Which of the following statements about noncovalent bonding interactions is NOT true?
Which of the following statements about noncovalent bonding interactions is NOT true?
All noncovalent bond interactions are inherently electrostatic in nature.
Van der Waals interactions, also known as dispersion forces, are the weakest of the attractive noncovalent bonding interactions.
Charge-induced dipole interactions are inversely proportional to the square of the distance between the two atoms.
A charge may induce formation of a dipole in a nearby polarizable molecule.
no
To determine which of the statements about noncovalent bonding interactions is NOT true, let's carefully analyze each option:
1. All noncovalent bond interactions are inherently electrostatic in nature.
To determine whether this statement is true or not, we need to consider what noncovalent bonding interactions are. Noncovalent bonds involve electrostatic interactions between atoms or molecules, such as hydrogen bonding, ion-dipole interactions, and charge-induced dipole interactions. Since all noncovalent bonding interactions involve electrostatic forces, this statement is TRUE.
2. Van der Waals interactions, also known as dispersion forces, are the weakest of the attractive noncovalent bonding interactions.
To determine whether this statement is true or not, we need to compare the strengths of various noncovalent bonding interactions. Van der Waals interactions, including London dispersion forces, are generally considered to be the weakest of the noncovalent bonding interactions. So, this statement is TRUE.
3. Charge-induced dipole interactions are inversely proportional to the square of the distance between the two atoms.
To determine whether this statement is true or not, we need to understand charge-induced dipole interactions. Charge-induced dipole interactions occur when a charged species interacts with a polarizable molecule, leading to the formation of a temporary dipole in the latter. The strength of charge-induced dipole interactions depends on the magnitude of the charge and the distance between the two atoms. Generally, these interactions are inversely proportional to the distance between the atoms, but not necessarily to the square of the distance. So, this statement is NOT TRUE.
4. A charge may induce the formation of a dipole in a nearby polarizable molecule.
To determine whether this statement is true or not, we need to understand the concept of charge-induced dipoles. When a charged species is near a polarizable molecule, the charge can attract or repel the electrons in the molecule, leading to a temporary separation of charge and the formation of a temporary dipole. This process is known as charge-induced dipole interactions. Therefore, this statement is TRUE.
Based on our analysis, the statement that is NOT true is statement number 3:
"Charge-induced dipole interactions are inversely proportional to the square of the distance between the two atoms."