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Chapter 8: Problem 78

A new compound is made that has a \(\mathrm{C}-\mathrm{N}\) bond length of $118 \mathrm{pm}$. Is this bond likely to be a single, double, or triple C-N bond?

Short Answer

Expert verified
The given C-N bond length is \(118\mathrm{~pm}\), which is closest to the standard triple C-N bond length (\(120\mathrm{~pm}\)). Therefore, it is likely that the C-N bond in the compound is a triple bond.

Step by step solution

01

Gather standard bond lengths for C-N bonds

First, we will need to know the standard bond lengths for single, double, and triple C-N bonds. These values can be found in a chemistry reference book or online. The standard bond lengths are as follows: - Single C-N bond: \(147\mathrm{~pm}\) - Double C-N bond: \(130\mathrm{~pm}\) - Triple C-N bond: \(120\mathrm{~pm}\).
02

Compare the given bond length to standard bond lengths

Now that we have the standard bond lengths of single, double, and triple C-N bonds, we can compare the given bond length (\(118\mathrm{~pm}\)) to these values: - \(147\mathrm{~pm} - 118\mathrm{~pm} = 29\mathrm{~pm}\) (Difference between single bond and given bond length) - \(130\mathrm{~pm} - 118\mathrm{~pm} = 12\mathrm{~pm}\) (Difference between double bond and given bond length) - \(120\mathrm{~pm} - 118\mathrm{~pm} = 2\mathrm{~pm}\) (Difference between triple bond and given bond length)
03

Determine the likely bond type based on bond length differences

Looking at the differences calculated in Step 2, the smallest difference is between the given bond length and the triple bond length, with just a difference of 2 pm. Therefore, it is likely that the C-N bond in the compound is a triple bond.

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Most popular questions from this chapter

For each of the following molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: (a) \(\mathrm{SO}_{2}\), (b) \(\mathrm{SO}_{3}\) (c) \(\mathrm{SO}_{3}^{2-}\). (d) Arrange these molecules/ions in order of increasing \(\mathrm{S}-\mathrm{O}\) bond length.

Which of these elements are unlikely to form ionic bonds? $\mathrm{Mg}, \mathrm{Al}, \mathrm{Si}, \mathrm{Br}, \mathrm{I}$.

Write Lewis structures that obey the octet rule for each of the following, and assign oxidation numbers and formal charges to each atom: $(\mathbf{a}) \mathrm{OCS},(\mathbf{b}) \mathrm{SOCl}_{2}(\mathrm{~S}$ is the central atom), (c) \(\mathrm{BrO}_{3}^{-}\), (d) \(\mathrm{HClO}_{2}(\mathrm{H}\) is bonded to \(\mathrm{O})\).

A common form of elemental phosphorus is the white phosphorus, where four \(\mathrm{P}\) atoms are arranged in a tetrahedron. All four phosphorus atoms are equivalent. White phosphorus reacts spontaneously with the oxygen in air to form \(\mathrm{P}_{4} \mathrm{O}_{6} .\) (a) How many valance electron pairs are in the \(\mathrm{P}_{4} \mathrm{O}_{6}\) molecule? (b) When $\mathrm{P}_{4} \mathrm{O}_{6}\( is dissolved in water, it produces a \)\mathrm{H}_{3} \mathrm{PO}_{3}\(, molecule. \)\mathrm{H}_{3} \mathrm{PO}_{3}$ has two forms, \(\mathrm{P}\) forms 3 covalent bonds in the first form and \(\mathrm{P}\) forms 5 covalent bonds in the second form. Draw two possible Lewis structures of \(\mathrm{H}_{3} \mathrm{PO}_{3}\). (c) Which structure obeys the octet rule?

Acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and nitrogen \(\left(\mathrm{N}_{2}\right)\) both contain a triple bond, but they differ greatly in their chemical properties. (a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formation of acetylene and nitrogen. Which compound is more stable? (c) Write balanced chemical equations for the complete oxidation of \(\mathrm{N}_{2}\) to form \(\mathrm{N}_{2} \mathrm{O}_{5}(g)\) and of acetylene to form \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O (g) .\) (d) Calculate the enthalpy of oxidation per mole for \(\mathrm{N}_{2}\) and for $\mathrm{C}_{2} \mathrm{H}_{2}\( (the enthalpy of formation of \)\mathrm{N}_{2} \mathrm{O}_{5}(g)\( is \)11.30 \mathrm{~kJ} / \mathrm{mol}\( ). \)(\mathbf{e})$ Both \(\mathrm{N}_{2}\) and \(\mathrm{C}_{2} \mathrm{H}_{2}\) possess triple bonds with quite high bond enthalpies (Table 8.3). Calculate the enthalpy of hydrogenation per mole for both compounds: acetylene plus \(\mathrm{H}_{2}\) to make methane, \(\mathrm{CH}_{4}\); nitrogen plus \(\mathrm{H}_{2}\) to make ammonia, \(\mathrm{NH}_{3}\).
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