# Why are alkali metal compounds like sodium hydride or sodium amide strong bases but weak nucleophiles?

I understand why compounds such as $$\ce{NaH}$$ or $$\ce{NaNH2}$$ are weak nucleophiles: as they aren't very soluble in organic solvents, they react only on the clusters' surface. But why are they strong bases?

I could understand why they are in water, as they are soluble in water, but in my organic chemistry class it was said that they accelerate E2 reactions. So how can they be strong bases in organic solvents if they aren't soluble in organic solvents?

• Huh, you provide somewhat surprising reasoning. I'd be interested how valid it. Major problem is they aren't exactly "soluble" in water - while they "dissolve" they also react and that's driving the process forward. Another thing is that they aren't completely insoluble in organic solvents, at least in the ones they are actually used. – Mithoron Dec 11 '19 at 1:44