C4H10 (butane) has four carbon atoms and ten hydrogen atoms. In the lewis structure of C4H10, there are three single bonds between the four carbon atoms. The left carbon and right carbon are attached with three hydrogen atoms, and the two center carbons are attached with two hydrogen atoms. And none of the atoms has a lone pair.
Here’s how you can draw the C4H10 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 C4H10 has four carbon atoms and ten hydrogen atoms, so…
Valence electrons of four carbon atoms = 4 × 4 = 16
Valence electrons of ten hydrogen atoms = 1 × 10 = 10
And the total valence electrons = 16 + 10 = 26
- Second, find the total electron pairs
We have a total of 26 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 = 26 ÷ 2 = 13
- 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 four atoms remaining and all four atoms are carbon, so we can assume any one as the central atom.
Let’s assume that the central atom is left carbon.
Therefore, place carbons in the center and hydrogens on either side.
- And finally, draw the rough sketch
#2 Mark Lone Pairs
Here, we have a total of 13 electron pairs. And thirteen 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 (left carbon) forms an octet. Hence, the octet rule is satisfied.
Therefore, this structure is the stable lewis structure of C4H10.
Next: ICl Lewis Structure