Questions: Determine the oxidation state of the highlighted atom in KNO3: species oxidation state of highlighted atom ------ Cl2(g) 0 KNO3(s) Fe2+(aq) CuCl(s)

Determine the oxidation state of the highlighted atom in KNO3:

species oxidation state of highlighted atom
------
Cl2(g) 0
KNO3(s)
Fe2+(aq)
CuCl(s)

Transcript text: Determine the oxidation state of the highlighted atom in KNO3: \begin{tabular}{|c|c|} \hline species & \begin{tabular}{c} oxidation state of \\ highlighted atom \end{tabular} \\ \hline $\mathrm{Cl}_{2}(g)$ & 0 \\ \hline $\mathrm{KNO}_{3}(s)$ & $\square$ \\ \hline $\mathrm{Fe}^{2+}(a q)$ & $\square$ \\ \hline $\mathrm{CuCl}_{(s)}$ & $\square$ \\ \hline \end{tabular}

Solution

Solution Steps

Step 1: Identify the compound and the highlighted atom

The compound given is potassium nitrate, \( \mathrm{KNO}_3 \). The highlighted atom is nitrogen (N).

Step 2: Determine the oxidation states of known elements

Potassium (K) is in Group 1 of the periodic table and has an oxidation state of \( +1 \).
Oxygen (O) typically has an oxidation state of \( -2 \).

Step 3: Set up the equation for the sum of oxidation states

The sum of the oxidation states in a neutral compound must equal zero. Let \( x \) be the oxidation state of nitrogen (N).

The formula for potassium nitrate is \( \mathrm{KNO}_3 \), so we have: \[ (+1) + x + 3(-2) = 0 \]

Step 4: Solve for the oxidation state of nitrogen

\[ 1 + x - 6 = 0 \] \[ x - 5 = 0 \] \[ x = +5 \]

Final Answer

\[ \boxed{+5} \]

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