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Chapter 10: Problem 111

Which is stronger, a dipole–dipole 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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