Oxygen differs from the other elements of the group. Compounds of oxygen with metals are more ionic in nature and hydrogen bonding is more important for oxygen compounds. Oxygen is never more than divalent beacasue when it hs formed two covalent bonds, there are no low energy orbitals which can be used for form. further bonds. However, the elements S,Se,Te and Po have empty d- orbitals which may be used for bonding, and they can form four or six bonds by unpairing electrons. The higher oxidation states become less stable on decending the group.
The bond between S and O, or Se and O, are much shorter than might be expected for a single bond owing to `rho pi - dpi` interaction between the p- orbital of oxygen and d- orbital of S or Se.
Which of the following statemet is incorrect ?

Options

A. Oxo-anions of sulpher have little tendency to pholymerise compared with the phosphates and sillicates.
B. In pyrosulphurous acid `(H_(2)S_(2)O_(5))` the oxidation states of both the sulpher atoms are not same, they are `+V and +III`
C. Concentrated `HNO_(3)` oxidises both sulpher and selenium to `H_(2)SO_(4)` (+VI)` and `H_(2) SeO_(4)(+VI)` respectively.
D. Most metal oxides are ionic and basic in nature while non-metallic oxides are usually covalent and acidic in nature.

Explanation

To determine which statement is incorrect based on the information provided, we will analyze each statement one by one.

### Step-by-Step Solution:

1. **Statement 1: "Oxo anion of sulphur have little tendency to polymerize as compared to phosphate and silicates."**
- This statement is **correct**. Sulphur oxoanions are generally smaller in size compared to phosphate and silicate ions, which leads to less tendency for polymerization.

2. **Statement 2: "In Pyrosulphurous acid H2S2O5 the oxidation state of both sulphur atoms are not the same; they are +5 and +3."**
...