Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction:
FeO (s) + 2 HClO4 (aq) → Fe(ClO4) (aq) + H2O (l)
So here we're asked to figure out the net ionic equation for the following reaction, that means we're going to have to get the molecular equation then the total or complete ionic equation and then finally get our net ionic equation. So the equation here that they give to us is iron 2 oxide as a solid plus 2 moles of perchloric acid gives us iron 2 perchlorate plus water. Now remember, when we're doing the complete or total ionic we can only break up aqueous things. So this and this would break up and nothing else would.
So we get iron 2 oxide as a solid plus 2 H+ ions because the 2 gets distributed plus 2 perchlorates gives us FE2+ aqueous plus 2 perchlorates again plus water as a liquid. Now remember we get rid of the spectator ions, ions that look the same on both sides. In this case it'll be the perchlorate ion. Everything else comes down and that'll be our net ionic equation. So this is what we would have at the very end. We remove the spectator ions so my net ionic equation would be this here at the end.