[trbngr]

I'm studying for a big chemistry exam, and i came across a question that confuses me. Basically i'm supposed to write the formula for dissolving zinc in hydrochloric acid. The answer says Zn(s) + 2H⁺(aq) -> Zn²⁺(aq) + 2H²(g), as if it's obvious that zinc would form a +2 ion. Since I'm not that good (or experienced) at chemistry, i don't know what ions specific d-block metals "usually" forms. I understand that the 4s orbital is higher in energy than the 3d orbital (when occupied) for most (all?) d-block metals, and this would explain why zinc, for example, is inclined to loose two electrons when forming an ion. I guess my question is this: does d-block metals always form ions that corresponds to stable electronic configuration (filled and half-filled shells) or does this only apply to some elements?

Sorry if this is all a little incoherent... my brain is a bit scrambled at the moment.

[Mitch]

Scrambled brains are fine. Transition elements are know to have an array of oxidation states. Zn and Cd are unique in that they will only form +2 in solution. There are some other ones you should know too like Au and Ag.

[weakling103]

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