Copper is one example. There are several different types of copper so the name gives it away rather than needing to have the ions present.
Calcium
No element on its own has a charge. However, in all of its compounds sodium forms a positive ion.
Chlorine always forms ions of charge -1. However in its compounds, it also shows oxidation states of +1,+3,+5 and +7.
Type 1 binary ionic compounds are those in which the cation has only one form, or charge. Type 2 binary ionic compounds are those in which the cation can have multiple forms.
Carbon is the element that forms maximum number of compounds
Calcium
Calcium forms a 2+ ion.
Mg, magnesium forms compounds containing Mg2+ ion.
No element on its own has a charge. However, in all of its compounds sodium forms a positive ion.
Chlorine always forms ions of charge -1. However in its compounds, it also shows oxidation states of +1,+3,+5 and +7.
Type 1 binary ionic compounds are those in which the cation has only one form, or charge. Type 2 binary ionic compounds are those in which the cation can have multiple forms.
The charge that bromine forms in compounds is -1. This is because it is a type of halogen that takes electrons to fill its outer shell.
CaO. Calcium forms a +2 charge, and oxygen a -2 charge. They bond in a 1:1 ratio because ionic compounds combine in lowest terms.
Carbon is the element that forms maximum number of compounds
Its the electrons! Iodine forms a "charge transfer" complex with starch which is ythebest known of its charge transfer complexes. It also forms charge transfer compexes with other compounds which are not blue. In iodine the charge transfer occurs because of an electonic transition (that causes the color), this causes a small amount of charge to move from the iodine molecule to the starch.
The chlorine can be replaced in this case, and hence it forms various compounds.
The charge on individual ions when they form compounds is decreased or increased depending on if the ion needed or had too many electrons. I think....think that is the answer, so, get back to your textbook :)