Which of the following metals (M) will form an ionic compound with nitrogen with the general formula M3N2? Hint: Think about how many positive charges you need to balance out the negative charges from nitrogen.

Metal elements from group 2 will make ionic bond with nitrogen.

Elements from group 2 will make ionic bond with nitrogen by complete transferring of electrons from metals to nitrogen atom. Three atoms of group 2 metals will provide 6 electrons which needed by the two nitrogen atoms.

Three positive charges are needed by the metal atom in order to balance the negative charges present on nitrogen atom because nitrogen has 5 electrons in its outermost shell and needs 3 more electrons to complete its outermost shell and become stable so we can conclude that for completing its outermost shell, nitrogen takes 3 electrons from 3 metal atoms.

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Explanation:

The question is incomplete but i will try to give you all the necessary guide that you need in order to answer the question.

When compounds are formed, atoms exchange valency. The valency of nitrogen is three while that of the metal is two. The exchange yields M3N2.

If the compound has been specifically mentioned to be a metal, then it must be a group two element. It could be any of Mg, Ca, Sr, Ba or Ra. I did not mention Be here because most of its compounds are covalent.

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> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.