Draw and Explain the Lewis Structure of C2H6

The Lewis structure of C₂H₆ (ethane) can be drawn by following these steps:

1. Count the total number of valence electrons: Carbon (C) has 4 valence electrons, and Hydrogen (H) has 1 valence electron. Since there are 2 carbon atoms and 6 hydrogen atoms, the total number of valence electrons is (2 × 4) + (6 × 1) = 14 electrons.
2. Draw the skeletal structure: Place the two carbon atoms in the center and arrange the hydrogen atoms around them. Each carbon atom will be bonded to three hydrogen atoms.
3. Distribute the electrons: Start by forming single bonds between the carbon atoms and the hydrogen atoms. Each single bond uses 2 electrons. After forming these bonds, you will have used 12 electrons (6 bonds × 2 electrons).
4. Complete the octets: The remaining 2 electrons will form a single bond between the two carbon atoms. This ensures that each carbon atom has a complete octet (8 electrons).

The final Lewis structure of C₂H₆ looks like this:

    H   H
    |   |
H—C—C—H
    |   |
    H   H

In this structure, each carbon atom is bonded to three hydrogen atoms and one carbon atom, satisfying the octet rule for both carbon atoms. The hydrogen atoms each have 2 electrons, fulfilling their duet rule.