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Chapter 6: Q. 6.83 (page 203)

The molecule ${CO}_{2}$ is nonpolar, but $CO$ is a polar molecule. Explain.

Short Answer

Expert verified

Due to electronegativity difference between carbon and oxygen atom ${CO}_{2}$ is nonpolar, but $CO$ is a polar molecule.

Step by step solution

01

Given information

We are given ${CO}_{2}$ is nonpolar, but $CO$ is a polar molecule

02

Simplify

Because the electronegativities of carbon and oxygen differ from each other, electrons are not shared equally between the two atoms.
However, because ${CO}_{2}$ geometry is linear, the two bond dipole moments cancel out, leaving no net molecule dipole moment.
The molecule is thus non-polar.

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Most popular questions from this chapter

Which of the following pairs of elements are likely to form an ionic compound?

a. lithium and chlorine

b. oxygen and bromine

c. potassium and oxygen

d. sodium and neon

c. cesium and magnesium

f. nitrogen and fluorine

Identify the major intermolecular forces between each of the

following atoms or molecules:

a. $P H_{3}$

b. $N O_{2}$

c. localid="1652945006972" $C H_{3_{}} N H_{2}$

d.localid="1652945003975" $A r$

Identify each of the compounds in problem 6.89 as ionic or molecular.

Determine the total number of valence electrons in each of the

following:

a. ${COCl}_{2}$

b. $N_{2} O$

c. ${SeCl}_{2}$

For each of the following bonds, indicate the positive end with $δ^{+}$ and the negative end with $δ^{-}$ . Draw an arrow to show the dipole for each.
a. $P$ and $Cl$
b. $Se$ and $F$
c. $Br$ and $F$
d. $N$ and $H$
e. $B$ and $Cl$

See all solutions

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