Oct 14, 2015 · At this point calculating formal charge of those two coordinate bonded oxygen gives total formal charge of −2 and the formal charge on $\ce S$ and the double bonded $\ce O$ is zero. Thus the minus 2 charge on $\ce{SO4^2-}$ can be shown but initially all the atoms were neutral. While making bonds electrons were shared only.

Mar 20, 2019 · This leaves behind the sulfate ion: $$\ce{H2SO4 -> 2H+ + SO4^2-}$$ When the $\ce{H^+}$ ion departs, it leaves its electron behind, so it has to go somewhere (it remains with the $\ce{O}$ atom). Hypothetically if $\ce{SO4}$ existed, with all $\ce{O}$ atoms double-bonded to the $\ce{S}$ , then the sulfur would have a total of 16 electrons in its ...

The S-O bond length in $\ce{SO4^{2-}}$ is 149 pm, which is shorter than that observed in sulfuric acid (157 pm) and very close to the gas-phase bond length of sulfur monoxide which is 148 pm. So, at the end of the day, an electron dot structure is a type of model that describes bonding.

C, N, and O are from groups 4, 5, and 6, and their atomic numbers are 6, 7, and 8. (1) Give a reasonable Lewis structure for CN2−, including formal charges (N.B. the C is the central atom). 2 (2) Give a reasonable Lewis structure for CO2−, including formal charges (N.B. the C is the central atom). 3 (3) Give a reasonable Lewis structure for O2−, including formal charges. 2 …

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Jun 17, 2018 · My question is, why can't the dissociation reaction happen like this: $$\ce{H2SO4 -> 2H^+ +SO4^{2-}}$$ I know hydrogen is a diatomic gas, but here I don't know if H will dissociate as a gas or as a liquid (since $\ce{H2SO4}$ is a liquid, not a gas).

Sep 5, 2015 · $$\ce{HSO4- (aq) + H2O <-> H3O+ (aq) + SO4^2- (aq)}$$ The sulfate ion should be a weak conjugate base, and hence the sodium sulfate salt should be a weak base. This was my line of reasoning, until today my friends told me it is actually a neutral salt, which was confirmed by searching online.

Jan 17, 2018 · I do understand the potential for the second $\pu{1.68 V}$ since for the second reaction the underlying redox pair is $\ce{Pb^4+ + 2 e- -> Pb^2+} $. For this redox pair the electrochemical standard potential is $\pu{1.69 V}$. But for the first reaction I think that the underlying redox pair has to be $\ce{Pb^2+ + 2 e- -> Pb}$.

Oct 7, 2018 · Why is $\ce{OH-}$ preferentially discharged over $\ce{SO4^2-}$ in the anode? One explanation I've found is that because $\ce S$ in $\ce{SO4^2-}$ has an oxidation number of $+6$ which is a maximum and thus cannot be oxidized any further.

In the equation $\ce{2SO4^2- -> S2O8^2- + 2e-}$ sulfate is being oxidized. This is different from oxygen being oxidized. The statement in the OP "In this reaction 2 of the oxygen ions change from $-2$ to $-1$ " is incorrect. Instead, each sulfate ion, taken as a whole, loses 1 electron.