| Formula | Electron Dot Structure | Number of Electron Groups | Electron Group Arrangement | Number of Bonded Atoms | Shape | Polarity |
|---|---|---|---|---|---|---|
| H2O | H:·Ö·H | 2 | Bent | 2 | Bent | Polar |
| SF2 | F:·S:F | 6 | Bent | 2 | Bent | Polar |
| NI3 | I:·N:I<br/>I:N:I | 5 | Trigonal pyramidal | 3 | Trigonal pyramidal | Polar |
| SiBr4 | Br:·Si:Br<br/>Br:Si:Br<br/>Br:Si:Br | 4 | Tetrahedral | 4 | Tetrahedral | Nonpolar |
| SO3 | O:·S:O<br/>O:S:O | 6 | Trigonal planar | 2 | Trigonal planar | Polar |
* The electron dot formula shows the valence electrons of each atom in a molecule.
* The number of electron groups is the number of regions of electron density around the central atom.
* The electron group arrangement is the three-dimensional shape of the electron groups around the central atom.
* The number of bonded atoms is the number of atoms that are directly bonded to the central atom.
* The shape of the molecule is determined by the electron group arrangement and the number of bonded atoms.
* Polarity is a measure of the uneven distribution of electrons in a molecule. A molecule is polar if it has a dipole moment.
The polarity of a molecule is important for its physical and chemical properties. For example, polar molecules are attracted to each other, while nonpolar molecules are not. Polar molecules are also more likely to dissolve in polar solvents, such as water, than nonpolar molecules.