C2H6 (ethane) has two carbon atoms and six hydrogen atoms. In the lewis structure of C2H6, there is a single bond between the two carbon atoms, and each carbon is attached with three hydrogen atoms, and none of the atoms has a lone pair.
Here’s how you can draw the C2H6 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
Hence, carbon has four valence electrons and hydrogen has one valence electron.
Since C2H6 has two carbon atoms and six hydrogen atoms, so…
Valence electrons of two carbon atoms = 4 × 2 = 8
Valence electrons of six hydrogen atoms = 1 × 6 = 6
And the total valence electrons = 8 + 6 = 14
- Second, find the total electron pairs
We have a total of 14 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 = 14 ÷ 2 = 7
- Third, determine the central atom
Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.
Now there are only two atoms remaining and both atoms are carbon, so we can assume any one as the central atom.
Let’s assume that the central atom is right carbon.
- And finally, draw the rough sketch
#2 Mark Lone Pairs
Here, we have a total of 7 electron pairs. And seven bonds are 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 carbon) forms an octet. Hence, the octet rule is satisfied.
Therefore, this structure is the stable lewis structure of C2H6.
Next: COCl2 Lewis Structure