When an element forms two or more ions how are the ions distinguished to indicate the charge?

Answer 1

An ion is different from its parent atom in the differing number of electrons. As the number of electrons goes up, the charge becomes more negative. Correspondingly, as the atom loses electrons, the net charge goes positive.

Answer 2

usually when a compound dissociates, one of the element may be more electronegative(1) and other may be less electro negative(2). hence (1) forms negative ion. but electron transfer is the only determining factor for the formation of charges. protons are immobile hence they are not involved in movement hoever they also contribute for the positiveness of an ion.

Answer 3

When an element has a variable oxidation state, it forms many compounds. For example, in the case of Sulfur, it forms ions such as SO42- and SO32- . Note the the oxidation numbers of Sulfur are 6+ and 4+ here. Now lets say we have 2 solutions containing these ions. There is a test to distinguish which solution has which ion. Add a solution of Barium nitrate, and a white precipitate will form in the solution which contains the SO42- . There will be no change if it is SO32- . For different substances, there are different methods to distinguish the oxidation number of different ions of the same element. In transition metals, such as Vanadium, we usually see the color of the solution to determine which oxidation number the vanadium ion has. V5+ has a yellow color, V4+ has a blue color, V3+ has a green color, and V2+ has a violet color. So there is no single specific method. You can use different ways for different elements.

Answer 4

The ions are distinguished by using Roman numerals in parentheses after the element's name. The Roman numeral indicates the charge of the ion formed by the element. For example, iron can form Fe(II) and Fe(III) ions to indicate charges +2 and +3, respectively.