Indicate which molecule in each of the following pairs of...

Indicate which molecule in each of the following pairs of mole- cules is more polar.
a. BrCl and BrI
b. $\mathrm{CO}_2$ and $\mathrm{SO}_2$
c. $\mathrm{SO}_3$ and $\mathrm{NF}_3$
d. $\mathrm{H}_3 \mathrm{CF}$ and $\mathrm{Cl}_3 \mathrm{CF}$

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Key Concepts

Electronegativity

Electronegativity refers to the ability of an atom to attract electrons toward itself in a chemical bond. Differences in electronegativity between atoms result in polar bonds, where electrons are unequally shared, contributing to the molecule's polarity.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms within a molecule. The shape of a molecule determines how individual bond dipoles add up or cancel each other out, influencing the overall dipole moment and polarity of the molecule.

Dipole Moment

The dipole moment is a quantitative measure of the overall separation of charge within a molecule. It is determined by the vector sum of individual bond dipoles and serves as an indicator of molecular polarity, affecting how molecules interact with electric fields.

Molecular Symmetry

Molecular symmetry pertains to how uniformly the elements in a molecule are arranged. A highly symmetrical molecule can have polar bonds that cancel out, resulting in a nonpolar molecule, whereas asymmetrical molecules tend to have a net dipole moment and are polar.

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