Question

(a) The PH \(_{3}\) molecule is polar. Does this offer experimental proof that the molecule cannot be planar? Explain. (b) It turns out that ozone, \(\mathrm{O}_{3},\) has a small dipole moment. How is this possible, given that all the atoms are the same?

Short answer

(a) The polarity of PH\(_3\) molecule offers experimental proof that it cannot be planar, as its trigonal pyramidal geometry is not symmetrical. This asymmetry leads to a net dipole moment, confirming that it is not planar. (b) Ozone (O\(_3\)) has a small dipole moment even though all its atoms are the same because of its bent molecular geometry and resonance structures. The uneven distribution of electron density due to alternating single and double bonds results in a net dipole moment.

Step-by-step solution

Understand the molecular geometry of PH\(_3\)

PH\(_3\) is a trigonal pyramidal molecule because it has one phosphorus atom surrounded by three hydrogen atoms and a lone pair of electrons on the phosphorus atom. In a trigonal pyramidal structure, the bond angles are approximately 107.5 degrees.

Polarity and planarity of PH\(_3\)

A molecule is considered polar if there is a net dipole moment in the molecule, which is a result of the presence of polar bonds and an asymmetrical molecular geometry. In PH\(_3\), phosphorus and hydrogen have different electronegativities, making the P-H bonds polar. However, the trigonal pyramidal geometry is also asymmetrical, indicating that the dipole moment of the molecule does not cancel out. This means that PH\(_3\) is a polar molecule. Since PH\(_3\) has an asymmetrical trigonal pyramidal geometry, it is not a planar molecule. Therefore, the polarity of PH\(_3\) can be considered as experimental evidence that it is not planar. For part (b):

Understanding the molecular geometry of O\(_3\) (ozone)

Ozone (O\(_3\)) has a bent molecular geometry with two resonance structures. One structure has a double bond between one pair of oxygen atoms and a single bond between the other pair, while the other structure has the double bond and single bond switched between the pairs of oxygen atoms.

Polarity of O\(_3\)

Despite all the atoms in ozone being the same (oxygen), the molecule is still polar because of its bent molecular geometry and resonance structure. The bent geometry means that the molecule is not symmetrical, and the two resonance structures mean that the electron density is not evenly distributed. The alternating single and double bonds in the resonance structures create an uneven distribution of electron density, resulting in a net dipole moment in the ozone molecule. This explains how ozone (O\(_3\)) can have a small dipole moment even though all the atoms are the same.

Key concepts

Trigonal Pyramidal Structure

Molecules with a trigonal pyramidal structure, like PH₃, play a fundamental role in understanding molecular geometry. This shape is reminiscent of a pyramid with a triangular base. The molecule consists of a central atom, which in the case of PH₃ is phosphorus, surrounded by three atoms at the corners of the pyramid and a lone pair of electrons at the apex. The presence of the lone pair increases the electron-electron repulsion, leading to a bond angle slightly less than 109.5 degrees typical for tetrahedral arrangements. The resulting angle is closer to 107 degrees, giving the molecule a distinct three-dimensional structure.

It is this pyramidal form that prevents the molecule from being planar and contributes to its polarity. The three-dimensional structure of the molecule, enhanced by the angles created around the central atom, can determine physical and chemical properties, including reactivity and interaction with other molecules.

Dipole Moment

Understanding the dipole moment is key to grasping molecular polarity. A dipole moment arises from the differences in electronegativity between two atoms in a bond, leading to a partial positive charge on one end and a partial negative charge on the other. The dipole moment is a vector quantity, with both magnitude, measured in Debye units, and direction, pointing from the positive to the negative charge.

For example, in PH₃, phosphorus and hydrogen have distinct electronegativities, causing the P-H bonds to be polar. If you imagine each bond as an arrow (vector) pointing from hydrogen to phosphorus, the vectors do not cancel each other out due to the trigonal pyramidal shape, resulting in a net dipole moment. The larger the difference in electronegativity and the more asymmetrical the molecule's shape, the higher the dipole moment, leading to increased molecular polarity.

Molecular Polarity

Closely related to dipole moments is the concept of molecular polarity. A molecule is polar if it has an uneven distribution of electron density, resulting in a positive and a negative side. This polarity affects how molecules interact with each other and with different substances. For example, water (H₂O) is a polar molecule, which is why it's such a good solvent for many different substances.

PH₃'s polarity can be deduced not only from the differences in electronegativity between phosphorus and hydrogen but also from its trigonal pyramidal geometry, which ensures an asymmetrical electron distribution. As a result, PH₃ has a net dipole and is polar, meaning it can engage in dipole-dipole interactions with other polar substances.

Resonance Structures

When discussing resonance structures, ozone (O₃) is a fascinating example. Some molecules cannot be adequately represented by a single Lewis structure. Instead, they have several contributing forms which together represent the true nature of the molecule. These are known as resonance structures and they depict the delocalization of electrons within a molecule.

Ozone's two resonance structures have alternating single and double bonds between the three oxygen atoms. No one structure can accurately depict the true electron distribution within ozone, which is a hybrid, or average, of these resonance structures. The delocalization described by the resonance structures leads to an uneven electron density distribution, which contributes to a molecule's polarity.

Electron Density Distribution

The electron density distribution within a molecule is fundamental to understanding its physical and chemical properties. It is the distribution that dictates how a molecule will interact with light, other molecules, and electric fields. The shape of the molecule, the electronegativity of its atoms, and the presence of lone pairs all influence electron density distribution.

In PH₃ and O₃, the distribution is not uniform. In PH₃, the electron density is greater around the phosphorus atom due to its higher electronegativity compared to hydrogen. For O₃, the resonance structures result in an electron density that is spread out more evenly amongst the oxygen atoms but still leads to a region of slight negative charge due to the bent geometry of the molecule, enabling polarity to arise even in a molecule composed entirely of the same element.