One of the compounds in Figure P 10.16 is insoluble in water; the other has a water solubility o

step 1 Again, we need to draw the Lewis structures for the two compounds that are given in P10 .16. The

One of the compounds in Figure P 10.16 is insoluble in...

One of the compounds in Figure $\mathrm{P} 10.16$ is insoluble in water; the other has a water solubility of $0.87 \mathrm{g} / 100 \mathrm{mL}$ at $20^{\circ} \mathrm{C} .$ Identify which is which, and explain your reasoning.

Key Concepts

Like Dissolves Like Principle

The 'like dissolves like' principle states that polar solvents typically dissolve polar substances, while nonpolar solvents dissolve nonpolar substances. This concept is essential when predicting solubility, as it explains why more polar compounds are generally soluble in water, a polar solvent, whereas nonpolar compounds are not.

Polarity

Polarity refers to the uneven distribution of electrical charge within a molecule. Polar molecules have regions of partial positive and negative charge, which enable them to interact effectively with other polar substances like water. The degree of polarity in a molecule directly influences its water solubility.

Hydrogen Bonding

Hydrogen bonding is a specific type of dipole-dipole interaction that occurs when hydrogen is bonded to a highly electronegative atom such as oxygen or nitrogen. Molecules capable of hydrogen bonding with water tend to be more water-soluble because they can form stable, attractive interactions with water molecules.

Molecular Structure and Functional Groups

The presence and arrangement of functional groups within a molecule, such as hydroxyl, carboxyl, or amino groups, greatly affect its overall polarity. These groups can either enhance or diminish water solubility depending on whether they increase the molecule’s ability to interact with water via dipole interactions or hydrogen bonding.

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