Question

Can someone help me with redox reactions using this as an example? What is the formula, including charge (if any), and state of the products of the reaction consistent with the display of reactants. Do not balance. Separate your answers by a comma. If there is no reaction, type NONE.
Zn(s) + Ag+(aq) →

Answer 1

Zn (s) is neutral
Ag+ has a 1+ charge

Zn is the reducing agent and it will oxidized
Ag+ is the oxidizing agent and it will be reduced

-> Zn+2 + Ag (s)

Answer 2

no balanced

Answer 3

well actually you have to look at a table of reduction potential to see if this will happen spontaneously, i assumed it would, but thats not necessarily the case

Answer 4

I'm confused why Ag has a charge when it's a transition metal, and Zn is neutral. I thought transition metals were neutral in charge. Also, I'm confused because I thought the charges were always supposed to add up to 8, which I don't see these adding up to.

Answer 5

as it is stated in the equation Ag has a 1+ charge no?

Zn is elemental and so it does not have a charge

the charges do not have to add up to eight, you're talking bout valence electrons

Answer 6

in redox reactions, you're dealing with exchange of electrons between molecules or elements

Answer 7

I see, so the charges are what it acquiring or giving away?

Answer 8

charges in the form of electrons

Answer 9

I see. What do you mean by Zn being an elemental? Is Ag the same, but different in this instance due to the problem?

Answer 10

elemental means it is neutral the (s) means that it is solid and that gives it away when it is by itself. Ag has a plus charge in the question, that means it's oxidation state is +1, meaning it's lost an electron

Answer 11

http://www.khanacademy.org/science/chemistry/oxidation-reduction
watch these vids

Answer 12

Thank you so much!

Answer 13

no problem !

Answer 14

That really helps a lot.

Answer 15

yeah those vids are pretty awesome. if you want more, search youtube. there is TONS

Answer 16

there are* haha