Organic compounds 2

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The structure of 1,3-butadiene shows the presence of two carbon-carbon double bonds. Load structure.

Hybrid orbitals

1. Inspecting that structure we can conclude that the following carbon atoms use sp³ hybrid orbitals in their bonding to other atoms:

	Wrong. A sp3 hybridization involves connections around a carbon atom. None of these atoms meet that condition because      the C = C double bond computed as one.
	Wrong. A sp3 hybridization involves connections around a carbon atom. None of these atoms meet that condition because      the C = C double bond computed as one.
	Right. None of the carbon atoms presents sp3 hybridization.

2. Inspecting that structure we can conclude that the following carbon atoms use sp² hybrid orbitals in their links to other atoms:

	Wrong. C1 y C4 atoms present sp2 hybridization but they are not the only ones.
	Wrong. C2 y C3 atoms present sp2 hybridization but they are not the only ones.
	Right. The four carbon atoms present sp2 hybridization.

3. The double bond between carbon atoms in addition to a sigma bond Csp²-Csp² there is:

One additional C-C sigma bond	Wrong. You can not have two sigma bonds between two carbon atoms.
One π bond in addition to a σ bond.	Right. The σ portion of the bond is located in the internuclear area, while the π portion is located on top of this axis. The π bond.. See the smaller overlap of the π lobes.

4. A single bond and a double bond are different because single bond is:

	Not right. The single bond, or σ bond, is stronger than a π bond. However a single bond is weaker than a double bond that has two contributors, one σ and one π contributions.
	Right. The stronger is the bond the shorter is. The single bond is weaker and longer than a double bond.