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 the total number of valence electrons

O has 6 valence electrons, and each F has 7 valence electrons. So for \(F_2O\), the total number of valence electrons is \(6 + 2\times7=20\).

Step2: Draw the Lewis structure

O is the central atom. Each F forms a single - bond with O. After forming two single bonds (using 4 electrons), 16 electrons are left. These 16 electrons are distributed as lone pairs: O has 2 lone pairs (\(2\times2 = 4\) electrons) and each F has 3 lone pairs (\(2\times3\times2= 12\) electrons). The Lewis structure is \(F - O - F\) with appropriate lone pairs.

Step3: Calculate the formal charge

The formula for formal charge is \(FC=V - N-\frac{B}{2}\), where \(V\) is the number of valence electrons in the free atom, \(N\) is the number of non - bonding electrons, and \(B\) is the number of bonding electrons.

• For O: \(V = 6\), \(N=4\), \(B = 4\). Then \(FC=6-4-\frac{4}{2}=0\).
• For F: \(V = 7\), \(N = 6\), \(B = 2\). Then \(FC=7 - 6-\frac{2}{2}=0\).

Answer:

The formal charge of O is \(0\) and the formal charge of F is \(0\).