Question

acetone (ch₃coch₃) ethanol (ch₃ch₂oh) lewis structure polar? y/n intermolecular forces

Explanation:

Step1: Draw Lewis structure of acetone

In acetone ($CH_3COCH_3$), the central carbon of the carbon - oxygen double - bond is bonded to two methyl ($CH_3$) groups. Carbon has 4 valence electrons, oxygen has 6. The Lewis structure has a carbon - oxygen double bond and single bonds between carbon and hydrogen atoms in the methyl groups.

Step2: Determine polarity of acetone

The carbon - oxygen double bond in acetone creates a dipole moment due to the electronegativity difference between carbon and oxygen. The molecule is polar (Y).

Step3: Identify intermolecular forces in acetone

The main intermolecular force in acetone is dipole - dipole interaction due to its polar nature, along with London dispersion forces which are present in all molecules.

Step4: Draw Lewis structure of ethanol

In ethanol ($CH_3CH_2OH$), there is a methyl group ($CH_3$), a methylene group ($CH_2$) and a hydroxyl group ($OH$). The oxygen in the hydroxyl group has two lone pairs of electrons.

Step5: Determine polarity of ethanol

The presence of the polar $O - H$ bond and the overall molecular geometry makes ethanol polar (Y).

Step6: Identify intermolecular forces in ethanol

Ethanol has hydrogen bonding due to the $O - H$ group, in addition to dipole - dipole interactions and London dispersion forces.

Answer:

	Acetone ($CH_3COCH_3$)	Ethanol ($CH_3CH_2OH$)
Polar? Y/N	Y	Y
Intermolecular Forces	Dipole - dipole, London dispersion	Hydrogen bonding, dipole - dipole, London dispersion