Question

(a) What conditions must be met if a molecule with polar bonds is nonpolar? (b) What geometries will give nonpolar molecules for \(\mathrm{AB}_{2}, \mathrm{AB}_{3}\), and \(\mathrm{AB}_{4}\) geometries?

Short answer

(a) For a molecule with polar bonds to be nonpolar, it must have a symmetrical distribution of bond dipoles, resulting in the vector sum of all bond dipoles being zero. (b) The nonpolar geometries for AB_2, AB_3, and AB_4 molecules are linear, trigonal planar, and tetrahedral, respectively.

Step-by-step solution

Identify conditions for a molecule with polar bonds to be nonpolar

For a molecule with polar bonds to be nonpolar, the bond dipoles must cancel each other out. This can happen if the molecule has a symmetrical distribution of these bond dipoles. In other words, the molecule must have a geometry where the vector sum of all the bond dipoles is zero.

Determine geometry for nonpolar AB2 molecules

For an AB_2 molecule to be nonpolar, the bond dipoles must cancel each other out. This can happen when the A atom is in the center and the two B atoms are in a linear orientation. The bond dipoles will be equal and opposite, thus canceling each other out. So, the nonpolar geometry for an AB_2 molecule is linear.

Determine geometry for nonpolar AB3 molecules

For an AB_3 molecule to be nonpolar, the bond dipoles must cancel each other out. This can happen when the A atom is in the center and the three B atoms are in a trigonal planar orientation. The bond dipoles will be equal in magnitude and in a symmetrical distribution, thus canceling each other out. So, the nonpolar geometry for an AB_3 molecule is trigonal planar.

Determine geometry for nonpolar AB4 molecules

For an AB_4 molecule to be nonpolar, the bond dipoles must cancel each other out. This can happen when the A atom is in the center and the four B atoms are in a tetrahedral orientation. The bond dipoles will be equal in magnitude and in a symmetrical distribution, thus canceling each other out. So, the nonpolar geometry for an AB_4 molecule is tetrahedral.

Key concepts

Polar Bonds

Polar bonds occur when two atoms share a pair of electrons, but the sharing is not even. One atom pulls the electrons closer due to its higher electronegativity, creating a difference in electric charge. This uneven distribution of charge creates what we call a dipole moment. It is essential to remember that just because a molecule has polar bonds, it doesn't necessarily mean the whole molecule is polar. There are other factors at play, like the molecule's shape, that can influence the overall polarity. Understanding polar bonds is crucial for predicting how a molecule will interact with others, influencing properties such as solubility and boiling points.

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms within a molecule. It is a significant factor in determining whether a molecule with polar bonds is overall polar or nonpolar. Specific geometries allow the bond dipoles to cancel each other out, resulting in a nonpolar molecule despite the presence of polar bonds. For example:

• Linear geometry (e.g., AB₂) can lead to nonpolar molecules if the dipoles are exactly opposite.
• Trigonal planar geometry (e.g., AB₃) can be nonpolar when dipoles are evenly distributed at 120 degrees.
• Tetrahedral geometry (e.g., AB₄) achieves nonpolarity when the dipoles are symmetrically arranged around the central atom.

Thus, understanding molecular geometry helps in predicting whether the molecule's polar bonds cancel out or not.

Bond Dipoles

A bond dipole arises when electrons in a bond are unevenly shared between two atoms, creating a miniature electric "push and pull" along the bond. This dipole can be visualized as an arrow pointing toward the more electronegative atom. It's like having a little battery in each bond where one side is slightly positive, and the other is slightly negative. These bond dipoles can add together to affect the whole molecule's polarity. If bond dipoles in a molecule point in different directions and do not cancel out, the molecule is polar as a whole. In contrast, if they cancel out, the molecule becomes nonpolar overall, regardless of having polar bonds.

Symmetrical Distribution

Symmetrical distribution in molecules with polar bonds is key to achieving nonpolarity. When the bond dipoles distribute uniformly around the central atom, they can effectively cancel each other out. In such arrangements, the vector of each dipole is balanced by another, leading to a net dipole moment of zero. This means the molecule does not have a positive or negative side, appearing neutral in terms of electric charge. Symmetry is crucial in determining the overall nonpolar nature in molecules such as CO₂, where linear geometry ensures opposite dipoles counterbalance each other, resulting in no net dipole moment.