Transition elements are unique in their ability to form ions with multiple charges due to their d-orbitals, which allow for variable oxidation states. While fluorine typically forms a -1 anion as fluoride, it is important to note that other elements, including main group elements like tin and sulfur, can exhibit multiple oxidation states. For instance, tin can form both ##\mathrm{Sn^{2+}}## and ##\mathrm{Sn^{4+}}## ions, and sulfur can range from -2 to +6. The peroxide ion ##\mathrm{O_2^{2-}}## demonstrates that even oxygen can have different charge states under specific conditions.
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Who said so? Most main group elements can have several oxidation states, e.g. tin forms both ##\mathrm{Sn^{2+}}## and ##\mathrm{Sn^{4+}}## ions. It is true that fluorine and oxygen mostly form ions with charge -1 and -2, respectively, however, even for oxygen, there are other possibilities, like the peroxide ion ##\mathrm{O_2^{2-}}## where each oxygen only bears one negative charge. Elements like sulfur come in a wealth of oxidation states ranging from -2 to +6.Murtuza Tipu said:Why can't elements other than transition elements form ions with different charges?