Question

24 mark for review in which of the following species does sulfur have the same oxidation number as it does in h2so4? a h2so3 b s2o3^2- c s^2- d so2cl2

Explanation:

Step1: Calculate oxidation number of S in \(H_2SO_4\)

Let oxidation number of \(S\) be \(x\). Oxidation number of \(H = + 1\) and \(O=-2\).
Using formula: \(2\times(+1)+x + 4\times(-2)=0\) (since overall charge of neutral molecule is \(0\))
\(2 + x-8 = 0\)
\(x=+6\)

Step2: Calculate oxidation number of S in \(H_2SO_3\)

Let oxidation number of \(S\) be \(y\).
\(2\times(+1)+y + 3\times(-2)=0\)
\(2 + y - 6=0\)
\(y = + 4\)

Step3: Calculate oxidation number of S in \(S_2O_3^{2 -}\)

Let oxidation number of \(S\) be \(z\).
\(2z+3\times(-2)=-2\)
\(2z-6=-2\)
\(2z = 4\)
\(z = + 2\)

Step4: Calculate oxidation number of S in \(S^{2-}\)

Oxidation number of \(S=-2\) (as it is an ion with charge \(-2\))

Step5: Calculate oxidation number of S in \(SO_2Cl_2\)

Let oxidation number of \(S\) be \(w\). Oxidation number of \(O=-2\) and \(Cl=-1\)
\(w+2\times(-2)+2\times(-1)=0\) (neutral molecule)
\(w - 4-2=0\)
\(w=+6\)

Answer:

D. \(SO_2Cl_2\)