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Chapter 6: Problem 33

Why are hydrogen bonds considered a special class of dipole-dipole interactions?

Short Answer

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Answer: Hydrogen bonds are considered a special type of dipole-dipole interaction because they involve a hydrogen atom bonded to a highly electronegative atom (F, O, N) and are generally stronger and more directional than other types of dipole-dipole interactions. The unique properties of hydrogen bonds play essential roles in the properties of various substances and biological systems.

Step by step solution

01

Define Dipole-Dipole Interactions

Dipole-dipole interactions are attractive forces between polar molecules. These occur when two or more polar molecules with partial positive and negative charges attract each other due to their charges. Examples of polar molecules are water (H2O) and hydrogen chloride (HCl).
02

Explain Hydrogen Bonds

A hydrogen bond is a particular type of dipole-dipole interaction that occurs when a hydrogen atom (H) is bonded to a highly electronegative atom such as fluorine (F), oxygen (O), or nitrogen (N). In this case, the hydrogen atom has a partial positive charge due to the electronegativity difference, and the highly electronegative atom has a partial negative charge. These partially charged atoms can form an attractive force with other nearby polar molecules, creating a hydrogen bond.
03

Characteristics of Hydrogen Bonds

Hydrogen bonds are generally stronger than other dipole-dipole interactions for two main reasons: (1) the significant electronegativity difference between hydrogen and the highly electronegative atoms (F, O, N), which causes a greater partial charge in both atoms, leading to a stronger attraction, and (2) the small size of the hydrogen atom allows for a closer approach of the interacting molecules, also resulting in a stronger attraction.
04

Examples of Hydrogen Bonds

Examples of hydrogen bonding can be found in many substances, including water, where hydrogen bonds give it unique properties such as high boiling and melting points, high heat capacity, and the ability to dissolve a wide range of substances. Hydrogen bonding is also essential in biological systems, for example in DNA, where hydrogen bonds between base pairs are crucial for the formation of the double helix structure.
05

Conclude Why Hydrogen Bonds Are a Special Type of Dipole-Dipole Interaction

In conclusion, hydrogen bonds are considered a special class of dipole-dipole interactions because they involve a hydrogen atom bonded to a highly electronegative atom (F, O, N) and are generally stronger and more directional than other types of dipole-dipole interactions. The unique properties of hydrogen bonds play essential roles in the properties of various substances and biological systems.

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Most popular questions from this chapter

In each of the following pairs of compounds, which compound is likely to be more soluble in \(\mathrm{CCl}_{4} ?\) a. \(C C 1_{4}\) or \(C H C l_{3}\) b. \(\mathrm{CH}_{3} \mathrm{OH}\) or \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{CH}_{2} \mathrm{OH}\) c. \(\mathrm{NaF}\) or \(\mathrm{MgO}\) d. \(\mathrm{CaF}_{2}\) or \(\mathrm{BaF}_{2}\)

Which of the following substances have little solubility in water? (a) benzenc, \(\mathrm{C}_{6} \mathrm{H}_{6} ;\) (b) \(\mathrm{KBr} ;\) (c) \(\mathrm{Ar}\)

(Before solving the following problems, you may find it useful to review Section 4.1 on the strengths of ionic bonds.) In an aqueous solution containing chloride, bromide, and iodide salts, which anion would you expect to experience the strongest ion-dipole interactions with surrounding water molecules?

The mercury level in a capillary tube inserted into a dish of mercury is below the surface of the mercury in the dish. Why?

Two liquids- one polar, one non polar have the same molar mass. Which one is likely to have the higher boiling point?
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