An allotrope of phosphorous, exhibits a phenomenon of phosphorescence, produces compound 'A' which on reacition with `O_(2)` gives 'B'. The number of oxygen atoms bonds to each central atom in 'A' and 'B' are 'X' and 'Y' respectively. When 'A' is heated to `210^(@)C` it decomposes to an oxide 'D' and another allotrope of phosphorus 'C'.
This allotrope of phosphorous reacts with halogens to produce the pentahalides but nitrogen does nto give pentahalides. The reason is:

Options

A. Smaller size, more electronegativity and nonavailability of d-orbitals in nitrogen
B. Larger size and more electronegativity of nitrogen
C. Phosphorous is less reactive than nitrogen
D. More bond energy in `P_(4)` molecule than `N_(2)`

Answer

A

Explanation

`A = P_(4)O_(6),B = P_(4)O_(10)`
`P_(4)O_(6) overset(210^(@)C)rarr P_(4)O_(8) +` red phosphorus