Final Answer:
The Lewis structure for nitrosyl fluoride (NOF) is:[Image B]
Step-by-step explanation:
To draw the Lewis structure for NOF, we need to first determine the number of valence electrons for each atom in the molecule. Nitrogen has five valence electrons, oxygen has six, and fluorine has seven.
First, we'll draw the atoms in the molecule and their bonds:
[Image A]
Next, we'll place the electrons in the molecule. Nitrogen has five valence electrons, so it has one electron in its outermost energy level. Oxygen has six valence electrons, so it has two electrons in its outermost energy level. Fluorine has seven valence electrons, so it has three electrons in its outermost energy level.
Now, we'll place the electrons in the bonds between the atoms. The nitrogen atom has one bond with the oxygen atom, which requires two electrons. So, we'll place two electrons in that bond. The oxygen atom has two bonds with the fluorine atoms, which require four electrons in total. We'll place four electrons in those bonds.
Finally, we'll place the remaining electrons in the molecule. Nitrogen has one electron left over, so we'll place that electron in the last energy level. Oxygen has two electrons left over, so we'll place those two electrons in the last energy level. Fluorine has three electrons left over, so we'll place those three electrons in the last energy level.
The final Lewis structure for NOF is:[Image B]