Question

Disulfur decafluoride is intermediate in reactivity between ${\mathbf{SF}}_{\mathbf{4}}$ and ${\mathbf{SF}}_{\mathbf{6}}$. It disproportionates at 150 C to these monosulfur fluorides. Write a balanced equation for this reaction, and give the oxidation state of S in each compound.

Short answer

The balanced equation for the disproportionation reaction can be given as

${\mathrm{S}}_2{\mathrm{F}}_{10}\left(\mathrm{g}\right)\to {\mathrm{SF}}_4\left(\mathrm{g}\right)+{\mathrm{SF}}_6\left(\mathrm{g}\right)$

The oxidation state of sulfur in $S_2{F}_{10}$is +5.

The oxidation state of sulfur in is +4.

The oxidation state of sulfur in is +6.

Step-by-step solution

Disproportionation reactions

Reactions in which a reactant undergoes both oxidation and reduction are called disproportionation reactions.

These reactions occur at high temperatures, and more than one product will be formed from a single reactant.

Disproportionation reactions can be identified by determining the atom's oxidation state in the reactants and products. The atom will have a higher oxidation state in one of the products and a lower oxidation state in the other.

The oxidation state of an atom

The number of electrons lost or gained by an atom during the formation of an ion is represented by its oxidation state. The oxidation of an atom includes the removal of electrons. The reduction of an atom includes the addition of electrons.

The oxidation state of an atom in a compound can be determined by equating the sum of charges of all the atoms in the compound to its total charge. Neutral compounds will have a zero charge, as the positive charges and negative charges in the compound will be equal.

Disproportionation of disulfur decafluoride

Disulfur decafluoride disproportionates to sulfur tetrachloride and sulfur hexafluoride. A balanced chemical equation will have the same number of each atom on the reactant and product sides.

The balanced equation for disproportionation of sulfur decafluoride is given as

$S_2{F}_{10}\left(g\right)\to S{F}_4\left(g\right)+S{F}_6\left(g\right)$

All three compounds contain sulfur and fluorine. Fluorine is a halogen, and its oxidation state is -1.

Disulfur decafluoride is a neutral compound containing two sulfur atoms and ten fluorine atoms.

Let the oxidation state of sulfur be x. Then, it can be determined as