HSO4– Structure, Properties and more than

Hydrogen sulphate also known as bisulphate, is an odorless anion in the form of a white powder. It is made up of one hydrogen, one sulphur and four oxygen atoms. The Lewis structure of this molecule has to exist known first to better understand its physical and chemical properties. The construction will aid in understanding the organization of atoms, bond formation and shape of the molecule.

Chemical Name Hydrogen Sulfate
HSO4 – Valence electrons 32
Molecular Weight/ Molar Mass 97.064 g/mol
Boiling Point N/A
Melting Point 59 °C
Chemic Formula HSO 4–

In this blog post, we will look at the HSO4 – construction and properties. But for knowing the Lewis structure of whatever molecule, we commencement need to know the total number of valence electrons.

HSO4 – Valence electrons

The electrons present in the outer vanquish of the cantlet are the ones that participate in bond formation and are known equally valence electrons.

To know the Lewis structure we will first summate the full number of valence electrons for HSO4 –

Total number of valence electrons – Valence electrons of Hydrogen + Valence electrons of Sulfur+Valence electrons of Hydrogen

Sulfur has 6 valence electrons in its outer shell.

Oxygen has six valence electrons in its outer shell, but equally we know there are four oxygen atoms in this molecule. Hence we will multiply the number by 4. And then now there are 24 valence electrons for all oxygen atoms.

However hydrogen has two valence electrons in this structure.

= half dozen+24+2

= 32 valence electrons

So for the HSO4 –  Lewis structure, we have a total of 32 valence electrons.

HSO4 –  Lewis structure

A Lewis structure is a pictorial presentation of how atoms are arranged in the molecule. As sulfur atom is the least electronegative, nosotros will put it in the heart. Now nosotros have four Oxygen atoms that volition exist kept around the Sulfur atom, so the Hydrogen cantlet will go on the outside of one of the Oxygen.

We'll beginning put a pair of electrons between atoms to form bonds. Place a pair of electrons between each Oxygen and Sulfur atom to show bonds. Repeat the same for ii Hydrogen atoms. Placing electrons for showing bonds will utilize upwards 12 valence electrons out of 32. After sharing valence electrons Hydrogen has attained a stable structure equally it only needs two electrons to complete its octet.

Then now we become around and fill up the octets for the Oxygen atoms as. Doing then will use all 32 valence electrons. As the central Sulfur atom is forming bonds with 6 atoms, it is sharing all its valence electrons. As sulfur is a grouping 13 element it tin can expand its orbitals to accommodate more than electrons.

Sulfur has more than than 8 valence electrons, each of the Oxygen atoms has an octet, and the Hydrogen, hither, has 2, then that its outer beat out is consummate. But equally Sulfur is in period three on the periodic tabular array, let us check the formal charges on each atom to make certain they're every bit shut to zero as possible.

When we check the formal charges, we can see that Sulfur in the center has a +2 charge, where each of the Oxygen atoms have a -one accuse. As we would like those formal charges to be as closer to zero if possible, nosotros accept a pair of electrons from the exterior of the Oxygen and course a double bail with the Sulfur, that volition alter the formal charges so that this Oxygen now has a formal charge of 0 and the Sulfur has a accuse of +1.

So let's practise that once again over here. Afterwards forming a double bond here, we now take a formal charge of 0 on this Oxygen and the Sulfur is 0. That leaves us with a -ane formal charge on this Oxygen here. Due to such arrangement, the molecule has a negative accuse up there. So the overall accuse on this is -1, just like in the HSO4- chemical formula correct here. The last thing we demand to exercise is put brackets around this, because it has a negative charge.

Hence this is the most stable Lewis structure for HSO4-.

hso4-lewis structure

Properties of HSO4-

  • Sodium Bisulfate (NaHS04) which is the pure substance starts melting at 185°C and begins to lose water and forms the hydrogen sulphate ion (HSO4). The structure is like to that of methyl hydride.
  • It is classified as a weak acid as it partially dissociates to form H+ and SO4^ii-.
  • Hydrogen sulfate forms hydronium ion and sulfate ion when treated with water. The chemical equation is given below.

HSO4– + H2o → H3O+ + SO42-

  • Hydrogen sulfate reacts with nitrate ion forming nitrous acid and sulfate ion. The chemical equation is given below.

HSO4– + NO2– → SO42- + HNO2