Which of the following is not an example of an intermolecular attraction?
dipole-dipole interactions
london dispersion forces
hydrogen bonding
Answer:
Covalent bonding is a form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms. (or intramolecular bonding)
Intermolecular forces are: Ionic interactions,
Hydrogen bonds, Dipole-dipole interactions, and Van der Waals' forces.
london dispersion forces are Van der Waals forces which are non-covalent or intermolecular forces.
covalent bonding
covalent bonding is between two atoms within the same molecule, which is called an intramolecular force.
dipole-dipole, london dispersion (aka van der waals), and hydrogen bonding are examples of attractions between separate molecules, which are called intermolecular forces.
Hydrogen bonding is a special type of dipole/dipole interaction and dispersion forces are another name for induced dipole/induced dipole attraction. Therefore covalent bonding is not an example. Covalent bonding is an interatomic attraction rather than an intermolecular attraction.
Covalent bonds only occur within atoms within the same molecule, not between different molecules. Covalent bonding is therefore not intermolecular and is not an example of intermolecular attraction. The other interactions are more often thought of as occurring between different molecules but can have significant consequences within single complex molecules such as proteins. This is particularly true of hydrogen bonding, which can be classified as a particularly strong kind of dipole-dipole interaction.
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