Question

For each pair of bonds, indicate the more polar bond, and use an arrow to show the direction of polarity in each bond. (a) \(\mathrm{C}-\mathrm{O}\) and \(\mathrm{C}-\mathrm{N}\) (b) \(\mathrm{P}-\mathrm{Br}\) and \(\mathrm{P}-\mathrm{Cl}\) (c) \(\mathrm{B}-\mathrm{O}\) and \(\mathrm{B}-\mathrm{S}\) (d) \(\mathrm{B}-\mathrm{F}\) and \(\mathrm{B}-\mathrm{I}\)

Short answer

(a) C-O is more polar (C→O); (b) P-Cl is more polar (P→Cl); (c) B-O is more polar (B→O); (d) B-F is more polar (B→F).

Step-by-step solution

Understanding Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons. In a pair of atoms, the difference in their electronegativities will determine the bond polarity; the larger the difference, the more polar the bond.

Comparing C-O and C-N bonds

Refer to the electronegativity values: Carbon (C) ~2.55, Oxygen (O) ~3.44, Nitrogen (N) ~3.04. For the C-O bond, the electronegativity difference is 0.89, while for C-N, it is 0.49. The C-O bond is more polar. Draw an arrow pointing towards oxygen in the C-O bond: C→O.

Comparing P-Br and P-Cl bonds

Refer to the electronegativity values: Phosphorus (P) ~2.19, Bromine (Br) ~2.96, Chlorine (Cl) ~3.16. For P-Br, the difference is 0.77, while for P-Cl, it's 0.97. The P-Cl bond is more polar. Draw an arrow pointing towards chlorine in the P-Cl bond: P→Cl.

Comparing B-O and B-S bonds

Refer to the electronegativity values: Boron (B) ~2.04, Oxygen (O) ~3.44, Sulfur (S) ~2.58. For B-O, the difference is 1.40, whereas for B-S, it is 0.54. The B-O bond is more polar. Draw an arrow pointing towards oxygen in the B-O bond: B→O.

Comparing B-F and B-I bonds

Refer to the electronegativity values: Boron (B) ~2.04, Fluorine (F) ~3.98, Iodine (I) ~2.66. For B-F, the difference is 1.94, while for B-I, it is 0.62. The B-F bond is more polar. Draw an arrow pointing towards fluorine in the B-F bond: B→F.

Key concepts

Bond Polarity

At the heart of chemical interactions lies bond polarity, which occurs when there is an unequal sharing of electrons between two atoms in a chemical bond. This unequal distribution creates a dipole moment, where one end of the bond becomes partially negative, while the other becomes partially positive.
The extent of polarity in a bond depends on the difference in the electronegativity values of the bonded atoms. If two atoms have significantly different electronegativities, the electrons are drawn more towards the more electronegative atom, resulting in a polar bond. Conversely, if the electronegativity difference is small, the electrons are shared more equally, leading to a nonpolar bond.

Electronegativity Difference

A key determinant of bond polarity is the difference in electronegativity between the two atoms involved. Electronegativity is essentially the ability of an atom to attract electrons toward itself in a chemical bond. To determine which bond is more polar, one can subtract the electronegativity of one atom from that of the other.
For instance, in a C-O bond, if carbon has an electronegativity of 2.55 and oxygen 3.44, subtracting these gives a difference of 0.89. As a rule of thumb:

• If the difference is greater than about 0.5, the bond is considered polar.
• If the difference is less than 0.4, it is generally considered nonpolar.

Recognizing and calculating this difference is crucial in predicting how molecules will interact with each other chemically.

Chemical Bonding

Chemical bonding is all about the interactions that hold atoms together in a molecule. These bonds can either be ionic, covalent, or metallic based on how the electrons are used in the bond.
In covalent bonds, atoms share electrons, and the polarity of these bonds often results from differences in electronegativity. Ionic bonds, on the other hand, involve the transfer of electrons and typically occur between metals and nonmetals. Finally, metallic bonds feature a "sea" of electrons shared among a lattice of metal ions.
Understanding these basic types of chemical bonds helps clarify why different molecules and compounds exhibit distinct chemical and physical properties.

Polarity Arrows

Polarity arrows are a visual tool used to indicate the direction of polarity in a molecular bond. Often represented as an arrow with a plus sign on one end (the positive side) and a pointed end (the negative side), it shows where the electrons are more concentrated.
For instance, in the P-Cl bond, a polarity arrow would point towards chlorine, which bears a higher electronegativity than phosphorus. This simple notation helps depict the flow of electron density between atoms and offers quick insight into the molecular structure.
These arrows are especially useful when comparing molecules or explaining reactions, as they provide an immediate sense of the bond's polar nature.