Draw the Lewis dot structure for Mg and S. Is it an ionic or covalent bond?

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This is an ionic bond.  Magnesium, found in group 2, has 2 valence electrons and needs to release them to become stable.  Sulfur, found in group 16, has 6 valence electrons and takes two from magnesium to become stable.

I like to say, "Eight is Great," to help students remember that atoms need eight electrons in the valance (outer energy level) to be stable.

It could be shown as [Mg 2+]  [S 2-].  The Mg would have no dots, and the S would have 8 around it, two on each side, top, and bottom.  The dots would be drawn inside the brackets  around the symbols.  The 2+ and 2- should be smaller and towards the top.

Mg becomes more positive and the S becomes more negative because electrons are negatively charged.

 

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The Lewis dot structure for Magnesium is an Mg with 2 dots which stand for its two valence electrons.

The Lewis dot structure for Sulfur is an S with 6 dots which stand for its six valence electrons.

These two elements when bonded together form an ionic bond as the Magnesium loses its two valence electrons to the Sulfur atom.  Both atoms then have complete outer electron shells.  The Magnesium atom has a +2 charge and the Sulfur atom has a -2 charge.  This is what causes the attraction that bonds these two atoms.

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