[hsebast1]

SnH4 SbH3 or TeH2. i believe that  TeH2 is the strongest because it lost most of its H+ hence it disociates more than the others, am i rite

[csrscience.com]

These are all hydrides - AKA strong bases.

In this case the H isn't in the H+ oxidation state, but rather the H-, and it is the oxidizer AFAIK.

Sorry I can't help you more...

[Borek]

the H-, and it is the oxidizer

Quite the opposite. It has excess of electrons and gives one happily away.

[BluRay]

One of the strongest acid is a solution of antimony pentafluoride in fluosulphuric acid: SbF₅ + HSO₃F.

http://en.wikipedia.org/wiki/Super_acid

[csrscience.com]

"Quite the opposite. It has excess of electrons and gives one happily away."

So it loses electrons?

remember the saying OIL RIG?

Oxidation is lose[of electrons] Reduction is gain [of electrons].

We might be misinterpreting one another (I see I said it kind of confusingly and I'm pretty sure we are...my fault ) but the H- on a hydride is the equivalent of the O-2 on an oxide. So in order to form a hydride, Hydrogen acts like an oxidizer.


I've got this right, right?

[Borek]

No, H^- is a strong reducing agent. It gives its electrons (if you give something away, you no longer have it, hence loss - and OIL - H^- gets oxidized in the process) lowering oxidation state of other substance (other substance receives electrons, or gains them - RIG - gets reduced).

[BluRay]

"Quite the opposite. It has excess of electrons and gives one happily away."

So it loses electrons?

remember the saying OIL RIG?

Oxidation is lose[of electrons] Reduction is gain [of electrons].

We might be misinterpreting one another (I see I said it kind of confusingly and I'm pretty sure we are...my fault ) but the H- on a hydride is the equivalent of the O-2 on an oxide. So in order to form a hydride, Hydrogen acts like an oxidizer.


I've got this right, right?

To know if you are right or not, write the exact equation you want to discuss and specify *what kind* of hydrogen you are talking about.
Example 1: Zn + 2H⁺ --> Zn⁺⁺ + H₂
here H⁺ is the oxidant.

Example 2: H₂ + F₂ --> 2HF
here H₂ is the reducing.

Example 3: 2K + H₂ --> 2KH
here H₂ is the oxidant.

Example 4: H^- + H₂O --> H₂ + OH^-
here H^- is the reducing and water the oxidant.

...