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Chapter 10: Problem 42

How many pi bonds and sigma bonds are there in the tetracyanoethylene molecule?

Short Answer

Expert verified
There are 9 pi bonds and 7 sigma bonds present in a tetracyanoethylene molecule.

Step by step solution

01

Understand the Molecule

Tetracyanoethylene is a molecule with the formula (C2N2)2. It consists of two carbon (C) atoms in the center and four cyano groups (CN) attached to the carbon atoms. Each cyano group consists of 1 carbon atom and 1 nitrogen atom (N). Thus overall, the molecule has four Carbon atoms and four Nitrogen atoms.
02

Analyze the molecule

Carbon in the cyano group forms a triple bond with the Nitrogen atom. In a triple bond, one bond is a sigma bond, and the other two are pi bonds. Furthermore, the central carbon atoms form a double bond. A double bond consists of one sigma bond and one pi bond.
03

Calculations

There are four instances of a triple bond in the molecule (each of them in a CN group). Hence, the number of pi bonds in the molecule is 4*2 = 8. Moreover, the double bond in the center contributes one more pi bond, thus the total pi bonds would be 8 + 1 = 9. As for sigma bonds, there are four instances of a triple bond, contributing 4 sigma bonds and the double bond in the center contributes one more sigma bond. The connection between the two central carbon atoms and the neighboring carbon atoms of the cyano groups gives additional 2 sigma bonds. Hence the total number of sigma bonds is 4 + 1 + 2 = 7.

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Most popular questions from this chapter

Explain the significance of bond order. Can bond order be used for quantitative comparisons of the strengths of chemical bonds?

Sketch the bond moments and resultant dipole moments for these molecules: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{PCl}_{3}, \mathrm{XeF}_{4}, \mathrm{PCl}_{5}\) \(\mathrm{SF}_{6}\)

Draw Lewis structures and give the other information requested for the following molecules: (a) \(\mathrm{BF}_{3}\). Shape: planar or nonplanar? (b) \(\mathrm{ClO}_{3}^{-}\). Shape: planar or nonplanar? (c) \(\mathrm{H}_{2} \mathrm{O}\). Show the direction of the resultant dipole moment. (d) \(\mathrm{OF}_{2}\). Polar or nonpolar molecule? (e) \(\mathrm{SeO}_{2}\). Estimate the OSeO bond angle.

What hybrid orbitals are used by nitrogen atoms in these species? (a) \(\mathrm{NH}_{3},\) (b) \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{NH}_{2}\) (c) \(\mathrm{NO}_{3}^{-}\)

Arrange these species in order of increasing stability: \(\mathrm{Li}_{2}, \mathrm{Li}_{2}^{+}, \mathrm{Li}_{2}^{-}\). Justify your choice with a molecular orbital energy level diagram.
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