How can a Lewis structure be drawn for a water molecule?

To draw a Lewis structure for a water molecule ($H_{2}O$), you can follow a systematic approach based on the chemical bonding model introduced by Gilbert N. Lewis:

1. Count Valence Electrons: Determine the total number of valence electrons available for bonding. Oxygen has 6 valence electrons, and each of the two hydrogen atoms has 1, for a total of 8 electrons ($2\times 1+6=8$).12
2. Arrange Atoms: Place the oxygen atom in the center with the two hydrogen atoms as neighbors.12
3. Add Bonding Pairs: Place one bonding pair (represented by a line) between the oxygen atom and each hydrogen atom.12
4. Add Lone Pairs: Distribute the remaining electrons to ensure each atom achieves a stable configuration. For oxygen, this involves adding two pairs of nonbonding electrons, known as lone pairs, to satisfy the octet rule.12

The resulting structure shows the oxygen atom connected to two hydrogens by single bonds, with two lone pairs remaining on the oxygen. Note that while this topological representation illustrates the bonding pattern, it does not depict the actual bent molecular shape of water.12