C4H10 Lewis structure

C₄H₁₀ (butane) has four carbon atoms and ten hydrogen atoms.

In the C₄H₁₀ Lewis structure, 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.

Alternative method: Lewis structure of C₄H₁₀

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, carbon lies in group 14, and hydrogen lies in group 1.

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

Learn how to find: Carbon valence electrons and Hydrogen valence electrons

• 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

Lone pair

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.

Final structure

The final structure of C₄H₁₀ consists of a continuous chain of four carbon atoms, with hydrogen atoms linked to each carbon to fill their remaining valencies. In this layout, each of the four carbon atoms forms four single covalent bonds to satisfy the octet rule, while every hydrogen atom achieves a stable duet. Within this configuration, the two internal carbon atoms are each bonded to two other carbons and two hydrogens, whereas the two terminal carbon atoms are bonded to one carbon and three hydrogens. This arrangement represents the most stable state for the linear molecule because it results in a formal charge of zero for every atom involved. Consequently, this specific electronic distribution serves as the definitive and most accurate Lewis representation of n-butane.

Next: ICl Lewis structure

External video

• C4H10 Lewis Structure: How to Draw the Lewis Structure for C4H10 – YouTube • Wayne Breslyn

External links

• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/C4H10-Lewis-structure.html
• https://topblogtenz.com/butane-c4h10-lewis-structure-molecular-geometry-polar-or-non-polar/