Groups 1 & 2 and 6 & 7 are the Most Likely to Form Ions
The elements that most readily form ions are those in Group 1,2,6 and 7
Group 1 and 2 elements are metals and they lose elections to form positive ions (cations)
Group 6 and 7 elements are non-metals. They gain electrons to form negative ions (anions)
Elements in the same group all have the same number of outer electrons. So they have to lose or gain the same number to get a full outer shell. And this means that they form ions with the same charges
A sodium atom (Na) is in Group 1, so it will lose 1 electron. Na → Na+ + e-. It will have the same electronic structure as neon
A magnesium atom (Mg) is in Group 2, so it will lose 2 electrons. Mg → Mg2+ + 2e-. It will have the same electronic structure as neon
A chlorine atom (Cl) is in Group 7, so it will gain 1 electron. Cl + e- →Cl-. It will have the same electronic structure as argon
An oxygen atom (O) is in Group 6 so it will gain 2 electrons. O + 2e- → O2-. It will have the same electronic structure as neon
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