Question

What is the hybridization of carbon in

Short answer

Answer: The carbon atoms in ethylene are sp^2 hybridized.

Step-by-step solution

Draw the Lewis structure of ethylene

To understand the bonding in ethylene, start by drawing its Lewis structure. Each carbon atom has four valence electrons, and each hydrogen atom has one valence electron. There are two carbon atoms and four hydrogen atoms in ethylene, so there are 12 valence electrons in total. 1. Place the two carbon atoms next to each other, and connect them with a double bond. The double bond consists of one sigma bond and one pi bond. 2. Arrange the four hydrogen atoms around the two carbon atoms, forming single bonds with each carbon atom. The Lewis structure should look like this: H H \ / C==C / \ H H

Determine the number of sigma bonds and lone pairs on each carbon atom

In ethylene, each carbon atom forms a sigma bond with two hydrogen atoms and one sigma bond with the other carbon atom (in addition to the pi bond). Since there are no lone pairs on the carbon atoms, each carbon atom forms three sigma bonds and has zero lone pairs.

Determine the hybridization of the carbon atoms in ethylene

The hybridization of an atom can be determined using the formula: Hybridization = number of sigma bonds + number of lone pairs For each carbon atom in ethylene: Hybridization = 3 sigma bonds + 0 lone pairs = 3 When the hybridization value is 3, the atom is sp^2 hybridized. Therefore, both carbon atoms in ethylene are sp^2 hybridized.