I thought (NO3) Would be (3 x -2 for oxygen = -6, meaning N =+6) But then I read somewhere that NO3 has a negative charge overall, so Im assuming then N=5?
So, if there is - overall for the Nitrogen Trioxide, does that mean that Mn is +1?
I thought (NO3) Would be (3 x -2 for oxygen = -6, meaning N =+6) But then I read somewhere that NO3 has a negative charge overall, so Im assuming then N=5?
So, if there is - overall for the Nitrogen Trioxide, does that mean that Mn is +1?
Wait sorry, forgot about the 2
So, does that mean then
Mn = +2
N =+10
O =-12?
Mn is +2 but you won't need to double the oxidation states for nitrogen or multiply by 6 oxygen. They refer to the individual atoms within each molecule: so O is still -2 and N is still +5.
NiO2 + 2 H2O + Fe Ni(OH)2 + Fe(OH)2 in basic solution
So can you walk me through the oxidation numbers again please? Will actually paypal you £10
Ni = +4 because O2 =-4? Im such a ****ing idiot
The oxidation state rules are simple.
1. The sum of all oxidation states = the charge on the species. 2. Oxygen is always -2 except in peroxides (or with fluorine) 3. S block metals are always +1 in compounds 4. Elements are always 0
1. The sum of all oxidation states = the charge on the species. 2. Oxygen is always -2 except in peroxides (or with fluorine) 3. S block metals are always +1 in compounds 4. Elements are always 0
So yes, in NiO2 nickel is +4
Next step, balance the oxygens and then the hydrogens, yeah?
1. The sum of all oxidation states = the charge on the species. 2. Oxygen is always -2 except in peroxides (or with fluorine) 3. S block metals are always +1 in compounds 4. Elements are always 0
So yes, in NiO2 nickel is +4
Wait, actually
Fe --> Fe(OH)2 Therefore, = Oxidation of + 2 NiO2 --> NiOH Therefore = Reduction of -2
NiO2 + 2H2O
I get that the oxygens have been balanced here, by virtue of the water molecules. But, what about balancing the hydrogens?
Do I add up all the oxidation numbers?
H2O (So that is +2 and -2) + NiO2 (which is +4 and -4 respectively)
Confused now
The answers state:
2 H 2O + NiO2+2e-
Bit lost where the +2e came from. Is that simply because I have already worked that out, or?
See, this is where I am getting tripped up, the rules and limits etc regarding basic solution, acidic solution and alkaline solution
I worked through your stuff though (thanks very much btw, eloquently and clearly written) and I am beginning to see HOW and WHY things fit in the way they do
See, this is where I am getting tripped up, the rules and limits etc regarding basic solution, acidic solution and alkaline solution
I worked through your stuff though (thanks very much btw, eloquently and clearly written) and I am beginning to see HOW and WHY things fit in the way they do
Then I split the equation to get my two half equations.
2CN- +Au ---> Au(CN)-2 +2e-
Got confused with the reduction equation.
O2 -----> H2O2
RHS has 2 Hydrogens so to balance:
O2 + 2H+ ----> H2O2
Total charge on LHS I thought was 2, (because oxygen here is elemental, ergo, no charge and 2 from the 2 hydrogens I just added) and the RHS was -2 (+2 for the hydrogen, -4 for the oxygen).
Therefore, I would add 4 electrons to LHS?
Ohhhh! Wait! The RHS, that is a peroxide, so it balances out with overall charge of 0?
Ergo, then, that means to make LHS =RHS, we must add 2 electrons not 4 electrons to LHS ?