Answer
See the explanation
Work Step by Step
Use the localized electron model to describe the bonding in $H_{2}O$.
In the localized electron model, the bonding in H2O can be described as follows:
The oxygen atom has 6 valence electrons, and it forms covalent bonds with two hydrogen atoms, each contributing 1 valence electron. This results in the formation of two O-H covalent bonds.
The oxygen atom also has two lone pairs of electrons, which are not involved in bonding. The presence of these lone pairs and the two covalent bonds results in a tetrahedral arrangement of the electron pairs around the oxygen atom.
The bond angle between the two O-H bonds is approximately 104.5°, which is slightly less than the ideal tetrahedral angle of 109.5°. This deviation is due to the repulsive interactions between the lone pairs and the bonding pairs of electrons.
The localized electron model accurately describes the overall shape and bond angles in the H2O molecule, which is a bent or angular molecule.
