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I have been trying to balance this chemical reaction in an "acidic" medium without using oxidation number or ion electron method: [$\ce{Fe^2+ + Cr2O7^2- -> Cr^3+ + Fe^3+}$].

Though I can balance number of atoms on both the sides $[\ce{Fe^2+ + Cr2O7^2- + 14H+ -> 2 Cr^3+ + Fe^3+ + 7 H2O}]$, but charge is still unbalanced. I am not sure why? I don't have any intuition about what's going on here.

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    $\begingroup$ I think you mean $\ce{Cr2O7^2-}$. $\endgroup$
    – Mathew Mahindaratne
    Commented Aug 4, 2019 at 19:12
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    $\begingroup$ This gives a pretty good step-by-step guide on how to go about the task: ck12.org/book/CK-12-Chemistry-Concepts-Intermediate/section/… $\endgroup$
    – Buck Thorn ♦
    Commented Aug 4, 2019 at 21:29
  • $\begingroup$ $\ce{6Fe^2+ + Cr2O7^{2-} + 14H+ -> 2 Cr^3+ + 6Fe^3+ + 7 H2O}$ $\endgroup$
    – Adnan AL-Amleh
    Commented Aug 5, 2019 at 4:38
  • $\begingroup$ You need not to use oxidation number, they are just convenient guidance. Good chemists can balance equation by their intuition, as they can easily see the proper way to do it. Other need to follow 2 fundamental rules of nature: 1/ Law of the total charge conservation 2/ Law of the element mass conservation. $\endgroup$
    – Poutnik
    Commented Aug 14, 2019 at 16:16

1 Answer 1

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A balanced equation must have a mass balance i.e., the masses should be equal on both sides and charges must be balanced as well. Oxidation number is just a way of book-keeping. Nothing fundamental there.

$$\ce{Fe^2+ + Cr2O7 + 14H+ -> 2 Cr^3+ + Fe^3+ 7 H2O}$$

What are you forgetting? It is mass balanced. Does $\ce{Cr2O7}$ exist? Hint: It is potassium dichromate.

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