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Chapter 6: Problem 40

Consider the two molecules \(\mathrm{CO}\) and \(\mathrm{CO}_{2}\). They are both made of the same elements, and yet only one is polar. Why is this so?

Short Answer

Expert verified
In conclusion, the CO molecule is polar due to its linear geometry and bond dipole not canceling out, whereas the CO2 molecule is nonpolar because its linear geometry results in equal and opposite bond dipoles that cancel each other out.

Step by step solution

01

Determine the Electronegativity Difference

The first step is to check the difference in electronegativity between the two elements (C and O) present in both molecules. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. A bond can be considered polar if there is a significant difference in electronegativity between the atoms involved. In this case, the electronegativity value of Carbon (C) is 2.55, and Oxygen (O) has a value of 3.44. The electronegativity difference between C and O is \(3.44 - 2.55 = 0.89\) Since 0.89 is greater than 0.5, the bond between C and O can be considered polar.
02

Analyze Molecular Geometry

Next, we need to consider the molecular geometry of the given molecules to determine their overall polarity. For CO molecule: The molecule CO has two atoms bonding with each other. So it's a linear molecule, and the bond dipole doesn't cancel out. This makes the CO molecule polar. For CO2 molecule: The CO2 molecule consists of one central carbon atom bonded to two oxygen atoms. The molecule has a linear geometry, as the oxygen atoms are at 180 degrees from each other. Oxygen is more electronegative than carbon, leading to a bond dipole for each CO bond.
03

Check for Cancellation of Bond Dipoles

In the CO2 molecule, since the bond dipoles are equal in magnitude and opposite in direction, they cancel each other out, making the molecule nonpolar. In conclusion, CO is a polar molecule due to its bond dipole not being canceled out in its linear geometry, while CO2 is nonpolar because its linear geometry cancels out the bond dipoles.

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Most popular questions from this chapter

Consider all the hydrogen halide molecules \(\mathrm{HX}\), where \(X\) is a group VIIA atom. (a) Which is the most polar? Why? (b) Which is the least polar? Why? (c) Draw all these molecules, showing their relative bond dipole moments.

Consider the \(\mathrm{PX}_{3}\) molecule, where \(\mathrm{X}\) is either \(\mathrm{H}\) or \(\mathrm{F}\). (a) For \(\mathrm{X}=\mathrm{H}\), the entire molecule is nonpolar. Why is this so? (Hint: Consider electronegativities.) (b) For \(\mathrm{X}=\mathrm{F}\), the entire molecule is polar. Draw two molecules next to one another in proper orientation so as to yield a dipolar intermolecular attraction, and explain why the attraction occurs.

Using lines, solid wedges, and dashed wedges, draw the three-dimensional shape of chloromethylacetylene, \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{Cl}\). Indicate the numeric value of all bond angles.

Consider the molecules \(\mathrm{CH}_{4}, \mathrm{CH}_{3} \mathrm{Cl}, \mathrm{CH}_{2} \mathrm{Cl}_{2}, \mathrm{CHCl}_{3}\) and \(\mathrm{CCl}_{4}\). Which are polar and which are nonpolar?

True or false? All molecules that contain polar bonds must be polar. Explain your answer.
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