Specify the product of a combination reaction between magnesium metal, Mg(s), and gaseous fluorine, F2(g). (Omit states-of-matter from your answer.)
Write a balanced equation for this reaction. (Include states-of-matter under the given conditions in your answer.)

By telling us this is a "combination" reaction, we know that both reactants "combine" to form a larger compound. We also know magnesium (Mg) is a metal and is willing to give up electron(s). Fluorine (F) is a halogen that is willing to accept electron(s).

From the periodic table, we see that Mg is in Group 2. So it has 2 electrons in its outer shell - called the valence electrons. This means it has up to 2 electrons it can share or give. Fluorine is in Group 17, the halogens. Elements in this group want a single electron to complete their valence shells. One more electron will take F's valence electrons from 7 to 8, making it a full valence shell.

So we can predict that one Mg will react with 2 F atoms: MgF2. The two valence electrons from the 2 magnesium atoms are largely given/shared with the 2 fluorine atoms. Both elements are happy (a "metric" term for complete valence shells, a lower energy state).

So we can predict:

Mg + 2F = MgF2

Specify the product of a combination reaction between magnesium metal, Mg(s), and gaseous fluorine, F2(g). (Omit states-of-matter from your answer.) Write a balanced equation for this reaction. (Include states-of-matter under the given conditions in your answer.)

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Specify the product of a combination reaction between magnesium metal, Mg(s), and gaseous fluorine, F2(g). (Omit states-of-matter from your answer.)
Write a balanced equation for this reaction. (Include states-of-matter under the given conditions in your answer.)