The number of oxygen atoms bonded to each phosphorus centre in P4O6, and P4O10 respectively, are
3 and 4
Phosphorus Oxygen Structures: P4O6 and P4O10
Let's understand the structures of phosphorus oxides, specifically P4O6 and P4O10, to determine the number of oxygen atoms bonded to each phosphorus atom.
Both P4O6 and P4O10 have cage-like structures derived from a tetrahedral arrangement of phosphorus atoms.
P4O6 Structure
- The structure of P4O6 can be visualized as four phosphorus atoms ($\text{P}$) forming a tetrahedron.
- Six oxygen atoms ($\text{O}$) are inserted along the edges of this tetrahedron, bridging between each pair of phosphorus atoms.
- Each oxygen atom bridges between two phosphorus atoms.
- In this arrangement, each phosphorus atom is connected to three oxygen atoms. These three oxygen atoms link that phosphorus atom to the other three phosphorus atoms in the structure.
So, in $\text{P}_4\text{O}_6$, each phosphorus centre is bonded to 3 oxygen atoms.
P4O10 Structure
- The structure of P4O10 is based on the P4O6 structure.
- It retains the central P4 tetrahedron with bridging oxygen atoms between phosphorus atoms.
- Additionally, in P4O10, there are four more oxygen atoms compared to P4O6. These four additional oxygen atoms are terminally bonded to each of the four phosphorus atoms.
- Each of these four terminal oxygen atoms is double-bonded to one phosphorus atom.
- Therefore, each phosphorus atom in P4O10 is bonded to three bridging oxygen atoms (single bonds) and one terminal oxygen atom (double bond).
So, in $\text{P}_4\text{O}_{10}$, each phosphorus centre is bonded to a total of 3 bridging oxygen atoms + 1 terminal oxygen atom = 4 oxygen atoms.
Oxygen Atoms Bonded to Phosphorus Summary
Based on the structures:
- In P4O6, each phosphorus atom is bonded to 3 oxygen atoms.
- In P4O10, each phosphorus atom is bonded to 4 oxygen atoms.
The number of oxygen atoms bonded to each phosphorus centre in P4O6 and P4O10 respectively are 3 and 4.
Important Questions from p - Block
Which of the following has the lowest boiling point?
Which of the following reaction(s) do(es) NOT occur
(i) [NPCl2]3 + 6 NaF \(\rm \xrightarrow[reflux]{MeCN}\) [NPF2]3 + 6 NaCl
(ii) n PCl5 + n NH4Cl \(\rm \xrightarrow[reflux]{C_6H_5Cl}\) [NPCl2]n + 4 n HCl [n = 3, 4, 5]
(iii) n PF 5 + n NH 4 F \(\rm \xrightarrow[reflux]{C_6H_5Cl}\) [NPF 2 ] n + 4 n HF [n = 3, 4, 5]
Choose the correct statement(s) from the following:
(i) The trend in Lewis acidity among silicon halides is SiI4 < SiBr4 < SiCl4 < SiF4.
(ii) Tin(II) chloride can act as a Lewis acid and not as a Lewis base.
(iii) Aluminosilicates can display Brønsted acidity.
Consider following statements
A. PbCl2 has low solubility in water.
B. Sulfides of As(III) and Sb(III) are soluble in ammonium sulfide.
C. SnS is soluble in yellow ammonium sulfide.
D. MnS is precipitated by passing H2S through acidic MnCl2.
Correct statements are
Which of the statements (A‐D) given below are correct for B2H6 molecule:
A. Addition of Et2O•BF3 to NaBH4 in a polyether solvent produces B2H6.
B. It has D2d symmetry.
C. Reaction of B2H6 with NMe3 gives Me3N•BH3.
D. It is diamagnetic.
