Given below are two statements
Statement I: The chlorides of Be and Al have Cl-bridged structure. Both are soluble in organic solvents and act as Lewis bases.
Statement II: Hydroxides of Be and Al dissolve in excess alkali to give beryllate and aluminate ions.
In the light of the above statements. Choose the correct answer from the options

We need to evaluate both statements about the diagonal relationship between Be and Al.

Statement I: "The chlorides of Be and Al have Cl-bridged structure. Both are soluble in organic solvents and act as Lewis bases."

Analysis of Statement I:

It is true that $$BeCl_2$$ and $$AlCl_3$$ both have chlorine-bridged structures. $$BeCl_2$$ has a polymeric chain with Cl bridges, and $$Al_2Cl_6$$ has a dimeric structure with Cl bridges.

It is also true that both are soluble in organic solvents due to their covalent character.

However, the statement says they act as Lewis bases. This is incorrect. Both $$BeCl_2$$ and $$AlCl_3$$ are electron-deficient species and act as Lewis acids (electron pair acceptors), not Lewis bases.

Therefore, Statement I is false.

Statement II: "Hydroxides of Be and Al dissolve in excess alkali to give beryllate and aluminate ions."

Analysis of Statement II:

Both $$Be(OH)_2$$ and $$Al(OH)_3$$ are amphoteric hydroxides. They dissolve in excess alkali (NaOH):

$$ Be(OH)_2 + 2NaOH \rightarrow Na_2[Be(OH)_4] \text{ (sodium beryllate)} $$

$$ Al(OH)_3 + NaOH \rightarrow Na[Al(OH)_4] \text{ (sodium aluminate)} $$

Therefore, Statement II is true.

Conclusion: Statement I is false but Statement II is true.

The correct answer is Option D: Statement I is false but Statement II is true.