1) Are fluorine oxides more stable than iodine oxides? 2) what is the middle row anomaly for bromine oxides? Why can't it form multiple bonds with oxygen like cl?

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The oxides of chlorine, bromine and iodine are well known. They have various compositions. The oxides of chlorine 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 structure of $C l_{2} O_{7}$ is $O_{3} C l - O - C l O_{3}$ The Cl - O-Cl bond angle is:

Which oxide of chlorine is colourless?

Q. The highest oxidation state of manganese in fluorides is 4+ (MnF₄) but the highest oxidation state in oxides is 7+ (Mn₂O₇) because:

Select the correct statements among the following.

I)

V_{2} O_{5}

and

C r_{2} O_{3}

are amphoteric oxides.

I I)

Interstitial compounds of transition elements have an exact formulae.

I I I)

In its higher oxidation states, manganese forms stable compounds with oxygen and fluorine.

why is fluorine more electronegative than chlorine,bromine and iodine?

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