Question

use the references to access important values if needed for this question.
determine the oxidation state for each of the elements below.
the oxidation state of zinc in tetrahydroxozincate ion $zn(oh)_4^{2 - }$ is.
the oxidation state of chlorine in hypochlorous acid $hclo$ is.
the oxidation state of sulfur in thiosulfate ion $s_2o_3^{2 - }$ is.

Explanation:

Step1: Calculate oxidation state of Zn in \(Zn(OH)_4^{2 -}\)

Let oxidation state of Zn be \(x\). Oxidation state of \(OH^-\) is \(- 1\).
For the ion \(Zn(OH)_4^{2 -}\), we have \(x+4\times(-1)=-2\)
\(x - 4=-2\)
\(x = + 2\)

Step2: Calculate oxidation state of Cl in \(HClO\)

Let oxidation state of Cl be \(y\). Oxidation state of H is \(+1\) and of O is \(-2\).
For \(HClO\), \(+1 + y+(-2)=0\)
\(y - 1=0\)
\(y = + 1\)

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

Let oxidation state of S be \(z\). Oxidation state of O is \(-2\).
For \(S_2O_3^{2 -}\), \(2z+3\times(-2)=-2\)
\(2z-6 = - 2\)
\(2z=4\)
\(z = + 2\)

Answer:

Zinc: \(+2\), Chlorine: \(+1\), Sulfur: \(+2\)