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 co₂(g) nh₃(g) h₂o(l) co(g)

Explanation:

Step1: Determine oxidation state of \(C\) in \(CO_2\)

Let oxidation state of \(C\) be \(x\). Oxidation state of \(O=-2\).
For \(CO_2\): \(x + 2(-2)=0\) (since molecule is neutral).
\(x-4 = 0\) → \(x = +4\).

Step2: Determine oxidation state of \(N\) in \(NH_3\)

Let oxidation state of \(N\) be \(y\). Oxidation state of \(H = +1\).
For \(NH_3\): \(y+3(+1)=0\) (since molecule is neutral).
\(y + 3=0\) → \(y=-3\).

Step3: Determine oxidation state of \(O\) in \(H_2O\)

Let oxidation state of \(O\) be \(z\). Oxidation state of \(H = +1\).
For \(H_2O\): \(2(+1)+z = 0\) (since molecule is neutral).
\(2+z=0\) → \(z=-2\).

Step4: Determine oxidation state of \(C\) in \(CO\)

Let oxidation state of \(C\) be \(w\). Oxidation state of \(O=-2\).
For \(CO\): \(w+(-2)=0\) (since molecule is neutral).
\(w - 2=0\) → \(w=+2\).

Answer:

species	oxidation state of highlighted atom
\(NH_3(g)\)	\(-3\)
\(H_2O(l)\)	\(-2\)
\(CO(g)\)	\(+2\)