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Chapter 11: Problem 15

Write Lewis structures for the following molecules, and then label each \(\sigma\) and \(\pi\) bond. (a) \(\mathrm{HCN} ;\) (b) \(\mathrm{C}_{2} \mathrm{N}_{2}\) (c) \(\mathrm{CH}_{3} \mathrm{CHCHCCl}_{3} ;\) (d) HONO.

Short Answer

Expert verified
The Lewis structures of the molecules are: (a) H-C≡N (b) \(-C≡C-)-N=N- (c) H_3C-CHCHCCl_3 (d) H-O-N=O. In (a), there are two \(\sigma\) bonds and two \(\pi\) bonds; in (b), there are three \(\sigma\) bonds and four \(\pi\) bonds; in (c), there are nine \(\sigma\) bonds and no \(\pi\) bonds; and in (d), there are three \(\sigma\) bonds and one \(\pi\) bond.

Step by step solution

01

Draw Lewis Structures

A Lewis structure is a visual representation of the molecule that shows how the valence electrons are distributed among the atoms in the molecule. Lewis structures can be drawn for each of the molecules as follows: (a) \( \mathrm{HCN} \) (b) \(\mathrm{C}_{2} \mathrm{N}_{2}\) (c) \(\mathrm{CH}_{3} \mathrm{CHCHCCl}_{3}\) (d) HONO.
02

Identify Sigma and Pi Bonds

Each molecule can now be examined for sigma (\(\sigma\)) and pi (\(\pi\)) bonds. A sigma bond (\(\sigma\)) bond is formed by the end-to-end overlapping and Pi bond (\(\pi\)) is formed by the lateral or side by side overlapping of atomic orbitals. In each molecule, single bonds represent \(\sigma\) bonds. Each double bond has one \(\sigma\) and one \(\pi\) bond while each triple bond has one \(\sigma\) and two \(\pi\) bonds.
03

Label Sigma and Pi Bonds

Now each bond in the molecule is labelled as either a sigma (\(\sigma\)) or pi (\(\pi\)) bond based on the type of overlap forming the bond. Label each single bond as a \(\sigma\) bond. Label one of the bonds in a double bond as a \(\sigma\) bond and the other as a \(\pi\) bond. For a triple bond, label one of the bonds as a \(\sigma\) bond and the other two as \(\pi\) bonds.

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Most popular questions from this chapter

The best electrical conductor of the following materials is (a) \(\mathrm{Li}(\mathrm{s}) ;\) (b) \(\mathrm{Br}_{2}(\mathrm{l}) ;\) (c) \(\mathrm{Ge}(\mathrm{s}) ;\) (d) \(\mathrm{Si}(\mathrm{s})\).

Describe the molecular geometry of \(\mathrm{CCl}_{4}\) suggested by each of the following methods: (a) Lewis theory; (b) valence-bond method using simple atomic orbitals; (c) VSEPR theory; (d) valence-bond method using hybridized atomic orbitals.

Show that both the valence-bond method and molecular orbital theory provide an explanation for the existence of the covalent molecule \(\mathrm{Na}_{2}\) in the gaseous state. Would you predict \(\mathrm{Na}_{2}\) by the Lewis theory?

In your own words, define the following terms or symbols: (a) \(s p^{2} ;\) (b) \(\sigma_{2 p}^{*} ;\) (c) bond order; (d) \(\pi\) bond.

Consider the molecules \(\mathrm{CO}^{+}\) and \(\mathrm{CN}^{-}\) and use molecular orbital theory to answer the following: (a) Write the molecular orbital configuration of each ion (ignore the 1 s electrons). (b) Predict the bond order of each ion. (c) Which of these ions is paramagnetic? Which is diamagnetic? (d) Which of these ions do you think has the greater bond length? Explain.
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