Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For a molecule of fluorous acid, the atoms are arranged as HOFO.

What is the formal charge on each of the atoms?

Question

Jaydan Welch

Chemistry

25 August, 06:49

Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For a molecule of fluorous acid, the atoms are arranged as HOFO.

What is the formal charge on each of the atoms?

+1

Answers (1)

Know the Answer?

Karla Maxwell · Answer 1

The formal charge for H, O, F, O = 0,0, 1, - 1

Explanation:

The octet of electrons acquired by oxygen and fluorine atoms in this structure and the formal charges add to zero. Assigning of a formal charge + 1 to an electro-negative atom as fluorine indicates that a structure does not occur. Fluorine normally forms one oxyacid HOF.