for \(\mathrm{HC}_{3} \mathrm{H}_{2} \mathrm{O}_{2}=1.75 \times 10^{-5}\) \(K_{\mathrm{a}}\) for \(\mathrm{HPO}_{4}^{2-}=4.8 \times 10^{-13}\) (A) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{H}_{2} \mathrm{PO}_{4}\) (B) \(\mathrm{HPO}_{4}^{2-}\) and \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) (C) \(\mathrm{HC}_{3} \mathrm{H}_{2} \mathrm{O}_{2}\) and \(\mathrm{NaC}_{3} \mathrm{H}_{2} \mathrm{O}_{2}\) (D) \(\mathrm{NaOH}\) and \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

\(14 \mathrm{H}^{+}(a q)+\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+3 \mathrm{Ni}(s) \rightarrow\) \(2 \mathrm{Cr}^{3+}(a q)+3 \mathrm{Ni}^{2+}(a q)+7 \mathrm{H}_{2} \mathrm{O}(l)\) In the above reaction, a piece of solid nickel is added to a solution of potassium dichromate. Which species is being oxidized and which is being reduced? \(\quad\) Oxidized \(\quad\) Reduced (A) \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q) \quad \mathrm{Ni}(s)\) (B) \(\mathrm{Cr}^{3+}(a q) \quad \mathrm{Ni}^{2+}(a q)\) (C) \(\mathrm{Ni}(s) \quad \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)\) (D) \(\mathrm{Ni}^{2+}(a q) \quad \mathrm{Cr}^{3+}(a q)\)

\(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)\) 2.0 mol of \(\mathrm{CO}(g)\) and 2.0 mol of \(\mathrm{O}_{2}(g)\) are pumped into a rigid, evacuated \(4.0-\mathrm{L}\) container, where they react to form \(\mathrm{CO}_{2}(g) .\) Which of the following values does NOT represent a potential set of concentrations for each gas at a given point during the reaction? (A) 0.5 0.5 0 (B) 0 0.25 0.5 (C) 0.25 0.25 0.5 (D) 0.25 0.38 0.25
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