based on their lewis diagrams, which of the following pairs of liquids are most soluble in each other? a b c d

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# Brief Explanations:
- **Option A**:
    - The first molecule is ethanol ($CH_3CH_2OH$). It has a hydroxyl ($-OH$) group which can form hydrogen bonds with water ($H_2O$).
    - Water also has $O - H$ bonds and can form hydrogen bonds. According to the "like - dissolves - like" principle (substances with similar intermolecular forces are soluble in each other), both ethanol and water can form hydrogen bonds (a type of strong dipole - dipole interaction).
- **Option B**:
    - Carbon tetrachloride ($CCl_4$) is a non - polar molecule (symmetrical tetrahedral structure, the bond dipoles cancel out).
    - Water ($H_2O$) is a polar molecule. Non - polar and polar substances do not mix well as their intermolecular forces are different (non - polar has London dispersion forces and polar has dipole - dipole and hydrogen bonding in the case of water).
- **Option C**:
    - Methanol ($CH_3OH$) is polar (due to the $O - H$ and $C - O$ bonds) and pentane ($C_5H_{12}$) is non - polar (hydrocarbon, symmetrical enough for the bond dipoles to cancel out to a large extent). Polar and non - polar substances do not have similar intermolecular forces for good solubility.
- **Option D**:
    - Methanol ($CH_3OH$) is polar and hexane ($C_6H_{14}$) is non - polar.  Polar and non - polar substances do not dissolve well in each other as their intermolecular forces (dipole - dipole for methanol and London dispersion for hexane) are not similar.

# Answer:
A. $CH_3CH_2OH$ and $H_2O$

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