Got a question about oxidation numbers...any help?
The question is, does Cl change oxidation numbers here?
According to my understanding of oxidation numbers, Cl is a halogen, so it should be a negative one in both the first and the second one. Al goes from a +3 to a 0 oxidation number, correct? But where do the electrons come from that it gets?! Wouldn't Na only go from a 0 to a +1? So where do the other two electrons come from? Doesn't a REDOX reaction have to be balanced? Or not? Can someone un-confuse me here...
Answer:
Cl does not change - it is -1 the whole time. Al is reduced and Na is oxidized.
The problem is that the equation isn't properly balanced. There should be a 3 in front of Na and NaCl.
Cl does not change oxidation numbers. The balanced reaction should be AlCl3+ 3Na -->3NaCl +Al
You are on the right track. Oxidation number Al is +3 so you would need 3 Cl atoms to accept all of those electrons.
To balance your equation, place a 3 coefficient in front of your Na atom on the reactant side and a 3 coefficient in front of the salt (NaCl) on the product side.
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