Question

neutral compounds
in a neutral compound, the sum of the oxidation states is zero. note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. in h₂o, for example, each hydrogen atom has an oxidation state of +1 and each oxygen atom has an oxidation state of - 2 for a total of 2(+1)+(-2)=0.
part a
what is the oxidation state of an individual sulfur atom in mgso₄?
express the oxidation state numerically (e.g., +1).
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part b
what is the oxidation state of an individual nitrogen atom in hno₃?
express the oxidation state numerically (e.g., +1).
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Explanation:

Step1: Recall oxidation - state rules for MgSO₄

In a neutral compound, the sum of oxidation states is 0. Magnesium (Mg) has an oxidation state of +2, and oxygen (O) has an oxidation state of -2. Let the oxidation state of sulfur (S) be \(x\).

Step2: Set up the equation

For MgSO₄, we have \(+2 + x+4\times(-2)=0\).

Step3: Solve the equation for \(x\)

\[

$$\begin{align*} +2 + x-8&=0\\ x&=8 - 2\\ x&=+6 \end{align*}$$

\]

Step4: Recall oxidation - state rules for HNO₃

In a neutral compound, the sum of oxidation states is 0. Hydrogen (H) has an oxidation state of +1, and oxygen (O) has an oxidation state of -2. Let the oxidation state of nitrogen (N) be \(y\).

Step5: Set up the equation

For HNO₃, we have \(+1 + y+3\times(-2)=0\).

Step6: Solve the equation for \(y\)

\[

$$\begin{align*} +1 + y-6&=0\\ y&=6 - 1\\ y&=+5 \end{align*}$$

\]

Answer:

Part A: +6
Part B: +5