How to balance the following equation using oxidation states?

Sn+HNO3-------> SnO2 + NO2 + H2O

How do I balance this using oxidation stateS?

Can't you use the example I showed you earlier and apply it to this problem?

The only species changing oxidation state are:

Sn(zero) --> Sn⁴⁺ + 4e
N⁵⁺ + 1e --> N⁴⁺

now take it from there...

Ohh I understand! but one question; in the AQA book it says Oxygen's oxidation state is always -2, except for in Peroxides where it is -1.

Isn't SnO2 a peroxide? so therefore it should be -2 for O2 and thus +2 for Sn?

Or am I missing something?

Thanks, much appreciated

No, SnO₂ isn't a peroxide.

The oxygen is in the usual -2 state.

How would you know this though?

Good question. Experience I guess.

Peroxides only appear in group 1 group 2 and organic compounds. The most common peroxides in inorganic chemistry are sodium and barium peroxides, Na₂O₂ and BaO₂

ohh thanks, hopefully a compound that I am used to will come up in the exam.

Also one last question, sorry for bothering you, but doesn't Oxygen's oxidation state change?

Sn+HNO3-------> SnO2 + NO2 + H2O

LHS: -2x3=-6 RHS: (-2x2)+(-2x2)+-2=-10

no, the equation isn't balanced yet, so you can't 'count up'

I meant as in shouldn't I list oxygen the same way these 2 were listed:

Sn(zero) --> Sn4+ + 4e
N5+ + 1e --> N4+

and then see if oxygen has been reduced/oxidised?

Can't you use the example I showed you earlier and apply it to this problem?

The only species changing oxidation state are:

Sn(zero) --> Sn⁴⁺ + 4e
N⁵⁺ + 1e --> N⁴⁺

now take it from there...

uve made a mistake geez, u forgot to do hydrogen.

Sn+HNO3-------> SnO2 + NO2 + H2O

+1 and +1x2 = 2+

becos hydrogens oxidaton nr has gone from 1 to 2, it means electron has been lost, so its oxidised

OP, please disregard this post.

I'm sure you have more experience, but isn't he right ? lol

it's the same as the oxygen question. You cannot compare oxidation states in this way. if the equation is not balanced there is no way you can add up species on both sides.

This is the idea of balancing the equation in the first place.

You have to follow a methodology and balance the equation by considering the individual oxidation states of the components.

Sn + hno₃ -----> sno₂ + no₂ + h₂o

left hand side
------------------

sn (element) = zero
------------------------------

hno₃

h = +1
n = +5
o = -2

-----------------------------
right hand side
------------------

sno₂
sn = +4
o = -2

-----------------------------

no₂
n = +4
o = -2

-----------------------------

h₂o
h = +1
o = -2

----------------------------

so, conclusion: The only elements that change their oxidation state are sn and n

now you follow a system to balance the equation using this information (as previously outlined)