Answer
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Work Step by Step
To describe the bonding in ethane (C2H6) and ethanol (C2H5OH) using the localized electron model, we can consider the following:
Ethane (C2H6):
In ethane, each carbon atom forms four single bonds - three C-H bonds and one C-C bond. The carbon atoms have a tetrahedral arrangement, with the bond angles close to 109.5 degrees. This is because the carbon atoms use sp3 hybridization, where the s orbital and three p orbitals combine to form four equivalent sp3 hybrid orbitals. These sp3 hybrid orbitals then participate in the formation of the C-H and C-C sigma (σ) bonds. The hydrogen atoms are also involved in the formation of these sigma bonds, contributing their 1s orbitals.
Ethanol (C2H5OH):
In ethanol, the carbon atoms also exhibit sp3 hybridization, similar to ethane. However, in ethanol, one of the hydrogen atoms on the second carbon is replaced by a hydroxyl (OH) group. The hydroxyl group is formed by the covalent bonding of the oxygen atom (which uses sp3 hybridization) and a hydrogen atom. The remaining three hydrogen atoms on the second carbon form C-H sigma bonds.
The localized electron model describes the bonding in ethane and ethanol as the formation of sigma bonds between the hybridized orbitals of the carbon and hydrogen atoms, as well as the formation of the sigma bond between the carbon and oxygen atoms in the hydroxyl group of ethanol.
