What will be the formula be if these ion's bond together?
Ag and I
the ag has a little plus symbol next to it and the I has a minus symbol next to it
Answers
They have the same number of electrons as protons, so the negative charges of the electrons is balanced by the positive charges of the protons. However, this is not always the case. Electrons can move from one atom to another; when they do, species with overall electric charges are formed. Such species are called ions. Species with overall positive charges are termed cations, while species with overall negative charges are called anions. Remember that ions are formed only when electrons move from one atom to another; a proton never moves from one atom to another. Compounds formed from positive and negative ions are called ionic compounds.
Individual atoms can gain or lose electrons. When they do, they become monatomic ions. When atoms gain or lose electrons, they usually gain or lose a characteristic number of electrons and so take on a characteristic overall charge. Table 3.6 “Monatomic Ions of Various Charges” lists some common ions in terms of how many electrons they lose (making cations) or gain (making anions). There are several things to notice about the ions in Table 3.6 “Monatomic Ions of Various Charges”. First, each element that forms cations is a metal, except for one (hydrogen), while each element that forms anions is a nonmetal. This is actually one of the chemical properties of metals and nonmetals: metals tend to form cations, while nonmetals tend to form anions. Second, most atoms form ions of a single characteristic charge. When sodium atoms form ions, they always form a 1+ charge, never a 2+ or 3+ or even 1− charge. Thus, if you commit the information in Table 3.6 “Monatomic Ions of Various Charges” to memory, you will always know what charges most atoms form. (In Chapter 9 “Chemical Bonds”, we will discuss why atoms form the charges they do.)
Table 3.6 Monatomic Ions of Various Charges
Ions formed by losing a single electron H+
Na+
K+
Rb+
Ag+
Au+
Ions formed by losing two electrons Mg2+
Ca2+
Sr2+
Fe2+
Co2+
Ni2+
Cu2+
Zn2+
Sn2+
Hg2+
Pb2+
Ions formed by losing three electrons Sc3+
Fe3+
Co3+
Ni3+
Au3+
Al3+
Cr3+
Ions formed by losing four electrons Ti4+
Sn4+
Pb4+
Ions formed by gaining a single electron F−
Cl−
Br−
I−
Ions formed by gaining two electrons O2−
S2−
Se2−
Ions formed by gaining three electrons N3−
P3−
Utilizing self-sacrificed transformation of the dual redox couples Ag/Ag+ and I−/(IO3)−, we developed a multiplex heterostructure Ag-AgI-AgIO3