Question

question 6 of 6
which of the following (is) are true?
the greater the charge of the ions the greater the ion-dipole force and the greater the dipole
the greater the difference in electronegativity of the atoms in a polar covalent molecule the greater the dipole force.
the greater the dipole force the greater the ion-dipole force.

Explanation:

• For the first statement: Ion - dipole force is given by \(F = k\frac{q_1q_2}{r^2}\), where \(q_1\) is the charge of the ion and \(q_2\) is the partial charge of the dipole. The dipole force (dipole - dipole force) is between two dipoles and is not directly related to the charge of ions. So, the first statement is false.
• For the second statement: In a polar covalent molecule, the dipole moment \(\mu= q\times d\). A greater difference in electronegativity leads to a larger partial charge \(q\) (where \(q\) is the partial charge separation in the dipole). So, the greater the difference in electronegativity of the atoms in a polar covalent molecule, the greater the dipole force. This statement is true.
• For the third statement: Ion - dipole force \(F = k\frac{q_1q_2}{r^2}\) (where \(q_1\) is ion charge and \(q_2\) is dipole partial charge) and dipole - dipole force \(F = k\frac{\mu_1\mu_2}{r^3}\) (\(\mu\) is dipole moment). They are different types of forces. The strength of dipole force does not directly determine the strength of ion - dipole force. So, the third statement is false.

Answer:

The second option: The greater the difference in electronegativity of the atoms in a polar covalent molecule the greater the dipole force.