Which of the following reactions would be classified as oxidation-reduction? Check all that apply. 2Na(s)+Cl2(g)→2NaCl(s) Na(s)+CuCl(aq)→NaCl(aq)+Cu(s) NaCN(aq)+CuCl(aq)→NaCl(aq)+CuCN(s)

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Which of the following reactions would be classified as oxidation-reduction? Check all that apply. 2Na(s)+Cl2(g)→2NaCl(s) Na(s)+CuCl(aq)→NaCl(aq)+Cu(s) NaCN(aq)+CuCl(aq)→NaCl(aq)+CuCN(s)

Chemistry
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what do you think?
i thought it was the first one and last one but i got it wrong...
let's look at this more closely

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Other answers:

electrons have to be transferred from one element to the other, in the process of the reaction, so one is oxidized and the other is reduced.
how do you know Na doesnt have a charge?
@marmar10 interesting point, that might be where the point of confusion is. For your reference: "Any pure element—even if it forms diatomic molecules like chlorine (Cl2)—has an oxidation state of zero. Examples of this are Cu or O2." Na(s)+CuCl(aq)→NaCl(aq)+Cu(s) |dw:1443492397750:dw| Na goes from 0 to +1 so it's oxidized Cu goes from +1 to 0 so it's reduced. so electrons are lost from sodium and electrons are gained from copper.
i think your point of confusion was that any pure element has an oxidation state of 0
yes it makes a lot more sense now. I was looking in my book and it gave examples of ions so no wonder i was confused. Thank you
@Marmar10 no problem
weird the answer was the first and second one
|dw:1443493401499:dw|
ugh.. yeah.. technically the first one can be classified as oxidation reduction too.
Sodium goes from 0 to +1 and chlorine goes from 0 to -1
ok haha makes sense

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