[lutesium]

Why do we need a 1A group Metal to form Hydride type reducing agents?
To stabilize the molecule.
What type of Protons do they give?
Hydrides (H- => A Hydrogen with Two Electrons).
Does the Metal effect the reducing power of the Reagent?
Yes. As the Electropositivity of the Metal increases so does the Reducing Power of the Reagent. As CsAlH4 is stronger than LiAlH4.

Are these true???


Lutesium...

[sjb]

A couple of thoughts

• I believe you can get things like Ca(BH₄)₂
• I wouldn't call the type of hydrogen generated from these "protons"

Based on the first point, there must be some reason it's available, I'm not sure about relative strengths.

[g-bones]

Why do we need a 1A group Metal to form Hydride type reducing agents?
To stabilize the molecule.
What type of Protons do they give?
Hydrides (H- => A Hydrogen with Two Electrons).
Does the Metal effect the reducing power of the Reagent?
Yes. As the Electropositivity of the Metal increases so does the Reducing Power of the Reagent. As CsAlH4 is stronger than LiAlH4.

Are these true???


Lutesium...

-1A group metals act as the counter ions much like a salt since the metal takes on a negative character it is necessary to have a possitive counter ion.  Ex: sodium borohydride is BH4- and Na+

-yes, they do act as hydride donors, so not protons. its still hydrogen its just the number of electrons that comes with it changes from zero to two

-The electropositivity is most likely refering to the metal on which the hydrides are bound, not the counter ion.  That is why AlH4- is a more powerful reducing agent than BH4-.  The selection of the counter ion is more based on Lewis acidity,  the stronger the lewis acidity of the counter ion, the stronger it activates the carbonyl to be reduced, through cooridination.