Using the electronegativities of Br and Cl, estimate the partial charges on the atoms in the Br-

step 1 We are asked in this problem to use electronegativities of bromine and chlorine, which I will lo

Using the electronegativities of Br and Cl, estimate the...

Using the electronegativities of $\mathrm{Br}$ and $\mathrm{Cl}$, estimate the partial charges on the atoms in the $\mathrm{Br}-\mathrm{Cl}$ molecule. Using these partial charges and the atomic radii given in Figure $7.7$, estimate the dipole moment of the molecule. The measured dipole moment is $0.57 \mathrm{D}$.

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Key Concepts

Electronegativity

Electronegativity is a measure of how strongly an atom attracts electrons in a chemical bond. In a molecule, differences in electronegativity between atoms lead to unequal sharing of electrons, which sets the foundation for determining electron distribution and the occurrence of polar bonds.

Partial Charges

Partial charges arise when there is an unequal sharing of electrons between atoms in a covalent bond due to differences in electronegativity. These charges are not full ionic charges, but they indicate regions of relative electron density (partial negative) and electron deficiency (partial positive) within a molecule.

Atomic Radii and Bond Length

Atomic radii provide an estimate of the size of an atom and, when used in combination with bonding considerations, help determine the bond length in a molecule. The bond length is a critical distance parameter in calculating separations of partial charges and, consequently, the dipole moment.

Bond Dipole Moment

The bond dipole moment is a vector quantity calculated as the product of the magnitude of the partial charge and the distance between the charge centers. It quantifies the polarity of a bond, and, in diatomic molecules, determines the overall molecular dipole moment.

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