Why does sulfate have this structure? - Chemistry Stack Exchange
The electron-dot model of bonding is so meaningful because it can be adapted to explain various experimental observables. You can draw two perfectly reasonable electron dot structures for $\ce{SO4^{2-}}$: one with all $\ce{S-O}$ single bonds and one with two $\ce{S=O}$ double bonds (and the additional resonance structures).
Correct representation of Lewis structure for sulphate ion
2020年7月3日 · $\begingroup$ Both structures might be accepted but the best way to draw it in the Lewis formalism is to put a double positive charge on sulphur and have all four oxygens be negatively charged. That also ensures complete equivalence of the oxygens without the need for resonance structures. $\endgroup$ –
How to calculate the formal charge of sulfate ion?
2013年4月27日 · Sulfate ion has two valid structures that you could draw, one with sulfur having a formal charge of zero and one with sulfur having a formal charge of +2. The structures below (from the Wikipedia page, released into the public domain) follow the annoying but allowable convention of replacing lone pairs with bars.
Bond angles in sulfate - Chemistry Stack Exchange
2015年9月25日 · However, the resonance structure on the left (and all of its equivalent representations) are more than likely acceptable for introductory chemistry classes. Note that no matter which resonance structure you think is a better representation of the sulfate ion, the bonds are all equivalent and therefore sulfate ion has the ideal tetrahedral bond ...
What is the chemical structure / hybridization of sulfuric acid?
2012年8月27日 · $\begingroup$ A structure with four double bonds in the sulphate ion would give the sulphur atom a formal charge of -2. This is not expected to be more stable than a configuration with two double bonds and two single bonds, because in the latter case the same amount of formal charge is more distributed, and lies mostly on a more electronegative ...
resonance - Why (SO4)^2- does not create 4 double bonds
2019年3月20日 · The sulfate ion is derived from the sulfuric acid molecule: When it undergoes chemical reactions, it typically donates both hydrogens as $\ce{H+}$ ions. 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).
How many resonance structures can be drawn from O3?
2024年5月25日 · The sulfate ion has four resonance structures. Wiki User. ∙ 9y ago. This answer is: ... AnswerBot. ∙ 5mo ago. Copy. There are two resonance structures that can be drawn for O3 (ozone). This is ...
Structures of Thiosulfate, Dithionate & Tetrathionate Ions
There ia a negative charge on the apical sulfur and another negative charge distributed across the 3 oxygens by resonance. Dithionate $\ce{[S2O6]^{-2}}$ There is one negative charge distributed by resonance over each group of 3 oxygens. Dithionite $\ce{[S2O4]^{-2}}$ There is one negative charge distributed by resonance over each group of 2 oxygens.
What is more stable: a carbonate ion or a sulphate ion?
2015年3月26日 · ‘more resonance structures’ (sulphate actually has only one significant resonance structure, carbonate three) geometrical features such as being tetrahedral. electronegativity (carbon is less electronegative, one would assume its anion to be more stable) resistance to reduction. an equilibrium with a gaseous compound
Most contributing resonance structure of phosphoric acid
2017年10月1日 · Structure having filled octet a for second row elements ($\ce {C, N, O, F}$) are stable. (followed by both structures) $\ce {H_3PO_4}$ is different from phosphate ion.None of the answers in the linked question directly state what would be the more contributing structure. They focus on the hybridisation of P in phosphate.