D-Glucose Functional Group Analysis

Step 1: Understanding the structure of D-glucose

D-glucose exists in two structural forms:

1. Open-chain form: The open-chain structure of D-glucose contains one aldehyde (-CHO) functional group and five hydroxyl (-OH) groups attached to the carbon atoms.
2. Cyclic (ring) form: When D-glucose undergoes cyclization to form a pyranose ring (as in the Haworth projection), the aldehyde group reacts with one of the hydroxyl groups to form a hemiacetal, resulting in the formation of a six-membered ring. In this form, the number of hydroxyl groups remains five.

Step 2: Identifying the correct answer

• In the open-chain form, there are five hydroxyl (-OH) groups.
• In the ring form, there are still five hydroxyl (-OH) groups (since the aldehyde group forms a hemiacetal but does not contribute an additional hydroxyl group).

Conclusion:

Thus, the correct answer is: (B) 5, 5

Paramagnetism of Cobalt Complexes Analysis

The paramagnetism of a complex is determined by the presence of unpaired electrons. For the given complexes:

• In , Co is in a +3 oxidation state (Co³⁺), which has a configuration, leading to fewer unpaired electrons and lower paramagnetism.
• In , Co is in a +2 oxidation state (Co²⁺), which has a configuration, allowing for more unpaired electrons and higher paramagnetism.
• In , Co is in a +2 oxidation state (Co²⁺), again with a configuration, which is paramagnetic but not as much as the next complex.
• In , Co is in a +3 oxidation state (Co³⁺), which leads to a configuration. The water ligands are weak field ligands, so the electrons do not pair up, resulting in the maximum number of unpaired electrons and the highest paramagnetism.

Conclusion:

Therefore, the complex is the most paramagnetic.

Note: There seems to be a contradiction within the provided reasoning. A configuration, in a *strong field* environment, leads to all electrons paired and *diamagnetism*. A weak field would have unpaired electrons and be *paramagnetic*. This needs careful checking against spectrochemical series and ligand field theory. The initial claim that [Co(H2O)6]3+ has *maximum* unpaired electrons needs rigorous justification.