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Establish the Lewis Structure of NF 3

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F

N

F

F

- Step 1: N is less electronegative than F, therefore it goes in the center
- Step 2: Count the valence electrons: N has 5 (2s22p3), F has 7 (2s22p5). Total : 5 + (3x7) = 26 valence electrons.
- Step 3: Draw up single bonds between the N and each F atom, then complete the octet on each atom (add a pair on N and 3 pairs on each F)
- Step 4: Check the number of electrons in the stucture, it should equal the number of valence electrons: 6 in three single bonds, 2 on nitrogen, 6 on each fluorine, ie 6 + 2 + 6x3 = 26 used.