Question

some chemical reactants are listed in the table below. complete the table by filling in the oxidation state of the highlighted atom.

species	oxidation state of highlighted atom
fe²⁺(aq)
cf₄(l)
h₃o⁺(aq)

Explanation:

Step1: Determine oxidation state of V in VO

Oxygen has an oxidation state of - 2 in most compounds. Let the oxidation state of V be \(x\). In a neutral compound, the sum of oxidation states is 0. So \(x+( - 2)=0\), solving for \(x\) gives \(x = + 2\).

Step2: Oxidation state of Fe in \(Fe^{2 +}\)

The charge on the ion is the oxidation state. So the oxidation state of Fe is + 2.

Step3: Determine oxidation state of C in \(CF_{4}\)

Fluorine has an oxidation state of - 1 in compounds. Let the oxidation state of C be \(y\). For the neutral compound \(CF_{4}\), \(y+4\times(-1)=0\), solving for \(y\) gives \(y = + 4\).

Step4: Determine oxidation state of O in \(H_{3}O^{+}\)

Hydrogen has an oxidation state of + 1 in most compounds. Let the oxidation state of O be \(z\). For the ion \(H_{3}O^{+}\), \(3\times(+1)+z= + 1\), solving for \(z\) gives \(z=-2\).

Answer:

species	oxidation state of highlighted atom
\(Fe^{2+}(aq)\)	+ 2
\(CF_{4}(l)\)	+ 4
\(H_{3}O^{+}(aq)\)	- 2