Oxygen has an oxidation state of +2 in...

Oxygen has an oxidation state of +2 in

`H_(2)O_(2)`

`OF_(2)`

`SO_(2)`

`H_(2)O`

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Oxygen has - 2 oxidation state in the compound

Oxygen has -1 oxidation state in the compound.

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Sulphur and rest of the elements of group 16 are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire ns^2 np^6 configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the same shell. As a result, they can show +4 and + 6 oxidation states. Oxygen exhibits +2 oxidation state in

Phosphorous has the oxidation state of +1 in :

Phosphorous has the oxidation state of +1 in:

Phosphorus has the oxidation state of +3 in

Account for the following : (i) Oxygen does not show an oxidation state of + 4 and + 6 like sulfur . (ii) NO_2 readily forms a dimer. (iii) Fluorine always exhibits and oxidation state of -1 only in its compunds

Why Al^(3+) is the only stable oxidation state of Al in its compounds while Tl has +1 and +3 oxidation states?

AAKASH INSTITUTE ENGLISH-REDOX REACTIONS-Assignment (Section A) (Objective type Questions (one option is correct))

The oxidation number of P in Mg(2)P(2)O(7) is
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Oxygen has an oxidation state of +2 in
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