H_{2} (hydrogen) has **two hydrogen** atoms. In the lewis structure of H_{2}, there is a single bond between the two hydrogen atoms, and none of the atoms has a lone pair.

## Steps

Here’s how you can draw the H_{2} lewis structure step by step.

Step #1: draw sketch

Step #2: mark lone pairs (if there are)

Let’s break down each step in detail.

### #1 Draw Sketch

- First, determine the total number of valence electrons

In the periodic table, hydrogen lies in group 1. Hence, hydrogen has **one** valence electron.

Since H_{2} has two hydrogen atoms, so…

Valence electrons of two hydrogen atoms = 1 × 2 = 2

So the **total valence electrons** = 2

- Second, find the total electron pairs

We have a total of 2 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the **total electron pairs** = 2 ÷ 2 = 1

- Third, determine the central atom

Here, there are only two atoms and both atoms are hydrogen, so we can assume any one as the central atom.

Let’s assume that the **central atom is right hydrogen**.

- And finally, draw the rough sketch

### #2 Mark Lone Pairs

Here, we have a total of 1 electron pair. And one H — H bond is already marked. So we do not have to mark any electron pair as a lone pair on the sketch.

And in the above structure, you can see that the central atom (right hydrogen) forms a duet. Hence, the duet rule is satisfied.

Therefore, this structure is the stable lewis structure of H_{2}.

**Next:** N_{3}^{–} Lewis Structure