Two questions: why do ionic compounds have to be neutral
every compound has to be neutral (not just ionic), local positive or negative charges are always counterbalanced by its opposite to get neutrality in macroscopic compounds. A stable, charged substance just will not exist.
I know the reason they are is because the anion's charge=cation's charge, but why do they have to be the same?
if for example the cation is 2+ the anion can be 1-, but then there would be 2 anions per 1 cation in the eventual compound to have neutrality again.
how would it apply to covalent compounds (Can you swap valencies with covalent compounds, and, if so, why can you do that? Do the two valencies always -or at least as a general rule of thumb- have to be equal so that valency1-valency2=0?)
covalent bonds work differently, they do not have the valency ionic bonds do. here you apply the
octet rule. Every atom likes to be surrounded by 8 electrons. For example, oxygen has 6 of its own in its outer shell, so likes to get 2 more through bonds, thus, oxygen likes to form 2 bonds. Carbon has 4 electrons in its outer shell, thus, carbon likes to obtain 4 more through bonds.