Final answer:
To draw the complete structure of the azide ion, N3-, you need to account for the total of 16 valence electrons and arrange them in a linear skeleton structure, leading to two double bonds between the nitrogen atoms and a set of lone pair electrons on a terminal nitrogen. The ion has a charge of -1, indicated outside the brackets.
Step-by-step explanation:
The azide ion, N3-, consists of three nitrogen atoms linearly arranged. When drawing the complete structure for the azide ion, you will need to account for the fact that nitrogen has five valence electrons, so for three nitrogen atoms, you will have 15 valence electrons. Because it's an ion with a -1 charge, you add one more electron for a total of 16 valence electrons.
Start with a skeleton structure with a single bond between the nitrogen atoms. Nitrogen typically forms three bonds, so you can place additional bonds between the nitrogen atoms. Once you have two N-N double bonds, you will notice that there is one electron pair left, which can be placed as a lone pair on one of the terminal nitrogens.
However, the actual structure of azide is an average of multiple resonance structures. One of the terminal nitrogens will carry a negative charge distributing across the ion.
In summary, the electron dot structure of azide ion will have a linear arrangement with alternating single and double bonds between the nitrogen atoms and a set of lone pair electrons on one of the terminal nitrogens. The charge of -1 should be placed at the brackets surrounding the structure to denote it is an ion.