The lewis structure of Magnesium nitride places eight electrons around N. 3 of these electrons are provided by Mg to get a stable conformation.
What is the Lewis structure?
The Lewis structure is a representation of electron pairs in bonds between the atoms that compose the molecule. It can also show the solitary electron pairs that remain for each atom.
Electrons
When adding the valence electrons of each atom, we get the total number of electrons in the molecule.
The valence value is the number of electrons placed in the last energetic level of the atom.
The compound that forms between magnesium and nitrogen is magnesium nitride, Mg₃N₂. This is a simple salt with an ionic bond between a metal and a non-metal element.
What are the Metalic atoms?
They are elements that express a tendency to lose valence electrons to get a stable electronic configuration. When they lose electrons, they remain positively charged. These are cations with positive charges and lose the valence electrons of their last level.
Mg has 2 electrons in its last level, so to get a complete stable configuration (2e-), it needs to lose 2 electrons.
Mg has two positive charges Mg ²⁺
What are the non-metalic atoms?
They are elements that gain electrons to complete their last level. These are the anions. When they get electrons, they remain negatively charged.
Because Nitrogen has 5 electrons in its last level, it needs to add 3 electrons. In this way, it gets to the complete stable configuration (8e-).
N has three negative charges N³⁻
So, to complete the Lewis structure, we need to add Mg ²⁺ and N³⁻.
We know that
- N needs to add three electrons.
According to this, N needs more than one Mg to complete its last level.
So, in our calculations, we need to have three Mg and two N.
- Two N need six electrons (-3e- x 2 = -6e-) to complete their last level
- Three Mg can provide six electrons (+2e- x 3 = +6e-)
You will find the final Lewis structure in the attached files.
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