The oxides of Cl, Br and I are well know...

The oxides of Cl, Br and I are well known. They have various composition. The oxides are thermally unstable and dangerously explosive. They react with alkali. The bromine oxides are thermally more stable than chlorine oxides. The structure of halogen oxides is explained on the basis of VSEPR theory.
The hydrides of chlorine, bromine and iodine can be made by direct synthesis an they are well strongly fuming become increasingly more powerful reducing agents. Halogens also form oxoacids of the form `HOX,HXO_(2) ,HXO_(3) " and " HXO_(4)` The acidic character of oxoacids and halogen oxides decreases from 'Cl' to 'I', however it increases with increase in oxidation number of halogen in them.
Which of the following does not dimerise?

`ClO_(2)`

`ClO_(3)`

`CH_(3)`

`CF_(3)`

Verified by Experts

The correct Answer is:

`ClO_(2)` does not dimerise as the odd electron is delocalidsed in the vacant d-orbitals

The oxides of Cl, Br and I are well known. They have various composition. The oxides are thermally unstable and dangerously explosive. They react with alkali. The bromine oxides are thermally more stable than chlorine oxides. The structure of halogen oxides is explained on the basis of VSEPR theory. The hydrides of chlorine, bromine and iodine can be made by direct synthesis an they are well strongly fuming become increasingly more powerful reducing agents. Halogens also form oxoacids of the form HOX,HXO_(2) ,HXO_(3) " and " HXO_(4) The acidic character of oxoacids and halogen oxides decreases from 'Cl' to 'I', however it increases with increase in oxidation number of halogen in them. Choose the correct statement about Cl_(2)O_(6)

It's most accepted structure has `Cl-Cl` bond.

It exists in liquid state as `ClO_(2)^(+)` and `ClO_(4)^(-)`

It is the dimer of `ClO_(3)`.

It does not exist in gaseous state.

`190^(@)`

`118^(@)37'`

`109^(@)28'`

`108.7^(@)`

`HOCI`

`CI_(2)O_(6)`

`KCIO_(4)`

`NaCIO_(3)`