Question

The oxidation state of Fe and S in FeS2 is​

Answer 1

Explanation:

The iron and sulphur atoms in FeS2 are arranged as Fe-S-S rather than S-Fe-S is the persulfide.

In FeS2, iron is assigned an oxidation number of 2+, since the persulfide has an oxidation number of - 2, where each sulphur atom is assigned an oxidation number of - 1.

Answer 2

The oxidation state of Fe and S is, (+2) and (-1)

Explanation :

Oxidation number : It represent the number of electrons lost or gained by the atoms of an element in a compound.

Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.

When the atoms are present in their elemental state then the oxidation number will be zero.

Rules for Oxidation Numbers :

The oxidation number of a free element is always zero.

The oxidation number of a monatomic ion equals the charge of the ion.

The oxidation number of  Hydrogen (H)  is +1, but it is -1 in when combined with less electronegative elements.

The oxidation number of  oxygen (O)  in compounds is usually -2, but it is -1 in peroxides.

The oxidation number of a Group 1 element in a compound is +1.

The oxidation number of a Group 2 element in a compound is +2.

The oxidation number of a Group 17 element in a binary compound is -1.

The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.

The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

The given compound is, $FeS_2$

Let the oxidation state of 'Fe' be, 'x'

As the oxidation number of  oxygen (O) in compounds is usually -2, but it is -1 in peroxides.  Similarly, oxidation number of sulfur (S) in compounds is usually -2, but it is -1 in peroxides.

In $FeS_2$, sulfur act as peroxide.

$x+2(-1)=0\\\\x-2=0\\\\x=+2$

Therefore, the oxidation state of Fe and S is, (+2) and (-1)

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