Hello, This question is from \'Chemistry: The Central Science 11th edition\' by

Question

Hello,

This question is from 'Chemistry: The Central Science 11th edition' by Brown.

Ch.4 4.53: Write balanced molecular and net ionic equations for the reactions of (b) chromium with hydrobromic acid; (c) tin with hydrochloric acid.

Attempts: b) Cr(s) + 2HBr(aq) CrBr2(aq) or CrBr3(aq)? + H2(g)

I got the left part of the reaction correct, but I can't figure out what charge chromium should have because it can have either +2 charge or +3 charge when it ionizes. The answer says that it should be CrBr2, but why can't it be CrBr3?

c) same thing for c. Why can't SnCl4 can be an answer?

Thank you

Explanation / Answer

You need a strong oxidizing compound (like potassium permanganate, potassium dichromate) to oxidize an element to the maximum charge. Hydracids, usually, are not strong enough.

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