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Chapter 11: Problem 101

What is the total number of (a) \(\sigma\) bonds and (b) \(\pi\) bonds in the molecule \(\mathrm{CH}_{3} \mathrm{NCO}\) ?

Short Answer

Expert verified
The molecule \(\mathrm{CH}_{3} \mathrm{NCO}\) has a total of 6 sigma bonds and 2 pi bonds.

Step by step solution

01

Break down molecule into structural formula

Firstly, it is necessary to know the molecular structure of \(\mathrm{CH}_{3} \mathrm{NCO}\). The structure is H3C-N=C=O, where the hyrdocarbon \(CH_{3}\) is bonded with Nitrogen, Nitrogen is double bonded with Carbon and Carbon is double bonded with Oxygen.
02

Count sigma bonds

Each single bond and each part of a double or triple bond is a sigma bond. So, in the molecule structure, there are three sigma bonds in the \(\mathrm{CH}_{3}\) group (between Carbon and Hydrogen atoms) and three more within the rest of the molecule (between Carbon-Nitrogen and Carbon-Oxygen). So, in total there are 6 sigma bonds.
03

Count pi bonds

Pi bonds are the 'extra' bonds in a double bond (N=C, C=O). For each double bond, there is one pi bond. Therefore, there are two pi bonds in the \(\mathrm{CH}_{3} \mathrm{NCO}\) molecule.

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Most popular questions from this chapter

A solar cell that is \(15 \%\) efficient in converting solar to electric energy produces an energy flow of \(1.00 \mathrm{kW} / \mathrm{m}^{2}\) when exposed to full sunlight. (a) If the cell has an area of \(40.0 \mathrm{cm}^{2}\), what is the power output of the cell, in watts? (b) If the power calculated in part (a) is produced at \(0.45 \mathrm{V},\) how much current does the cell deliver?

\(\mathrm{N}_{2}(\mathrm{g})\) has an exceptionally high bond energy. Would you expect either \(\mathrm{N}_{2}^{-}\) or \(\mathrm{N}_{2}^{2-}\) to be a stable diatomic species in the gaseous state? Explain.

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

Explain how it is possible to avoid the concept of resonance by using molecular orbital theory.

For each of the following species, identify the central atom(s) and propose a hybridization scheme for those $\operatorname{atom}(\mathrm{s}):(\mathrm{a}) \mathrm{CO}_{2} ;(\mathrm{b}) \mathrm{HONO}_{2} ;(\mathrm{c}) \mathrm{ClO}_{3}^{-} ;(\mathrm{d}) \mathrm{BF}_{4}^{-}$
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