NO3- Lewis Structure: How to Draw the Lewis Structure for NO3-

A step-by-step explanation of how to draw the NO3- Lewis Dot Structure (Nitrate ion).

For the NO3- structure use the periodic table to find the total number of valence electrons for the NO3- molecule. Once we know how many valence electrons there are in NO3- we can distribute them around the central atom with the goal of filling the outer shells of each atom.

In the Lewis structure of NO3- structure there are a total of 24 valence electrons. NO3- is also called Nitrate ion.

Also note that you should put the NO3- Lewis structure in brackets with as 1- on the outside to show that it is an ion with a negative one charge

Note that NO3- can have an Expanded Octet and have more than eight valence electrons. Because of this there may be several possible Lewis Structures. To arrive at the most favorable Lewis Structure we need to consider formal charges. See how to calculate formal charges:    • Formal Charges: Calculating Formal Ch...  

---- Steps to Write Lewis Structure for compounds like NO3 ------
1. Find the total valence electrons for the NO3- molecule.
2. Put the least electronegative atom in the center. Note: Hydrogen (H) always goes outside.
3. Put two electrons between atoms to form a chemical bond.
4. Complete octets on outside atoms.
5. If central atom does not have an octet, move electrons from outer atoms to form double or triple bonds.

---- Lewis Resources ----
• Lewis Structures Made Simple:    • How to Draw Lewis Structures: Five Ea...  
• More practice:    • Lewis Dot Structure Practice Problems...  
• Counting Valence Electrons:    • Finding the Number of Valence Electro...  
• Calculating Formal Charge:    • Formal Charges: Calculating Formal Ch...  
• Exceptions to the Octet Rule:    • Exceptions to the Octet Rule  

Lewis Structures, also called Electron Dot Structures, are important to learn because they help us understand how atoms and electrons are arranged in a molecule, such as Nitrate ion. This can help us determine the molecular geometry, how the molecule might react with other molecules, and some of the physical properties of the molecule (like boiling point and surface tension).

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