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The scheme below summarizes the results from a study into the optimum conditions needed for a key step in the synthesis of the proposed structure of carambolaflavone, a natural product that has antidiabetic properties. Note that $\ce{Sc^3+}$ acts as a Lewis acid in these reactions.
I'm very confused about how the acid is coordinating to the Benzene derivative here?
@Waylander provided a correct written explanation for your question. I'll expand on his comments by considering the effect of temperature and provide diagrams.
Using M+ = Sc+3 to save some space, the Lewis acid coordinates with the more basic of the two acetate oxygens in 1 to provide the reactive oxonium species 2. [The oxonium species is planar about the double bond but I have left it in the chair conformation as a space-saving device.] This step may be reversible. At room temperature there is not sufficient activation energy to permit substitution of the aromatic ring. Following the red arrows of phenolic species 3, axial attack of the phenol oxygen occurs on the oxonium ion 2 to form, kinetically, compound 4. At 50 oC this reaction is reversible catalyzed by Sc+3 to reform 2 and 3 via the blue arrows. Following the green arrows, now there is sufficient energy to disrupt the aromaticity of 3 and allow for axial attack by carbon on the oxonium ion 2 to form, kinetically, structure 5. An increase of temperature to 70 oC permits coordination of the tetrahydropyran oxygen with the Lewis acid permitting ring opening, bond rotation about the red bond in 6 and ring closure of conformation 7 forming the thermodynamically stable, all equatorial tetrahydropyran ring of 8. [Structures 6 and 7 may also be drawn as benzyl cations with the carbonyl oxygen protonated.]
