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Chapter 2: Problem 41

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 smallest bond angle between terminal atoms? (A) \(\mathrm{CO}_{2}\) (B) \(\mathrm{CO}_{3}^{2-}\) (C) \(\mathrm{NO}_{2}^{-}\) (D) \(\mathrm{NO}_{3}^{-}\)

Short Answer

Expert verified
So the molecule with the smallest bond angle among the options is NO2-.

Step by step solution

01

Understand Lewis Structures

Content for Step 1: You need to draw the Lewis structure of each molecule. Lewis structures show all valence electrons and therefore help to visualize molecular geometry.
02

Determine the Geometry

Content for Step 2: Using the Lewis structures, you can determine the geometry of each molecule. CO2 is linear, CO32- is trigonal planar, NO2- is bent, and NO3- is trigonal planar.
03

Evaluate Bond Angles

Content for Step 3: Then you need to denote the bond angles within each molecule. Linear molecules have bond angles of 180 degrees. Trigonal planar molecules have bond angles of 120 degrees. A bent molecule, on the other hand, due to the presence of lone pair(s) of electrons has bond angles less than120 degrees
04

Compare Angles

Content for Step 4: Lastly, compare the bond angles. The molecule with the smallest angle is the one having the bond angle less than 120 degrees that is present in the bent molecule -- NO2-, due to the existence of a lone pair of electrons.

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Most popular questions from this chapter

$$\mathrm{NH}_{4}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q) \rightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)$$ Increasing the temperature of the above reaction will increase the rate of reaction. Which of the following is NOT a reason that increased temperature increases reaction rate? (A) The reactants will be more likely to overcome the activation energy. (B) The number of collisions between reactant molecules will increase. (C) A greater distribution of reactant molecules will have high velocities. (D) Alternate reaction pathways become available at higher temperatures.

A solution contains a mixture of four different compound: \(\mathrm{KCl}(a q),\) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q), \mathrm{MgSO}_{4}(a q),\) and \(\mathrm{N}_{2} \mathrm{H}_{4}(a q) .\) Which of these compounds would be easiest to separate via distillation? (A) \(\mathrm{KCl}(a q)\) (B) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) (C) \(\mathrm{MgSO}_{4}(a q)\) (D) \(\mathrm{N}_{2} \mathrm{H}_{4}(a q)\)

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.

\(\mathrm{SF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{SO}_{2}(g)+4 \mathrm{HF}(g) \Delta H=-828 \mathrm{kJ} / \mathrm{mol}\) Which of the following statements accurately describes the above reaction? (A) The entropy of the reactants exceeds that of the products. (B) \(\mathrm{H}_{2} \mathrm{O}(l)\) will always be the limiting reagent. (C) This reaction is never thermodynamically favored. (D) The temperature of the surroundings will increase as this reaction Progresses.

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 or molecules exhibit \(s p^{2}\) hybridization around the central atom? (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 \(\mathrm{NO}_{3}^{-}\)
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