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Chapter 10: Problem 18

The bonds in beryllium hydride \(\left(\mathrm{BeH}_{2}\right)\) molecules are polar, and yet the dipole moment of the molecule is zero. Explain.

Short Answer

Expert verified
The \(BeH_2\) molecule has zero dipole moment despite containing polar bonds, because the molecule's linear geometry means these two bond dipoles are oppositely directional and cancel each other out, resulting in a net zero dipole moment of the molecule.

Step by step solution

01

Understand Polar Bonds

Polar bonds are formed when there is a significant electronegativity difference between the atoms involved in the bond. In this case \(BeH_2\), the electronegativity difference between Be and H atoms makes the bonds polar.
02

Understand Dipole Moment

Dipole moments occur when there is an overall polarity in the molecule, meaning a net positive charge and a net negative charge exist in two different locations within the molecule.
03

Understanding molecule geometry

The molecule \(BeH_2\) is linear in shape. This shape causes the polar bonds to be directly opposite each other. The geometrical arrangement of these bonds is such that individual bond dipoles cancel each other.
04

Collective Analysis

Despite being composed of two polar \(Be-H\) bonds, the entire \(BeH_2\) molecule has no net dipole moment because the dipole moments of the \(Be-H\) bonds are equal in magnitude but opposite in direction, essentially cancelling each other out. The key to understanding this is the linear shape of \(BeH_2\), where everything is balanced perfectly.

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