Given the following balanced equation: 2Na + Cl2 ---> 2NaCl

Question

A.List each element on the reactant side and each element on the product side and assign the correct oxidation number to each.
B.Identify which element is oxidized in the reaction and which is reduced. C.Identify the oxidizing agent in this reaction.

Answer 1

Am I doing this right?

A. Reactant
———————
Element(Na) Reactant(2) Product(2)
Element(Cl) Reactant(2) Product(1)
{Na and Cl are different element so I’m guessing there Reactant and Products are different from each other’s}

B. Oxidizing and Reduced
————————————
2Na+Cl2———>2NaCl
^ ^
| |
(Oxidized) (Reduced)
{Because at first it has a 2 then it gets taken away}

C. The Oxidizing Agent
———————————
2Na? or Na?
{Because it didn’t get reduced so I’m guessing it’s 2Na or Na}

Side note: I’m not good at chemistry but at least I tried. Can you help me if I’m wrong please?

Answer 2

For B) I was talking about the Cl’s lol the arrows had moved it the wrong place (I figured that would happen

Answer 3

2Na + Cl2 ---> 2NaCl

Na went from a state of zero, to a +1: it lost an electron, oxidized
Cl went from a state of zero, to a -1: it gained electron, reduced.