(b) Using these partial charges and the atomic radii given in Figure 7.8, estimate the dipole moment of the molecule.

Verified step by step guidance

1. Identify the atoms involved in the molecule and their respective partial charges (\( \delta^+ \) and \( \delta^- \)).
2. Determine the distance between the centers of the two atoms using their atomic radii. This distance is the bond length.
3. Use the formula for dipole moment: \( \mu = q \times d \), where \( q \) is the magnitude of the charge and \( d \) is the distance between the charges.
4. Substitute the values of the partial charge (\( q \)) and the bond length (\( d \)) into the formula.
5. Calculate the dipole moment, ensuring the units are consistent, typically in Debye (D).

Key Concepts

Dipole Moment

The dipole moment is a measure of the separation of positive and negative charges in a molecule. It is a vector quantity, represented by the product of the charge magnitude and the distance between the charges. A higher dipole moment indicates a greater polarity, which affects the molecule's interactions with electric fields and other polar substances.

Partial Charges

Partial charges arise in polar covalent bonds where electrons are not shared equally between atoms, leading to a slight positive charge (δ+) on one atom and a slight negative charge (δ-) on the other. These charges are crucial for determining the overall dipole moment of a molecule, as they indicate how charge is distributed within the molecule.

Atomic Radii

Atomic radii refer to the size of an atom, typically measured as the distance from the nucleus to the outermost electron shell. In the context of dipole moments, atomic radii help estimate the distance between partial charges in a molecule, which is essential for calculating the dipole moment accurately. Understanding atomic radii allows for better predictions of molecular behavior and interactions.