Question

What are the number of lone pairs and bond pairs in SO2? And how to draw its structure with this info.

Answer 1

Answer:

Explanation:

Sulphur dioxide, SO2

Sulphur dioxide could be drawn exactly the same as carbon dioxide (again without making any assumptions about the shape):

          O=S=O( is the structure)

The argument develops differently though. Sulphur has 6 electrons in its outer level, and the oxygens between them contribute another 4 (1 for each bond). That gives 10 electrons in total - 5 pairs. 4 pairs are needed for the bonds, leaving 1 lone pair. Each double bond uses 2 bond pairs and can be thought of as a single unit.

Answer 2

Answer:

There are four bond pairs and one lone pair of electrons in SO₂.

Concept:

Covalent Bond: The bond formed by sharing of electrons is called a covalent bond.

Lone pair of electrons: The pair of electrons that don't participate in bond formation is called the lone pair.

Bond pair of electrons: The pair of bonding electrons is called bond pair.

Solution:

We are given with a molecule of sulphur dioxide gas, i.e., SO₂.

The structure of SO₂ is like this -

$\huge{ \ddddot O=\huge \ddot S=\ddddot O}$

Dots represent the non-bonding electrons.

So, we can see clearly that SO₂ has two $\sigma$ bonds and two $\pi$ bonds.

For two  $\sigma$ bonds, bond pairs of electrons = 2

For two $\pi$ bonds, bond pairs of electrons = 2

Lone pair of electron on central atom, i.e., on S = 1

Total bond pairs = 2 + 2 = 4

Total lone pairs = 1

Hence, there are four bond pairs and one lone pair in SO₂.

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