What is the Lewis structure of H2SO4?

Answer 1

S is the central atom, with 2 single bonded Os around it and 2 double bonded ones. The two single bonded ones have the H atoms. S has an expanded octet and can have more than 8 valence electron. like this with a double bonded O on top and on bottom of the S atom

O=

H-O-S-O-H

O=

This is actually the Structural Formula of H2SO4. The Lewis structure would have dots instead of lines. You will have to use your smarts to change the lines into Lewis Structure dots.

Answer 2

The Lewis structure for H2SO4 is drawn with one sulfur atom in the center, surrounded by four oxygen atoms. Each oxygen atom is bonded to the sulfur atom through a single bond, and each oxygen atom has two lone pairs of electrons. The hydrogen atoms are bonded to the oxygen atoms through single bonds.

Answer 3

the centre atom is s and aroud it 4 oxygen in the right side oxygen gain one electron from h also the left oxygen gain one electrom from h.in the top oxygen gain two electron from s and oxygen didn't share any electron.same as also the bottom oxygen.

Answer 4

The structure of HSO4- is tetrahedral with the four oxygen atoms around the sulfur atom, and then bent with one of the oxygen atoms as the central atom and the hydrogen atom coming off of it. All of it is attached with single bonds.

Sulfur gives two of its electrons, 1 to two of the oxygen atoms, and because HSO4 is an ion it has an extra electron that is given to another oxygen atom. Thus the fourth oxygen atom yet to fill the octet rule bonds with the hydrogen.

Stephanie W.

10th grade chemistry

Lakota West High School I believe the answer above is incorrect. The structure of HSO4- (Bisulfate Ion) is certainly tetrahedral, but is centered around the sulfur atom. The Sulfur atom does not obey the octet rule as many atoms of the 3rd period do not. Therefore, there is a hydroxyl group (-OH) attached to the Sulfur atom (the oxygen has two pairs of nonbonded electrons), and two double bonded Oxygens (each with two pairs of nonbonded electrons). Finally, there is a single bonded Oxygen atom, carrying three pairs of nonbonded electrons and a negative charge. The molecule shows a classic case of resonant behavior, as the oxygen atoms bonded to the sulfur atom (excluding the one in the hydroxyl group) share the pi bond character. In other words, the negative charge is "floating" among the three oxygen atoms. Soor Kothari This dot structure begins with the S atom in the center. In one direction is an O atom doubly bonded with two pairs of dots. In the other three directions, an O atom is singly bonded and has three pairs of dots. The entire structure is bracketed and superscripted with a 1-.

Answer 5

it would normally be: ..

:O:

.. | ..

:O-S-O:

.. | ..

:O:

..

the formal charge of S being 2

and the formal charge of O being -1

so you get 2-4=-2 the overall charge of the ion

however there is a better way to form this ion due to formal charge the best way would be by having an atom have 0 as its formal charge as so:

..

O

.. ..

:O-S-O:

.. ..

O

..

here the formal charge of S is 0

the formal charge of the double bonded O is 0

and the formal charge of the single bonded O is -1

giving you 0+0-2=-2

Answer 6

Sulfer is central atom (least electro negative) srounnded by the 4 oxygen, two double bonds with the oxgyens to complete the octet rule tetraheral

Answer 7

the name of h2so3

Answer 8

O

Na O S O Na

O