Draw the Skeletal Lewis Structure for Ethane

After determining the total valence electrons (14) for C₂H₆, arrange the atoms to form a stable, bonded molecule.

1) Identify the central atom(s)

Carbon (C) is less electronegative than hydrogen (H) and forms four bonds, so carbon atoms are central. With two carbons present, they form the backbone by bonding to each other.

2) Create the skeletal structure

Connect the two carbon atoms with a single bond:

C – C

This uses 2 of the 14 valence electrons (12 electrons remaining).

3) Attach terminal atoms (hydrogen)

Distribute the six hydrogens evenly: each carbon bonds to three hydrogens so that each carbon makes four total bonds.

4) Final skeletal (Lewis) structure of ethane

 H H
 | |
H – C – C – H
 | |
 H H
 

Molecule: C₂H₆ (ethane)

5) Check the electron count

• Count bonds: 7 single bonds (1 C–C and 6 C–H).
• Count electrons: 7 bonds × 2 electrons per bond = 14 electrons (all valence electrons accounted for).

6) Check octets/duets

• Hydrogen: 1 bond (2 electrons) → duet rule satisfied.
• Carbon: 4 bonds (8 electrons) → octet rule satisfied.

Since all 14 valence electrons are used and each atom meets its duet/octet requirement, this is the correct Lewis structure for ethane.