Final answer:
The Lewis structure for ethanol involves a chain of two carbon atoms with a hydroxyl group attached, while dimethyl ether has two methyl groups attached to an oxygen atom. Both molecules exhibit tetrahedral geometry around carbon atoms, with bond angles close to 109.5°. The intermolecular forces present in ethanol result in a higher boiling point compared to dimethyl ether.
Step-by-step explanation:
Ethanol and Dimethyl Ether Lewis Structures and Molecular Geometry
To draw the Lewis structure for ethanol (C2H5OH), begin by arranging two carbon atoms in the center, connected by a single bond. Each carbon atom should further connect to three hydrogen atoms, with the first carbon also connecting to a hydroxyl group (OH). Ethanol has a tetrahedral geometry around each carbon atom, resulting in bond angles close to 109.5° due to the sp3 hybridization.
The Lewis structure for dimethyl ether (CH3OCH3) begins with an oxygen atom in the center, with two single bonds connecting to two methyl groups (CH3). The molecular geometry around the carbon atoms in dimethyl ether is also tetrahedral, with approximately 109.5° bond angles due to sp3 hybridization. However, the central oxygen atom exhibits a bent shape similar to a water molecule, with angles around 109.5°.
These structures are critical for understanding the properties of these molecules. For example, the presence of a hydroxyl group in ethanol allows for hydrogen bonding, leading to a higher boiling point compared to dimethyl ether, which only exhibits weak Van der Waals forces.