Magnesium reacts with a certain element to form a compound with the general formula MgX. What would the most likely formula be for the compound formed between 10 assum and element X? K_(2)X KX_(2) K_(2)X_(3) K_(2)X_(2)

The chemical formula indicates that magnesium (Mg) is combining with element X in a 1:1 ratio. Since magnesium typically has a +2 charge (as it is in group 2 of the periodic table and loses two electrons to achieve a noble gas configuration), we can infer that element X must have a -2 charge to balance the charge of magnesium in the compound .Now, considering the element potassium (K), which is in group 1 of the periodic table, it typically has a +1 charge because it loses one electron to achieve a noble gas configuration. To form a neutral compound with element X (which we have determined has a -2 charge), we would need two potassium ions to balance the -2 charge of a single X ion. This would result in a formula of , where the subscript 2 indicates that there are two potassium ions for every one ion of element X.Let's evaluate the given options:- : This formula shows two potassium ions for every one ion of element X, which is correct based on our charge balance reasoning.- : This formula suggests one potassium ion for every two ions of element X, which would not be charge balanced since potassium has a +1 charge and X has a -2 charge.- : This formula suggests two potassium ions for every three ions of element X, which would also not be charge balanced.- : This formula suggests two potassium ions for every two ions of element X, which would not be charge balanced either.