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 formula is \(F = \frac{kq_1q_2}{r^2}\), where \(q_1\) is the ion charge and \(q_2\) is the dipole charge. As \(q_1\) (ion charge) increases, \(F\) (ion - dipole force) increases.
• For the second statement: In a polar covalent molecule, dipole moment \(\mu= q\times d\). A greater electronegativity difference leads to a larger \(q\) (partial charge), so the dipole force (which is related to the dipole moment) is greater.
• For the third statement: Ion - dipole force depends on ion charge and dipole properties. Just because dipole force is greater (e.g., due to a larger dipole moment from a non - ion situation like in a pure polar covalent molecule - molecule interaction), it doesn't directly mean ion - dipole force (which needs an ion) is greater.

Answer:

• The first statement: “The greater the charge of the ions the greater the ion - dipole force and the greater the dipole” is True.
• The second statement: “The greater the difference in electronegativity of the atoms in a polar covalent molecule the greater the dipole force” is True.
• The third statement: “The greater the dipole force the greater the ion - dipole force” is False.