Answer
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Step 1: Determine the total number of valence electrons in the molecule.
Nitrogen (N) is in the 15th group of the periodic table, so it has 5 valence electrons. Fluorine (F) is in the 17th group, so it has 7 valence electrons. There are 3 fluorine atoms in NF^3, so the total number of valence electrons in the molecule is: \text{Total valence electrons} = 5(\text{N}) + 3 imes 7(\text{F}) = 5 + 21 = 26
Step 2: Place the central atom and arrange the remaining atoms around it.
Nitrogen will be the central atom, and we will arrange the three fluorine atoms in a trigonal planar geometry since nitrogen forms three bonds in this molecule.
Final Answer
The Lewis structure for NF^3 is shown above, with a central nitrogen atom surrounded by three fluorine atoms in a trigonal planar geometry. The formal charges are shown next to each atom.
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