Question

Which bond do you expect to be more polar-an O-F bond or an S-O bond?

Short answer

The S-O bond is more polar than the O-F bond.

Step-by-step solution

Understand the Concept of Bond Polarity

Bond polarity arises from the difference in electronegativity between two atoms. The larger the difference in electronegativity, the more polar the bond. Thus, to determine which bond is more polar, we need to compare the electronegativities of the atoms involved.

Identify the Electronegativity Values

Find the electronegativity values for each atom. Oxygen has an electronegativity of approximately 3.44, fluorine is about 3.98, and sulfur is around 2.58.

Calculate Electronegativity Differences

For the O-F bond, the difference in electronegativity is \[ |3.44 - 3.98| = 0.54 \]For the S-O bond, the difference in electronegativity is \[ |2.58 - 3.44| = 0.86 \]

Compare Electronegativity Differences

Compare the calculated differences: the O-F bond has a difference of 0.54, while the S-O bond has a difference of 0.86. The bond with the larger electronegativity difference is more polar.

Conclusion on Bond Polarity

Since the S-O bond has a greater electronegativity difference than the O-F bond, the S-O bond is more polar.

Key concepts

Electronegativity

Electronegativity is a measure of how strongly an atom can attract electrons in a chemical bond. It is crucial in predicting how electrons are shared in bonds and whether a bond is considered polar or non-polar. In general, the higher the electronegativity of an atom, the stronger its ability to attract electrons. This concept is fundamental in understanding the nature of different types of chemical bonds.
Electronegativity values are not fixed and can vary slightly depending on different scales or contexts, but they provide a useful basis for comparison. The Pauling scale is a commonly used reference for these values, and elements like fluorine rank highly with a value around 3.98, indicating a very strong electronegativity.

• Fluorine: 3.98
• Oxygen: 3.44
• Sulfur: 2.58

By comparing these values for the atoms forming a bond, you can predict how the electrons will be distributed in that bond, affecting its polarity.

Polar Bonds

A polar bond is essentially a chemical bond where the distribution of electrons between the two atoms forming the bond is unequal. This occurs when there is a difference in electronegativity between the atoms involved. The more unequal the distribution, the more polar the bond.
In a polar bond, the atom with higher electronegativity will attract the shared electrons more strongly, resulting in a partial negative charge, while the other atom ends up with a partial positive charge. This creates a dipole moment, which is a measure of the bond's polarity. To determine bond polarity: - Compare the electronegativity of the two atoms. - Calculate the difference between these electronegativity values. - The greater the difference, the more polar the bond. For example, in the S-O bond with an electronegativity difference of 0.86, it is more polar than the O-F bond with a difference of 0.54. This means that in the S-O bond, the electrons are shared less equally than in the O-F bond, making it more polar.

Chemical Bonding Concepts

Chemical bonding is a fundamental concept in chemistry that explains how atoms combine to form molecules. It involves interactions that hold atoms together, governed by forces and the sharing of electrons. Among the different kinds of bonds, the most common types are ionic and covalent. - **Ionic Bonds**: Formed when there is a complete transfer of electrons from one atom to another, typically between a metal and a non-metal. For example, the bond in sodium chloride (NaCl). - **Covalent Bonds**: Formed when atoms share electrons to achieve stability, usually happening between non-metal atoms. Depending on how equally electrons are shared, these can be non-polar or polar covalent bonds. Understanding chemical bonding involves examining how electronegative interactions contribute to bond characteristics. For covalent bonds, especially, electronegativity differences influence whether a bond will be more ionic or more covalent, and consequently, more polar or non-polar. Recognizing these variations helps predict the behavior of substances in chemical reactions and their physical properties.