Draw the Lewis Formula and a Three Dimensional Structure for Butane (C4H10): Indicate Hybridization and Bond Angles at Each Carbon Atom

To draw the Lewis structure of butane (C₄H₁₀), we start by calculating the total number of valence electrons. Each carbon atom contributes 4 valence electrons, and each hydrogen atom contributes 1. Hence, the total is:

• Carbon: 4 x 4 = 16 electrons
• Hydrogen: 10 x 1 = 10 electrons
• Total = 16 + 10 = 26 valence electrons

Now we arrange the carbon atoms in a chain, since butane is an alkane with a linear structure. Each carbon atom forms four bonds:

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

In the Lewis structure, each line represents a bond between atoms. Every hydrogen atom is bonded to a carbon atom, and this fully satisfies their valence.

For the three-dimensional structure, we can visualize butane as having a zigzag formation due to the tetrahedral geometry around each carbon:

      H   H
       \ /
        C
       / \
H—C      C—H
       \ /
        C
       / \
      H   H

Each carbon atom in butane is sp³ hybridized because they are each bonded to four other atoms (either C or H), resulting in a tetrahedral geometry around each carbon. The bond angles around each carbon atom are approximately 109.5 degrees.

In summary:

• Hybridization: Each carbon atom is sp³ hybridized.
• Bond angles: Approximately 109.5 degrees