Question

According to Lewis dot theory, what types of electron pairs would you find surrounding the central atom of the sulfate ion?

Answer 1

Answer : The type of electron pair present in the surrounding of the central atom of the sulfate ion is, bonding electron pair.

Explanation :

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.

In the Lewis-dot structure the valance electrons are shown by 'dot'.

The representation of valence electrons of an atom by dots around the symbol of an element is said to be the Lewis-dot symbol.

In the representation of Lewis-symbol, one electron dot must put on each side of the element symbol then paired the electrons.

The given ion is, sulfate ion
`(SO_4^(2-))`

As we know that sulfur and oxygen has '6' valence electrons.

Therefore, the total number of valence electrons in
`SO_4^(2-)` = 6 + 4(6) + 2 = 32

According to Lewis-dot structure, there are 12 number of bonding electrons and 20 number of non-bonding electrons.

From the Lewis-dot structure we conclude that, the bonding pair of electrons present in the surrounding of the central atom of the sulfate ion.

The Lewis-dot structure of sulfate ion is shown below.

Answer 2

Bonding electron pairs

Step-by-step explanation:

Sulfate (SO₄²⁻)

Valence electrons of sulfur = 6

Valence electrons of oxygen = 6

Charge = 2 (Negative which means that the electrons are being added)

The total number of the valence electrons = 6 + 4(6) + 2 = 32

The Lewis structure is drawn in such a way that the octet of each atom and duet for the hydrogen in the molecule is complete. So,

The Lewis structure is:

`\begin{bmatrix}& .. & \\& :O: & \\& : & \\ :\ddot {O}&: S :& \ddot {O}:\\& : & \\& :O: & \\& .. & \\ \end{bmatrix}^(2-)`

Since, all the electrons pairs around the central atom, sulfur is bonded. So, the electron pairs are bonding electron pairs.