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Chapter 6: Problem 36

Which of these molecules is the least polar? (a) \(\mathrm{CH}_{2} \mathrm{O}\) (b) \(\mathrm{F}_{2}\) (c) \(\mathrm{CH}_{3} \mathrm{~F}\) (d) \(\mathrm{CH}_{3} \mathrm{Cl}\)

Short Answer

Expert verified
The least polar molecule among the given options is (b) F2, as it is a nonpolar diatomic molecule with no electronegativity difference between the two fluorine atoms.

Step by step solution

01

Understanding Molecular Polarity

Molecular polarity refers to the uneven distribution of electrical charges across a molecule, resulting from the differences in electronegativity between the atoms in the molecule. A molecule with a greater difference in electronegativity between its atoms has more polar bonds, leading to a more polar molecule.
02

Analyzing CH2O (formaldehyde)

CH2O has a trigonal planar molecular geometry with a central carbon atom bonded to two hydrogen atoms and one oxygen atom. The electronegativity difference between carbon and hydrogen is small, resulting in nonpolar C-H bonds. However, the C-O bond is polar due to the electronegativity difference between carbon and oxygen. The molecule has an overall polarity, as the C-O bond polarity is not canceled out by the nonpolar C-H bonds.
03

Analyzing F2

F2 is a diatomic molecule with two fluorine atoms bonded together. Since the electronegativity difference between the two atoms is zero, the bond is nonpolar. Therefore, the F2 molecule is nonpolar.
04

Analyzing CH3F (fluoromethane)

CH3F has a tetrahedral molecular geometry with a central carbon atom bonded to one fluorine atom and three hydrogen atoms. The C-F bond is polar due to the electronegativity difference between carbon and fluorine, while the C-H bonds are relatively nonpolar. The molecule has an overall polarity as the bond polarities do not cancel each other out.
05

Analyzing CH3Cl (chloromethane)

CH3Cl, like CH3F, has a tetrahedral molecular geometry with a central carbon atom bonded to one chlorine atom and three hydrogen atoms. The C-Cl bond is polar due to the electronegativity difference between carbon and chlorine, while the C-H bonds are relatively nonpolar. The molecule has an overall polarity, with the bond polarities not canceling each other out.
06

Comparing and Determining the Least Polar Molecule

From the analysis, we can see that F2 (option b) is a nonpolar molecule, while CH2O, CH3F, and CH3Cl are polar molecules. Therefore, the molecule with the least polarity is: (b) F2

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Most popular questions from this chapter

The atoms in the molecule HSCN are connected in the order given in the formula. (a) Draw the dot diagram. (b) Draw the molecule's three-dimensional shape, and label the numeric value of all bond angles. (c) Draw in the individual bond dipole moments. (d) Is the molecule polar? If yes, draw the molecular dipole moment vector.

Is phosphorus trichloride, \(P C l_{3}\), a polar molecule? If it is, draw the dipole moment vector for the entire molecule and show where the \(\delta+\) and \(\delta-\) regions of the molecule are.

Consider the phosphonium ion, \(\mathrm{PH}_{4}^{+}\). (a) Draw the dot diagram. (b) Draw the ion's three-dimensional shape, and label the numeric value of all bond angles. (c) What is the shape of this polyatomic ion? (d) Draw in the individual bond dipole moments.

An atom has no lone pairs of electrons on it and four other atoms bound to it. Why is \(109.5^{\circ}\) the bond angle adopted by this molecule?

$$ \mathrm{C}_{2} \mathrm{Cl}_{2} \text { , which is connected } \mathrm{Cl}-\mathrm{C}-\mathrm{C}-\mathrm{Cl} . $$
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