H2O’s oxygen atom undergoes sp^3 hybridization, forming 4 hybrid orbitals that accommodate 2 lone pairs and form 2 sigma bonds with hydrogen atoms. This results in a tetrahedral electronic geometry, but a bent molecular shape due to lone pair repulsion, with an observed bond angle of 104.5°, deviating from the ideal tetrahedral angle (109.5°) due to the electron pair repulsion theory.
H2O Hybridization
The hybridization of the atoms in H2O can be determined by examining the molecular geometry and electron arrangement of the molecule. In H2O, the oxygen atom is bonded to two hydrogen atoms, resulting in a bent or V-shaped molecular geometry.
To determine the hybridization of the oxygen atom in H2O, we need to consider the electron arrangement around it. Oxygen has six valence electrons, and in H2O, four of these electrons are involved in two covalent bonds with the hydrogen atoms. The remaining two electrons are in lone pairs.
The presence of two lone pairs and two bonding pairs around the oxygen atom in H2O indicates that the oxygen atom undergoes sp3 hybridization. This means that one s orbital and three p orbitals of the oxygen atom combine to form four sp3 hybrid orbitals. The four sp3 hybrid orbitals are oriented in a tetrahedral arrangement, with two of them forming sigma bonds with the hydrogen atoms and the other two containing the lone pairs.
The hybridization of the hydrogen atoms in H2O can also be determined. Each hydrogen atom has one valence electron, which is involved in a sigma bond with the oxygen atom. Since each hydrogen atom is only bonded to one other atom and has no lone pairs, the hybridization of the hydrogen atoms is simply the s orbital.
The hybridization of the atoms in H2O can be summarized in the following table:
| Atom | Hybridization | Orbital Type |
|---|---|---|
| Oxygen | sp3 | sp3 hybrid |
| Hydrogen | s | s orbital |
The hybridization of the oxygen atom in H2O influences the molecule’s bonding and shape. The sp3 hybrid orbitals of the oxygen atom allow for the formation of sigma bonds with the hydrogen atoms and the accommodation of the lone pairs. This results in a bent or V-shaped molecular geometry, with the oxygen atom at the center.
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