Do not skip or try to rearrange any step during your learning process, as it is important to understand and implement each step to correctly design these structures. Place the last 2 electrons as a lone pair on the oxygen, and now it has 8 electrons in its outer energy level. Phosphorus has 5 valence electrons so like nitrogen it is also very happy with zero formal charge on it. For every covalent bond, an atom gives one electron so number of bonds around each atom will give the number of electrons used in making covalent bonds. Let’s practice step one “count the total valence electrons’ on molecules and polyatomic ions. Covalent bonds share electrons and generally occur between 2 nonmetals. This structure is wrong because N cannot have more than 8 electrons around it .In the above structure we have made 6 bonds around Nitrogen means 6*2 (2 electrons in each bond) =12 electrons .Now we need to replace two of the double bonds of the oxygen atom with nitrogen into single bond .To complete the octet of these oxygen, we need to put one extra lone pair on each of them and in the structure you can see two singly bonded oxygen atoms with three lone pairs. COMPLETE THE OCTET OF THE MOST  ELECTRONEGATIVE ATOM  WITH MINIMUM FORMAL CHARGES. {"smallUrl":"https:\/\/www.wikihow.com\/images\/thumb\/3\/30\/Draw-Lewis-Dot-Structures-Step-1-Version-4.jpg\/v4-460px-Draw-Lewis-Dot-Structures-Step-1-Version-4.jpg","bigUrl":"\/images\/thumb\/3\/30\/Draw-Lewis-Dot-Structures-Step-1-Version-4.jpg\/aid2387611-v4-728px-Draw-Lewis-Dot-Structures-Step-1-Version-4.jpg","smallWidth":460,"smallHeight":306,"bigWidth":728,"bigHeight":485,"licensing":"

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