2 interactive concept widgets for Redox Reactions. Drag any slider, change any number, and watch the formula and the answer update live. Built so you understand how each NEET problem actually works, not just the final number.
See oxidation states assigned to every atom in 15 compounds and ions. Each step traces the rules applied (free element, monatomic ion, O = −2, H = +1, sum rule).
Select a compound to find the oxidation state of every element with step-by-step reasoning. Covers KMnO₄, K₂Cr₂O₇, H₂O₂, and 12 more.
Select a compound to see the oxidation state of each element with step-by-step reasoning using the standard rules.
Key rules (in order of priority)
1. Free elements: ox. state = 0 (Fe, O₂, H₂...)
2. Monoatomic ions: ox. state = charge (Na⁺ = +1)
3. O = −2 (exception: O₂ = 0; H₂O₂ = −1; OF₂ = +2)
4. H = +1 bonded to non-metals; H = −1 in metal hydrides
5. F = −1 always (most electronegative)
6. Halogens Cl, Br, I = −1 unless bonded to O or more electroneg. element
7. Sum of all ox. states = 0 (neutral) or = ionic charge
KMnO₄
+1
K (×1)
+7
Mn (×1)
-2
O (×4)
1
O is −2 (4 × −2 = −8)
2
K is +1 (Group 1)
3
Sum = 0: +1 + Mn + (−8) = 0
4
Mn = +7
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Four preset redox reactions balanced step by step using the ion-electron method. Identify oxidation/reduction half-reactions, balance atoms and charge, then combine.
Walk through the ion-electron (half-reaction) method step by step for 4 NEET-relevant redox reactions including KMnO₄, K₂Cr₂O₇, and disproportionation.
Walk through the half-reaction method for balancing redox equations. Reveal each step in sequence.
Unbalanced
MnO₄⁻ + Fe²⁺ → Mn²⁺ + Fe³⁺
Medium: acidic
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