Question

Which statement is wrong bout structure of phosphorus (V) oxide? (a) Each 'P'atom is sp \(^{3}\) hybridized (b) It has \(6 \mathrm{P}-\mathrm{O}-\mathrm{P}\) bonds. (c) IT has POP angle of \(180^{\circ}\). (d) It has two types of \(\mathrm{P}-\mathrm{O}\) bond lengths.

Short answer

Option (c) is incorrect; P-O-P angles aren't \( 180^{\circ} \).

Step-by-step solution

Understanding Phosphorus (V) Oxide Structure

Phosphorus (V) oxide, or diphosphorus pentoxide, is represented by the chemical formula \( P_4O_{10} \). The structure consists of a central ring of four phosphorus atoms, each connected by relatively shorter P=O bonds and longer P-O-P bonds. Each phosphorus atom is bonded to its neighboring phosphorus atoms through an oxygen bridge, forming a cage-like structure.

Analyzing Hybridization

Each phosphorus atom in the \( P_4O_{10} \) molecule uses \( sp^{3} \) hybridization. This gives the phosphorus atoms a tetrahedral geometry in their local environment. Option (a) is therefore a correct statement about the hybridization of phosphorus atoms.

Counting P-O-P Bonds

In \( P_4O_{10} \), the structure features six P-O-P bonds. These are the bridge oxygens connecting the phosphorus atoms within the cage-like network. Therefore, option (b) correctly describes the presence of 6 P-O-P bonds.

Examining P-O-P Bond Angles

P-O-P bonds in \( P_4O_{10} \) do not have an angle of \( 180^{\circ} \). In fact, the angles are significantly less than \( 180^{\circ} \) because the structure does not form a linear bond due to its cage-like arrangement. Thus, option (c) is incorrect.

Identifying Types of P-O Bond Lengths

The structure of \( P_4O_{10} \) has non-equivalent P-O bonds; the terminal P=O bonds are shorter compared to the bridging P-O-P bonds, which are longer. Therefore, it is correct that there are two types of P-O bond lengths, making option (d) correct.

Key concepts

sp3 Hybridization

In the structure of phosphorus (V) oxide, each phosphorus atom is characterized by \( sp^3 \) hybridization. This type of hybridization occurs when one \( s \) orbital mixes with three \( p \) orbitals to form four equivalent \( sp^3 \) hybrid orbitals. These orbitals arrange themselves in a tetrahedral shape.
This geometry allows each phosphorus atom to form a total of four bonds: one double bond with an oxygen atom and three single bonds with other oxygen atoms, which either connect to neighboring phosphorus atoms or terminate as a lone oxygen. As a result, every phosphorus atom retains a tetrahedral arrangement around itself.
This hybridization gives clues about the molecular geometry and is crucial in understanding how the phosphorus atoms link together in the compound's framework.

P-O-P Bonds

The phosphorus (V) oxide molecule includes six P-O-P bonds, essential components connecting the phosphorus atoms in a network. These bonds form from phosphorus atoms joining through oxygen bridges.
The P-O-P bonds act as bridges, holding the framework together, contributing to the characteristic "cage-like" structure of the molecule. These bridges are longer than the P=O bonds, reflecting their unique bonding role.
Understanding the P-O-P bonds helps to appreciate the molecular interactions within the phosphorus (V) oxide compound, portraying how the atoms interact and stabilize in the structure.

Cage-like Molecular Structure

Phosphorus (V) oxide, \( P_4O_{10} \), is known for its distinct cage-like molecular structure. The arrangement consists of a core of four phosphorus atoms arranged in a ring-like feature. These phosphorus atoms are interconnected by oxygen atoms that act as bridges.
This cage-like arrangement allows for stability and symmetry within the molecule. Each phosphorus atom interacts with neighboring atoms, contributing to the overall framework's integrity. This structural configuration is a key feature that gives phosphorus (V) oxide its unique chemical properties.
Visualizing this cage-like structure can aid in comprehending how the atoms bond in three dimensions and how it impacts the molecule's functionality and interactions with other substances.

Bond Angles in Molecules

In the phosphorus (V) oxide structure, bond angles are crucial in understanding the molecule's shape and behavior. The P-O-P bridge bonds do not form a linear arrangement, which means the bond angles are not \( 180^\circ \).
These angles are generally less than \( 180^\circ \) due to the spatial constraints imposed by the cage-like geometry. The presence of bridge oxygens forces the bonds to bend, resulting in smaller bond angles.
These non-linear bonding arrangements help stabilize the structure and are prominent factors influencing the physical and chemical properties of the molecule, making bond angle analysis a critical aspect of understanding molecular geometry.