Final answer:
C-O bonds are polar and hydrophilic, so compounds containing C-O bonds can be soluble in water, whereas C-H bonds are typically non-polar and hydrophobic. C-O bonds do not have more potential energy than C-H bonds; it is generally the opposite. Finally, the C-O bond is polar, not non-polar as erroneously stated in one of the choices.
Step-by-step explanation:
Understanding the Solubility in Water and Polarity of Bonds
When considering the properties of the C-H and C-O bonds, it is important to recognize that the C-O bond is indeed polar because of the difference in electronegativity between carbon and oxygen. This polarity means that compounds with C-O bonds tend to be hydrophilic and can be soluble in water, as water is a polar solvent capable of forming hydrogen bonds with other polar molecules. On the other hand, C-H bonds are generally non-polar because the difference in electronegativity between carbon and hydrogen is not as great. Consequently, molecules with mostly C-H bonds do not mix well with water and are hydrophobic. Additionally, the potential energy of a bond is related to the bond strength and the difference in electronegativity; strong bonds with larger differences in electronegativity (like C-O) usually have lower potential energy compared to weaker bonds (like C-H).
To clarify the given options, molecules composed of mostly C-H or C-O could be soluble in water if they have significant polar character, particularly in the case of C-O. The statement that C-H bonds are hydrophilic at high pH is misleading; pH does not change the inherent polarity of a bond. Moreover, saying that molecules with C-H bonds will be able to interact with water and ones with C-O bonds will not is incorrect. Indeed, it is the C-O bond with its polar nature that can interact more readily with water. Lastly, the claim that the C-O bond is a non-polar covalent bond is incorrect as well because it is polar due to the difference in electronegativity between carbon and oxygen.