Question

draw the most important lewis structure for the f₂o molecule and then assign formal charges to the o and f atoms.

Explanation:

Step1: Determine valence electrons

O has 6 valence electrons, each F has 7 valence electrons. Total valence electrons: \(6 + 2\times7=20\).

Step2: Draw Lewis structure

O is central atom. Each F forms single bond with O. After bonding, O has 2 lone pairs, each F has 3 lone pairs.

Step3: Calculate formal charge

Formal charge formula: \(FC = V - N - \frac{B}{2}\), where \(V\) is valence electrons, \(N\) is non - bonding electrons, \(B\) is bonding electrons.
For O: \(V = 6\), \(N = 4\), \(B = 4\). \(FC=6 - 4-\frac{4}{2}=0\).
For F: \(V = 7\), \(N = 6\), \(B = 2\). \(FC = 7-6-\frac{2}{2}=0\).

Answer:

Atom	Formal Charge
F	0