Question

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the “real” and “model” modes. Explain the difference observed.

Short answer

The lone pairs are larger in the "real" mode, and hydrogens are compressed as a result. As a result, the smaller angle of${104.5}^{\circ }$.

Step-by-step solution

Definition of molecule

A molecule is a particle made up of two or more atoms that are chemically bonded together. The number of atomic nuclei making up a molecule is a determinate number.

Explanation

In this case the structures are very similar.

In the "real" mode, the lone pairs are larger, and because of that hydrogens are being compressed. Ultimately that leads to the smaller angle of${104.5}^{\circ }$.

In the model mode, each electron group occupies the same amount of space; therefore the bond angle is shown as${109.5}^{\circ }$.

Therefore,the structures are nearly identical in this situation.

The lone pairs are larger in the "real" mode, which compresses hydrogens. Finally, a lower angle of ${104.5}^{\circ }$ is obtained.

The bond angle is shown as ${109.5}^{\circ }$ in the model mode because each electron group occupies the same amount of space.