How to calculate the formal charge of sulfate ion?
2013年4月27日 · The sulfur atom has a partial positive charge (#2) (note that partial charges, unlike formal charges, have some experimental basis). The four oxygen atoms have equivalent partial negative charges (#2). The partial negative charges on the oxygen atoms add to more than $-2$ but not anywhere near $-4$ (#1).
Why is negative charge more stable on sulphur than on oxygen?
2021年3月21日 · We know about the aromaticity of certain ring ketones in which the electronegative oxygen atom imparts a positive charge to a three- or seven-membered carbon ring. It turns out that despite what an elctronegativity table might suggest, the higher electron affinity of sulfur and selenium versus oxygen causes this characteristic to carry over to ...
How is (SO4)^2- Charged if S and O all are Neutral Themselves?
2015年10月14日 · As far as I understand $\ce{SO4^2-}$ structure, sulfur makes two coordinate bonds with two oxygen atoms and two double bonds are formed with oxygen after sulfur expands it's valance shell to 6. 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 ...
Oxidation state of the sulfur atoms in the thiosulfate Ion
2015年2月11日 · Similar to peroxide (as described in the IUPAC Gold Book), each sulfur is considered oxidation state -1. Now, we add an oxygen to one of those sulfurs. Oxygen is (almost) always -2. To keep the overall charge -2, that means that the newly bonded sulfur is oxidation state +1. Oxidizing that sulfur again gives sulfurs of +3 and -1.
Why does sulfate have this structure? - Chemistry Stack Exchange
You can't hybridize a d orbital and even get the proper tetrahedral geometry here. Reducing formal charges to 0 makes no real world sense, when sulfur has a measured empirical charge of around 1.7 in sulfate. Sulfate is 4 single bonds. The bond length difference is due to the fact that the sulfur carries extra charge, as does the oxygens.
Why do compounds like SF6 and SF4 exist but SH6 and SH4 don't?
In summary, the electronic structure of this system is best described as a sulfur center with a charge somewhere between $2+$ and $3+$; the corresponding negative charge is distributed among the equivalent fluorine atoms. Shown in Figure 12 is the orbital occupation of the sulfur center, $\ce{3s^1 3p^{2.1} 3d^{0.19} 5p^{0.03} 4f^{0.01}}$.
What is the charge of the sulfide ion? - Answers
2024年5月22日 · What is the net charge of a single sulfide ion? The net charge of a single sulfide ion is -2. This is because sulfur typically gains two electrons to achieve a stable electron configuration ...
What is the charge for Sulfur? - Answers
2024年6月2日 · Sulfur typically carries a charge of -2 in ionic compounds due to its position in Group 16 of the Periodic Table, where it tends to gain two electrons to achieve a stable electron configuration.
Sulfur trioxide structure - Chemistry Stack Exchange
2014年11月11日 · The charge-separation method. predicts a bond order of $1.33$ which is much closer to $1.4$ requires mesomery of three structures to explain the three equal bond lengths. I for my part prefer the mesomeric charge-separation description, because we have no trouble drawing benzene in the same way and because I like the octet rule.
Can a sulfur atom form six single bonds with six other sulfur atoms?
2020年1月30日 · The next element to come to mind was sulfur because it was the next element that could form solely single bonds, fill its valence shell (by reaching into the d orbital), and have a neutral formal charge. So can sulfur atoms form 6 single bonds with 6 other sulfur atoms?