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Chapter 10: Problem 111

Which is stronger, a dipole鈥揹ipole interaction between two molecules or a covalent bond between two atoms within the same molecule? Explain.

Short Answer

Expert verified
A covalent bond between two atoms within the same molecule is generally stronger than a dipole-dipole interaction between two molecules. Covalent bonds involve the direct sharing of electrons, leading to strong attractive forces between bonding atoms, with bond energies ranging from approximately 150 to 1100 kJ/mol. In contrast, dipole-dipole interactions involve attraction between charged centers of different molecules and have lower associated energies, typically in the range of 5 to 25 kJ/mol.

Step by step solution

01

Understanding dipole-dipole interactions

Dipole-dipole interactions occur between polar molecules that have positive and negative charge centers (dipoles). These interactions arise when the positive end of one polar molecule is attracted to the negative end of another polar molecule. The strength of a dipole-dipole interaction depends on the magnitudes of the molecular dipoles and the distance between the interacting molecules. In general, dipole-dipole interactions are weaker than covalent bonds.
02

Understanding covalent bonds

A covalent bond is a type of chemical bond that involves the sharing of electrons between two atoms within the same molecule. Covalent bonds are formed when atoms within a molecule share electrons to achieve a more stable electronic configuration, usually by completing their outer electron shells. The strength of a covalent bond depends on various factors, including the electronegativity difference between the bonded atoms and the distance between their nuclei. In general, covalent bonds are much stronger than dipole-dipole interactions.
03

Comparing the strength

To determine which interaction is stronger, we will compare the energies associated with each interaction type. Covalent bonds can have bond energies ranging from approximately 150 to 1100 kJ/mol, whereas dipole-dipole interactions typically have energies in the range of 5 to 25 kJ/mol. This indicates that, in general, covalent bonds are much stronger than dipole-dipole interactions.
04

Conclusion

Based on the energies associated with each interaction type, we can conclude that a covalent bond between two atoms within the same molecule is stronger than a dipole-dipole interaction between two molecules. This difference in strength can be attributed to the direct sharing of electrons in covalent bonds, which leads to strong attractive forces between the bonding atoms. In contrast, dipole-dipole interactions involve attraction between the charged centers of different molecules, which is intrinsically weaker than electron sharing in covalent bonds.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Dipole-Dipole Interaction
Dipole-dipole interactions occur in polar molecules. Polar molecules have regions with partial positive and negative charges, creating dipoles. These arise due to differences in electronegativity between atoms in a molecule. When two polar molecules come close, the positive end of one is attracted to the negative end of the other. This is a dipole-dipole interaction.

These interactions depend on the strength of the dipoles and how close the molecules are. Stronger dipoles and shorter distances increase the interaction strength.

While important for molecular behavior, these interactions are relatively weak compared to other types of bonds. They play a significant role in determining properties like boiling points and solubility.
Molecular Interactions
Molecular interactions refer to forces between molecules that influence their physical and chemical properties. Understanding these interactions helps explain why substances hold together in certain ways.

There are several types of molecular interactions, including:
  • Dipole-dipole interactions
  • Hydrogen bonding 鈥� a stronger type of dipole interaction
  • Dispersion forces (also known as London forces)
  • Ionic interactions
These determine states of matter, reactivity, and even biological function. Recognizing these interactions helps in understanding reactions and designing new materials.
Bond Strength
Bond strength is crucial in determining how molecules behave and react. Stronger bonds are stable and require more energy to break. Bond strength is affected by several factors such as bond length and electronegativity differences between atoms.

Covalent bonds, the sharing of electrons between atoms, exhibit significant strength, often between 150 to 1100 kJ/mol. The strong bonds form the backbone of molecular structures by tightly holding atoms together.

On the other hand, dipole-dipole interactions, ranging from 5 to 25 kJ/mol, are much weaker. Despite this, they crucially influence molecular interactions and behavior, especially in liquids and solids.
Chemical Bonding
Chemical bonding involves the forces that hold atoms together in molecules. It forms the basis for the structure and properties of matter. There are several key types of chemical bonds, including:

  • Covalent bonds 鈥� where atoms share electrons
  • Ionic bonds 鈥� where transfer of electrons occurs between atoms
  • Metallic bonds 鈥� involving a 'sea' of electrons shared among many metal atoms
Covalent bonds are particularly strong due to their electron-sharing nature and play a critical role in the molecules鈥� stability and chemistry. This bond strength explains why chemical bonding is fundamental to studying molecular chemistry.

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Most popular questions from this chapter

Rubidium chloride has the sodium chloride structure at normal pressures but assumes the cesium chloride structure at high pressures. (See Exercise \(71 . )\) What ratio of densities is expected for these two forms? Does this change in structure make sense on the basis of simple models? The ionic radius is 148 \(\mathrm{pm}\) for \(\mathrm{Rb}^{+}\) and 181 \(\mathrm{pm}\) for \(\mathrm{Cl}^{-} .\)

A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties, since one is a molecular solid and the other is an ionic solid. How do the properties differ and why?

A 20.0 -g sample of ice at \(-10.0^{\circ} \mathrm{C}\) is mixed with 100.0 g water at \(80.0^{\circ} \mathrm{C}\) . Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of \(\mathrm{H}_{2} \mathrm{O}(s)\) and \(\mathrm{H}_{2} \mathrm{O}(l)\) are 2.03 and \(4.18 \mathrm{J} / \mathrm{g} \cdot^{\circ} \mathrm{C},\) respectively, and the enthalpy of fusion for ice is 6.02 \(\mathrm{kJ} / \mathrm{mol} .\)

Pyrolusite is a mineral containing manganese ions and oxide ions. Its structure can best be described as a body-centered cubic array of manganese ions with two oxide ions inside the unit cell and two oxide ions each on two faces of the cubic unit cell. What is the charge on the manganese ions in pyrolusite?

Calcium has a cubic closest packed structure as a solid. Assuming that calcium has an atomic radius of \(197 \mathrm{pm},\) calculate the density of solid calcium.
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