Final answer:
Without a specific molecular context in the question, it's generally true that hydrogens close to electronegative atoms, such as in a carbon-oxygen double bond, are more deshielded due to the withdrawal of electron density, while those farther from such influences are more shielded.
Step-by-step explanation:
The hydrogens connected to the carbon-carbon double bond can be described as being either shielded or deshielded based on the electron density around them and the presence of electronegative atoms. Since the question does not provide a detailed molecular context for the hydrogens in relation to other substituents and their exact positions, we have to consider general principles. In most cases, hydrogens that are closer to electronegative atoms or groups, such as a carbon-oxygen double bond, are more deshielded due to the electronegative atom drawing electron density away from the hydrogen. Conversely, hydrogens that are farther away from such withdrawing groups would be more shielded.
Based on the interaction with electronegative atoms, hydrogen atoms adjacent to carbons with double bonds to more electronegative atoms (like oxygen in the described carbon-to-oxygen double bond from the reference material) will generally be more deshielded than those attached to carbons without such electroattractive influences. However, the exact nature of the deshielding or shielding effect could vary, depending on the rest of the molecular structure and the relative positioning of other functional groups or atoms.