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The oxidation number of an element is the "charge" the element would have if all of...

The oxidation number of an element is the "charge" the element would have if all of its bonds were completely ionic; that is, if the electron pairs of each bond were transferred to the more electronegative atom.

For monatomic ions the oxidation number is simply the charge of the ion. For covalently bonded elements the oxidation number is a bookkeeping device and does not mean that the element carries an actual charge.

Determine the oxidation state for each of the elements below.

The oxidation state of silver in silver bromide AgBr is __

The oxidation state of nitrogen in nitrogen dioxide NO2 is __.

The oxidation state of xenon in xenon gas Xe is __.

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Answer #1

AgBr , Br will have --1 oxidation in general

Ag ( OS) + Br ( OS) = 0                     ( OS mean Oxidation state , total compound charge = 0 )

Ag( OS) + ( -1) = 0

Ag (OS) = +1

NO2   has O in -2 state , hence N is +4

Xe oxidation state in Xe gas = 0                 ( since Xe gas exists as Xe atoms , and single neutral atom oxidation state = 0 )

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