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Chapter 5: Problem 19

The number of \(\sigma\) bonds and \(\pi\) bonds in \(\mathrm{CO}_{2}\) molecule are \(\quad\) respectively.

Short Answer

Expert verified
Answer: In a CO₂ molecule, there are 2 sigma (σ) bonds and 2 pi (π) bonds.

Step by step solution

01

Determine the molecular structure of CO₂

First, we need to figure out the structure of the CO₂ molecule. A CO₂ molecule consists of one carbon atom double bonded to two oxygen atoms (O=C=O).
02

Identify the sigma (σ) and pi (π) bonds in the molecule

In a double bond, there is always one sigma (σ) bond and one pi (π) bond. As there are two double bonds in CO₂ molecule (each between the carbon and an oxygen atom), we can now calculate the number of sigma (σ) and pi (π) bonds:
03

Calculate the number of sigma (σ) bonds

Since there is one σ bond in each double bond, CO₂ will have: 1 σ bond (from C=O) + 1 σ bond (from C=O) = 2 σ bonds
04

Calculate the number of pi (π) bonds

As there is one π bond in each double bond, CO₂ will have: 1 π bond (from C=O) + 1 π bond (from C=O) = 2 π bonds In conclusion, the number of sigma (σ) bonds and pi (π) bonds in a CO₂ molecule are 2 and 2, respectively.

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Most popular questions from this chapter

In the formation of a \(\mathrm{Br}_{2}\) molecule, the overlapping of orbitals takes place.

Although the number of bond pair of electrons in the valence shell of phosphorus in a \(\mathrm{PCl}_{3}\) molecule is 3 , its shape is not trigonal planar. Why?

How is the strength of the covalent bond related to overlapping of the orbitals?

The shape of \(\mathrm{BF}_{3}\) molecule is

Why is \(\mathrm{BeCl}_{2}\) molecule linear, but \(\mathrm{BF}_{3}\) is trigonal planar?
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