Multiple Choice
What is the oxidation state of manganese (Mn) in Mn(ClO4)3?
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6. Chemical Quantities & Aqueous Reactions
Calculate Oxidation Numbers
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What is the oxidation state of manganese (Mn) in the compound Mn(CrO4)2?
A
+2
B
+3
C
+4
D
+6
Verified step by step guidance1
Identify the overall charge of the compound Mn(CrO4)2. Since no charge is given, assume it is neutral (charge = 0).
Determine the oxidation state of the chromate ion (CrO4)^{2-}. The chromate ion has a charge of -2 overall.
Assign the oxidation state of oxygen as -2. Since there are 4 oxygen atoms, the total oxidation from oxygen is 4 \times (-2) = -8.
Let the oxidation state of chromium (Cr) be x. The sum of oxidation states in CrO4^{2-} is x + (-8) = -2. Solve for x: x - 8 = -2, so x = +6.
Since there are two chromate ions, the total negative charge contributed by the two CrO4^{2-} ions is 2 \times (-2) = -4. To balance this, the oxidation state of Mn must be +4 to make the compound neutral.
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