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Chapter 8: Problem 140

Look up the energies for the bonds in \(\mathrm{CO}\) and \(\mathrm{N}_{2}\). Although the bond in \(\mathrm{CO}\) is stronger, \(\mathrm{CO}\) is considerably more reactive than \(\mathrm{N}_{2}\). Give a possible explanation.

Short Answer

Expert verified
Carbon monoxide (CO) is more reactive than nitrogen gas (N鈧�) despite having a stronger bond energy (\(1076.6 \, kJ \cdot mol^{-1}\) for CO and \(941 \, kJ \cdot mol^{-1}\) for N鈧�) due to the polar nature of CO. The polarity of CO makes it more prone to interact with other molecules. In contrast, N鈧� has a non-polar, highly stable triple bond structure between nitrogen atoms, making it less likely to interact with other molecules and exhibit chemical reactivity.

Step by step solution

01

Identifying the bond energies

The bond energies can be looked up in various sources such as textbooks or online databases. Bond energy for CO: The bond strength between carbon (C) and oxygen (O) in a carbon monoxide (CO) molecule can be found to be around \(\require{cancel} 1076.6 \, \cancel{kJ} \cdot \cancel{mol^{-1}}\). Bond energy for N鈧�: The bond strength between nitrogen atoms in a nitrogen gas (N鈧�) molecule can be found to be around \(\require{cancel} 941 \, \cancel{kJ} \cdot \cancel{mol^{-1}}\).
02

Analyzing the molecular properties

To understand the difference in reactivity while the bond between C and O is stronger, we need to examine the molecular structure and processes that affect the chemical reactivity. CO: Carbon monoxide has a triple bond structure, and it is a polar molecule鈥攁 molecule with a net dipole as a result of the opposing charges. Due to this polarity, CO is prone to exhibit reactiveness with other molecules. N鈧�: Nitrogen gas molecules (N鈧�) have a triple bond structure between the two nitrogen atoms. This triple bond makes the molecule highly stable and less prone to react with other molecules. Furthermore, N鈧� is a non-polar molecule, which means it does not possess a net dipole. This reduces its chances of reacting with other molecules as well.
03

Formulating an explanation

Comparing the molecular properties and structures of the CO and N鈧�, we can now provide a possible explanation for differences in reactivity: Carbon monoxide (CO) is more reactive than nitrogen gas (N鈧�) even though the bond energy between C and O in CO is stronger. This difference in reactivity is due to the polar nature of the CO molecule, making it more prone to interact with other molecules. On the other hand, the non-polar nature and triple bond stability of N鈧� make it a less reactive molecule as it remains stable and is less likely to interact with other molecules during chemical reactions.

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Most popular questions from this chapter

Give an example of an ionic compound where both the anion and the cation are isoelectronic with each of the following noble gases. a. Ne c. \(\mathrm{Kr}\) b. \(\mathrm{Ar}\) d. Xe

Place the species below in order of the shortest to the longest nitrogen- oxygen bond. \(\begin{array}{lllll}\mathrm{H}_{2} \mathrm{NOH}, & \mathrm{N}_{2} \mathrm{O}, & \mathrm{NO}^{+}, & \mathrm{NO}_{2}^{-}, & \mathrm{NO}_{3}^{-}\end{array}\) \(\left(\mathrm{H}_{2} \mathrm{NOH}\right.\) exists as \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{OH} .\).

Identify the five compounds of \(\mathrm{H}, \mathrm{N}\), and \(\mathrm{O}\) described below. For each compound, write a Lewis structure that is consistent with the information given. a. All the compounds are electrolytes, although not all of them are strong electrolytes. Compounds \(\mathrm{C}\) and \(\mathrm{D}\) are ionic and compound \(\mathrm{B}\) is covalent. b. Nitrogen occurs in its highest possible oxidation state in compounds \(\mathrm{A}\) and \(\mathrm{C}\); nitrogen occurs in its lowest possible oxidation state in compounds \(\mathrm{C}, \mathrm{D}\), and \(\mathrm{E}\). The formal charge on both nitrogens in compound \(\mathrm{C}\) is \(+1\); the formal charge on the only nitrogen in compound \(\mathrm{B}\) is \(0 .\) c. Compounds A and E exist in solution. Both solutions give off gases. Commercially available concentrated solutions of compound \(\mathrm{A}\) are normally \(16 M .\) The commercial, concentrated solution of compound \(\mathrm{E}\) is \(15 M\). d. Commercial solutions of compound \(\mathrm{E}\) are labeled with a misnomer that implies that a binary, gaseous compound of nitrogen and hydrogen has reacted with water to produce ammonium ions and hydroxide ions. Actually, this reaction occurs to only a slight extent. e. Compound \(\mathrm{D}\) is \(43.7 \% \mathrm{~N}\) and \(50.0 \% \mathrm{O}\) by mass. If compound D were a gas at STP, it would have a density of \(2.86 \mathrm{~g} / \mathrm{L}\). f. A formula unit of compound \(\mathrm{C}\) has one more oxygen than a formula unit of compound D. Compounds \(\mathrm{C}\) and \(\mathrm{A}\) have one ion in common when compound \(\mathrm{A}\) is acting as a strong electrolyte. g. Solutions of compound \(\mathrm{C}\) are weakly acidic; solutions of compound \(\mathrm{A}\) are strongly acidic; solutions of compounds \(\mathrm{B}\) and \(\mathrm{E}\) are basic. The titration of \(0.726 \mathrm{~g}\) compound \(\mathrm{B}\) requires \(21.98 \mathrm{~mL}\) of \(1.000 M \mathrm{HCl}\) for complete neutralization.

Which of the following statements is(are) true? Correct the false statements. a. The molecules \(\mathrm{SeS}_{3}, \mathrm{SeS}_{2}, \mathrm{PCl}_{5}, \mathrm{TeCl}_{4}, \mathrm{ICl}_{3}\), and \(\mathrm{XeCl}_{2}\) all exhibit at least one bond angle which is approximately \(120^{\circ}\) b. The bond angle in \(\mathrm{SO}_{2}\) should be similar to the bond angle in \(\mathrm{CS}_{2}\) or \(\mathrm{SCl}_{2}\) c. Of the compounds \(\mathrm{CF}_{4}, \mathrm{KrF}_{4}\), and \(\mathrm{SeF}_{4}\), only \(\mathrm{SeF}_{4}\) exhibits an overall dipole moment (is polar). d. Central atoms in a molecule adopt a geometry of the bonded atoms and lone pairs about the central atom in order to maximize electron repulsions.

Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers. a. \(\mathrm{NaCl}, \mathrm{KCl}\) b. \(\mathrm{LiF}, \mathrm{LiCl}\) c. \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgO}\) d. \(\mathrm{Fe}(\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}\) e. \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{O}\) f. \(\mathrm{MgO}, \mathrm{BaS}\)
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