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?
The charge on a fluorine ion is -1. This is because fluorine has 7 valence electrons, and it needs one more electron to complete its octet, giving it a negative charge.
Transition elements, also known as transition metals, are elements located in the middle of the periodic table. They have partially filled d orbitals and exhibit similar chemical properties, such as forming colored compounds and having multiple oxidation states.
The charge on a fluorine ion makes it highly reactive. This is because the negative charge makes it attract positively charged ions, allowing it to easily bond with other elements and form compounds.
Transition elements have multiple oxidation states due to the availability of electrons in their d orbitals. These electrons can be easily gained or lost to form different ions with varying charges, resulting in multiple oxidation states.
Fluorine is used in many industries, such as in the production of refrigerants, plastics, and pharmaceuticals. Transition elements have various uses, including as catalysts in chemical reactions, in electronics, and in the production of alloys.