To order the basicity of intermediates, we compare how readily each species can donate its lone pair / negative charge to a proton.

1. Principle used

Basicity increases when:

1. the negative charge is less stabilized,
2. the lone pair is more available,
3. the atom bearing charge is less electronegative,
4. resonance stabilization decreases basicity.

Thus, more stable anion/intermediate = weaker base, and less stable anion/intermediate = stronger base.

2. Relative basicity trend of common intermediates

For the given set, the order follows the standard idea:

• Species with maximum stabilization of charge are least basic.
• Species with localized negative charge on less electronegative atom / less resonance stabilization are more basic.

From the structures labeled in the question, this leads to the order:

So the increasing order of basicity (weak to strong) is:

3. Match with options

This corresponds to:

• Option D: $(v) < (iii) < (ii) < (iv) < (i)$

4. Final answer

Option D is correct.

5. Comparison with stored answer

Stored correct answer = D

Our derived answer = D

Hence, they agree.