lewis structures: complete the table\n| | water (h₂o) | hexane (ch₃ch₂ch₂ch₂ch₂ch₃) |\n|--|--|--| \n| lewis…

Explanation:

Step1: Determine Lewis structure of water

Oxygen has 6 valence - electrons and hydrogen has 1. In $H_2O$, oxygen is the central atom. It forms single bonds with two hydrogen atoms and has two lone - pairs of electrons. The Lewis structure is: H - O - H with two lone - pairs on oxygen.

Step2: Determine polarity of water

The electronegativity of oxygen is greater than that of hydrogen. The $O - H$ bonds are polar, and due to the bent molecular geometry, the bond dipoles do not cancel out. So, water is polar (Y).

Step3: Identify intermolecular forces in water

Water has hydrogen bonding (due to the $O - H$ bonds), dipole - dipole forces (because it is polar), and London dispersion forces (present in all molecules).

Step4: Determine Lewis structure of hexane

Hexane is a hydrocarbon. Each carbon atom has 4 valence - electrons and hydrogen has 1. Carbon atoms form single bonds with each other and with hydrogen atoms to satisfy the octet rule. The Lewis structure has a chain of six carbon atoms with appropriate number of hydrogen atoms attached to each carbon.

Step5: Determine polarity of hexane

Hexane is a non - polar molecule. The $C - C$ and $C - H$ bonds have very small electronegativity differences, and the molecule has a symmetrical structure. So, hexane is non - polar (N).

Step6: Identify intermolecular forces in hexane

Since hexane is non - polar, the only intermolecular forces present are London dispersion forces.

Answer:

	Water ($H_2O$)	Hexane ($CH_3CH_2CH_2CH_2CH_2CH_3$)
Lewis Structure	H - O - H with two lone - pairs on oxygen	Chain of six carbon atoms with appropriate hydrogen atoms attached to each carbon
Polar? Y/N	Y	N
Intermolecular Forces	Hydrogen bonding, dipole - dipole, London dispersion	London dispersion