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The molecular geometry of a compound can be determined using the Valence Shell Electron Pair Repulsion (VSEPR) theory. This theory states that the shape of a molecule is primarily determined by the repulsion between electron pairs in the valence shell of the central atom.
The molecular geometry of a compound can be determined using the Valence Shell Electron Pair Repulsion (VSEPR) theory. This theory states that the shape of a molecule is primarily determined by the repulsion between electron pairs in the valence shell of the central atom.
To determine the molecular geometry of PO(OH)₃, we first need to identify the central atom, which is the atom that is single and is attached to other atoms. In this case, the central atom is Phosphorus (P).
Next, we need to determine the number of bonding pairs and lone pairs of electrons on the central atom. The Phosphorus atom in PO(OH)₃ has four bonding pairs (one with the Oxygen atom in the PO bond and three with the Hydrogen atoms in the OH bonds) and no lone pairs.
According to the VSEPR theory, a molecule with four bonding pairs and no lone pairs has a tetrahedral molecular geometry. Therefore, the molecular geometry of PO(OH)₃ is tetrahedral.
In a tetrahedral molecular geometry, the bond angles are approximately 109.5 degrees. This is because in a tetrahedron, the bonds are as far apart from each other as possible, which minimizes the repulsion between the electron pairs and results in a stable molecular structure.
In summary, the molecular geometry of PO(OH)₃ is tetrahedral, with bond angles of approximately 109.5 degrees. This is determined using the Valence Shell Electron Pair Repulsion (VSEPR) theory, which considers the number of bonding pairs and lone pairs of electrons on the central atom.
To determine the molecular geometry of PO(OH)₃, we first need to identify the central atom, which is the atom that is single and is attached to other atoms. In this case, the central atom is Phosphorus (P).
Next, we need to determine the number of bonding pairs and lone pairs of electrons on the central atom. The Phosphorus atom in PO(OH)₃ has four bonding pairs (one with the Oxygen atom in the PO bond and three with the Hydrogen atoms in the OH bonds) and no lone pairs.
According to the VSEPR theory, a molecule with four bonding pairs and no lone pairs has a tetrahedral molecular geometry. Therefore, the molecular geometry of PO(OH)₃ is tetrahedral.
In a tetrahedral molecular geometry, the bond angles are approximately 109.5 degrees. This is because in a tetrahedron, the bonds are as far apart from each other as possible, which minimizes the repulsion between the electron pairs and results in a stable molecular structure.
In summary, the molecular geometry of PO(OH)₃ is tetrahedral, with bond angles of approximately 109.5 degrees. This is determined using the Valence Shell Electron Pair Repulsion (VSEPR) theory, which considers the number of bonding pairs and lone pairs of electrons on the central atom.
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