Element X has the following valence electron configuration: [core]ns2np5. Element M has the following valence electron configuration: [core]ns2. What ionic compound would most likely result from the reaction between ions of M and X?

The kind of ionic compound formed is MX2.

Explanation:

Element X electron configuration is represented as [core] ns2np5. The group in the periodic table this element belong to is group 7A. The element group is called the halogen family. Element X cannot be stated specifically, because the number is represented with n. Element X will behave as an anions when it react with a metal (cations). Element X has a charge of - 1. The element X will gain electron when it bond with a metal. Element X is a non metal. Elements in this group are fluorine, chlorine, bromine, iodine, astatine, and tennessine. The element X have 7 valency electrons.

Element M electronic configuration is represented as [core]ns2. The group in the periodic table this element belong to is group 2A. The element group is called the alkaline earth metals family. Element M will behave as a cation when it bond with a non metal. Element M is a metal, therefore it will likely lose electron to form cations during bonding. The charge of element M is 2+. Element M is positively charged. Elements that belong to this group includes beryllium, magnesium, calcium, strontium, barium and radium. Element M has 2 valency electrons.

The reaction between this 2 ions will likely form an ionic compound. The element M is the cations while the element X is the anions. The element M will lose 2 electron while 2 atoms of element X will gain 2 electrons. Element M will lose 2 electron to attain a stable configuration while 2 atoms of element X will gain a single electron each to attain a stable configuration.

M² + and F-. This will form MX2 when you cross multiply the charge. The kind of ionic compound formed is MX2.